Name: Period: AP Take Home Practice Test for Unit 0.5 Exam

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1 Name: Period: AP Take Home Practice Test for Unit 0.5 Exam 1. Which of the following is a correctly balanced equation? a. Al 2(SO 4) CaCl 2 2 CaSO AlCl 3 b. Al 2(SO 4) CaCl 2 3 CaSO AlCl 3 c. Al 2(SO 4) 3 + CaCl 2 CaSO 4 + AlCl 3 d. Al 2(SO 4) CaCl 2 3 CaSO 4 + AlCl 3 2. In the reaction shown in question #1 above, the reactants are: a. Al 2(SO 4) 3 and AlCl 3 b. CaCl 2 and CaSO 4 c. Al 2(SO 4) 3 and CaCl 2 d. CaCl 2 and AlCl 3 3. A glass of iced tea containing excess sugar at the bottom is said to be : a. saturated b. unsaturated c. supersaturated d. homogeneous 4. At chemical equilibrium, the rates of the forward reaction and reverse `reaction are : a. equal to zero. b. equal to each other. c. at a maximum. d. at a minimum. 5. The most concentrated solution from among those listed below is? a. 200 ml of 0.15 M NaNO 3 b. 150 ml of 0.18 M NaOH c. 75 ml of 0.23 M KNO 3 d. 100 ml of 0.25 M KCl 6. What is the molarity of a 200 ml aqueous solution in which a 0.2 mole of sodium bromide is dissolved? a M b. 1.0 M c M d. 4.0 M 1 7. Which of the following is an empirical formula? a. C 2H 4 b. C 2H 2 c. C 2Cl 2 d. CCl 4 8. In a neutral solution, the [H ] is: a b. zero c. 1.0 x 10 7 M d. equal to [OH ] 9. With solutions of strong acids and strong bases, the word strong refers a. to molality b. to molarity c. to solubility d. to degree of ionization 10. What is the ph of a solution in which the [H ] = 1.0 x 10 12? a. 1.0 b. 2.0 c. 2.0 d What is the molecular electronic geometry of CH 4? a. linear b. bent/angular c. trigonal planar d. tetrahedral 12. If the [H ] in an aqueous solution increases, the [OH ]: a. will increase b. will equal 1.0 x c. will decrease d. will remain the same

2 13. Catalysts increase the rate of a chemical reaction by what means? a. Increasing the concentration of reactants b. Increasing collision energy c. Increasing temperature d. Lowering activation energy. 14. With pressure constant, the temperature of a gas is increased from 300 K to 900 K. The volume will. a. increase by 20% b. triple c. remain the same d. decrease by one-half 15. The volume of a gas is doubled while the temperature is held constant. The pressure of the gas: a. remains unchanged b. is reduced by one-half c. is doubled d. Answer depends on the molar mass of the gas. 16. In comparing 1.00 mole of nitrogen monoxide gas (NO) and 1.00 mole of carbon dioxide gas (CO 2), each at 25 C and 1.00 atmospheres, which of the following is true? a. They have the same mass. b. They have the same number of atoms. c. They occupy the same volume. d. All of the above selections are true. 17. Which element has an electron configuration of 1s 2, 2s 2, 2p 6, 3s 2, 3p 5? a. iron. b. chlorine. c. bromine. d. phosphorous. 18. The modern periodic table is arranged in order of increasing: a. atomic mass. b. atomic number. c. atomic size. d. atomic radius. 19. When a strontium atom loses two electrons to become a Sr 2+ ion, the electrons are lost from the: a. 5s orbital b. 5p orbital c. 3d orbital d. 4f orbital 20. The vertical columns of the periodic table are called: a. groups b. rows c. periods d. sublevels 21. When freezing of water occurs a. heat energy is consumed b. heat energy is released c. the process is endothermic d. the process is isothermic 22. The electron configuration of a fluoride ion, F, is: a. 1s 2, 2s 2, 2p 5. b. the same as that of the neon atom. c. 1s 2, 2s 2, 2p 6, 3s 1. d. the same as that of the potassium atom. 23. Metals are good conductors of electricity because they: a. contain ions. b. are ductile. c. contain mobile valence electrons. d. bend easily. 24. Which of the following elements does not exist as a diatomic molecule? a. I b. F c. H d. He 2

3 25. A covalent bond forms: a. when an element becomes a noble gas. b. when atoms share electrons. c. between metals and nonmetals. d. when electrons are transferred from one atom to another. For questions #31 #33 below, refer to the following Diagram for Phase Change of Water: 26. Which of the following compounds is not molecular? a. SCl 2 b. KCl c. CO 2 d. S 2Cl How many significant digits are in the number ? a. 2 b. 3 c. 4 d The energy required to raise the temperature of one gram of any substance 1 C is defined as for that substance. a. one joule b. one calorie c. the melting point d. the specific heat 29. Which of the following elements would probability NOT react with a Group 2 metal? a. Cl b. Ne c. O d. S 30. Electrostatic attraction between cations and anions occurs in a. ionic bonds b. nonpolar covalent bonds c. polar covalent bonds d. metallic bonds 31. Which segments of the curve represent changes in temperature? a. 1 and 3 b. 2 and 4 c. 1, 3 and 5 d. all segments 32. Which segments of the curve represent phase changes? a. 1 and 2 b. 1 and 3 c. 1, 3 and 5 d. 2 and Which segments of the curve represent times when liquid is present? a. 3 only b. 2 and 3 c. 2, 3 and 4 d. 3 and 4 3

4 34. How does the collision theory explain the effect of temperature on the rate of reaction? a. Increasing the temperature increases the rate of reaction because particles move faster at higher temperatures. b. Increasing the temperature decreases the rate of reaction because few collisions occur at higher temperatures. c. Decreasing the temperature increases the rate of reaction because particles are closer together at lower temperatures d. The collision theory cannot explain the effect of changing the temperature. 35. How does the collision theory explain the effect of changing the concentration of reactants on the rate of reaction? a. Increasing the concentration decreases the rate of reaction because reactants are too crowded to collide. b. Increasing the concentration increases the rate of reaction because there are more reactant particles to take part in the collision. c. Decreasing the concentration increases the rate of reaction because there is more room for particles to rebound after collision. d. The collision theory cannot explain the effect of changing the concentration of reactants. 36. Which of the following operations usually makes a substance dissolve faster in a solvent? a. agitation b. raising the solvent temperature c. crushing the substance to a powder d. all of the above 37. Le Chatelier s principle states that if a system is in equilibrium and a condition is changed the equilibrium will. a. remain unchanged b. shift to minimize the amount of reactants c. shift to minimize the amount of products d. shift in the direction to restore the original conditions 38. The breaking of bonds is a. exothermic b. isothermic c. endothermic 39. A reaction that releases heat is said to. a. run uphill b. be isothermic c. be endothermic d. be exothermic Questions 40-42: Choose from the following list: a. Carbon b Silicon c. Strontium 40. a metal 41. a nonmetal 42. a semimetal/metalloid Questions 43-46: Choose form the following list: a. Argon b. Zinc c. Iodine d. Magnesium e. Lithium 43. an alkali metal 44. an alkaline earth metal 45. a halogen 46. a noble gas 4

5 47. Which of the following is a member of the p block elements a. Lead b. Uranium c. Zinc d. Sodium 48. How many significant figures are in the answer to this calculation? (46.86 * /45) a. 2 b. 3 c. 4 d Which statement describes the particles of an ideal gas according to the kinetic molecular theory? a. The gas particles are arranged in a regular geometric pattern. b. The gas particles are in random, constant, straight-line motion. c. The gas particles are separated by very small distances, relative to their sizes. d. The gas particles are strongly attracted to each other. 53. Which Lewis electron-dot diagram represents a molecule having a nonpolar covalent bond? 49. Which statement describes the distribution of charge in an atom? a. A neutral nucleus is surrounded by one or more negatively charged electrons. b. A neutral nucleus is surrounded by one or more positively charged electrons. c. A positively charged nucleus is surrounded by one or more negatively charged electrons. d. A positively charged nucleus is surrounded by one or more positively charged electrons. 50. Which pair represents two forms of an element in the same phase at STP but with different structures and different properties? a. I 2(s) and I 2(g) b. H 2(g) and Hg (g) c. O 2(g) and O 3(g) d. H 2O(s) and H 2O(l) 51. A mixture of sand and table salt can be separated by filtration because the substances in the mixture differ in a. boiling point b. density at STP c. freezing point d. solubility in water Questions 54-57: Choose from the following list: a. Ammonia b. Carbon Dioxide c. Hydrofluoric acid d. Lithium hydroxide e. Sulfuric acid 54. Strong base 55. Strong Acid 56. Weak acid 57. Weak base 5

6 Questions 58-62: Choose from the following list: a. CO b. HBr c. KOH d. MgO e. NaF ab. NaH 58. Nonmetal oxide 59. Metal oxide 60. Metal hydride 61. Metal hydroxide 62. Salt Questions 63-65: Choose from the following list identify a molecule whose strong force of attraction between molecules is: a. CH 4 b. C diamond c. HOH d. MgO e. SO London Force, 64. Dipole-dipole force, 65. Hydrogen bond Questions 66-69: Choose from the following list: a. C diamond b. Pb c. HOH d. MgO 66. ionic solid 67. molecular solid 68. metallic solid 69. network covalent solid Questions 70-81: Choose from the following list: a. 1 b. 2 c. 3 d. 4 e. 5 ab. 6 ac. 7 ad. 8 ae. 9 bc What is the atomic number of 7 Li? 71. How many protons are found in a neutral atom of 7 Be? 72. How many electrons are found in the ion O 2-? 73. How many neutrons are present in 7 Be? 74. How many valance electrons are found in N? 75. How many valance electrons are found in N 3-? 76. What is the core charge of the atom N? 77. What is the core charge of the cation Na +? 78. What is the core charge of the anion O 2-? 79. Grams of Carbon in mole of carbon? 80. Moles of carbon atoms in 1 mole of C 4H 10? 81. Moles of atoms in 1 mole of Ca(NO 2) 2? 82. NH 4CI(s) + heat NH 3(g) + HCI(g) What kind of change will shift the reaction above to the right to form more products? A a decrease in total pressure B an increase in the concentration of HCl C an increase in the pressure of NH 3 D a decrease in temperature 6

7 83. NO 2(g) + CO(g) NO(g) + CO 2(g) The reaction shown above occurs inside a closed flask. What action will shift the reaction to the left? A pumping CO gas into the closed flask B raising the total pressure inside the flask C increasing the NO concentration in the flask D venting some CO 2 gas from the flask Questions 84-88: Choose from the list below a. Ca(s) + 2 H2O(l) H2(g) + Ca(OH)2 (aq) b. 2 NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g) c. NH3(g) + HCl(g) NH 4Cl(s) d. HCl(aq) + NaHS(aq) H2S(g) + NaCl(aq) e. (CH3)2O(l) + 3 O2(g) 3H2O(g) + 2 CO2(g) 84. synthesis reaction, 85. combustion reaction, 86. decomposition reaction, 87. single replacement reaction, 88. double replacement reaction Questions 89-91: Choose from the list below a. Cd(s) + SnCl2(aq) Sn(s) + CdCl2(aq) b. 2 K3PO4(aq) +3Zn(NO 3 )2(aq) Zn3(PO4)2(s) + 6 KNO 3(aq) c. H3PO4(aq) + KOH(aq) KH2PO4(aq) + H 2O(l) 89. an acid base reaction 90. an oxidation reduction reaction 91. a precipitation reaction Questions 92-95: Which of the following has the a. F b. Na c. Cl d. Li 92. highest first ionization energy 93. lowest first ionization energy 94. has the largest radius 95. has the smallest radius Questions 96-99: Which of the following has the a. F - b. Na+ c. Cl - d. Br smallest radius? 97. largest radius? Questions 98-99: Which of the following has the a. F b. Na c. Cl d. Li 98. highest electronegativity 99. lowest electronegativity 100. The line-emission spectrum of an atom is caused by the energies released when electrons do what? A. jump from a lower energy level to a higher energy level B. jump from a higher energy level to a lower energy level C. jump from the ground state to an excited state D. none of the above 7

5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons

5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons 1. Which substance can be decomposed by a chemical change? (A) beryllium (B) boron (C) methanol (D) magnesium 2. The particles in a crystalline solid are arranged (A) randomly and far apart (B) randomly