Chemistry Released

NameRELEASED FORM Chemistry Form A Chemistry R EL Public Schools of North Carolina www.ncpublicschools.org State Board of Education Department of Public Instruction Division of Accountability Services/North Carolina Testing Program Raleigh, North Carolina 27699-6314 © 2009 All rights reserved. This document may not be reproduced by any means, in whole or in part, without prior written permission from the North Carolina Department of Public Instruction, Raleigh, North Carolina. EA North Carolina Test of SE D A NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 1. How many protons and electrons are + in a 64 Cu2 ion? 29 4. Why did most of the alpha particles go straight through the gold foil in Rutherford’s experiment? A B C Most of an atom is empty space. A B C D 27 protons, 29 electrons 27 protons, 31 electrons 29 protons, 27 electrons 29 protons, 31 electrons Alpha particles are positively charged. Alpha particles move with high velocity. The center of an atom is positively charged. 2. What is the name of the compound with the chemical formula CrCl3 ? A B C D chromium tetrachloride chromium trichloride chromium(II) chloride chromium(III) chloride EA C D 3. If two oxygen atoms combine to make a molecule, what type of bond will they form? A B C an ionic bond R EL a hydrogen bond a double covalent bond D a metallic bond Page 1 SE D D 5. How does an S 2 ion differ from an electrically neutral sulfur atom? mass number − A B atomic number nuclear charge number of electrons 6. A gas under a pressure of 74 mmHg and at a temperature of 75°C occupies a 500.0-L container. How many moles of gas are in the container? A B C D 1.7 moles 7.9 moles 13 moles 59 moles Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 7. A chemistry student is given 5 samples of a metal. The student measures and records the mass and the volume of each sample and then graphs the data, as shown below. Mass vs. Volume of a Metal 600 What is the identity of the metal? A B C D aluminum iron nickel lead R EL 8. A Which orbital notation represents an s-block element in the third period? 1s B 1s C 1s 2s D 1s EA 2s 2s 2p 3s 2p 3s 3p 2s 2p 3s 3p 4s 3d Page 2 SE D 400 300 200 100 0 10 20 30 40 50 Volume (cm3) 500 Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 9. What is the volume of 2.00 moles of nitrogen gas (N 2) at STP? A B C D 11.2 L 28.0 L 44.8 L 56.0 L 10. According to this balanced chemical equation, what volume of C2H2 is required to form 40.0 L of CO2 ? 2C2H2 (g) + 5O2 (g) → 2H2O (g) + 4CO2 (g) A B C D 20.0 L 44.8 L 80.0 L 100 L R EL Page 3 Go to next page EA SE D NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 11. In an experiment, 2.62 g of iron react completely with 1.50 g of sulfur. What is the empirical formula for the compound produced? A B C D FeS FeS2 12. What do the ions K +, Ca 2+, and Cl − have in common? A B C They have the same number of protons. They will form covalent bonds with oxygen. They have the same electron configuration as argon. They are larger than their corresponding atoms. Fe2S Fe2S3 R EL Page 4 Go to next page EA SE D D NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 13. This graph represents a heating curve of a substance. Heating Curve 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 I IV V II Which region on the graph represents the solid phase? A I R EL B C II III D IV Page 5 EA 0 6 12 18 24 30 36 42 48 54 60 66 72 78 84 90 Time (min) SE D III Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 14. 42 When 19 K undergoes radioactive decay, the result is two products, one 15. This graph is a potential energy diagram for a chemical reaction. of which is calcium-42. What is the other product? A B C D 4 2 Potential Energy Diagram He 2 4 He 1 1 e e 0 −1 EA A B C D R EL Page 6 Go to next page SE D V VI II IV III I Reaction Coordinate Which energy measure will remain unchanged with the addition of a catalyst? II IV V VI NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 16. What type of chemical reaction is represented by this balanced equation? 19. Which substance can act as either an acid or a base according to the Brønsted-Lowry definition? A B C H3O1 + NH1 + 4 HOH HCl S8 (s) + 8O2 (g) → 8SO2 ( g) A B C D synthesis decomposition single replacement double replacement 17. Which chemical equation is balanced? A B C D LiOH + CO2 → Li2CO3 + H2O 2LiOH + CO2 → Li2CO3 + H2O LiOH + 3CO2 → 2Li2CO3 + H2O EA D 4LiOH + CO2 → Li2CO3 + 2H2O 18. Neutralization occurs when 15.0 mL of KOH react with 25.0 mL of HNO3 . If the molarity of HNO3 is 0.750 M, what is the molarity of the KOH? R EL A 1.67 M 1.25 M B C 0.600 M 0.450 M D Page 7 SE D D 20. A −2 What is the oxidation number of sulfur in BaSO4 ? B 0 C +1 +6 Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 21. This diagram represents a phase diagram for a substance. Phase Diagram 2 1 5 6 At which point do solid, liquid, and gas phases exist in equilibrium? A B C D 1 2 4 R EL Page 8 Go to next page EA 3 SE D 4 3 Temperature (K) NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 22. Using the solubility graph provided, a student performs an experiment to find the solubility of a substance. The student finds the amount of substance needed to make a saturated solution in 100 g of water at different temperatures. The student’s data are shown in the table below the graph. Solubility Graph 140 130 120 110 100 90 80 70 60 50 40 30 20 10 Sodium Nitrate R EL Trial 1 2 A Sodium Nitrate What is the identity of the substance? B C Potassium Nitrate Sodium Chloride Potassium Chlorate D Page 9 EA 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C) Student Data Temperature (°C) Salt in 100 g of water (g) of Water 25 40 68 126 SE D Potassium Iodide Potassium Nitrate Sodium Chloride Potassium Chlorate 150 Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 23. What is the correct chemical formula for sodium sulfate? A B C D NaSO4 Na 2SO4 26. What are the differences between these isotopes of hydrogen shown below? 1 1 H , 2 H , and 3 H 1 1 A Na(SO4 )2 Na 2(SO4 )2 24. Which compound contains both covalent and ionic bonds? A B C D CaCO3 CO2 H2O NaCl EA A B C D 28. 25. R EL A 10.2 L 76.6 L 92.4 L In a flexible container, 15.9 L of gas is under 589 kPa of pressure at a temperature of 56.5°C. If the pressure and temperature change to STP, what is the new volume? B C D 112 L Page 10 SE D B the number of electrons and the atomic number the number of protons and the atomic number C the number of neutrons and the mass number the number of electrons and protons D 27. What is the correct name for the acid whose chemical formula is H2SO4 ? hydrosulfuric acid hydrosulfurous acid sulfurous acid sulfuric acid Which element is located in Group 2 (IIA) and Period 6 of the periodic table? A B C D barium (Ba) molybdenum (Mo) radium (Ra) tungsten (W) Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 29. How many moles are in 325 g of (NH4)2Cr2O7 ? A B C D 32. 0.732 mole 0.776 mole Considering this balanced chemical equation, how many grams of HgO will be produced when 44 g of Hg react with excess O2 ? 2Hg (l) + O2 ( g) → 2HgO (s) 1.29 moles 1.37 moles 30. Which compound contains the greatest percent of oxygen by mass? A B C D CO2 NO2 SO2 SiO2 EA B C D 31. This balanced equation represents a chemical reaction: 2KClO3 (s) Δ 2KCl (s) + 3O2 (g) R EL A B C 1.06 moles 2.13 moles 4.25 moles How many moles of KCl are produced when 4.25 moles of KClO3 decompose? D 8.50 moles Page 11 SE D B C A 28 g 44 g 48 g D 96 g 33. Which electron transmission in the hydrogen atom will result in the emission of red light? A n = 2 to n = 3 n = 2 to n = 4 n = 3 to n = 2 n = 4 to n = 2 34. What can be said of a closed system when an exothermic reaction proceeds in an aqueous solution? A B C D There is a net energy loss. There is a net energy gain. Heat is transferred from the water to the reactants. Heat is transferred from the reactants to the water. Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 35. In which group are the particles arranged in order of decreasing mass? A B C D alpha, beta, neutron 37. What is the best reason for using iron filings instead of an iron nail in a chemical reaction? A B C to decrease the amount of catalyst during the reaction to increase the molecular structure during the reaction alpha, neutron, beta neutron, beta, alpha neutron, alpha, beta 36. Consider this incomplete chemical equation: Ba + CuCl2 → What are the products of this equation? A B C D BaCl2 and CuCl2 BaCuCl2 and Ba BaCl2 and Cu EA C D BaCu and Cl2 R EL Page 12 Go to next page SE D to decrease the rate of reaction D to increase the surface area of the reaction 38. Which is a characteristic of a strong acid? A It has a pH greater than 7. B It completely ionizes in solution. It contains many hydroxide ions. It reacts only with a strong base. NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 39. Consider this balanced chemical equation: Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) Which is the oxidation half-reaction? A B C D Zn → Zn 2 + + 2e − Zn + 2e − → Zn 2 + 2H + → H2 + 2e − 2H + + 2e − → H 2 40. What is the net ionic equation for the reaction between Pb ( NO3 )2 and HCl ? A B C D Pb 2 + (aq) + 2Cl − (aq) → PbCl 2 (s) − 2NO3 (aq) + 2H+ (aq) → 2HNO3 (aq) Pb(NO3)2 (aq) + 2HCl (aq) → PbCl 2 (s) + 2 HNO3 (aq) − − Pb 3 + (aq) + 2 NO3 (aq) + 2 H + (aq) + 2Cl − (aq) → PbCl 2 (s) + 2 H + (aq) + 2 NO3 (aq) R EL Page 13 Go to next page EA SE D NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 41. When combined, two gases have a pressure of 4.0 atm. If one gas has a pressure of 1.5 atm, what is the pressure of the second gas? A B C D 1.5 atm 43. Which elements have the same number of neutrons? A B C 10 5 B and 12 6 C 56 26 55 25 Mn and Ag and Fe Cd 2.0 atm 2.5 atm 5.5 atm 42. What compound has the chemical formula MgI2 ? A B C D di-iodide magnesium iodide(II) magnesium magnesium(I) iodine(II) R EL Page 14 Go to next page EA magnesium iodide SE D D 197 79 108 47 112 48 Au and 201 80 Hg NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 44. This chart represents the melting point of several substances. Substance Cl 2 Na NaCl Melting Point (°C) 101.5 97.72 801 What best explains the high melting point of the salt? A B C D the strong electrostatic attraction between Na 0 and Cl0 the weak electrostatic attraction between Na 0 and Cl 0 the weak electrostatic attraction between Na + and Cl the strong electrostatic attraction between Na + and Cl 45. Based on the VSEPR theory, what is the molecular geometry of CO2 ? A B C D linear tetrahedral trigonal planar R EL Page 15 Go to next page trigonal pyramidal EA SE D − − NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 46. This graph represents a phase diagram for a substance. Phase Diagram 200 150 100 50 0 — 80 What is the state of the substance at point I? A B C D gas liquid liquid and gas solid and liquid R EL 47. Which one of these compounds is soluble in water? A aluminum sulfide EA 48. In which block does an element with the electron configuration [Xe] 6s24 f 145d106 p1 belong? A B C D s block p block d block B C calcium carbonate iron(III) hydroxide potassium sulfate D Page 16 SE D H I G E K —40 0 40 Temperature (°C) 80 F S f block Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 49. Which statement is true for the reaction represented by this equation? CH4 + 2O2 → CO2 + 2H2O 51. Which orbital notation shows the lowest energy arrangement of valence electrons for 1s22s22p3 ? A 2s 2s 2p A 1 gram of CH4 is required to react with 2 grams of O2 . 1 gram of CH4 is required to react with 4 grams of O2 . B C B C 1 mole of CH4 is required to react with 2 moles of O2 . D 1 mole of CH4 is required to react with 4 moles of O2 . EA B C D 50. What is the percent by mass of N in Ca ( CN )2 ? A B C D 15.21% 21.19% 30.42% 42.39% R EL Page 17 Go to next page SE D 2s 2s 2p 2p D 52. What is the molarity of 28.9 g of CaCl2 dissolved in water to make 0.78 L of solution? A 0.33 M 0.69 M 1.5 M 3.0 M NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 53. The half-life of phosphorus-32 is 14.3 days. How much of a sample of phosphorus-32 will remain after 57.2 days? A 1 32 55. What is the [ H + ] of an HCl solution if the pH is measured to be 6? A B 1 × 10 — 7 M 1 × 10 — 6 M M B 1 16 1 8 1 4 C D 54. how much energy is required? A B C D 1.67 × 104 J 8.20 × 103 J 8.08 × 103 J 1.95 × 103 J R EL Page 18 Go to next page EA To increase the temperature of 100.0 g of H2O (s) from — 50.0° C to —10.0° C, SE D C 6 × 10 8 × 10 — 6 D — 1 M NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 56. This balanced equation represents a chemical reaction. 2C4H10 (g) + 13O2 (g) → 8CO2 (g) + 10H2O (g) What type of chemical reaction is represented by the equation? A B C D combustion decomposition double replacement single replacement 57. This balanced equation represents a chemical reaction using palladium, Pd, as a catalyst. (Pd) CO2 (g) + H2O (l) ⎯⎯⎯ H2CO3 (l) → Without palladium the reaction is slow and produces low concentrations of product. How does the palladium increase the speed of the reaction? A EA B C D The palladium reacts with the water. The palladium lowers the activation energy. R EL C The palladium purifies the carbon dioxide. D B The palladium increases the reaction temperature. Page 19 SE D 58. Which pair of substances will likely undergo a single replacement reaction? A Na and BaCl2 Zn and BaCl2 Ca and BaCl2 K and BaCl2 Go to next page NCDPI North Carolina Test of Chemistry. Form A RELEASED Fall 2009 59. What is the net ionic equation for the reaction between aqueous solutions of LiBr and AgNO3 ? 60. A B C D Ag + (aq) + Br — (aq) → AgBr (s) Li + (aq) + NO3 (aq) → LiNO3 (s) Li + (aq) + Br — (aq) → LiBr (s) — A scientist hypothesizes that a colorless gas produced during a chemical reaction is carbon dioxide. Which observation would confirm this hypothesis? A B The gas will react violently with water. A glowing splint placed in the gas will burn brighter. Burning the gas in the presence of oxygen will produce water. — Ag + (aq) + NO3 (aq) → AgNO3 (s) R EL Page 20 Go to next page EA SE D C D Bubbling the gas through lime water will make the lime water cloudy. STOP End of Chemistry Test North Carolina Test of Chemistry Form A RELEASED Fall 2009 Answer Key Item Number 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 41 42 Correct Answer C D C A D A D B C A A C A D B A B B C D D B B A B C D A C A C C C D B C D B A A C C Goal 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 4 – Energy Changes in Chemistry 4 – Energy Changes in Chemistry 4 – Energy Changes in Chemistry 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 4 – Energy Changes in Chemistry 4 – Energy Changes in Chemistry 4 – Energy Changes in Chemistry 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter R EL 6 August 2009 EA SE D Page 1 North Carolina Test of Chemistry Form A RELEASED Fall 2009 Answer Key 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 B D A C D B C C D A B B B A B D A D 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 2 – Structures & Properties of Matter 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 3 – Regularities in Chemistry 4 – Energy Changes in Chemistry 4 – Energy Changes in Chemistry 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions 5 – Chemical Reactions R EL 6 August 2009 Page 2 EA SE D North Carolina Test of Chemistry Form A RELEASED Fall 2009 Raw to Scale Score Conversion Raw Score 0 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 41 Scale Score 120 121 121 122 122 123 124 124 125 126 126 127 128 129 130 131 132 133 134 135 136 137 138 139 140 141 142 143 144 145 146 147 148 149 149 150 151 152 153 153 154 155 R 10 August 2009 EL EA SE Page 1 D North Carolina Test of Chemistry Form A RELEASED Fall 2009 Raw to Scale Score Conversion 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 156 156 157 158 159 160 160 161 162 163 164 165 166 168 169 171 173 175 178 R 10 August 2009 EL Page 2 EA SE D