XIX.Chemistry, High School High School Chemistry Test The spring 2012 high school Chemistry test was based on learning standards in the Chemistry content strand of the Massachusetts Science and Technology/Engineering Curriculum Framework (2006). These learning standards appear on pages 69–73 of the Framework. The Science and Technology/Engineering Curriculum Framework is available on the Department website at www.doe.mass.edu/frameworks/current.html. Chemistry test results are reported under the following four MCAS reporting categories: ■ Atomic Structure and Periodicity ■ Bonding and Reactions ■ Properties of Matter and Thermochemistry ■ Solutions, Equilibrium, and Acid-Base Theory Test Sessions The high school Chemistry test included two separate test sessions, which were administered on consecutive days. Each session included multiple-choice and open-response questions. Reference Materials and Tools Each student taking the high school Chemistry test was provided with a Chemistry Formula and Constants Sheet/Periodic Table of the Elements. Copies of both sides of this formula sheet follow the final question in this chapter. Each student also had sole access to a calculator with at least four functions and a square-root key. The use of bilingual word-to-word dictionaries was allowed for current and former English language learner students only, during both Chemistry test sessions. No other reference tools or materials were allowed. Cross-Reference Information The table at the conclusion of this chapter indicates each item’s reporting category and the framework learning standard it assesses. The correct answers for multiple-choice questions are also displayed in the table. 330 Chemistry Session 1 DIRECTIONS This session contains twenty-one multiple-choice questions and two open-response questions. Mark your answers to these questions in the spaces provided in your Student Answer Booklet. You may work out solutions to multiple-choice questions in the test booklet. ID:252678 A Common EQ 1 ● ID:229504 A Common EQ Which of the following statements describes the difference between endothermic and exothermic chemical reactions? A. Energy is absorbed in endothermic reactions but is released in exothermic reactions. B. Energy is conserved in endothermic reactions but is not conserved in exothermic reactions. C. Endothermic reactions involve changes in the nucleus of an atom, but exothermic reactions do not involve changes in the nucleus. D. Endothermic reactions occur when electrons are shared between atoms, but exothermic reactions occur when electrons are transferred between atoms. 2 ● Cobalt has an atomic mass of 59 and an atomic number of 27. What does this information reveal about most cobalt atoms? A. They contain more neutrons than protons. B. They naturally have a net negative charge. C. They attract protons more strongly than electrons. D. They form ions with a charge of 127 in compounds. 331 Pure water 1 Water-sucrose solution 100 100 Temperature (°C) Temperature (°C) 332 . Water-sucrose solution C. 1 Water-sucrose solution D. Which of the following graphs best represents vapor pressure as a function of temperature for the two liquids? A. Pure water Vapor Pressure (atm) 1 Water-sucrose solution Vapor Pressure (atm) Pure water 1 100 100 Temperature (°C) Temperature (°C) Vapor Pressure (atm) Pure water Vapor Pressure (atm) B.eps [opt_a0 D Common EQ Session 1 3 ● A liquid boils when its vapor pressure equals the pressure of the atmosphere.Chemistry ID:260036 vp_graphsVH48. A student creates a graph of vapor pressure as a function of temperature for pure water and for a solution of water and sucrose. C B. electrons only H B. neutrons only C. and electrons 333 . neutrons. 5 ● H H C H Which of the following is a balanced equation for the synthesis of methane from carbon and hydrogen? A. C D. protons and neutrons D.Chemistry ID:229678 3210287_AR1. C2 H H 2H2 4H CH4 CH4 CH4 CH4 Which of the following subatomic particles can be found inside the nucleus of an atom? A. C4 C. protons.eps C Common EQ Session 1 ID:216946 C Common EQ ● 4 The diagram below represents one molecule of methane (CH4 ). ice and liquid mercury B.Chemistry ID:252153 A Common EQ Session 1 6 ● The table below contains data for mercury and water at standard pressure. which of the following pairs of substances could exist at the same temperature? A.0 Boiling Point (°C) 357 100 Based on the data in the table. water vapor and solid mercury D. Substance mercury water Melting Point (°C) 39 0. liquid water and solid mercury C. liquid water and mercury vapor 334 . using larger pieces of iron B. The balloon with argon will decrease most in volume because argon is a noble gas. B.Chemistry ID:206670 D Common EQ Session 1 ID:261470 D Common EQ 7 ● Three identical balloons each contain one mole of gas. increasing the concentration of the CuCl 2 solution ID:281962 B Common EQ 10 ● The equation below shows the reaction of ammonia with water. H2O ( l ) NH 4 ( aq ) OH ( aq ) ID:275846 B Common EQ 8 ● NH3 ( g ) How many electrons are in the outermost energy shell of a calcium atom? A. H 2O + C. which of the following is acting as the acid for the forward reaction? A. C. NH 3 B. 6 D. Fe(s) CuCl 2 (aq) FeCl 2 (aq) Cu(s) Which of the following changes would most likely increase the reaction rate? A. OH– 335 . Which of the following changes in volume will happen if the balloons are placed in a warmer room? A. 1 B. decreasing the volume of the CuCl 2 solution D. NH 4 D. 8 According to the Brønsted-Lowry theory of acids and bases. The balloon with oxygen will increase most in volume because oxygen has the largest molecules. performing the reaction in an ice bath C. All of the balloons will decrease in volume equally because the temperature increased. D. All of the balloons will increase in volume equally because they have equal numbers of molecules. 2 C. One balloon contains oxygen. one contains nitrogen. 9 ● A student adds iron filings to a copper(II) chloride solution at room temperature. and one contains argon. A balanced equation for the reaction that occurs is shown below. eps Common EQ 11 ● The diagrams below show a 0. The pH of the 0. or computations) in your Student Answer Booklet. • Show all your work (diagrams. based on the diagrams of the solutions and the definition of pH. • If you do the work in your head. explain in writing how you did the work. Explain your answer. Session 1 • BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION.1 M aqueous solution of HCl and a 0. Identify HCl and HF as acids or bases.1 M HCl 0. 336 . 0.1 M HF solution. Write your answer to question 11 in the space provided in your Student Answer Booklet.1 M HCl solution is expected to be lower than the pH of the 0. tables.1 M HF H+ Cl– H+ Cl– Cl– H+ H+ Cl– H+ H+ Cl– Cl– H+ Cl– H+ Cl– H+ Cl– H+ Cl– HF HF F– HF HF HF H+ F– HF HF HF H+ a.1 M aqueous solution of HF.Chemistry Question 11 is an open-response question. Explain why. b. ID:206688 206688_acid_base. Water molecules on the surface overcome intermolecular forces and change into the gas phase. D. 13 ● Which of the following is a correct Lewis dot structure for potassium chloride? A. C.Chemistry Session 1 Mark your answers to multiple-choice questions 12 through 22 in the spaces provided in your Student Answer Booklet. K [ Cl ] C. K2 [ Cl ]2 D. ID:287584 B Common EQ 12 ● ID:288254 AVEBRY075_potassiumchlori A Common EQ Which of the following statements best describes what happens to water during evaporation? A. but you may work out solutions to multiple-choice questions in the test booklet. K [ Cl ] B. B. Water molecules on the surface come in contact with air molecules and are pulled into the gas phase. K2 [ Cl ]2 337 . Do not write your answers in this test booklet. The temperature of the water increases until the water molecules separate and form oxygen and hydrogen gas. The temperature of the water increases until the water molecules react with nitrogen in the air. Nuclei gain electrons during fission and release electrons during fusion. Fission generates potential energy. 15 ● Iron(II) chloride (FeCl ) is a product of 2 the reaction between iron metal (Fe) and hydrochloric acid (HCl). B. C. Nuclei split during fission and combine during fusion. Fission forms heavier elements. and fusion forms lighter elements. and fusion generates kinetic energy. D. as shown in the equation below.Chemistry ID:287569 A Common EQ Session 1 ID:275840 A Common EQ 14 ● Which of the following statements best describes a difference between nuclear fission and nuclear fusion reactions? A. from 0 to 2 2 338 . from D. Fe 2 HC1 FeC12 H2 What is the change in oxidation number of iron in this reaction? A. from 1 to 2 2 1 to C. from 0 to B. The equation for this reaction at equilibrium is shown below. H2 (g) CO2 (g) H2O(g) CO(g) Which of the following changes in concentration occur when more water vapor is added to the system under equilibrium conditions? A. [CO 2] decreases. [CO] decreases 339 .Chemistry ID:260041 D Common EQ Session 1 16 ● The reduction of carbon dioxide by hydrogen gas takes place at 420°C to produce water vapor and carbon monoxide. [H 2] increases. [H 2] decreases. [H 2] decreases. [CO 2] increases. [H 2] increases. [CO] decreases C. [CO 2] increases. [CO] increases D. [CO 2] decreases. [CO] increases B. D. alkaline-earth metals C. To which of the following groups of elements does it belong? A. 18 ● A neutral atom has an outer shell electron configuration of 2s22p6. alkali metals B. halogens B. noble gases C. 340 . D.eps [opt_a C Common EQ Session 1 ID:216949 D Common EQ 17 ● Which of the following models best represents the shape of a compound with trigonal planar geometry? A.Chemistry ID:258965 014_shape_opts. Li C. F. The force of attraction between neighboring polar water molecules is weak. Be. Be D. Li. F B. The force of attraction between neighboring nonpolar water molecules is weak. F. O. Be. F. Li. O. 20 ● In which of the following lists are the elements shown in order of increasing electronegativity? A. B. C. O 341 . D. The force of attraction between neighboring polar water molecules is strong. The force of attraction between neighboring nonpolar water molecules is strong. O.Chemistry D:260762 B Common EQ Session 1 ID:264340 A Common EQ 19 ● Which of the following statements best explains why water has a high surface tension? A. Li. Be. gas to solid B.Chemistry ID:229235 B Common EQ Session 1 ID:264310 B Common EQ 21 ● The balanced equation below represents the reaction of NaOH with H 3PO 4. 9 g of water is produced. 60 g C. liquid to solid 342 . liquid to gas C. How 3PO 4 many grams of NaH 2PO 4 are produced? A. gas to liquid D. NaOH H3PO4 NaH2 PO4 H2O When 20 g of NaOH reacts with 49 g of H . 78 g 22 ● The average distance between molecules always increases during which of the following phase changes? A. 11 g B. 69 g D. b. Identify two chemical properties of zinc from the list.Chemistry Question 23 is an open-response question. or computations) in your Student Answer Booklet. Session 1 • BE SURE TO ANSWER AND LABEL ALL PARTS OF EACH QUESTION. Explain why the properties you identified are physical properties and not chemical properties. Write your answer to question 23 in the space provided in your Student Answer Booklet. • Show all your work (diagrams. 343 . ID:261154 Common EQ 23 ● Several properties for zinc (Zn) are listed below: • • • • • • • brittle at room temperature. Identify two physical properties of zinc from the list. tables. • If you do the work in your head. but malleable between 100°C and 150°C bluish-white in color burns in air at high temperatures. explain in writing how you did the work. Explain why the properties you identified are chemical properties and not physical properties. giving off zinc oxide (ZnO) gas conducts heat and electricity sinks in water reacts with acids and bases exposed surfaces tarnish in moist air a. carbon-14 undergoes decay to become nitrogen-14. tetracarbon chloride D. D. oxidation ID:252564 A Common EQ 25 ● Which of the following ideas was proposed by Niels Bohr? A. C. carbon 4-chloride B. 14 6C 26 ● Carbon reacts with chlorine to form CCl 4. fusion B. nuclear D. 1-carbon 4-chloride C. You may work out solutions to multiple-choice questions in the test booklet. 344 . Electrons occupy specific energy levels within an atom.Chemistry Session 2 DIRECTIONS This session contains nineteen multiple-choice questions and three open-response questions. An atom is a solid sphere that cannot be separated into smaller parts. neutralization C. ID:216947 C Common EQ 24 ● ID:229517 D Common EQ In radiocarbon dating. An atom consists of negative charges embedded in a positively charged sphere. The nucleus of an atom contains neutrons as well as protons. B. What is the name of this compound? A. carbon tetrachloride → 14 7N 1 0 −1 e What type of reaction is this? A. Mark your answers to these questions in the spaces provided in your Student Answer Booklet. 0 g 3 D.0 g 3 C.Chemistry ID:287582 C Common EQ Session 2 27 ● A student has 84. P 5 84.0 g 3 1 mol 3 R 3 500 L 28 g B. P 5 28 g 3R 1 mol 500 L 345 .0 g of N 2 gas in a sealed 500 L container at 20°C. P 5 84. P 5 84.0 g 3 28 g 3 R 3 293 K 3 500 L 1 mol 1 mol 3 R 3 293 K 28 g 500 L 84. Which of the following equations should the student use to calculate the gas pressure? A. 5 C. 4.5 D.0 atm.9 B. 6.Chemistry ID:258930 A Common EQ Session 2 28 ● A walk-in cooler has a volume of 1.0 102 mol 104 mol 105 mol 1023 mol 346 . 2. 4. If the temperature inside the cooler is 3°C and the gas pressure is 1.1 104 L. how many moles of gas are inside the cooler? A. 1 g/mol. Water has high surface tension. 128 g D. Al 2 O3 31 ● The chemical equation below represents sulfur trioxide (SO 3) in the atmosphere mixing with rainwater to form sulfuric acid (H 2SO 4). 105 g C. mixing baking soda and salt 347 . Water is a highly polar molecule. boiling water B. Water has a higher boiling point than predicted by its molar mass. dissolving salt in water D. 98. AlO B. What is the chemical formula for aluminum oxide? A. SO3(g) H 2 O(l ) H 2 SO 4 (l ) The molar mass of SO 3 is 80. AlO 2 C.0 g of SO 3 mixes with rainwater? A. Oxygen (O) needs two electrons to complete its outer shell.1 g ID:258937 B Common EQ 30 ● Which of the following statements best explains why ionic solids dissolve in water? A. D. C. How much H SO 2 4 is produced when 128.1 g/mol and the molar mass of H 2SO 4 is 98. Al 2 O D. 157 g ID:275834 B Common EQ Which of the following actions decreases the entropy of a system? A.Chemistry ID:216953 D Common EQ Session 2 ID:273206 D Common EQ 29 ● Aluminum (Al) has three electrons in its outer shell. Water is more dense as a liquid than as a solid. which is a major component of acid rain. freezing water C. 32 ● B. B. Explain why you identified this reaction as decomposition.Chemistry Question 33 is an open-response question. explain in writing how you did the work. Write your answer to question 33 in the space provided in your Student Answer Booklet. Reaction 1 Reaction 2 Reaction 3 Reaction 4 Reaction 5 2Mg Ca(OH)2 NH3 CaCO3 2 HCl HCl PbO 2 O2 CaO CaCl 2 NH 4 Cl Pb O2 CO 2 2H 2O 2 MgO a. Describe a combustion reaction. ID:287891 Common EQ 33 ● Five chemical reactions are listed in the table below. b. Write a balanced chemical equation for a combustion reaction using some or all of the substances from the table below. • Show all your work (diagrams. Identify one chemical reaction from the list that is a decomposition reaction. or computations) in your Student Answer Booklet. Explain why you identified this reaction as synthesis. c. tables. d. Session 2 • BE SURE TO ANSWER AND LABEL ALL PARTS OF EACH QUESTION. C 3H 8 O2 C CO 2 H 2 H 2O 348 . Identify one chemical reaction from the list that is a synthesis (combination) reaction. • If you do the work in your head. C. ID:258935 B Common EQ 35 ● A 6. solution of plasma and liquid. Buffers catalyze chemical reactions in the body cells. and more dense chemicals like diesel fuel and tar. 6 mL B. crude oil can best be classified as a A.0 M solution would be used to prepare 100. 36 ● After crude oil is pumped out of the ground. B. Buffers maintain a constant pH in the blood. How many milliliters of the 6. Buffers decompose food molecules during digestion. D.Chemistry Session 2 Mark your answers to multiple-choice questions 34 through 43 in the spaces provided in your Student Answer Booklet. 17 mL C. 33 mL D. B. D.” The tower separates it into less dense chemicals like butane and gasoline.0 M solution of HCl is diluted to 1. Based on this information. Buffers dissolve salts and minerals in the blood.0 mL of the diluted 1. 100 mL 349 . but you may work out solutions to multiple-choice questions in the test booklet.0 M solution? A. it must be processed in a “cracking tower. mixture of compounds. C. Do not write your answers in this test booklet.0 M. pure compound. mixture of pure elements. ID:275928 A Common EQ 34 ● ID:251804 B Common EQ Which of the following statements explains why the human body produces chemical buffers? A. 56. Their positions are becoming fixed in crystals. Their average distance from adjacent molecules is increasing. Their valence electrons are being lost. B. a metal in group 14 (4A) C. a metal in group 1 (1A) B. which of the following is happening to the molecules of the liquid? A.Chemistry ID:229652 A Common EQ Session 2 ID:274061 B Common EQ 37 ● When a cup of hot chocolate cools from 90°C to 80°C. Physical Properties: shiny silver-colored solid easily flattened with small hammer denser than water has 4 valence electrons • • • • Chemical Properties: • does not react with sodium • reacts slowly with oxygen Based on this information.6% C. 3. C. 39 ● The table below provides some information about an unidentified element.00% B. Their rate of motion is decreasing. a nonmetal in period 4 D. What is the percent yield if the theoretical yield is 18.1% 350 . D. a metalloid in period 5 ID:275857 C Common EQ 38 ● A reaction yields 6.81 g? A.3% D. the unidentified element is best classified as which of the following? A. 33. 10.26 g of a product. 6 4. Element carbon fluorine hydrogen oxygen Electronegativity 2. carbon–hydrogen B. B. A gamma ray has no mass.4 Which of the following bonds is the most polar? A. A gamma ray has a positive charge.0 2. C.2 3. fluorine–fluorine D.Chemistry ID:281286 A Common EQ Session 2 ID:246822 B Common EQ 40 ● Which of the following statements describes a gamma ray? A. A gamma ray can be converted into a beta particle. hydrogen–oxygen 351 . 41 ● The table below shows the electronegativities of four elements. carbon–fluorine C. A gamma ray can be stopped by a sheet of paper. D. removing the stopper C. decreasing the water temperature D. 352 . The number of molecules in the bubbles remains the same. pouring off half the water D. C. 43 ● When a scuba diver is deep underwater and exhales. The number of molecules in the bubbles increases. Erlenmeyer flask Water at 20°C Cube of NaCl Which of the following changes will cause the cube to dissolve more quickly? A. and the diameter of the bubbles decreases. swirling the flask B. air bubbles form and rise to the surface of the water. and the diameter of the bubbles decreases. and the diameter of the bubbles increases. The number of molecules in the bubbles decreases.eps A Common EQ Session 2 ID:273212 C Common EQ 42 ● The diagram below shows a cube of sodium chloride beginning to dissolve in water. B. Which of the following statements best describes what happens to the air bubbles as they rise to the surface? A. and the diameter of the bubbles increases.Chemistry ID:208301 208301_saltflask. The number of molecules in the bubbles remains the same. ID:281306 Common EQ 44 ● The elements helium. 353 . or computations) in your Student Answer Booklet. tables. Explain why the atomic number increases from helium to neon to xenon.Chemistry Questions 44 and 45 are open-response questions. Write your answer to question 44 in the space provided in your Student Answer Booklet. neon. a. neon. explain in writing how you did the work. c. and xenon are located in group 18 (8A) in the periodic table. and xenon and explain how the location of these elements in the periodic table relates to their chemical reactivity. • Show all your work (diagrams. neon. • If you do the work in your head. and xenon are located in different periods in the periodic table. Session 2 • BE SURE TO ANSWER AND LABEL ALL PARTS OF EACH QUESTION. Describe the chemical reactivity of helium. b. Explain why helium. formed when 100 mol of O 2 is released. Calculate the amount of glucose. Show your calculations and include units in your answer. 6 CO 2 6H 2 O sunlight C6 H12 O6 6 O2 a. 354 .Chemistry Session 2 Write your answer to question 45 in the space provided in your Student Answer Booklet. Assume excess water is available. c. ID:287607 Common EQ 45 ● Glucose (C ) is formed in plants by the process of photosynthesis. The net equation for 6H 12O 6 photosynthesis is shown below. Show your calculations and include units in your answer. b. in grams. Explain how the amount of carbon dioxide consumed by a plant can be determined from measuring the amount of oxygen released by the plant. Calculate the molar mass of glucose. 4 L/mol Ideal Gas Constant: R 5 0.Massachusetts Comprehensive Assessment System Chemistry Formula and Constants Sheet Common Polyatomic Ions Ion Ammonium Carbonate Hydroxide Nitrate Phosphate Sulfate Combined Gas Law: P1 V1 PV 5 2 2 T1 T2 Ionic Formula NH41 CO32OHNO3PO43SO42- Ideal Gas Law: PV 5 nRT Dilution Formula: M1V1 5 M2V2 Molar Volume of Ideal Gas at STP: 22.31 L • kPa/mol • K STP: 1 atm (101.02 3 1023 particles/mol Nuclear Symbols Name Alpha particle Beta particle Gamma ray Neutron Symbol or 4 2 He b or −0 1e 1 0n 355 .3 kPa).0821 L • atm/mol • K 5 8. 273 K (0°C) Absolute Temperature Conversion: K 5 °C 1 273 Definition of pH: pH 5 log [H3O1] 5 log [H1] Avogadro’s Number: 6. 09 N 7 Nitrogen 30.62 88.50 164.60 Br 34 35 Selenium Bromine 126.69 63.01 20.94 9.Massachusetts Department of ELEMENTARY & SECONDARY Massachusetts Comprehensive Assessment System Periodic Table of the Elements 8A 18 Group (Family) 1A 1 1.87 K Cr Mn 27 Cobalt 28 Nickel 29 Copper (98) 95.59 In 49 Indium 204. “Atomic Weights of the Elements 2007.91 140.41 Ga 114.91 144.01 H Key: 4.22 92.10 40.55 65.42 107.04 La Ce Pr 59 Praseodymium Nd 60 238.71 As 31 33 32 Gallium Germanium Arsenic 121.39 Na 8B 9 10 1B 11 2B 12 5B 5 50.97 Cd 48 Cadmium 200.” .91 137. 138.33 6 72 73 74 75 76 Hafnium Tantalum Tungsten Rhenium Osmium (267) (268) (271) (272) (277) (276) Cs Ba Hf T a W Re Os Ir 77 Iridium Pt 78 Platinum (281) Au 79 Gold (280) Hg 80 Mercury Tl 81 Thallium Pb 82 Lead Bi Po At 83 84 85 Bismuth Polonium Astatine Rn 86 Radon 55 Cesium 56 Barium (223) (226) 7 104 Rutherfordium Fr Rf Db Sg Bh Ra Hs Mt Ds 110 Darmstadtium Rg 111 Roentgenium 87 88 Francium Radium 105 107 108 109 106 Dubnium Seaborgium Bohrium Hassium Meitnerium Mass numbers in parentheses are those of the most stable or most common isotope.06 F 9 Fluorine 35.96 Cl 17 Chlorine 79.01 6A 16 16.96 Period 4 26 Iron 101.96 157.03 Pm 61 (237) Sm 62 (244) Eu (243) Gd (247) Tb (247) Dy (251) Ho 65 63 67 64 66 Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium (252) Er 68 Erbium (257) Tm (258) Yb (259) Lu 69 70 71 Thulium Ytterbium Lutetium (262) 231.85 186.91 106.85 58.99 24.47 87.95 3 Lithium 4 Beryllium 22.95 195.08 44.07 102.97 O 8 Oxygen 32.93 58.94 Mg 6B 6 7B 7 47.93 173.38 Sn 50 Tin 207.29 356 Zr Mo 42 Molybdenum 183.24 (145) 150.98 Li Be B C 6 Carbon 28.18 2 5 Boron 26.45 Ne 10 Neon 39.82 Ge 118.93 162.90 Ar 18 Argon 83.00 6.22 19 20 21 22 23 24 25 Potassium Calcium Scandium Titanium Vanadium Chromium Manganese 85.12 140.94 91.04 Actinide Series 89 Actinium Ac Th Pa U Np Pu Am 92 94 90 93 91 95 Thorium Protactinium Uranium Neptunium Plutonium Americium Cm 96 Curium Bk 97 Cf 98 Es 99 Fm 100 Berkelium Californium Einsteinium Fermium Md 101 Mendelevium No Lr 102 103 Nobelium Lawrencium *Revised based on IUPAC Commission on Atomic Weights and Isotopic Abundances.91 Kr 36 Krypton 131.08 Rb Tc Ru Sr Y Nb Rh Pd Ag 47 Silver 196.21 190.93 167.04 174.72 Si 14 Silicon 72.26 168.00 7A 17 19.88 Al 13 Aluminum 69.75 Se 127.91 5 43 44 178.98 T e 51 52 Antimony Tellurium (209) (210) I 53 Iodine Xe 54 Xenon (222) 37 38 Rubidium Strontium 39 40 41 Yttrium Zirconium Niobium 45 46 Technetium Ruthenium Rhodium Palladium 132.91 Ca Sc Ti V Fe Co Ni Cu Zn 30 Zinc 112.01 1 atomic weight Symbol atomic number Name 3A 13 10.80 39.00 54.36 151.25 158.2 Sb 208.00 He 2 Helium 1 Hydrogen 1 2A 2 4A 14 5A 15 14.49 180.81 12.97 Lanthanide Series 57 58 Lanthanum Cerium (227) 232.23 192.94 52.59 P 15 Phosphorus 74.31 3 4B 4 8 55.92 11 12 Sodium Magnesium 3B 3 S 16 Sulfur 78. 2 7.5 3.4 7.5 A B B A C B A C A D C A D B D B B A A A D C D B A B B Correct Answer (MC)* A A D C C A D B D B 357 .4 2.3 1.1 7.3 4. Equilibrium and Acid Base Theory Properties of Matter and Thermochemistry Properties of Matter and Thermochemistry Bonding and Reactions Atomic Structure and Periodicity Atomic Structure and Periodicity Standard 6.5 8.5 5.4 3. and Correct Answers* Item No. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 Page No.3 5.3 7.3 1. Equilibrium and Acid Base Theory Solutions.2 6.1 4.2 2. Equilibrium and Acid Base Theory Bonding and Reactions Atomic Structure and Periodicity Bonding and Reactions Atomic Structure and Periodicity Atomic Structure and Periodicity Properties of Matter and Thermochemistry Properties of Matter and Thermochemistry Atomic Structure and Periodicity Atomic Structure and Periodicity Bonding and Reactions Properties of Matter and Thermochemistry Properties of Matter and Thermochemistry Bonding and Reactions Solutions. 331 331 332 333 333 334 335 335 335 335 336 337 337 338 338 339 340 340 341 341 342 342 343 344 344 344 345 346 347 347 347 347 348 349 349 349 350 350 350 351 Reporting Category Properties of Matter and Thermochemistry Atomic Structure and Periodicity Solutions.1 8.7 8. Equilibrium and Acid Base Theory Solutions.2 8.5 6.High School Chemistry Spring 2012 Released Items: Reporting Categories.2 4.2 6.2 2.2 1.2 6.1 5. Equilibrium and Acid Base Theory Bonding and Reactions Properties of Matter and Thermochemistry Bonding and Reactions Solutions.1 2.1 2.3 4. Equilibrium and Acid Base Theory Properties of Matter and Thermochemistry Bonding and Reactions Atomic Structure and Periodicity Bonding and Reactions Solutions.6 4. Standards.2 1.4 2.1 6.6 2.4 5.6 3. Equilibrium and Acid Base Theory Bonding and Reactions Atomic Structure and Periodicity Properties of Matter and Thermochemistry Properties of Matter and Thermochemistry Atomic Structure and Periodicity Solutions.1 2. Equilibrium and Acid Base Theory Solutions.6 6.4 7. 351 352 352 353 354 Reporting Category Bonding and Reactions Solutions. which are indicated by shaded cells.3 7. will be posted to the Department’s website later this year. Equilibrium and Acid Base Theory Properties of Matter and Thermochemistry Atomic Structure and Periodicity Bonding and Reactions Standard 4.1 5.3 Correct Answer (MC)* B A C * Answers are provided here for multiple-choice items only. Sample responses and scoring guidelines for open-response items.Item No.1 3. 41 42 43 44 45 Page No.3 6. 358 .