KEY FinalExamStudyGuide Fall2013
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Leaming-Focused® Notebook©2005 Learning Concepts Student Learning Map Unit Topic: How do scientists study Chemistry? Instructional Tools Key Learning(s): A. Scientific Community Chemical Changes Lab B. Quantifying and measuring matter. Island of Rapone Dimensional Analysis Game Unit Essential Questions: A. What is the difference between observation and interpretation? Density Demonstration B. How are scientific measurements calculated accurately? C. What is matter? Concept: Concept: Concept: Concept: Scientific Method SI System Significant Figures Matter Lesson EQ: Lesson EQ: Lesson EQ: Lesson EQ: How is the scientific method used? What is the SI system? List four steps for solving problems. What are the parts of the scientific method? What are the units of the SI system? What is uncertainty? What are physical properties and changes? How does the scientific community communicate? How are units converted in the SI system? What is a significant figure? What are chemical properties and changes? How are significant figures used in calculations? What is density? How do variables affect an observed result? How is matter classified? Explain the difference between a substance and a mixture? Vocabulary: Vocabulary: Vocabulary: Vocabulary: Scientific method (parts) Prefix Accuracy Mass Theory Base unit Precision Volume Law Derived unit Uncertainty Density Observation Conversion factors Significant digit Matter Interpretation Dimensional Analysis Percent Error Mixture Scientific Notation Filtration/Distillation Variable and Control Reproduction of this page for classroom and planning use by owner of this book is permitted. 05_Chem_GRSW_Ch02.SE/TE 6/11/04 3:27 PM Page 11 Name ___________________________ 2 Date ___________________ Class __________________ MATTER AND CHANGE SECTION 2.1 PROPERTIES OF MATTER (pages 39–42) This section helps you distinguish extensive from intensive properties and identify substances by their properties. It teaches you how to differentiate the three states of matter. It also defines a physical property and lists examples of physical properties and physical changes. Describing Matter (page 39) mass 1. The ______________________ of an object is a measure of the amount of matter the object contains. 2. How does an extensive property differ from an intensive property? An extensive property depends on the amount of matter, while an intensive property depends on the type of matter. Identifying Substances (page 40) 3. Matter that has a uniform and definite composition is called a substance ______________________ . © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 4. Is the following sentence true or false? All samples of a substance have false different physical properties. ______________________ 5. A physical property is a quality or condition of a substance that can be observed measured ______________________ or ______________________ without changing the substance’s composition. 6. Circle the letter of the term that is NOT a physical property. a. hardness c. boiling point b. color d. melting 7°C 7. Look at Table 2.1 on page 40. What is the melting point of bromine? ______ 8. Look at Table 2.1 on page 40. Circle the letter of the substance that is a yellow solid and melts at 115°C. a. sulfur b. chlorine c. gold d. copper Chapter 2 Matter and Change 11 05_Chem_GRSW_Ch02.SE/TE 6/11/04 3:27 PM Page 12 Name ___________________________ Date ___________________ Class __________________ CHAPTER 2, Matter and Change (continued) 9. Is the following sentence true or false? Physical properties can help a chemist true identify a substance. ______________________ States of Matter (pages 41–42) 10. Circle the letter of the term that is NOT a physical state of matter. a. water b. gas c. liquid d. solid 11. Complete the table about properties of three states of matter. Use these terms: definite, indefinite, easily, and not easily. Properties of the States of Matter Property Liquid Gas or Vapor Shape definite indefinite indefinite Volume definite definite indefinite Can be compressed not easily not easily easily 12. Match each arrangement of the particles in matter with a physical state. Physical State Arrangement c ______ gas a. packed tightly together b ______ liquid b. close, but free to flow a ______ solid c. spaced relatively far apart 13. Is the following sentence true or false? The words gas and vapor can be used false interchangeably. ______________________ 14. The term gas is limited to those substances that exist in the gaseous state at room temperature ______________________ . 12 Guided Reading and Study Workbook © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Solid Physical Changes (page 42) 16. phase Chapter 2 Matter and Change 13 . cut. ______________________ 4. 1. What is true about all physical changes that involve a change of state? They are all reversible. melt.2 MIXTURES (pages 44–47) This section explains how to classify a mixture as heterogeneous or homogeneous. Circle the letter of the term that describes a part of a sample with uniform composition and properties. What are some words that describe physical changes? boil.. and crush 18. publishing as Pearson Prentice Hall. split. dissolve. grind.05_Chem_GRSW_Ch02. true ______________________ 2. Inc. a. All rights reserved. freeze. break. What is another name for a homogeneous mixture? a solution ______________________ 5. crack. condense. 3.SE/TE 6/11/04 3:27 PM Page 13 Name ___________________________ Date ___________________ Class __________________ 15. mixture c. A physical change alters a given material without changing its chemical composition ______________________ . solution b. Is the following sentence true or false? A heterogeneous mixture is one that false has a completely uniform composition. Is the following sentence true or false? Most samples of matter are mixtures. It also describes ways to separate mixtures. 17. ____________________________________________________________________________ SECTION 2. Classifying Mixtures (pages 44–45) © Pearson Education. state d. What does vapor describe? Vapor describes the gaseous state of a substance that is generally a liquid or solid at room temperature. What is a mixture? A mixture is a physical blend of two or more components. distilled water . tap water D Distillation flask B C Cold water in Receiver flask E 14 Guided Reading and Study Workbook © Pearson Education.05_Chem_GRSW_Ch02. The process that separates a solid from a liquid in a heterogeneous mixture is filtration called ______________________ . Match each term with its location in the diagram. condenser A C ______ 16.. publishing as Pearson Prentice Hall. E ______ 19. what is used to separate mixtures? differences in physical properties 8. 9. Inc. Homogeneous ______________________ two or more b. In general. What happens during a distillation? A liquid is boiled to produce a vapor that is then condensed into a liquid. D ______ 15.SE/TE 6/11/04 3:27 PM Page 14 Name ___________________________ Date ___________________ Class __________________ CHAPTER 2. All rights reserved. Matter and Change (continued) 6. Heterogeneous ______________________ Separating Mixtures (pages 46–47) 7. heat source Cold water out A ______ 17. How many phases exist in these types of mixtures? one a. thermometer B ______ 18. What are the two groups into which substances can be classified? Substances can be classified are elements and compounds. Compounds are substances that can be separated into simpler substances chemical only by ______________________ means. All rights reserved. If the composition of a sample is fixed. Distinguishing Substances and Mixtures (page 50) 7. which is a pale yellow gas ______________________ . Inc. SECTION 2.SE/TE 6/11/04 3:27 PM Page 15 Name ___________________________ Date ___________________ Class __________________ Reading Skill Practice By looking carefully at photographs and drawings in textbooks. 5.. false simpler substances. What important idea does this drawing communicate? This drawing shows that the components of a mixture can be separated based on differences in their physical properties. Distinguishing Elements and Compounds (pages 48–49) 1. publishing as Pearson Prentice Hall. All living and nonliving things are made up of building blocks called elements ______________________ . It also summarizes the process for classifying substances and mixtures.3 ELEMENTS AND COMPOUNDS (pages 48–52) This section explains a key difference between an element and a compound. you can better understand what you have read. 2.8 on page 44. Look carefully at Figure 2. Complete this sentence. and chlorine. ______________________ 6. Describe one way to decide whether a sample of matter is a substance or a mixture. which metal is a soft ______________________ . the sample is a mixture. Is the following sentence true or false? Elements can be easily separated into © Pearson Education.05_Chem_GRSW_Ch02. Is the following sentence true or false? The properties of compounds are true different from those of their component elements. compound Sodium chloride (table salt) is a ______________________ of sodium. and describes how chemical symbols and formulas are used to represent elements and compounds. ______________________ 4. the sample is a substance. Chapter 2 Matter and Change 15 . If the composition of a sample may vary. 3. publishing as Pearson Prentice Hall. What are chemical symbols used for? Chemical symbols are used to write the chemical formulas of compounds. ______________________ 16 Guided Reading and Study Workbook Uniform. Compound __________ (Examples: water. sodium chloride) d. 11.or two-letter chemical symbol.05_Chem_GRSW_Ch02. Element __________ (Examples: carbon. Symbols and Formulas (pages 51–52) Homogeneous __________ . Matter and Change (continued) 8. Heterogeneous f. Matter _________ Can be separated physically Substance _________ Definite composition (homogeneous) Mixture of substances Variable composition Can be separated chemically c. Inc. distinct phases 9. also called a solution © Pearson Education. oxygen) __________ e. a. 12. Is the following sentence true or false? The elements that make up a compound are always present in the same true proportions. Nonuniform. All rights reserved. b.. What is used to represent an element? An element is represented by a one. 10.SE/TE 6/11/04 3:27 PM Page 16 Name ____________________________________ Date __________ Class ___________________ CHAPTER 2. Complete the labels in the diagram below. hydrogen. Subscripts in chemical formulas are used to indicate the relative proportions compound of the elements in the ______________________ . sometimes b. Is the following sentence true or false? Chemical properties are observed only true when a substance undergoes a chemical change. ______________________ 3. rarely c. Chemical Changes (page 53) 1. Use Table 2. never 6. 5. In chemical reactions. 2.05_Chem_GRSW_Ch02. It also teaches the law of conservation of mass. A change in the composition of matter _______ occurs during a chemical reaction. Circle the letter of the term that best completes the sentence.. What is the symbol for gold? ______________________ antimony c. Which representation of a chemical reaction is correct? a. always d. Stibium is the Latin name for which element? ______________________ SECTION 2. lead a. reactants ➞ products Chapter 2 Matter and Change 17 . the substances present at the start of the reaction are reactants called ______________________ and the substances produced are products called ______________________ . Inc.SE/TE 6/11/04 3:27 PM Page 17 Name ____________________________________ Date __________ Class ___________________ 13.4 CHEMICAL REACTIONS (pages 53–55) This section provides clues to help you recognize a chemical change. products ➞ reactants b. Pb is the symbol for what element? ______________________ Au b. All rights reserved.2 on page 52 to answer the following questions. What is a chemical property? A chemical property is the ability of a substance to undergo a specific chemical change. What happens during a chemical reaction? One or more substances change into one or more new substances. 4. © Pearson Education. publishing as Pearson Prentice Hall. a. The mass of the product is the same as the mass of the reactants. mass is neither ______________________ nor destroyed ______________________ . 12.05_Chem_GRSW_Ch02. Matter and Change (continued) Recognizing Chemical Changes (page 54) 7.15 on page 55. false you can be certain that a chemical change has taken place. Inc.SE/TE 6/11/04 3:27 PM Page 18 Name ___________________________ Date ___________________ Class __________________ CHAPTER 2.. ______________ 9. publishing as Pearson Prentice Hall. The law of conservation of mass states that in any physical change or created chemical reaction. Look at Figure 2. or the formation of a precipitate 8. During a chemical reaction. A precipitate is a solid that forms and settles out of a liquid mixture. Is the following statement true or false? If you observe a clue for chemical change. 11. Conservation of Mass (page 55) 10. a change in color. the mass of the products is always equal to reactants the mass of the ______________________ . How do you know that mass was conserved? 18 Guided Reading and Study Workbook © Pearson Education. ____________________________________________________________________________________ . List the four possible clues to a chemical change? transfer of energy. the production of a gas. All rights reserved. Define a precipitate. 000 is written correctly in scientific notation. and Error (pages 64–65) 4. Using and Expressing Measurements (page 63) 1. 5. 503 million Accuracy. b. and error in measurements. Is the following sentence true or false? To decide whether a measurement has good precision or poor precision. © Pearson Education. publishing as Pearson Prentice Hall. the measurement must be made more than true once. d. All rights reserved. The coefficient is always a number greater than or equal to one and less than ten.03 108 d. 503 106 c. the exponent is positive. a. Writing out all the zeros in such numbers can be very cumbersome. precision.000. Scientific notation makes it easier to work with these numbers. 5. The power of 10 is called the exponent. a.05_Chem_GRSW_Ch03. Precision.03 10–7 b. For numbers less than one.SE/TE 6/11/04 3:29 PM Page 19 Name ___________________________ 3 Date ___________________ Class __________________ SCIENTIFIC MEASUREMENT SECTION 3. c. ______________________ Chapter 3 Scientific Measurement 19 . A number expressed in scientific notation is written as the product of a coefficient and a power of 10. Circle the letter of each sentence that is true about numbers expressed in scientific notation. Inc..1 MEASUREMENTS AND THEIR UNCERTAINTY (pages 63–72) This section describes the concepts of accuracy. 2. Circle the letter of the answer in which 503. Why are numbers used in chemistry often expressed in scientific notation? Numbers used in chemical calculations are often very large or very small. 3. It also explains the proper use of significant figures in measurements and calculations. Eight measurements were spread over a wide range. 9. 13. 11. All rights reserved. A __________ 7. P __________ 5. and the fifth varied from the others in value by less than 1%. darts that are closest to the bull’s-eye have been thrown with the greatest accuracy. draw three darts to represent three tosses of lower precision. Four of five repetitions of a measurement were numerically identical. Is the following sentence true or false? The value of an error must be false positive. 8. 2% c. and the experimental value is 198 cm. Inc. For an experimental measurement. On the second target. On a dartboard. the error experimental value minus the accepted value is called the _________________ . 2% b. First target Second target The accepted value is the correct value based on reliable references.05_Chem_GRSW_Ch03. What is the meaning of “accepted value” with respect to an experimental measurement? . publishing as Pearson Prentice Hall.SE/TE 6/11/04 3:29 PM Page 20 Name ___________________________ Date ___________________ Class __________________ CHAPTER 3. 10. 1% 20 Guided Reading and Study Workbook © Pearson Education. Scientific Measurement (continued) Label each of the three following sentences that describes accuracy with an A. Complete the following sentence. Relative error is also called _____________________________ . _________________ percent error 12.. Circle the letter of the value that shows the percent error of this measurement. The accepted value of a length measurement is 200 cm. Label each sentence that describes precision with a P. 1% d. A single measurement is within 1% of the correct value. but higher accuracy than the darts on the first target. a. P __________ 6. Zeros to the left of the decimal point that act as placeholders for the first nonzero digit to the left of the decimal point are not significant. Inc. In the measurement 43. 4 c. All rightmost zeros to the right of the decimal point are always significant. a. 3 d. 3 d. b. Is the following sentence true or false? An answer is as precise as the most false precise measurement from which it was calculated.SE/TE 6/11/04 3:29 PM Page 21 Name ___________________________ Date ___________________ Class __________________ Significant Figures in Measurements (pages 66–67) 14.145 meters to 4 significant figures. a. © Pearson Education. If a thermometer is calibrated to the nearest degree. Leftmost zeros acting as placeholders in front of nonzero digits in numbers less than one are not significant. 4 b.15 meters 20. ______________________ 100°C 21. Every nonzero digit in a reported measurement is assumed to be significant..05_Chem_GRSW_Ch03. 2 c. Round 65. which digit is the most uncertain? a. ______________________ Chapter 3 Scientific Measurement 21 . a. Circle the letter of each sentence that is true about significant figures. When the measurement involves exactly defined quantities. c. 18.80 m. Circle the letter of the correct number of significant figures in the measurement 6. 65. Zeros appearing between nonzero digits are never significant. d. 2 16. e.1°C to 1 significant figure. 5 b. All rights reserved. When the measurement involves counting. b. Circle the letter of the correct digit. to what part of a degree one tenth of a degree can you estimate the temperature it measures? ____________________________ 15.52 cm. ______________________ Round the following measurements as indicated. publishing as Pearson Prentice Hall. Significant Figures in Calculations (pages 68–71) 19. 5 17. List two situations in which measurements have an unlimited number of significant figures. Round 100. Round 155 cm to two significant figures. publishing as Pearson Prentice Hall. Units and Quantities (pages 74–79) 1. Scientific Measurement (continued) 160 cm 22.” Derived units are combinations of base units. ______________________ 65. 22 Guided Reading and Study Workbook © Pearson Education. The International System of Units (SI) is a revised version of the metric system ______________________ .SE/TE 6/11/04 3:29 PM Page 22 Name ___________________________ Date ___________________ Class __________________ CHAPTER 3. Inc. or are derived from base units. or speed. Round 65. Round 0. ______________________ SECTION 3.1 meters 24. All metric units of length are based on multiples of _______ 3. temperature. All SI units are base units. All rights reserved. Possible responses are units of volume. and energy in the International System of Units (SI). Complete the table showing selected SI base units of measurement.. Time SI base unit . Units of Measurement Quantity Length Mass Temperature Symbol meter m kilogram kg kelvin K second s 10 . 4. Explain what is meant by a “derived unit. Students’ responses will vary. 2.145 meters to three significant figures.05_Chem_GRSW_Ch03. 5.000 718 kilograms to two significant figures. ______________________ 0. volume. density.00072 kilograms 23. Give at least one example of a derived unit.2 THE INTERNATIONAL SYSTEM OF UNITS (pages 73–79) This section defines units of measurement for length. mass. b _______ 7. A box of cookies b. The SI unit for volume is derived from the meter. The liter is an SI unit.SE/TE 6/11/04 3:29 PM Page 23 Name ___________________________ Date ___________________ Class __________________ 6. 1 m a _______ 9. Example Unit of Volume b _______ 13. the SI unit for length. Circle the letter of each sentence that is true about units of volume. There are 1000 cm3 in 1 L. Match each of the three descriptions of a volume to the appropriate metric unit of volume. Thickness of about 10 sheets of paper b. 1 mm © Pearson Education. 1 km d _______ 8. Metric Units of Length Unit Symbol Factor Multiplying Base Unit Meter m 1 Kilometer km 1000 Centimeter cm 102 Millimeter mm 103 Nanometer nm 109 Match each metric unit with the best estimate of its length or distance. 1 m3 c _______ 15.05_Chem_GRSW_Ch03. Distance along a road spanning about 10 telephone poles c. The space occupied by any sample of matter is called its ___________________ . b. Inc. The liter (L) is a unit of volume. and there are also 1000 mL in 1 L. 1 L a _______ 14. 1 mL Chapter 3 Scientific Measurement 23 . a. Complete the following table showing some metric units of length. 12. Interior of an oven a. Height of a stove top above the floor a. volume 11. All rights reserved. Remember that the meter is the SI base unit for length. d. publishing as Pearson Prentice Hall. Width of a key on a computer keyboard d. One-quarter teaspoon c. 1 cm c _______ 10. c.. so 1 cm3 is equal to 1 mL. lower temperature higher temperature ➞ 24 Guided Reading and Study Workbook © Pearson Education. Circle the letter of the unit of mass commonly used in chemistry that equals 1/1000 kilogram. A liter bottle of soda b. platform balance d. a. scale c. or will it be the same weight? Explain. 18.. Mass Unit of Mass c _______ 20. Inc. Circle the letter of the instrument shown that is used to measure mass. Its weight will be less. The volume of any solid. liquid. 1 kg a _______ 21. Scientific Measurement (continued) 16. 1 dm3 c. analytical balance 24. will a mass have more or less weight than it did on the surface of Earth. gram b. Five aspirin tablets c. Draw an arrow below the diagram. showing the direction of heat transfer between two objects. publishing as Pearson Prentice Hall. 1 L of liquid water at 4°C .05_Chem_GRSW_Ch03. When brought to the surface of the moon. milligram c. and the force of gravity on the moon is one-sixth what it is on Earth. 1 mg 23. a. Is the following sentence true or false? The mass of an object changes with false location. A volume of 1 L is also equal to a. 1 g b _______ 22. A kilogram was originally defined as the mass of __________________________ 19. A few grains of sand a.SE/TE 6/11/04 3:29 PM Page 24 Name ___________________________ Date ___________________ Class __________________ CHAPTER 3. 1000 cm 17. or gas will change with temperature ______________________ . because weight is a measure of gravitational force. 1000 mL b. ______________________ 25. balance beam . 26. milliliter Match each unit of mass with the object whose mass would be closest to that unit. All rights reserved. b. ________________________________________________ Chapter 3 Scientific Measurement 25 .. As the temperature falls. How are the two parts of a conversion factor related? They are equivalent. This expansion forces the liquid higher in the thermometer tube as the temperature rises. Inc. One calorie is the quantity of heat that raises the temperature of 1g 1°C ______________________ of pure water by ______________________ . What properties explain the behavior of liquid-filled thermometers? Almost all liquids expand in volume with an increase in temperature. 28. Celsius © Pearson Education. publishing as Pearson Prentice Hall. 0 K. the liquid contracts and its level in the tube drops.SE/TE 6/11/04 3:29 PM Page 25 Name ___________________________ Date ___________________ Class __________________ 27.3 CONVERSION PROBLEMS (pages 80–87) This section explains how to construct conversion factors from equivalent measurements.15 K ________ 373.15 K ________ Kelvin 100 divisions 32. What are the two reference temperatures on the Celsius scale? The freezing point of water is 0°C and the boiling point of water is 100°C. All rights reserved. A change of temperature equal to one Kelvin is equal to a change of 1°C temperature of how many degrees Celsius? ______________________ 31. 100 divisions 0°C ________ 100°C ________ Freezing point of water Boiling point of water 273. SECTION 3. It also describes how to apply the techniques of dimensional analysis to a variety of conversion problems.05_Chem_GRSW_Ch03. Conversion Factors (pages 80–81) 1. on the Kelvin scale called? absolute zero ______________________ 30. Complete the diagram to show the reference temperatures in the Celsius and Kelvin scales. What is the zero point. 29. There are 225 mL per cup. the smaller number is part of the larger quantity that has the ______________________ unit. The larger number is part smaller of the quantity that has the ______________________ unit.SE/TE 6/11/04 3:29 PM Page 26 Name ___________________________ Date ___________________ Class __________________ CHAPTER 3. 26 Guided Reading and Study Workbook © Pearson Education. ______________________ 4. Circle the letter of the conversion factor you would use to find its length in inches. All rights reserved. 2.0 cm long when it is new. of the measurements. because the measurement true being converted is multiplied by unity. 1 in. of 2 cups of oil. publishing as Pearson Prentice Hall. 2. Inc. 3. 1 cup Volume 2 cups 0. Look at Figure 3. Dimensional Analysis (pages 81–83) 7. The correct conversion factor has the ______________ unit unknown in the denominator and the ______________ unit in the numerator. 60 minutes 1 hour and 1 hour 60 minutes 5.54 cm 1 in.05_Chem_GRSW_Ch03. Scientific Measurement (continued) 2. in milliliters. What is dimensional analysis? Dimensional analysis is a way to analyze and solve problems. Write two conversion factors based on the relationship between hours and minutes. A student is asked to calculate the volume. or dimensions. The student calculates the volume as follows: . The average lead for a mechanical pencil is 6.54 cm a.11. 1 in. c. b.0 cm 6. In a conversion factor.08 cup 25 mL List three errors the student made. The unit in the answer is incorrect. 6. 6.5. using the units.0 cm d. The conversion factor was inverted. 1 in. Is the following sentence true or false? The actual size of a measurement multiplied by a conversion factor remains the same.. Reread Sample Problem 3. known 8. 25 mL was used instead of 225 mL. 4 fluid ounces a.25 m to centimeters 100 cm 0. Circle the conversion factor needed to find the mass of water that 5 identical containers can hold. Complex conversions between units may require using __________________________ conversion factor. 1 L/1000 mL Chapter 3 Scientific Measurement 27 .2 dL 10 dL _______________________________________ more than one 13.2 dL to liters 1L 4.05_Chem_GRSW_Ch03. 1 tablespoon 1 tablespoon b.. 65 g water 65 g water c. 9. 1 mL/1 cm3. 5 containers a. 15 mL © Pearson Education.8 g 1000 g _______________________________________ c. 35 ms to seconds 1s 35 ms 1000 ms _______________________________________ d. All rights reserved.25 m 1m _______________________________________ b. Circle the letter of the conversion factor that you would use to convert tablespoons to milliliters.8 g to kilograms 1 kg 9. 1 container 65 g water d. 65 g water 1 container b. Inc. 15 mL d. 11. 4. 4 fluid ounces 1 tablespoon c.SE/TE 6/11/04 3:29 PM Page 27 Name ___________________________ Date ___________________ Class __________________ 9. Show the calculation you would use to convert the following: a. publishing as Pearson Prentice Hall. 14. 0. Converting between units is easily done using ____________________________ . 1 tablespoon 12. 5 containers Converting Between Units (pages 84–85) dimensional analysis 10. How many conversion factors would you need to use to find the number of liters in a cubic decimeter? What are they? Three conversion factors are needed: 1000 cm3/1 dm3. A container can hold 65 g of water. 1 cm 1 m/102 cm 109 nm/1 m 8. Mass g 1000 g 1 kg kg ? Volume Density mm3 ? 1 m3 109 mm3 g/m3 cm3 ? 1 m3 106 cm3 g/m3 23. Calculate his average speed in kilometers per hour. Describe the steps you would use to solve this problem. A scientist has 0.1 cm? 8. density. Scientific Measurement (continued) 15.05_Chem_GRSW_Ch03. How would you calculate the number of nanometers in 8. how much would they spend on flooring for the dining room? The dimensions of the dining room on the floor plan are 40 mm 32 mm. A man can run a mile in 4 minutes. A normal concentration of glucose.1 107 nm 16..95 g/L 22. Complex units can be converted using dimensional analysis. 95 mg/dL 10 dL/1 L 1 g/1000 mg 0. What is the equivalent of 0.2 km/h 28 Guided Reading and Study Workbook © Pearson Education. Replace each question mark in the table with the conversion factors needed to obtain the given units of density.2 lb 1000 g/1 kg 770 g 17. speed. If the homeowners wanted to purchase flooring that costs $10. In a scale drawing of a dining room floor plan. 1. gas mileage 20.89 per square yard.46 mL of a solution. Inc.35 lb in grams? 0. then to yards. How many grams of sugar would be present per liter of blood? Show the conversion factors you use. 3.35 lb 1 kg/2. in the blood is 95 mg/dL. publishing as Pearson Prentice Hall. Convert each dimension to meters. What technique can be used to convert complex units? 21. or sugar. . (1 mile 1.46 mL 1 L/103 mL 106 L/1 L 460 L 18.61 km/1 mi 60 min/1 h 24. How would she convert this volume to microliters? 0. 19. Multiply by the cost per yard to find the total cost. Multiply the lengths in yards to find the number of square yards. 2. All rights reserved.61 km) 1 mi/4 min 1. 10 mm equals 2 meters. Show your work. Name three common measurements that are expressed as a ratio of two units.SE/TE 6/11/04 3:29 PM Page 28 Name ___________________________ Date ___________________ Class __________________ CHAPTER 3. If she is at bat an average of 3 times per game. As a result. Which material has a greater density.05_Chem_GRSW_Ch03. How is density defined? Density is the ratio of the mass of an object to its volume. It explains that density is a characteristic property that depends on the composition of a substance. grams per cubic centimeter (g/cm3) 5. ice d. Is the mass of one pound of lead greater than. The mass of a sample is measured in grams. 4.. lead or feathers? ______________________ 3. how many hits will she make in 52 games? Show your work. Yes. and its volume is measured in cubic centimeters. or equal to the mass equal to of one pound of feathers? ______________________ lead 2. aluminum b. publishing as Pearson Prentice Hall.SE/TE 6/11/04 3:29 PM Page 29 Name ___________________________ Date ___________________ Class __________________ 24.254 (254 hits per 1000 at bats). Look at Table 3. The density of a substance generally decreases as its temperature increases. less than. Are there any exceptions to this statement? Explain. Over a small range of temperatures near the freezing point. gasoline Density and Temperature (pages 91–92) 6. Chapter 3 Scientific Measurement 29 . All rights reserved. a. Determining Density (page 89–90) 1. 52 games 3 at bats/1 game 254 hits/1000 at bats 39 or 40 hits SECTION 3.6 on page 90. not on the size of the sample. corn oil c.4 DENSITY (pages 89–93) This section defines density. Circle the letter of the material that will sink in liquid water at 4°C. the density of water decreases as the temperature decreases. In what units would its density be reported? © Pearson Education. Inc. A baseball player’s batting average is . ice floats on liquid water. Inc.0 107 kg (10 2 cm)3 20 g 1 kg 20 10 6 kg 3 103 m3 1 m3 1 cm 103 g 103 m3 2. 87. 8.71 101 ______________________ meters GUIDED PRACTICE PROBLEM 34 (page 85) 34. Divide. The radius of a potassium atom is 0. 2.227 nm.227 nm Step 2. 1 109 nm 102 cm 1m centimeter 2. Scientific Measurement (continued) GUIDED PRACTICE PROBLEMS GUIDED PRACTICE PROBLEM 3 (page 69) 3. Express this radius in centimeters.27 10–8 cm EXTRA PRACTICE (similar to Practice Problem 36. publishing as Pearson Prentice Hall. 1m 0. To round to three significant figures. Write the number in scientific notation.SE/TE 6/11/04 3:29 PM Page 30 Name ___________________________ Date ___________________ Class __________________ CHAPTER 3.227 102 109 Step 3.. 0.05_Chem_GRSW_Ch03. All rights reserved.073 rounds to _______ Step 2. page 86) 36. Use the conversion factors for nanometers and centimeters.1 87. Round 87.073 meters to three significant figures. Gold has a density of about 20 g/cm3. Simplify. round to the nearest tenth. Step 1. Complete the following steps to solve the problem. Step 1.0 10 4 kg/m3 30 Guided Reading and Study Workbook © Pearson Education. Estimate this density in kg/m3. . Write your answer in scientific notation. A student finds a shiny piece of metal that she thinks is aluminum. Calculate the density. Is the metal aluminum? ______________________ © Pearson Education. a density of about 2. Use dimensional analysis to convert 4.50 g/cm3 _____ Step 4. compare the density of the metal to the density of aluminum given in Table 3.34 g cm3 2 cm3 of boron Chapter 3 Scientific Measurement 31 .SE/TE 6/11/04 3:29 PM Page 31 Name ___________________________ Date ___________________ Class __________________ GUIDED PRACTICE PROBLEM 46 (page 91) 46. Inc. Because a density of 2.34 g 4.68 g 2. List the known values. In the lab.68 g of boron 4. Underline the correct word(s) that complete(s) this statement. Volume 245 cm3 612 g Mass _______ Step 2. Is the metal aluminum? Analyze Step 1. All rights reserved. the metal (is. she determines that the metal has a volume of 245 cm3 and a mass of 612 g. density ______________________ Calculate Step 3. 1 cm3 2. Evaluate Step 5..7 on no page 90. Remember to round your answer to three significant figures. publishing as Pearson Prentice Hall. Use the following relationship to find the density.05_Chem_GRSW_Ch03. The density of boron is 2.7 g/cm3. List the unknown.68 g of boron to cubic centimeters of boron. page 92) 48a.34 g/cm3.50 g/cm3 is nearly 10% less than 2. mass Density volume 612 g 245 _____ cm3 2. EXTRA PRACTICE (similar to Practice Problem 48a. Because the mass of the metal is about two and one-half times the volume. the density of aluminum.5 g/cm3 is reasonable. To determine whether the piece of metal is aluminum. is not) aluminum. How is electronic structure (e-) described in an atom? Concept: Concept: Concept: Concept: Scientific Method Atomic Theory Subatomic Particles Nuclear Lesson EQ: Lesson EQ: Lesson EQ: Lesson EQ: How is the scientific method used? What is Dalton’s atomic theory? What is the difference between mass number and atomic mass? How is average atomic mass calculated? What are the parts of the scientific method? How is a scientific model used? What is a theory? What are the main parts of lab report? How did the cathode ray and gold foil experiment effect the description of atomic structure? How did our understanding of the atom evolve? What is an isotope? What is radioactivity? What are the two naming conventions for isotopes? How are nuclear equations written? What is an ion? What is half life? What are the major components of a nuclear reactor? How is the Bohr atom represented? Vocabulary: Vocabulary: Vocabulary: Vocabulary: Scientific Method (parts) Cathode Ray Tube Atomic number Radioactivity Theory Gold Foil Experiment Atomic mass Radioactive Decay Model Planetary Model Independent Variable Dependent Variable Control Reproduction of this page for classroom and planning use by owner of this book is permitted. Atomic Theory Chemical Concoctions Inc Lab B. C. Applying the Scientific Method. Unit Essential Questions: A. Fission/Fusion . Electrons C. How are the steps Atomic Theory Cooperative Group Exercise in the scientific method applied? B. Decribe how atomic theory changed through time.Leaming-Focused® Notebook ©2005 Learning Concepts Student Learning Map Unit Topic: What is the Atom? Instructional Tools Key Learning: A. 05_Chem_GRSW_Ch04. suggested that matter is made up of tiny particles that cannot be divided. Atoms of different elements can physically mix together. however. Circle the letter of each sentence that is true about Dalton’s atomic theory. c. publishing as Pearson Prentice Hall.1 DEFINING THE ATOM (pages 101–103) This section describes early atomic theories of matter and provides ways to understand the tiny size of individual atoms. © Pearson Education. joined. The modern process of discovery about atoms began with the theories of an John Dalton English schoolteacher named ______________________ . Democritus. atoms of one element are never changed into atoms of another element by a chemical reaction. b. 4. They did not explain chemical behavior. whole-number ratios to form compounds. d. All rights reserved. All elements are composed of tiny. He atoms called these particles ______________________ . 2. or can chemically combine in simple. and they lacked experimental support because Democritus’s approach was not based on the scientific method. 5.SE/TE 6/11/04 3:29 PM Page 33 Name ___________________________ 4 Date ___________________ Class __________________ ATOMIC STRUCTURE SECTION 4. In the diagram. who lived in Greece during the fourth century B. 3.. Inc. List two reasons why the ideas of Democritus were not useful in a scientific sense. or rearranged. indivisible particles called atoms. (a) Atoms of element A (b) Atoms of element B compound mixture Chapter 4 Atomic Structure 33 . use the labels mixture and compound to identify the mixture of elements A and B and the compound that forms when the atoms of elements A and B combine chemically. An element is composed of several types of atoms. a.C. Chemical reactions occur when atoms are separated.. Early Models of the Atom (pages 101–102) 1. About how many atoms of copper when placed side by side would form a line 100. How is the atomic theory that is accepted today different from Dalton’s atomic theory? Atoms are now known to be divisible.. electrons 2. The smallest particle that could no longer be divided. electron d. All rights reserved. Suppose you could grind a sample of the element copper into smaller and smaller particles. an electrode with a positive charge d _______ 6. yet still an atom of copper has the chemical properties of copper. Subatomic Particles (pages 104–106) 1. The diagram shows electrons moving from left to right in a cathode-ray tube. They can be broken down into even smaller. a. Atomic Structure (continued) Sizing up the Atom (page 103) 6. more fundamental particles. cathode ray c.2 STRUCTURE OF THE NUCLEAR ATOM (pages 104–108) This section describes the experiments that led to the discovery of subatomic particles and their properties. 7. Inc.000 1 cm long? ______________________ SECTION 4. is _________________________________ . a negatively charged particle 7.000. High voltage Negative plate Slit Cathode Anode Vacuum pump 34 Guided Reading and Study Workbook Positive plate © Pearson Education. Thomson with the correct description. Draw an arrow showing how the path of the electrons will be affected by the placement of the negatively and positively charged plates. cathode b. a glowing beam traveling between charged electrodes b _______ 5.05_Chem_GRSW_Ch04. c _______ 3.SE/TE 6/11/04 3:29 PM Page 34 Name ___________________________ Date ___________________ Class __________________ CHAPTER 4. publishing as Pearson Prentice Hall. Which subatomic particles carry a negative charge? ______________________ Match each term from the experiments of J. an electrode with a negative charge a _______ 4. anode . J. a. 0 b. and electric charge. All rights reserved. 11. When a given number of positively charged particles combines with an equal number of negatively charged particles. Electric charges are carried by particles of matter. What two properties of an electron did Robert Millikan determine from his experiments? He determined the quantity of charge carried by an electron and its mass. What conclusion did he draw from these observations? He concluded that electrons must be parts of the atoms of all elements. none 13.05_Chem_GRSW_Ch04.67 10–24 9. 2 d. an electrically neutral particle is formed. Circle the letter of each sentence that is true about atoms. Thomson observed that the production of cathode rays did not depend on the kind of gas in the tube or the type of metal used for the electrodes. Properties of Subatomic Particles Particle Symbol Relative Electrical Charge Relative Mass Actual Mass (mass of proton 1) (g) Electron e– 1 1 1840 Proton p+ 1 1 1. 1 c. a. What charge does a neutron carry? ______________________ .11 10–28 Chapter 4 Atomic Structure 35 .SE/TE 6/11/04 3:29 PM Page 35 Name ___________________________ Date ___________________ Class __________________ 8. 9. d. Circle the letter next to the number of units of positive charge that remain if a hydrogen atom loses an electron. All atoms have an electric charge.. c. publishing as Pearson Prentice Hall. b. Electric charges always exist in whole-number multiples of a single basic unit. 10. The positively charged subatomic particle that remains when a hydrogen atom a proton loses an electron is called ______________________ . 12. Inc. 14.67 10–24 Neutron n0 0 1 1. 3 © Pearson Education. matter. Complete the table about the properties of subatomic particles. neutrons d. neutrons. a. The nucleus is composed of protons. and a few were deflected at very large angles. e. . An atom is mostly empty space. All the positive charge of an atom is concentrated in a small central region called the nucleus. They found that most alpha particles were not deflected at all. Explain why in 1911 Rutherford and his coworkers were surprised when they shot a narrow beam of alpha particles through a thin sheet of gold foil..3 DISTINGUISHING AMONG ATOMS (pages 110–119) This section explains how atomic number identifies an element. electrons b. SECTION 4. ______________________ 16. and how to calculate average atomic mass. d.05_Chem_GRSW_Ch04. how isotopes differ. c. Nearly all the mass of an atom is in its nucleus. protons c. The nucleus is large compared with the atom as a whole. how to use atomic number and mass number to find the number of protons. All rights reserved. Inc. a. Circle the letter of the term that correctly completes the sentence.SE/TE 6/11/04 3:29 PM Page 36 Name ___________________________ Date ___________________ Class __________________ CHAPTER 4. b. Is the following sentence true or false? An alpha particle has a double positive true charge because it is a helium atom that has lost two electrons. Circle the letter of each sentence that is true about the nuclear theory of atoms suggested by Rutherford’s experimental results. Elements are different because their atoms contain different numbers of _______ . publishing as Pearson Prentice Hall. and electrons in an atom. 17. Atomic Number (page 110) 1. nuclei 36 Guided Reading and Study Workbook © Pearson Education. They expected most of the alpha particles to pass easily through the foil with only a slight deflection. Atomic Structure (continued) The Atomic Nucleus (pages 106–108) 15. and mass number in the shorthand notation below. Atoms of Six Elements Name Symbol Atomic Number Number of Protons Number of Electrons Hydrogen H 1 1 1 Helium He 2 2 2 Lithium Li 3 3 3 Boron B 5 5 5 Carbon C 6 6 6 Oxygen O 8 8 8 Mass Number (pages 111–112) 3. All rights reserved. atomic number. Place the labels chemical symbol. How many protons.. and electrons are in the atom discussed in Questions 6 and 7? Protons: 10 Neutrons: 12 Electrons: 10 Chapter 4 Atomic Structure 37 . 4. What is the mass number of a helium atom that has two protons and two 4 neutrons? ______________________ 5. publishing as Pearson Prentice Hall. mass number atomic number 22 10 Ne chemical symbol 7. Designate the atom shown in Question 6 in the form “name of element”-“mass neon-22 number.” ______________________ 8.SE/TE 6/11/04 3:29 PM Page 37 Name ___________________________ Date ___________________ Class __________________ 2. How many neutrons does a beryllium atom with four protons and a mass 5 number of nine have? ______________________ 6. Complete the table showing the number of protons and electrons in atoms of six elements.05_Chem_GRSW_Ch04. neutrons. Inc. The total number of protons and neutrons in an atom is its mass number ______________________ . © Pearson Education. 37 amu 38 Guided Reading and Study Workbook © Pearson Education. most elements occur as a mixture of two or more isotopes. 35 amu b. Is the following sentence true or false? Isotopes are chemically alike because true they have identical numbers of protons and electrons. Isotopes of an element do not have a specific natural percent abundance. How do atoms of neon-20 and neon-22 differ? An atom of neon-22 has two more neutrons in its nucleus than an atom of neon-20. Circle the letter of the correct answer. hydrogen-2 b. tritium c _______ 13. deuterium Atomic Mass (pages 114–117) 15. Circle the letter of each statement that is true about the average atomic mass of an element and the relative abundance of its isotopes. hydrogen a _______ 14. the average atomic mass of natural hydrogen is 2 amu. publishing as Pearson Prentice Hall. Is the following sentence true or false? The atomic mass of an element is false always a whole number of atomic mass units. 11. Neon-20 and neon-22 are called ______________________ . b _______ 12.05_Chem_GRSW_Ch04. ______________________ Match the designation of each hydrogen isotope with its commonly used name. Why is the atomic mass unit (amu). there are three atoms of chlorine-35 for every one atom of chlorine-37. Atomic Structure (continued) Isotopes (pages 112–113) 9. Which atomic mass number is closer to the average atomic mass of chlorine? a. All rights reserved. The average atomic mass of an element is usually closest to that of the isotope with the highest natural abundance.. rather than the gram. 19. b. 12 amu 17. d. hydrogen-1 a. c. 16. ______________________ 18. Inc. 2 amu. hydrogen-3 c. respectively. What isotope of carbon has been chosen as the reference isotope for atomic mass units? What is the defined atomic mass in amu of this isotope? . isotopes 10.SE/TE 6/11/04 3:29 PM Page 38 Name ___________________________ Date ___________________ Class __________________ CHAPTER 4. When chlorine occurs in nature. carbon-12. Because hydrogen has three isotopes with atomic masses of about 1 amu. In nature. and 3 amu. usually used to express atomic mass? The values of atomic masses measured in grams are inconveniently small and impractical to work with. a. Distinguishing Among Atoms.3. Begin with the headings in the textbook. In the periodic table. Isotopes. Main heads should be Atomic Number. Chapter 4 Atomic Structure 39 . the elements are organized into groups based on a set of repeating properties ______________________________________________________________ . Then list the details that support the main idea. write the main idea. What are the horizontal rows in the periodic table called? periods Reading Skill Practice Outlining can help you understand and remember what you have read. Mass Number. Under each heading. Prepare an outline of Section 4. Subheads should indicate an understanding of each concept. The Periodic Table—A Preview (page 118) 21.. © Pearson Education. Inc. All rights reserved.SE/TE 6/11/04 3:29 PM Page 39 Name ___________________________ Date ___________________ Class __________________ 20.05_Chem_GRSW_Ch04. and Atomic Mass. publishing as Pearson Prentice Hall. Do your work on a separate sheet of paper. For carbon-12.2 to express the compositions of carbon-12.SE/TE 6/11/04 3:29 PM Page 40 Name ___________________________ Date ___________________ Class __________________ CHAPTER 4. and beryllium-9 in shorthand notation. 19 Step 2. Is your answer reasonable? Why? Yes it is.. because the mass number is greater than the atomic number. The number of protons in an atom is called its ______________________ number. Atomic Structure (continued) GUIDED PRACTICE PROBLEMS Fill in the write-on lines and boxes provided as you work through the guided practice problems. 6 The number of protons in an atom of carbon-12 is ___________ . Inc. publishing as Pearson Prentice Hall. Use Table 4. this number is ___________ .05_Chem_GRSW_Ch04. All rights reserved. mass number . 19 Step 3. The shorthand notation for fluorine-19 is: 9 F Step 4. The shorthand notation for carbon-12 is: 12 atomic number 6 C Evaluate Step 4. The atomic number of fluorine-19 is ____________ . GUIDED PRACTICE PROBLEM 18 (page 112) 18. the mass number of an isotope is always greater yes than its atomic number. Except for hydrogen-1. Calculate Step 2. The number of protons plus the number of neutrons in an atom is called 12 mass its ______________________ number. Analyze Carbon-12 atomic Step 1. Step 3. 40 Guided Reading and Study Workbook © Pearson Education. fluorine-19. Is the mass number reasonable? ____________ Fluorine-19 9 Step 1. Its mass number is ____________ . 9 Step 2.93 amu.05_Chem_GRSW_Ch04. Calculate the average atomic mass of copper. Average mass: 43. The atomic number of beryllium-9 is ____________ .2% 62. Solve Step 2. Because about 70% of the element consists of the lighter isotope. Analyze Step 1.SE/TE 6/11/04 3:29 PM Page 41 Name ___________________________ Date ___________________ Class __________________ Beryllium-9 4 Step 1.692 62. because the mass number is greater than the atomic number.6 amu 64.8% 64.2% for mass 62. the average atomic mass should be closer to the atomic mass number of 63 than 65. Inc. Three isotopes of sulfur are sulfur-32. including the atomic number and the mass number..6 amu 0. 9 Be Step 3.308 20.6 amu Evaluate Step 5.0 amu 63. Is your answer reasonable? Why? Yes it is. Chapter 4 Atomic Structure 41 .0 amu 43. It is closer to 63 than 65.93 amu Step 4. All rights reserved. For Cu-63: 69. and sulfur-34. The shorthand notation for beryllium-9 is: 4 Step 4.93 amu 0. Explain why your answer is reasonable. Its mass number is ____________ .93 amu and 30. sulfur-33.93 amu 20. publishing as Pearson Prentice Hall. sulfur-32 sulfur-33 sulfur-34 32 33 34 16 S 16 S S 16 © Pearson Education.8% for mass 64. The relative abundance and atomic masses are 69.93 amu Step 3. page 113) 19. For Cu-65: 30. GUIDED PRACTICE PROBLEM 23 (page 117) 23. EXTRA PRACTICE (similar to Practice Problem 19. The element copper has naturally occurring isotopes with mass numbers of 63 and 65. Write the complete symbol for each isotope. Will the average atomic mass be closer to 63 or to 65? Explain. 84%). Inc.. Calculate the atomic mass of rubidium. _________________________ © Pearson Education.16%) 85. publishing as Pearson Prentice Hall.05_Chem_GRSW_Ch04.47 amu and 86. The two isotopes of rubidium have atomic masses and relative abundancies of 84. All rights reserved. page 117) 24.91 amu (27.SE/TE 6/11/04 3:29 PM Page 42 Name ___________________________ Date ___________________ Class __________________ CHAPTER 4. 42 Guided Reading and Study Workbook .91 amu (72. Atomic Structure (continued) EXTRA PRACTICE (similar to Practice Problem 24. Leaming-Focused® Notebook ©2005 Learning Concepts Student Learning Map Unit Topic: How do electrons behave in an atom? Key Learning: A. How is electronic Hog Hotel Activity structure (e-) described in an atom? B. Electromagnetic Spectrum Atomic Emission Spectra Flame Tests Lab Unit Essential Questions: A. Describe the dual wave-particle nature of electrons. Vocabulary: . Concept: Concept: Concept: Wave-Particle Duality Electron Configurations Atomic Charge Lesson EQ: Lesson EQ: Lesson EQ: What is EMS? How is the Bohr atom represented? What is a cation? What is the relationship between wavelength and frequency? What is the quantum mechanical model of atomic structure? What are electron orbitals? What rules do electrons follow when filling their orbitals? How are ions formed? How are electron configurations used to describe location of electrons? Vocabulary: Vocabulary: Plank’s constant Bohr atom Cation Wavelength Aufbau Principle Anion Frequency Pauli Exclusion Principle Valence Electrons Quantum numbers Lesson EQ: What is an anion? Vocabulary: Photoelectric effect Concept: Hund’s Rule Reproduction of this page for classroom and planning use by owner of this book is permitted. Electron Configurations Instructional Tools B. Chapter 5 Electrons in Atoms 43 . Circle the letter of the term that completes the sentence correctly. All rights reserved. Bohr Most of an atom’s mass is concentrated in the small.1 MODELS OF THE ATOM (pages 127–132) This section summarizes the development of atomic theory. Electrons are arranged in concentric circular paths around the nucleus. The electrons surround the nucleus and the rest of the atom is empty space. Scientist Dalton Model of Atom The atom is a solid indivisible mass. Rutherford © Pearson Education. A quantum of energy is the amount of energy required to a. It also explains the significance of quantized energies of electrons as they relate to the quan– tum mechanical model of the atom. Complete the table about atomic models and the scientists who developed them. Thomson The atom is a ball of positive charge with electrons stuck into the ball. The Development of Atomic Models (pages 127–128) 1. positively charged nucleus. What is a small. move an electron from its present energy level to the next higher one 5. Is the following sentence true or false? The electrons in an atom can exist false between energy levels. publishing as Pearson Prentice Hall. the higher the electron is on the energy ladder. discrete unit of energy called? It is called a quantum. Inc..05_Chem_GRSW_Ch05.SE/TE 6/11/04 3:30 PM Page 43 Name ____________________________________ Date __________ Class ___________________ 5 ELECTRONS IN ATOMS SECTION 5. move an electron from its present energy level to the next lower one b. ______________________ The Bohr Model (pages 128–129) 3. In general. the farther ______________________ it is from the nucleus. maintain an electron in its present energy level c. 2. 4. They are all perpendicular to each other. _____________________________ orientations in space. py . . n © Pearson Education. All rights reserved. z z z x x x y y y px py pz p orbitals 12. publishing as Pearson Prentice Hall. the px . Inc. 2. Match each diagram below with the name of its p orbital. 14. 11. and pz orbitals are similar. py . atomic orbitals b. 7. Is the following sentence true or false? The quantum mechanical model of the atom estimates the probability of finding an electron in a certain position. Describe how the px . Principal energy levels are assigned values in order of ______________________ energy: n 1. Circle the letter of the term that correctly answers this question. principal quantum numbers (n) generally increasing 9. quantum mechanical numbers c. The quantum mechanical model is not based on the exact path an electron follows around the nucleus. py . 4.05_Chem_GRSW_Ch05. Electrons in Atoms (continued) The Quantum Mechanical Model (page 130) 6. The p orbitals are similar because they are all dumbbell shaped. Which name describes the major energy levels of electrons? a. or pz. Describe how the px . Circle the letter of the formula for the maximum number of electrons that can occupy a principal energy level. In the quantum mechanical model the regions where electrons are likely atomic orbitals to be found are called ______________________ and are denoted by letters ______________________ . 10. and pz orbitals are different. a. n2 44 Guided Reading and Study Workbook c. true ______________________ Atomic Orbitals (pages 131–132) 8. 2n2 b. Use n for the principal quantum number. Use the diagram above. and so forth.SE/TE 6/11/04 3:30 PM Page 44 Name ___________________________ Date ___________________ Class __________________ CHAPTER 5. 3.. What is the difference between the previous models of the atom and the modern Previous models described the motion of electrons the quantum mechanical model? __________________________________________________ same way as the motion of large objects. The p orbitals have different 13. 2n d. quantas d. 05_Chem_GRSW_Ch05.SE/TE 6/11/04 3:30 PM Page 45 Name ___________________________ Date ___________________ Class __________________ SECTION 5.2 ELECTRON ARRANGEMENT IN ATOMS (pages 133–136) This section shows you how to apply the aufbau principle, the Pauli exclusion principle, and Hund’s rule to help you write the electron configurations of elements. It also explains why the electron configurations for some elements differ from those assigned using the aufbau principle. Electron Configurations (pages 133–135) 1. The ways in which electrons are arranged around the nuclei of atoms are electron configurations called ___________________________________________ . Match the name of the rule used to find the electron configurations of atoms with the rule itself. b _______ 2. aufbau principle a. When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins. b. Electrons enter orbitals of lowest energy first. c. An atomic orbital may describe at most two electrons. c _______ 3. Pauli exclusion principle a _______ 4. Hund’s rule 5. Look at the aufbau diagram, Figure 5.7 on page 133. Which atomic orbital 4f is of higher energy, a 4f or a 5p orbital? _______ © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 6. Fill in the electron configurations for the elements given in the table. Use the orbital filling diagrams to complete the table. Electron Configurations for Some Selected Elements Orbital filling Element H He Li C N O F 1s 2s 2px 2py 2pz 3s Electron configuration 1s 1 1s 2 1s 22s1 1s 22s 22p 2 1s 22s 22p 3 1s 2 2s 22p 4 1s 22s 22p 5 Ne 1s 22s 22p 6 Na 1s 22s 22p 63s 1 Chapter 5 Electrons in Atoms 45 05_Chem_GRSW_Ch05.SE/TE 6/11/04 3:30 PM Page 46 Name ___________________________ Date ___________________ Class __________________ CHAPTER 5, Electrons in Atoms (continued) 7. In the shorthand method for writing an electron configuration, what does a superscript stand for? The superscript stands for the number of electrons occupying a given sublevel. 8. In the shorthand method for writing an electron configuration, what does the sum of the superscripts equal? The sum equals the number of electrons in the atom. Exceptional Electron Configurations (page 136) 9. Is the following sentence true or false? The aufbau principle works for false every element in the periodic table. ______________________ stable 10. Filled energy sublevels are more ______________________ than partially filled sublevels. filled 11. Half-filled levels are not as stable as ______________________ levels, but are more stable than other configurations. Reading Skill Practice The subheads of students’ outlines of the section should be Electron Configurations and Exceptional Electron Configurations. The section’s main ideas should form the next level of the outline. SECTION 5.3 PHYSICS AND THE QUANTUM MECHANICAL MODEL (pages 138–146) This section explains how to calculate the wavelength, frequency, or energy of light, given two of these values. It also explains the origin of the atomic emission spectrum of an element. Light (pages 138–140) 1. Match each term describing waves to its definition. b _______ amplitude a. the distance between two crests a _______ wavelength b. the wave’s height from the origin to the crest c _______ frequency c. the number of wave cycles to pass a given point per unit of time 46 Guided Reading and Study Workbook © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Outlining can help you understand and remember what you have read. Prepare an outline of Section 5.2, Electron Arrangement in Atoms. Begin your outline by copying the headings from the textbook. Under each heading, write the main idea. Then list the details that support, or back up, the main idea. Do your work on a separate sheet of paper. 05_Chem_GRSW_Ch05.SE/TE 6/11/04 3:30 PM Page 47 Name ___________________________ Date ___________________ Class __________________ 2. The units of frequency are usually cycles per second. The SI unit of hertz (Hz) cycles per second is called a(n) ______________________ . 3. Label the parts of a wave in this drawing. Label the wavelength, the amplitude, the crest, and the origin. Wavelength λ Crest Amplitude Origin 4. The product of wavelength and frequency always equals a(n) constant ______________________ , the speed of light. 5. Is the following sentence true or false? The wavelength and frequency of all true waves are inversely proportional to each other. ______________________ 6. Light consists of electromagnetic waves. What kinds of visible and invisible radiation are included in the electromagnetic spectrum? The following kinds of radiation are included in the electromagnetic spectrum: radio waves, microwaves, infrared waves, visible light, ultraviolet waves, x-ray, and gamma © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. rays. 7. When sunlight passes through a prism, the different wavelengths separate into spectrum a(n) ______________________ of colors. 8. Put the visible colors in order of frequency. 2 6 _______ orange _______ violet 4 _______ green 5 _______ blue 3 _______ yellow 1 _______ red 9. Look at Figure 5.10 on page 139. The electromagnetic spectrum consists of radiation over a broad band of wavelengths. What type of radiation has the lowest frequency? The highest frequency? Radio waves have the lowest frequency. Gamma rays have the highest frequency. Atomic Spectra (page 141) 10. What happens when an electric current is passed through the gas or vapor of an element? The element emits light as it is excited by the passage of the electric current. Chapter 5 Electrons in Atoms 47 What did Albert Einstein call the quanta of energy that is light? photons ______________________ 16. 17. Is the following sentence true or false? The new method of describing the motions of subatomic particles. Does the Heisenberg uncertainty principle apply to cars and airplanes? No. atoms. Is the following sentence true or false? The emission spectrum of an element can be the same as the emission spectrum of another element. 18. Inc. publishing as Pearson Prentice Hall. ______________________ 19. ______________________ true by experimental evidence. only to small particles. What is the lowest possible energy of an electron called? ____________________________ _ higher 14.SE/TE 6/11/04 3:30 PM Page 48 Name ___________________________ Date ___________________ Class __________________ CHAPTER 5. 12. Electrons in Atoms (continued) 11. false ______________________ An Explanation of Atomic Spectra (pages 142–143) ground state 13. 48 Guided Reading and Study Workbook © Pearson Education.05_Chem_GRSW_Ch05. Passing the light emitted by an element through a prism gives the atomic emission spectrum _________________________________________________ of the element. and molecules is called quantum true mechanics.. Only electrons moving from ______________________ to lower ______________________ energy levels lose energy and emit light. Is the following sentence true or false? de Broglie’s conclusions were supported . What did de Broglie’s equation predict about the behavior of particles? It predicts that all moving objects have wavelike motions. All rights reserved. Quantum Mechanics (pages 381–382) 15. What is the wavelength of red light in cm? Red light has a wavelength of about 700 nm. this radiation has a longer wavelength than red light. Therefore. Step 8. is greater than the wavelength of red light. Explain why you think your result makes sense? The magnitude of the frequency is about 105 times the magnitude of c. Chapter 5 Electrons in Atoms 49 . λ ___________ © Pearson Education. Step 3. Because frequency and wavelength are inversely proportional to each other. 2. Substitute the known quantities into the equation and solve. Evaluate Step 7.50 1013 s–1 )? Does this radiation have a longer or shorter wavelength than red light? Analyze Step 1. Solve c υ Step 4. because wavelength is measured in meters or fractions of a meter.05_Chem_GRSW_Ch05.00 10–5 m. Step 5. Are the units in your answer correct? How do you know? Yes. Compare the answer with the wavelength of red light.00 108 m/s.00 108 m/s 2.SE/TE 6/11/04 3:30 PM Page 49 Name ___________________________ Date ___________________ Class __________________ GUIDED PRACTICE PROBLEM GUIDED PRACTICE PROBLEM 14 (page 140) 14. What is the wavelength of radiation with a frequency of 1.501013 Hz (1. What is the equation for the relationship between frequency and c λυ wavelength? ______________________ Step 2. 7 10–7 m. Does the given radiation have a wavelength longer or shorter than that of red light? The answer. What does c represent and what is its value? It represents the speed of light. which can be converted to m by dividing by 109 nm/m. Inc.00 10–5 m 1.. 3. All rights reserved.50 1013 s Step 6. producing 7 10–7 m. the answer should be about 10 –5. which is 3. publishing as Pearson Prentice Hall. Solve the equation for the unknown. ionization energy. electron affinity. Vocabulary: . What is a periodic trend? Concept: Concept: Concept: History of the Periodic Table Periodic Table Organization Lesson EQ: Lesson EQ: Lesson EQ: Compare Mendeleev’s Periodic Table to a shoe store.Leaming-Focused® Notebook ©2005 Learning Concepts Student Learning Map Unit Topic: How is the Periodic Table be used? Instructional Tools Key Learning: A. Periodic Trends Unit Essential Questions: A. How is the periodic Density Trends in a Group Lab table organized? B. and electronegativity? Reproduction of this page for classroom and planning use by owner of this book is permitted. Periodic Table Alien Zoo Activity B. What are the major groupings on the periodic table? How does electron configuration explain periodic trends? How has the periodic table changed through time? How has it stayed the same? What is periodicity and how can it be used? What is shielding? Vocabulary: Vocabulary: Vocabulary: Mendeleev Periodicity Periodic Trend Moseley Blocks Radii Periodic law Group Shielding Effect Noble Gases Family Ionization Energy Lanthanides Row Electronegativity Actinides Period Concept: Trends Lesson EQ: What is the trend on the periodic table for atomic radius. Inc. What caused the rate of discovery to increase after 1700? Chemists began to use scientific methods to search for elements.. publishing as Pearson Prentice Hall. Searching For An Organizing Principle (page 155) 13 1. Nonmetals. Explain the color coding of the squares in the periodic table in Figure 6. How are the elements arranged in the modern periodic table? The elements are arranged in order by increasing atomic number. ______________________ Metals. ______________________ The Periodic Law (page 157) 7. 6. Yellow squares contain metals.1 ORGANIZING THE ELEMENTS (pages 155–160) This section describes the development of the periodic table and explains the periodic law. and metalloids.5.05_Chem_GRSW_Ch06. Mendeleev’s Periodic Table (page 156) Dmitri Mendeleev was a Russian chemist and teacher 4. Who was Dmitri Mendeleev? __________________________________________________ © Pearson Education. who developed a periodic table of elements. How many elements had been identified by the year 1700? ________________ 2. It also describes the classification of elements into metals. 5. Is the following statement true or false? The periodic law states that when elements are arranged in order of increasing atomic number. What property did Mendeleev use to organize the elements into a periodic table? Mendeleev arranged the elements in order of increasing atomic mass. there is a true periodic repetition of physical and chemical properties. 8. and Metalloids (pages 158–160) 9. 3. What did chemists use to sort elements into groups? Chemists used the properties of elements.SE/TE 6/12/04 9:57 AM Page 51 Name ___________________________ 6 Date ___________________ Class __________________ THE PERIODIC TABLE SECTION 6. Is the following sentence true or false? Mendeleev used his periodic table to true predict the properties of undiscovered elements. Chapter 6 The Periodic Table 51 . green squares contain metalloids. nonmetals. blue squares contain nonmetals. All rights reserved. 52 Guided Reading and Study Workbook © Pearson Education. a. Squares In The Periodic Table (pages 161–163) 1. Use the labels element name. . Why are Group A elements called representative elements? They exhibit a wide range of physical and chemical properties. _________________________________________________________________ Electron Configurations In Groups (pages 164–165) 3. Is the following statement true or false? The variation in properties among metals false is greater than the variation in properties among nonmetals. It also describes the use of electron configurations to classify elements. and average atomic mass. symbol. element symbol 12 element name Magnesium 24. ________________ 4. Inc.305 atomic number Mg average atomic mass state at room temperature a. All rights reserved. atomic number. _________________________________________________________________ electrons in each energy level b. The Periodic Table (continued) 10.2 CLASSIFYING THE ELEMENTS (pages 161–167) This section explains why you can infer the properties of an element based on the properties of other elements in the periodic table.9.SE/TE 6/12/04 9:57 AM Page 52 Name ___________________________ Date ___________________ Class __________________ CHAPTER 6. __________________ metal 12. high luster 11. malleable b. atomic number. Which property below is not a general property of metals. nonmetal Under other conditions. ductile c. you can discover about an element using the periodic table in Figure 6. a metalloid may behave like a __________________ . List three things. Label the sample square from the periodic table below. Is the following sentence true or false? The subatomic particles that play the key true role in determining the properties of an element are electrons. 2.05_Chem_GRSW_Ch06. and average atomic mass. element symbol. a metalloid may behave like a __________________ . Under some conditions. SECTION 6. other than the name. publishing as Pearson Prentice Hall. poor conductor of heat d.. _________________________________________________________________ whether an element is found in nature c. Representative elements Description of Electron Configuration s or p sublevels are filled s or p sublevels are only partially filled Transition metals s sublevel and nearby d sublevel contain electrons Inner transition metals s sublevel and nearby f sublevel contain electrons 8. Groups 1A and 2A and helium b. 4A. gallium a _______ 10. and 8A except for helium c. fluorine ______________________ 6. c _______ 9. halogen. chlorine ______________________ alkali metal f. how many electrons are in the highest occupied energy level? 3 a. Groups 3A. 6A. inner transition metals Match the category of elements with an element from that category. Noble gases a. calcium ______________________ alkaline earth metal g. alkali metal a. Group 8A ____________________ Transition Elements (page 166) 7. xenon ______________________ halogen b. Classify each of the following elements as a (an) alkali metal. a. Group 1A ____________________ 8 c. Complete the table about classifying elements according to the electron configuration of their highest occupied energy level.. For elements in each of the following groups. Circle the letter of the elements found in the p block. or noble gas. publishing as Pearson Prentice Hall.SE/TE 6/12/04 9:57 AM Page 53 Name ___________________________ Date ___________________ Class __________________ 5. Category Noble gases © Pearson Education. nobelium d _______ 11. 5A.05_Chem_GRSW_Ch06. Inc. potassium ______________________ alkaline earth metal c. argon b _______ 12. 7A. transition metals d. Inner transition metals d. Group 3A ____________________ 1 b. magnesium ______________________ halogen d. vanadium Chapter 6 The Periodic Table 53 . sodium ______________________ noble gas e. All rights reserved. Representative elements b. alkaline earth metal. Transition metals c. cobalt __________________________________ 1s 22s 22p 63s 23p 4 c. Write the electron configurations for the following elements. pick the element with the largest atom.SE/TE 6/12/04 9:57 AM Page 54 Name ___________________________ Date ___________________ Class __________________ CHAPTER 6. ______________________ 2. 54 Guided Reading and Study Workbook © Pearson Education. Helium and argon __________________________ potassium b. argon a. 4. publishing as Pearson Prentice Hall. What is an ion? An ion is an atom or group of atoms that has a positive or negative charge. sulfur __________________________________ SECTION 6. Trends in Atomic Size (pages 170–171) 1.3 PERIODIC TRENDS (pages 170–178) This section explains how to interpret group trends and periodic trends in atomic size. Potassium and argon __________________________ Ions (page 172) 6. Is the following sentence true or false? The radius of an atom can be measured false directly.12 on page 166. Inc. ionic size. _________________________________________________________________ 5. For each pair of elements. What are the two variables that affect atomic size within a group? the charge on the nucleus a. The atomic size decreases from left to right across a period. 3. The Periodic Table (continued) 13. All rights reserved.05_Chem_GRSW_Ch06. What is the general trend in atomic size within a group? Within a period? . What are the atomic radii for the following molecules? Hydrogen atomic radius Oxygen atomic radius Nitrogen atomic radius Chlorine atomic radius 30 pm __________ 68 pm __________ 70 pm __________ 102 pm __________ The atomic size increases within a group as atomic number increases. magnesium _____________________________ 2 2 6 2 6 7 2 1s 2s 2p 3s 3p 3d 4s b. _________________________________________________________________ the number of occupied energy levels b. ionization energy. Use Figure 6. and electronegativity.. 1s 22s 22p 63s 2 a. How are ions formed? An ion is formed when electrons are transferred between atoms. anion 8. Why does ionization energy tend to increase as you move across a period? The nuclear charge increases across a period but the shielding effect remains constant. Chapter 6 The Periodic Table 55 .05_Chem_GRSW_Ch06. 13. publishing as Pearson Prentice Hall. Why does ionization energy tend to decrease from top to bottom within a group? Atomic size increases from top to bottom within the group. Inc. There is a large increase in ionization energy between the second and the third ionization energies of a metal. ______________________ is the energy required to overcome the attraction of protons in the nucleus and remove an electron from a gaseous atom. 12. 11. an ion with a 2 charge Trends in Ionic Size (page 176) lose 14. All rights reserved. Anions Cations Charge negative positive Metal/Nonmetal nonmetal metal Minus sign/Plus sign plus sign minus sign Trends in Ionization Energy (pages 173–175) Ionization energy 10.SE/TE 6/12/04 9:57 AM Page 55 Name ___________________________ Date ___________________ Class __________________ 7. There is greater attraction of the electrons to the nucleus and more energy is required to remove an electron. 9. gain Nonmetallic elements tend to ______________________ electrons and negative form ______________________ ions. Atomic size increases from top to bottom within the group. Complete the table about anions and cations. an ion with cation a negative charge is called a(n) ______________________ . An ion with a positive charge is called a(n) ______________________ . The nuclear charge has a smaller effect on the electrons in the highest occupied energy level and less energy © Pearson Education.. is required to remove an electron. What kind of ion is the metal likely to form? Include the charge in your answer. Metallic elements tend to ______________________ electrons and form positive ______________________ ions. Use Table 6. Plot atomic number on the horizontal axis. The electronegativity values of the transition elements are all zero. The element with the highest electronegativity value is sodium. Use Figure 6. c. publishing as Pearson Prentice Hall. d. What property of an element represents its tendency to attract electrons when electronegativity it chemically combines with another element? _____________________________ 18. Summary of Trends (page 178) 20. a. c.SE/TE 6/12/04 9:57 AM Page 56 Name ___________________________ Date ___________________ Class __________________ CHAPTER 6. atomic radius d. a cation with a higher atomic number has a smaller ionic radius. Within a period. 19.2 on page 177. Circle the letter of each statement that is true about electronegativity values. ionic radius Reading Skill Practice A graph can help you understand comparisons of data at a glance. Anions are always smaller than the neutral atoms from which they form.05_Chem_GRSW_Ch06.2 on page 177. Electronegativity values can help predict the types of bonds atoms form. a. a. Students’ graphs should show a trend of increasing electronegativity values within a period as atomic number increases. Within a group. What trend do you see in the relative electronegativity values of elements within a group? Within a period? The electronegativity values decrease as you move down a group. The Periodic Table (continued) 15.22 on page 178. . electronegativity b. Circle the letter of each property for which aluminum has a higher value than silicon. first ionization energy c. a cation with a greater charge has a larger ionic radius. Use a range from 0 to 4. d. and a dramatic decrease in the electronegativity value between the Group 7A element in one period and the group 1A element in the next period. Use graph paper to make a graph of the data in Table 6. 56 Guided Reading and Study Workbook © Pearson Education. b. b. Circle the letter of the statement that is true about ion size. but increase as you move across a period. Label each period and the first element in each period. Cl – 16. All rights reserved. Plot electronegativity values on the vertical axis. Nonmetals have higher electronegativity values than metals. Cations are always smaller than the neutral atoms from which they form. Inc.. Which ion has the larger ionic radius: Ca2+ or Cl – ? ________ Trends in Electronegativity (page 177) 17. Solve d. 2p C _______ 5s Sr _______ 3d V _______ c. 22 2 6.05_Chem_GRSW_Ch06.SE/TE 6/12/04 9:57 AM Page 57 Name ___________________________ Date ___________________ Class __________________ GUIDED PRACTICE PROBLEM GUIDED PRACTICE PROBLEM 8 (page 167) 8. Start from the top left and move right across each period in Figure 6. Use Figure 6.12 to write the electron configurations of these elements. This sum should be equal to the atomic number for that element. Make sure the d-block is in the correct energy level. What is the highest occupied energy sublevel for each element. According to its position on the periodic table. how many electrons does each element have in the sublevel listed above? 2 C _______ 2 Sr _______ 3 V _______ © Pearson Education. strontium c. f.12 until you reach the highest occupied sublevel for each element. 1s 22s 22p 63s 23p 63d 104s 24p 65s 2 1s 22s 22p 2 C _________________________ Sr __________________________________________ __ 1s 22s 22p 63s 23p 63d 34s 2 V _____________________________________________ e. vanadium Analyze a. publishing as Pearson Prentice Hall. carbon b. Check your answers as outlined above. according to its position on the periodic table? Remember that the energy level for the d block is always one less than the period. Begin filling in electron sublevels.9 and Figure 6. a. All rights reserved. How can you check whether your answers are correct? Add all the superscripts in the electron configurations. What is the number of electrons for each element? 6 C _______ 38 Sr _______ 23 V _______ b. Inc.. equal to the atomic number C ________________________________________________________________________ 2 2 6 2 6 10 2 6 2 38. equal to the atomic number Sr ________________________________________________________________________ 2 2 6 2 6 3 2 23. equal to the atomic number V ________________________________________________________________________ Chapter 6 The Periodic Table 57 . VESPR Ionic Bonds Covalent Bonds Metallic Bonds Metal + Nonmetal Nonmetal + Nonmetal Metal + Metal Lesson EQ: Lesson EQ: Lesson EQ: Lesson EQ: How many valence electrons are in an element? How are ionic bonds formed? How are covalent bonds formed? How are metallic bonds formed? How are covalent molecules/compound formulas written? How are metal compound formulas written? What is polarity? What is an alloy and how are they used? How are ionic How are electrons in compound a covalent bond formulas named diagrammed? and written? How are multiple bonds diagrammed? Concept: How is molecular shape determined? Vocabulary: Vocabulary: Vocabulary: Vocabulary: Valence Electrons Ionic Bonds Covalent Bonds Alloy Octet Rule Cation Polarity Electron Dot Structure Anion Hybrid Orbital Lewis Structure Polyatomic ions Molecular formula resonance Empirical formula Reproduction of this page for classroom and planning use by owner of this book is permitted.Leaming-Focused® Notebook ©2005 Learning Concepts Student Learning Map Unit Topic: How do atoms bond together to form molecules and compounds? Key Learning(s): A. What are the main bonding theories? Atom Modeling B. What do compounds look like three dimensionally? Concept: Concept: Concept: Electron Dot & Lewis Structure. Molecular Shapes Conductivity Demonstration Unit Essential Question: A. . Atom Bonding Instructional Tools B. Metallic atoms tend to lose their valence electrons to produce a(n) ______________ . atoms tend to achieve the electron configuration of a noble gas. _________________ 4. 3. It also describes the formation of cations from metals and anions from nonmetals. which (except for helium) has eight electrons in its highest energy level. The valence electrons largely determine the __________________________ of an chemical bonds element and are usually the only electrons used in ________________________ . All rights reserved.. Draw the electron dot structure of each of the following atoms. Chapter 7 Ionic and Metallic Bonding 59 . iodine The Octet Rule (page 188) 6. Inc. Most nonmetallic atoms achieve a complete octet by sharing gaining or ________________ electrons. Ar a. chemical properties 2.05_Chem_GRSW_Ch07. What is the octet rule? In forming compounds. Is the following sentence true or false? The group number of an element in the true periodic table is related to the number of valence electrons it has.1 IONS (pages 187–193) This section explains how to use the periodic table to infer the number of valence electrons in an atom and draw its electron dot structure. cation 7. publishing as Pearson Prentice Hall. © Pearson Education. or a positively charged ion. 5. calcium Ca I c.SE/TE 6/11/04 3:31 PM Page 59 Name ___________________________ 7 Date ___________________ Class __________________ IONIC AND METALLIC BONDING SECTION 7. argon b. What is an electron dot structure? It is a diagram that shows the valence electrons as dots. Valence Electrons (pages 187–188) 1. What are valence electrons? Valence electrons are the electrons in the highest occupied energy level of an element’s atoms. or negatively charged ions. helium b. 1s 22s 22p 6 b _______ 11. Energy level 4s 3p 3s 2p 2s 1s Copper atom Cu Copper(I) ion Cu Formation of Anions (pages 191–192) 16. krypton d. Atoms of most nonmetallic elements achieve noble-gas electron anions configurations by gaining electrons to become ____________________ . 17. Write the electron configuration for zinc.SE/TE 6/11/04 3:31 PM Page 60 Name ___________________________ Date ___________________ Class __________________ CHAPTER 7. 1s 22s 22p 63s 23p 63d 104s 2 15. Al 1s 22s 22p 63s 23p 6 4s1 c.. 1s 22s 22p 6 2s 2 a.05_Chem_GRSW_Ch07. Inc. publishing as Pearson Prentice Hall. 60 Guided Reading and Study Workbook © Pearson Education. Mg 1s 22s 22p 6 3s23p1 b. Fill in the electron configuration diagram for the copper(I) ion. 1s 2 a _______ 10. 3d . c _______ 9. 1s 22s 22p 63s 23p 6 d _______ 12. K Match the noble gas with its electron configuration. What is the electron configuration called that has 18 electrons in the outer energy level and all of the orbitals filled? pseudo noble-gas configuration 14. 1s 22s 22p 63s 23p 63d 104s 24p 6 13. Write the electron configurations for these metals and circle the electrons lost when each metal forms a cation. neon c. All rights reserved. Ionic and Metallic Bonding (continued) Formation of Cations (pages 188–190) 8. argon a. What property of nonmetallic elements makes them more likely to gain electrons than lose electrons? They have relatively full valence shells. and name the noble gas with the same configuration. neon b. In an ionic compound. It also describes the use of these characteristics to explain the electrical conductivity of ionic compounds when melted and when in aqueous solutions. argon c. publishing as Pearson Prentice Hall. sulfide Br –. sulfur 2 _____________ 1 d.2 IONIC BONDS AND IONIC COMPOUNDS (pages 194–199) © Pearson Education. nitride O2–. Use figure on page 194 as a model. How many electrons will each element gain in forming an ion? 3 a.SE/TE 6/11/04 3:31 PM Page 61 Name ___________________________ Date ___________________ Class __________________ 18. Formation of Ionic Compounds (pages 194–195) 1. oxygen _____________ c.. All rights reserved.05_Chem_GRSW_Ch07. _________________ 19. Write the symbol and electron configuration for each ion from Question 19. N3–. Complete the electron dot structures below to show how beryllium fluoride (BeF2) is formed. This section lists the characteristics of an ionic bond. oxide S2–. bromine _____________ 20. 3. Is the following sentence true or false? Elements of the halogen family lose one false electron to become halide ions. 1s 22s 22p 63s 23p 63d 104s 24p 6. F F Be2 Be F F Chapter 7 Ionic and Metallic Bonding 61 . 1s 22s 22p 63s 23p 6. neon a. What is an ionic bond? It is the electrostatic force of attraction that binds oppositely charged ions. Inc. bromide SECTION 7. nitrogen _____________ 2 b. 1s 22s 22p 6. the charges of the ___________________ and _____________ neutral must balance to produce an electrically ___________________ substance. cations anions _ 2. 1s 22s 22p 6. krypton d. _________________ 12. Ionic compounds exist as collections of positively and negatively charged ions arranged in repeating three-dimensional patterns. but each fluorine atom only accepts one electron. 3 atoms of oxygen a.SE/TE 6/11/04 3:31 PM Page 62 Name ___________________________ Date ___________________ Class __________________ CHAPTER 7.. Fe2O3 _________________________________________________________________ ____ 1 atom of potassium. 6 13. List the numbers and types of atoms represented by these chemical formulas. A chemical formula shows the types and ______________________ of atoms in the smallest representative unit of a substance. Therefore. 4 atoms of oxygen b. There must be twice as many chloride ions (Cl–) to balance the magnesium ions (Mg2+) to form an electrically neutral compound. 4 atoms of hydrogen. Why do beryllium and fluorine combine in a 1 : 2 ratio? They combine in a 1 : 2 ratio because each beryllium atom gives up two electrons.05_Chem_GRSW_Ch07. Inc. Describe the structure of ionic compounds. 6. CH3 ______________________________________________________________________ 2 atoms of nitrogen. Properties of Ionic Compounds (pages 196–198) crystalline solids 10. What is the coordination number of the ions in a crystal of NaCl? _________________ 62 Guided Reading and Study Workbook © Pearson Education. 8. numbers 5. Is the following sentence true or false? Ionic compounds generally have low false melting points. 1 atom of manganese. All rights reserved. 2 atoms of iron. What is a formula unit? A formula unit is the lowest whole-number ratio of ions in an ionic compound. 4 atoms of hydrogen c. KMnO4 ___________________________________________________________________ 1 atom of carbon. Ionic and Metallic Bonding (continued) 4. Explain why the ratio of magnesium ions to chloride ions in MgCl2 is 1 : 2. two fluorine atoms are needed to react with each beryllium atom. . NH4NO3 __________________________________________________________________ 7. Most ionic compounds are _____________________________ at room temperature. 11. What does a coordination number tell you? It is the number of ions of opposite charge that surround an ion in a crystal. 3 atoms of oxygen d. publishing as Pearson Prentice Hall. 9. Chapter 7 Ionic and Metallic Bonding 63 .. When melted. b.3 BONDING IN METALS (pages 201–203) This section uses the theory of metallic bonds to explain the physical properties of metals. a. Different combinations of ions produce different repeating three-dimensional patterns. Is the following sentence true or false? Metals are made up of cations.SE/TE 6/11/04 3:31 PM Page 63 Name ___________________________ Date ___________________ Class __________________ 14. malleability 4. What important idea does this drawing communicate? Do your work on a separate sheet of paper. All rights reserved. They repel each other and the crystal shatters. 3. ionic compounds do not conduct electricity. Ionic compounds have very unstable structures. d. ionic compounds can conduct electricity. What are metallic bonds? Metallic bonds are the forces of attraction between free-floating valence electrons and positively charged metal ions. Look carefully at Figure 7. Crystalline Structure of Metals (page 202) compact 5. c. The shape of a crystalline solid depends on the composition of the ionic compound that forms the crystal. ductility c. What happens to an ionic crystal when a force is applied to it? The force tends to push ions of like charge into contact.9 on page 197. Inc. Metal atoms in crystals are arranged into very ____________________ and orderly patterns. _________________ 2. electrical conductivity b. Ionic compounds are electrically neutral. a. Name three properties of metals that can be explained by metallic bonding. publishing as Pearson Prentice Hall. 1.05_Chem_GRSW_Ch07. SECTION 7. you can better understand what you have read. Reading Skill Practice By looking carefully at photographs and drawings in textbooks. It also describes the arrangements of atoms in some common metallic crystal structures. Metallic Bonds and Metallic Properties (pages 201–202) © Pearson Education. When dissolved in water. Circle the letter of each statement that is true about ionic compounds. not true neutral atoms. copper d. 8 a 10. The most common use of nonferrous alloys is in _________________ . Label each of the following arrangements of atoms with the correct name. Is the following sentence true or false? Pure metals are usually harder and false more durable than alloys.05_Chem_GRSW_Ch07.. Circle the letter of each metal whose atoms form a face-centered cubic pattern. face-centered cubic b. magnesium c. 12. hexagonal close-packed ______ Alloys (page 203) 11. 12 a ______ 9. a. sodium b. body-centered cubic __________________________________ hexagonal close-packed __________________________________ face-centered cubic __________________________________ 7. body-centered cubic a. All rights reserved. Inc.SE/TE 6/11/04 3:31 PM Page 64 Name ___________________________ Date ___________________ Class __________________ CHAPTER 7. . 64 Guided Reading and Study Workbook © Pearson Education. is called alloy a(n) _________________ . publishing as Pearson Prentice Hall. _________________ coins 13. aluminum b ______ 8. at least one of which is a metal. A mixture of two or more elements. Match the arrangement with the number of neighbors each atom in the arrangement has. Ionic and Metallic Bonding (continued) 6. corrosion resistance b.05_Chem_GRSW_Ch07. Chapter 7 Ionic and Metallic Bonding 65 . publishing as Pearson Prentice Hall. cast iron iron. surgical steel d. What are the component elements for the following alloys? a. Inc. toughness 15. chromium. _________________ alloys have smaller atoms that fit into the spaces between Substitutional alloys have component atoms that are larger atoms.SE/TE 6/11/04 3:31 PM Page 65 Name ___________________________ Date ___________________ Class __________________ 14. sterling silver silver and copper b. roughly equal in size. What four properties make steel an important alloy? a. hardness d. nickel. brass copper and zinc c. All rights reserved. and molybdenum iron and carbon Interstitial 16. _________________ © Pearson Education. ductility c.. potassium reacts with iodine. write an equation that shows the formation of the ionic compound from the two elements. Use electron dot structures to determine formulas of the ionic compounds formed when a. Ionic and Metallic Bonding (continued) GUIDED PRACTICE PROBLEM GUIDED PRACTICE PROBLEM 12 (page 196) 12. Metal atoms _________ gain Nonmetal atoms _________ electrons when forming ionic compounds. publishing as Pearson Prentice Hall. must lose ______ 1 electron(s) in order Step 4. aluminum reacts with oxygen. 66 Guided Reading and Study Workbook © Pearson Education. Analyze yes. potassium Step 1. must gain ______ Step 5. to achieve an octet in the next-lowest energy level.. Solve Step 3. Write the electron dot structures for the two atoms potassium K _________________ iodine I _________________ potassium . Using electron dot structures. The metal atom. Make sure that the electrons lost equals the electrons gained. iodine . Step 2. b. + K + I →K I – KI Step 6. The nonmetal atom. a. All rights reserved. ______________ 1 electron(s) in order to achieve a complete octet.SE/TE 6/11/04 3:31 PM Page 66 Name ___________________________ Date ___________________ Class __________________ CHAPTER 7. which one? ____________________ lose their valence electrons when forming ionic compounds. Is one of the elements a metal? If so. potassium reacts with iodine. The chemical formula for the ionic compound formed is _____________ . Inc. _________ .05_Chem_GRSW_Ch07. O © Pearson Education. The chemical formula for the ionic compound formed is _____________ . Chapter 7 Ionic and Metallic Bonding 67 . Metal atoms _________ gain electrons when forming ionic compounds.. Step 2. publishing as Pearson Prentice Hall. Write the electron dot structures for the two atoms aluminum Al _________________ O oxygen _________________ aluminum .SE/TE 6/11/04 3:31 PM Page 67 Name ___________________________ Date ___________________ Class __________________ b. aluminum reacts with oxygen.05_Chem_GRSW_Ch07. aluminum Step 1. The metal atom. Using electron dot structures. Is one of the elements a metal? If so. The nonmetal atom. to achieve an octet in the next-lowest energy level. Al + Al O O Al 3+ Al 3+ → O 2– O 2– O 2– Al2O3 Step 6. _________ 2 electron(s) in order to achieve a complete octet. Make sure that the electrons lost equals the electrons gained. must lose ______ 3 electron(s) in order Step 4. which one? ____________________ lose their valence electrons when forming ionic compounds. write an equation that shows the formation of the ionic compound from the two elements. All rights reserved. Analyze yes. ______________ oxygen . must gain ______ Step 5. Nonmetal atoms _________ Solve Step 3. Inc. a. publishing as Pearson Prentice Hall. exist as gases or liquids at room temperature Chapter 8 Covalent Bonding 69 . molecules are called ______________________ 5. water c. exist as molecules. © Pearson Education.05_Chem_GRSW_Ch08. Circle the letter of the substances that do NOT exist as molecules in nature. All rights reserved. List two properties of molecular compounds. 3. Molecules and Molecular Compounds (pages 213–214) 1. oxygen b. neon d. What is a covalent bond? A covalent bond is a bond formed when two atoms share electrons. helium 6.1 MOLECULAR COMPOUNDS (pages 213–216) This section explains how to distinguish between ionic and molecular compounds.. Compounds that are formed when two or more atoms combine to form molecular compounds . 4. Inc. a. noble gases 2.SE/TE 6/12/04 11:10 AM Page 69 Name ___________________________ 8 Date ___________________ Class __________________ COVALENT BONDING SECTION 8. What is a molecule? A molecule is a neutral group of atoms joined together by covalent bonds. with the exception of the ______________________ . low melting and boiling points b. ozone e. Most elements found in nature. Is the following sentence true or false? A molecular formula shows the false arrangement of the atoms in a molecule. ammonia c. NH3 11. _______________ H H a 13. carbon dioxide a. ethane b. _______________ c 15. CO2 c _______10. _______________ 70 Guided Reading and Study Workbook N H H e 16. b _______ 8. All rights reserved. match the type of model or formula with its representation. What is a molecular formula? A molecular formula shows the types and numbers of atoms present in a molecule of a compound. C2H6 a _______ 9. molecular formula e. ball-and-stick model d. Match each compound with its molecular formula. space-filling molecular model b.SE/TE 6/12/04 11:10 AM Page 70 Name ___________________________ Date ___________________ Class __________________ CHAPTER 8. _______________ 17.. ______________________ In the diagram. perspective drawing H NH3(g ) b 12. a. Covalent Bonding (continued) Molecular Formulas (pages 215–216) 7. Inc. H N . structural formula c. _______________ N H H H N H H d 14. What is the arrangement of atoms within a molecule called? molecular structure ___________________________ H © Pearson Education.05_Chem_GRSW_Ch08. publishing as Pearson Prentice Hall. SE/TE 6/12/04 11:10 AM Page 71 Name ___________________________ Date ___________________ Class __________________ SECTION 8. Inc. Is the following sentence true or false? A shared pair of electrons is represented false by a double dash. © Pearson Education. How does electron sharing occur in forming covalent bonds? Sharing of electrons usually occurs so that atoms acquire the electron configurations of noble gases. O H H 5. and exceptions to the octet rule. H2O2 H c. NH3 H C H b. 4. H N H H H O O H H a. 7. CH4 Double and Triple Covalent Bonds (pages 221–222) 6.05_Chem_GRSW_Ch08. How many covalent bonds are in the nitrogen molecule? three ______________________ Chapter 8 Covalent Bonding 71 . The Octet Rule in Covalent Bonding (page 217) 1. Use the electron dot diagram below. It also describes and gives examples of coordinate covalent bonding. All rights reserved. Structural formulas show the arrangement of ______________________ in molecules. publishing as Pearson Prentice Hall. A chemical bond formed when atoms share two pairs of electrons is called a(n) double covalent bond . Complete the electron dot structure for each molecule. double. Single Covalent Bonds (pages 217–220) 2. Circle each unshared pair of electrons in a water molecule. resonance structures. and triple covalent bonds. ______________________ atoms 3.2 THE NATURE OF COVALENT BONDING (pages 217–220) This section uses electron dot structures to show the formation of single. Each molecule contains only single covalent bonds.. depending on the kind and number © Pearson Education. A compare/contrast table can help you do this. 1. publishing as Pearson Prentice Hall. Students’ tables should include the basic information about the three types of hybrid orbitals contained on pages 235–236.05_Chem_GRSW_Ch08.0 c. and sp3. Inc. Describe how electrons are shared in each type of bond. On a separate sheet of paper. nonpolar covalent c _______ 7. very polar covalent a _______ 8. charge? _______________________________________________________________________ therefore. 0. ionic d _______ 6. and. Write equally or unequally. or ionic. Is the following statement true or false? Covalent bonds differ in the way electrons are shared by the bonded atoms. 2.SE/TE 6/12/04 11:10 AM Page 75 Name ___________________________ Date ___________________ Class __________________ Reading Skill Practice You can increase your understanding of what you have read by making comparisons. Then list the characteristics that will form the basis of your comparison above each column. All rights reserved. bond? The polarity of the bond? ______________________ JKL Match the electronegativity difference range with the most probable type of bond that will form. equally unequally a. What symbols are used to represent the charges on atoms in a polar covalent or . Component Orbitals. attracts the bonding electrons slightly away from hydrogen.. and Bond Angle. Bond Polarity (pages 237–238) 1. Why does the chlorine atom in hydrogen chloride acquire a slightly negative Chlorine has a higher electronegativity than hydrogen. b _______ 5. Number of Bonds.0 b. 4. The column heads should be Number of Hybrid Orbitals.4 POLAR BONDS AND MOLECULES (pages 237–244) This section explains the use of electronegativity values to classify a bond as nonpolar covalent. moderately polar covalent Chapter 8 Covalent Bonding 75 .0–2. SECTION 8. sp 2.4–1. 0.0 d. ______________________ 2. polar covalent. The three heads for the rows should be sp. Polar bond ______________________ 3. draw a table to compare the three types of hybrid orbitals as explained on pages 235 and 236. Nonpolar bond ______________________ b.0–0. It also names and describes the weak attractive forces that hold groups of molecules together.4 a. true of atoms joined together. The strongest of the intermolecular forces are ______________________ . ___________________ Intermolecular Attractions and Molecular Properties (pages 243–244) 14. Is the following sentence true or false? Dispersion forces generally increase true in strength as the number of electrons in a molecule increases. or gas Melting point high low Solubility in water usually high high to low 76 Guided Reading and Study Workbook © Pearson Education. What determines the physical properties of a compound? The physical properties depend on the type of bonding in the compound. HCl ______________________ Attractions Between Molecules (pages 240–241) 11.05_Chem_GRSW_Ch08. they all line up with the same orientation in relation to the charged plates. When polar molecules are placed in an electric field. Covalent Bonding (continued) Polar Molecules (pages 239–240) 9. Complete the following table comparing ionic and covalent compounds. Characteristic Ionic Compound Covalent Compound Representative unit formula unit molecule Physical state solid solid. A molecule containing a polar bond is always polar.4 on page 244. c.. 10. Some regions of a polar molecule are slightly negative and some are slightly positive. 15. Circle the letter of each sentence that is true about polar molecules. CO2 ______________________ polar d. b. a. . All rights reserved.SE/TE 6/12/04 11:10 AM Page 76 Name ___________________________ Date ___________________ Class __________________ CHAPTER 8. d. Use Table 8. NH3 ______________________ nonpolar b. Are the following molecules polar or nonpolar? polar a. publishing as Pearson Prentice Hall. 12. What causes dispersion? Dispersion forces are caused by the motion of electrons. liquid. Inc. H2O ______________________ polar c. A molecule that has two poles is called a dipolar molecule. hydrogen bonds 13. difference 0 Step 3. Br 2.0. ______________________________ ionic b. difference 1 d. ______________________________ very polar covalent c.3 on page 238 to determine the most probable type of bond for each compound.0 moderately polar covalent__ _________________________ 1. moderately polar covalent a. Br 2. What is the most probable type of bond for each electronegativity difference range? Electronegativity Difference Range Most Probable Type of Bond 0. C and O d. a.5..8 .0 ionic _________________________ __ Calculate Step 2. Br and Br Analyze Step 1. Refer to Table 8. very polar covalent.4 nonpolar covalent _________________________ __ 0. From Table 6. determine the electronegativity values and differences for each pair of elements.8. ______________________________ Evaluate Step 4. K 0. ______________________________ nonpolar covalent d. K and Cl c. Br 2.0–2. or ionic. All rights reserved. difference 0. difference 2.1.SE/TE 6/12/04 11:10 AM Page 77 Name ___________________________ Date ___________________ Class __________________ GUIDED PRACTICE PROBLEM GUIDED PRACTICE PROBLEM 19 (page 239) 19. © Pearson Education.4–1.0–0.8 . How do you know that your answers are correct? The answers are consistent with the magnitudes of the electronegativity differences. Identify the bonds between atoms of each pair of elements as nonpolar covalent. Cl 3.7 b. Chapter 8 Covalent Bonding 77 .2 c. Inc.0 very polar covalent _________________________ __ 2. C 2.2 on page 177. O 3.5 . moderately polar covalent.8 .05_Chem_GRSW_Ch08. a. H 2. H and Br b. publishing as Pearson Prentice Hall. Circle the letter of the type of element that often has more than one common ionic charge. © Pearson Education. or 3A ion determined? The ionic charge is numerically equal to the group number.SE/TE 6/11/04 3:33 PM Page 79 Name ___________________________ 9 Date ___________________ Class __________________ CHEMICAL NAMES AND FORMULAS SECTION 9. and the suffix -ic to name the cation with the greater ______________________ charge. It also defines polyatomic ion and gives the names and formulas for the most common polyatomic ions. transition metal d. alkali metal b. alkaline earth metal c. publishing as Pearson Prentice Hall. a. 2A. Inc. How is the ionic charge of a Group 1A. or 7A is determined by subtracting 8 from the group number. Chapter 9 Chemical Names and Formulas 79 . The ______________________ of naming transition metal cations uses a Roman numeral in parentheses to indicate the numeric value of the ionic charge. How is the ionic charge of a Group 5A. Monatomic Ions (pages 253–256) 1. 6A.. 2. or 7A ion determined? The charge of an ion in Groups 5A. 6. 6A. An older naming system uses the suffix -ous to name the cation with the lesser ______________________ charge. 4. 7. What is a major advantage of the Stock system over the old naming system? The Stock system gives the actual charge of the ion. All rights reserved. nonmetal Stock system 5.1 NAMING IONS (pages 253–258) This section explains the use of the periodic table to determine the charge of an ion. 3. What are monatomic ions? Monatomic ions are ions consisting of only one atom.05_Chem_GRSW_Ch09. How many atoms make up the oxalate ion and what is its charge? It is made up of 6 atoms (2 carbon atoms and 4 oxygen atoms) and it has a charge of 2. 12. publishing as Pearson Prentice Hall. Inc.05_Chem_GRSW_Ch09. phosphate 13. Element Name Formula Fluorine fluoride ion F– Calcium calcium ion Ca2+ Oxygen oxide ion O2– Polyatomic Ions (pages 257–258) 9. What is the difference between the anions sulfite and sulfate? The sulfite ion has one less oxygen atom than the sulfate ion. Is the following sentence true or false? The names of polyatomic anions always false end in -ide. What is a polyatomic ion? A polyatomic ion is a tightly bound group of atoms that behaves as a unit and carries a charge.3 on page 257. a. ____________________________________________ 80 Guided Reading and Study Workbook © Pearson Education.. Chemical Names and Formulas (continued) 8. b. 10. ______________________ 11. All rights reserved. ____________________________________________ dihydrogen phosphate ion c. ammonium . Use the periodic table to write the name and formula (including charge) for each ion in the table below. acetate c. 14. oxalate d. Look at Table 9. Circle the letter of a polyatomic ion that is a cation.SE/TE 6/11/04 3:33 PM Page 80 Name ___________________________ Date ___________________ Class __________________ CHAPTER 9. What three hydrogen-containing polyatomic anions are essential components of living systems? hydrogen carbonate ion a. ____________________________________________ hydrogen phosphate ion b. Na. All rights reserved. S2 ______________________ 6. __________________ N phosphate ion b. O2 ______________________ Na2S c. What are two methods for writing a balanced formula? finding the least common multiple of the charges a. cupric nitride ______________________ MgCl2 c. What are the formulas for these compounds? LiBr a. What is the general name for compounds composed of two elements? They are binary compounds. Binary Ionic Compounds (pages 260–263) property 1. Traditionally. ____________________________________________________________________ 5. Inc.SE/TE 6/11/04 3:33 PM Page 81 Name ___________________________ Date ___________________ Class __________________ 15. publishing as Pearson Prentice Hall.05_Chem_GRSW_Ch09. the charges of the ions balance must ______________________ . ______________________ nitrate ion c. lithium bromide ______________________ Cu3N2 b. ______________________ SECTION 9. Cr3. 4. The name of a binary ionic compound is written with the name of the cation anion ______________________ first followed by the name of the ______________________ . © Pearson Education. magnesium chloride ______________________ 7. Cl ______________________ Cr2O3 b. What are the formulas for the compounds formed by the following pairs of ions? FeCl2 a.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS (pages 260–266) This section explains the rules for naming and writing formulas for binary ionic compounds and compounds containing a polyatomic ion. __________________________________________________ 3. Identify each of the ions shown below. Look at Figure 9. common names were based on some ______________________ of source a compound or its ______________________ . When writing the formula for any ionic compound. 3 1 1 P N ammonium ion a. 2. Fe2.5 on page 257. Chapter 9 Chemical Names and Formulas 81 .. ____________________________________________________________________ using the crisscross method b. Why are parentheses used to write the formula Al(OH)3? 13. MgCl2 __________________________________ aluminum selenide c. Inc. Complete the table for these ionic compounds containing polyatomic ions. How can you tell that cobalt(II) iodide is a binary ionic compound formed by a transition metal with more than one ionic charge? The name includes a Roman numeral representing the ionic charge of the transition metal cation.SE/TE 6/11/04 3:33 PM Page 82 Name ___________________________ Date ___________________ Class __________________ CHAPTER 9. 12. 9. Write the names for these binary ionic compounds. The parentheses indicate how many polyatomic ions are needed in the formula. Chemical Names and Formulas (continued) 8. PbS lead(II) sulfide __________________________________ magnesium chloride b. Cation Anion Name Formula NH4+ S2 ammonium sulfide (NH4)2S Fe3+ CO32– iron(III) carbonate Fe2(CO3)3 Ag+ NO3 K+ CN– 82 Guided Reading and Study Workbook silver nitrate potassium cyanide AgNO3 KCN © Pearson Education. All rights reserved. a. . publishing as Pearson Prentice Hall. Al2Se3 __________________________________ Compounds with Polyatomic Ions (pages 264–266) 10. What is a polyatomic ion? A polyatomic ion contains more than one element. 11..05_Chem_GRSW_Ch09. How do you write the formula for a compound containing a polyatomic ion? Write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges. Is the following sentence true or false? Two nonmetallic elements can combine false in only one way. All rights reserved. a metal and a nonmetal c. Naming Binary Molecular Compounds (pages 268–269) 1. octa- a. What method is used to distinguish between different molecular compounds Prefixes are used. P4S7 ____________________________________________ Writing Formulas for Binary Molecular Compounds (page 270) 9. nitrogen triiodide ______________________ ICl c. 8 d _______ 7.3 NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS (pages 268–270) This section explains the rules for naming and writing formulas for binary molecular compounds.05_Chem_GRSW_Ch09. tetra- b. N2O4 ____________________________________________ tetraphosphorus heptasulfide c. What are the names of the following compounds? boron trifluoride a.. nona- d.SE/TE 6/11/04 3:33 PM Page 83 Name ___________________________ Date ___________________ Class __________________ SECTION 9. two nonmetallic elements b. ______________________ 3. c _______ 4. BF3 ____________________________________________ dinitrogen tetroxide b. 7 b _______ 6. 4 a _______ 5. that contain the same elements? _________________________________________ © Pearson Education. What are the formulas for the following compounds? CBr4 a. publishing as Pearson Prentice Hall. Circle the letter of the type(s) of elements that form binary molecular compounds. tetraiodine nonaoxide ______________________ Chapter 9 Chemical Names and Formulas 83 . a. carbon tetrabromide ______________________ NI3 b. iodine monochloride ______________________ I4O9 d. Match the prefix with the number it indicates. two metals 2. hepta- c. Inc. 9 8. 05_Chem_GRSW_Ch09. Your summary should be shorter than the text on which it is based. What is the formula for hydrobromic acid? ______________________ . 4. Inc. H3PO3 Writing Formulas for Acids (page 272) 5. 2. Write a summary of the information in Section 9. Acids produce ______________________ ions when dissolved in water. What are the components of phosphorous acid? What is its formula? hydrogen ion and phosphite ion. When you write a summary. you can consider them to be combinations of anions hydrogen ______________________ connected to as many ______________________ ions as are necessary to create an electrically neutral compound. Do your work on a separate sheet of paper.4. publishing as Pearson Prentice Hall. Acid Name Formula Anion Name acetic acid HC2H3O2 acetate carbonic acid H2CO3 carbonate hydrochloric acid HCl chloride nitric acid HNO3 nitrate phosphoric acid H3PO4 phosphate sulfuric acid H2SO4 sulfate 84 Guided Reading and Study Workbook © Pearson Education.3 on pages 268–269.5 on page 272 to help you complete the table about acids. When naming acids.SE/TE 6/11/04 3:33 PM Page 84 Name ___________________________ Date ___________________ Class __________________ CHAPTER 9.. Use Table 9. All rights reserved.4 NAMING AND WRITING FORMULAS FOR ACIDS AND BASES (pages 271–273) This section explains the three rules for naming acids and shows how these rules can also be used to write the formulas for acids. Students’ summaries should focus on the main points of each subsection and include the information given in Table 9. Chemical Names and Formulas (continued) Reading Skill Practice Writing a summary can help you remember the information you have read. Naming Common Acids (pages 271–272) hydrogen 1. Names and formulas for bases are also explained. include only the most important points. HBr 3. SECTION 9. 5.05_Chem_GRSW_Ch09. not 1 : 1. The atomic mass of Li is 6. it contains 32 g of sulfur. Circle the whole-number mass ratio of Li to Cl in LiCl. How are bases named? Name the cation first followed by the anion (hydroxide ion). Inc. The atomic mass of C is 12. What is the law of multiple proportions? When two elements form more than one compound. the masses of the elements are always present in the same proportions. 5 : 1 c. No. the mass ratio of sulfur to oxygen is 1 : 1. The ratio 32 : 48 is equivalent to 2 : 3. A base is a compound that produces ______________________ when dissolved in water. 7. 1 : 12 b. the different masses of one element that combine with the same mass of the other element are in a ratio of small whole numbers.5 THE LAWS GOVERNING FORMULAS AND NAMES (pages 274–279) This section uses data to demonstrate that a compound obeys the law of definite proportions. SECTION 9. the atomic mass of Cl is 35. If the sample contains 48 g of oxygen.SE/TE 6/11/04 3:33 PM Page 85 Name ___________________________ Date ___________________ Class __________________ Names and Formulas for Bases (page 273) hydroxide ions 6. 12 : 1 4. In the compound sulfur dioxide. a.9. Is the sample sulfur dioxide? Explain. 2. Circle the whole-number mass ratio of carbon to hydrogen in C2H4. 1 : 6 c. It also explains how to use flow charts to write the name and formula of a compound. © Pearson Education. the atomic mass of H is 1. What is the law of definite proportions? In different samples of the same chemical compound. 6 : 1 d. Chapter 9 Chemical Names and Formulas 85 . publishing as Pearson Prentice Hall. 42 : 1 b.0. a.0. An 80-g sample of a compound composed of sulfur and oxygen contains 48 g of oxygen. All rights reserved. 1 : 5 3. a food preservative.5. The Laws of Definite and Multiple Proportions (pages 274–275) 1.. 3 g 4.05_Chem_GRSW_Ch09. 86 Guided Reading and Study Workbook © Pearson Education.55 1 Compound B 3. publishing as Pearson Prentice Hall. 8.. Prefixes d. Roman numeral e.SE/TE 6/11/04 3:33 PM Page 86 Name ___________________________ Date ___________________ Class __________________ CHAPTER 9.3 g 3.20 on page 277 to write the names of the following compounds: a. . Inc. Complete the table using the law of multiple proportions. An -ide ending generally indicates a ______________________ compound. NH4OH ___________________________________ d.1 2 Practicing Skills: Naming Chemical Compounds (pages 276–277) 7. How can a flowchart help you to name chemical compounds? It gives step-by-step directions for naming a compound. the net ionic charge is ______________________ .6 g 0. SnSe2 tin(IV) selenide ___________________________________ ammonium hydroxide c. ______________________ in a name generally indicate that the compound is molecular and show the number of each kind of atom in the molecule. Si3N4 trisilicon tetranitride ___________________________________ zero a. An -ite or -ate ending means there is a ______________________ ion that includes oxygen in the formula. 9. polyatomic c. Complete the following five rules for writing a chemical formula from a chemical name. Use the flowchart in Figure 9. A ______________________ after the name of a cation shows the ionic charge of the cation. binary b. HF hydrofluoric acid ___________________________________ e. Chemical Names and Formulas (continued) 6. In an ionic compound. Mass of Cu Mass of Cl Mass Ratio Cl : Cu Whole-number Ratio of Cl Compound A 8.6 g 1. CsCl cesium chloride ___________________________________ b. All rights reserved. potassium silicate ______________________ PCl5 b. Fill in the missing labels from Figure 9. publishing as Pearson Prentice Hall.05_Chem_GRSW_Ch09.3 for charges..1 for charges.SE/TE 6/11/04 3:33 PM Page 87 Name ___________________________ Date ___________________ Class __________________ Practicing Skills: Writing Chemical Formulas (page 278) 10. Inc. manganese(II) chromate ______________________ LiH d. Give charges for cations. diiodine pentoxide ______________________ Chapter 9 Chemical Names and Formulas 87 . All rights reserved. lithium hydride ______________________ I 2O5 e. phosphorus pentachloride ______________________ MnCrO4 c.22 to write the formulas of the following compounds: K2SiO3 a. Balance charges Use crisscross method. © Pearson Education. Use Table 9. Use the flowchart in Figure 9. Add parentheses for any multiple polyatomic ions. 11. Name of Compound Contains prefixes? yes Molecular compound Uses prefixes to write formula.22 on page 278. no Ionic compound Identify symbols Group A elements Roman numerals Polyatomic ions Use Table 9. ________________________________________________ Cu lost 1 electron. ________________________________________________ GUIDED PRACTICE PROBLEMS 10B AND 10C (page 263) 10. Fe3 b. Fe3 lost 3 electrons. 88 Guided Reading and Study Workbook 2 O 2 1 © Pearson Education. ___________ Li Evaluate Step 3. a. ________________________________________________ O 2 gained 2 electrons. b. How many electrons were lost or gained to form these ions? a.. Use the crisscross method to balance the formula. O2 c. Do the ions combine in a 1:1 ratio? No. Chemical Names and Formulas (continued) GUIDED PRACTICE PROBLEMS GUIDED PRACTICE PROBLEM 2 (page 256) 2. How do you know your formula is reasonable? The positive and negative charges are equal. Solve . Determine the number of electrons based on the size of the charge. Step 2. Determine whether the electrons were lost or gained based on the sign of the charge. Cu Step 1. O2– Analyze Step 1. publishing as Pearson Prentice Hall. Inc. Step 2. Write formulas for compounds formed from these pairs of ions. c. All rights reserved. Li20 Write the formula.05_Chem_GRSW_Ch09. the charges on the ions are not equal. b.SE/TE 6/11/04 3:33 PM Page 88 Name ___________________________ Date ___________________ Class __________________ CHAPTER 9. Li+ . Use the crisscross method to balance the formula. Ca 2 N 3 3 2 Ca3 N2 Write the formula. N3 Analyze Step 1. ___________ Evaluate Step 3. ____________________________ Cr 3 1 (NO3) 3 Chapter 9 Chemical Names and Formulas 89 . Cr(NO3)3 • Write the formula.05_Chem_GRSW_Ch09. Inc. Solve Step 2. How do you know this formula is reasonable? The positive and negative charges are equal. Ca2 . ________ • Use the crisscross method to balance the formula. It is ionic because it has no prefixes and it contains a metal. Write the formula for chromium(III) nitrate.SE/TE 6/11/04 3:33 PM Page 89 Name ___________________________ Date ___________________ Class __________________ c. because then the total charge would be negative. Will the calcium (Ca2+) and nitride (N3–) ions combine in a 1 : 1 ratio? How do you know? No. publishing as Pearson Prentice Hall. • Is the compound ionic or molecular? Explain.3 on page 257 to write the formula for NO3– the nitrate ion. All rights reserved. • Use Table 9.. GUIDED PRACTICE PROBLEM 13B (page 265) © Pearson Education. instead of neutral. 13b.
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