Semester 2 Honors Chemistry Final Review

Semester 2 Honors Chemistry Final Review Name: Chapter 8 - Chemical Reactions I can balance chemical equation using the law of conservation of mass. 1. Which coefficients correctly balance the formula equation CaCO 3 CaO + CO 2? a. 1, 1, 1 c. 2, 6, 3 b. 1, 3, 1 d. 3, 1, 2 2. Which coefficients correctly balance the formula equation H 2 O + Cl 2 O 7 HClO 4? a. 2, 1, 2 c. 1, 2, 1 b. 1, 1, 2 d. 2, 2, 2 For the following problems, balance the equation and use in the following three questions. Al(OH) 3 + H 2 SO 4 ---> Al 2 (SO 4 ) 3 + H 2 O 3. What would the coefficient on H 2 SO 4 be? a. 1 c. 3 b. 2 d. none of the above 4. What would the coefficient on Al(OH) 3 be? a. 1 c. 3 b. 2 d. none of the above 5. What would the coefficient of Al 2 (SO 4 ) 3 be? a. 1 c. 3 b. 2 d. none of the above 6. When the equation Si (s) + HF (aq) SiF 4 (g) + H 2 (g) is balanced, what is the coefficient for HF? a. 1 c. 3 b. 2 d. 4 I can write net ionic reactions. 7. The balanced net ionic equation for precipitation of CaCO 3 when aqueous solutions of Li 2 CO 3 and CaCl 2 are mixed is. a. Li + (aq) + Cl - (aq) LiC(aq) b. 2Li + (aq) + 2Cl - (aq) 2LiCl(aq) c. Li 2 CO 3 (aq) + CaCl 2 (aq) 2LiCl(aq) + CaCO 3 (s) d. Ca 2+ (aq) + CO 3 2- (aq) CaCO 3 (s) e. 2Li + (aq) + CO 3 2- (aq) Li 2 CO 3 (aq) I can predict products of simple chemical reactions. 8. Identify the solid product that forms when aqueous solutions are mixed: KNO 3 (aq) + BaCl 2 (aq) a. KCl c. BaNO 3 b. Ba(NO 3 ) 2 d. none of the above 9. Which of the following reactions would represent the reaction between aqueous zinc bromide and aqueous silver nitrate? a) ZnBr 2 (aq) + AgNO 3 (aq) ZnNO 3 (aq) + AgBr 2 (s) b) ZnBr 2 (aq) + AgNO 3 (aq) ZnNO 3 (aq) + AgBr (s) c) ZnBr 2 (aq) + 2 AgNO 3 (aq) Zn(NO 3 ) 2 (aq) + 2 AgBr (s) d) ZnBr 2 (aq) + AgNO 3 (aq) Zn(NO 3 ) 2 (aq) + AgBr (s)

I can predict the products for the decomposition of metallic carbonates, hydroxides, and chlorates. 10. Predict the products for the decomposition of sodium carbonate, NaCO 3 a. Na + CO 3 c. Na 2 O + CO 2 b. NaO + CO 3 d. Na + C + O 3 I can identify the 5 major types of reactions. I can identify if a single or double replacement reaction will occur. 11. The reaction 2K (s) + Br 2 (l) 2 KBr (s) is a(n) reaction. a. combustion c. decomposition b. synthesis d. none of the above 12. When a reaction has O 2 as a reactant, it is classified as a reaction. a. combustion c. decomposition b. synthesis d. none of the above 13. Ag + Cu(NO 3 ) 2 no reaction is an example of a reaction. a. synthesis c. single replacement e. combustion b. decomposition d. double replacement 14. The reaction of CH 3 CH 2 OH + 3O 2 2CO 2 + 3H 2 O is an example of a reaction. a. synthesis c. single replacement e. combustion b. decomposition d. double replacement Chapter 9 - Stoichiometry I can solve stoichiometrically for mass, volume, number of particles and moles of a given compound in a chemical reaction. The combustion of propane (C 3 H 8 ) produces CO 2 and H 2 O: C 3 H 8 + 5O 2 3CO 2 + 4H 2 O 15. The reaction of 2.5 mol of O 2 will produce mol of H 2 O. a. 4.0 c. 2.5 e. 1.0 b. 3.0 d. 2.0 Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N 2 + 3H 2 2NH 3 16. A 9.3g sample of hydrogen requires grams of N 2 for a complete reaction. a. 2.0 c. 3.9 x 10 2 e. 1.3 x 10 2 b. 43 d. 4.6 17. In the reaction Ca + Cl 2 CaCl 2, what is the mole ratio of chlorine to calcium chloride? a. 2:3 c. 1:2 b. 2:1 d. 1:1 18. What is the mole ratio of oxygen to phosphorus(v) oxide in the reaction: P 4 + 5O 2 P 4 O 10? a. 1:1 c. 5:1 b. 1:5 d. 4:10 I can manipulate the stoichiometric calculations to determine the limiting reactant in a chemical reaction. 19. What mass in grams of hydrogen is produced by the reaction of 4.73g of magnesium with 1.83g of water? Mg + 2H 2 O Mg(OH) 2 + H 2 a. 0.0162 c. 0.102 e. 0.494 b. 0.0485 d. 0.392

For #19 and 20 use the following reaction: Mg 3 N 2 + 3H 2 O 2NH 3 + 3MgO 20. How many moles of magnesium oxide are produced by the reaction of 3.82g of magnesium nitride with 7.73g of water? a. 0.0378 c. 0.113 e. 4.57 b. 0.429 d. 0.0756 I can use actual yield and theoretical yield to calculate percent yield. 21. The yield of MgO from the reaction in #20 is 3.60g. What is the percent yield in the reaction? a. 99.9 c. 94.5 e. 46.6 b. 79.1 d. 49.4 22. For the reaction Cl 2 + 2KBr 2KCl + Br 2, calculate the percentage yield if 200.g of chlorine react with excess potassium bromide to produce 410.g of bromine. a. 73.4% c. 91.9% b. 82.1% d. 98.9% 23. The measured amount of product obtained in lab from a chemical reaction is the a. percentage yield. c. theoretical yield. b. actual yield. d. mole ratio. Chapter 11 - Intermolecular Forces I can explain how a hydrogen bond is different from other dipole-dipole forces. 24. A hydrogen bond is a special form of a(n) a. covalent bond c. ionic bond b. dipole-dipole d. london dispersion force 25. A hydrogen bond forms between molecules that contain hydrogen bonded to a. a highly electronegative atom c. another hydrogen atom b. an atom with a low electronegativity d. none of the above I can describe London Dispersion Forces. 26. London dispersion forces are the only forces that occur between molecules that are a. highly polar c. nonpolar b. slightly polar d. all molecules whether they are polar or not 27. A London dispersion force is considered a dipole-dipole force because it a. affects all types of compounds c. affects polar molecules b. affects nonpolar molecules d. results from a temporary dipole I can identify systems that have multiple phases and determine whether they are at equilibrium. 28. A carbonated beverage over ice contains phases. a. one c. three b. two d. four 29. Which of the following will form the strongest hydrogen bonds? a. HF c. H 2 S b. HCl d. HBr I can rank substances to their intermolecular attractions. 30. Which of the following is most likely to have a high boiling point? a. F 2 c. CH 4 b. CO 2 d. H 2 O

31. A dipole-dipole force is strongest when the molecules are. a. far apart. c. strongly polar. b. nonpolar. d. large. I can relate the properties of a state to the energy content and particle arrangement of that state of matter. 32. A sample of matter whose particles are close together and cannot move past each other is. a. a solid. c. a liquid. b. a gas. d. viscous. 33. The attraction of particles for each other within a liquid is. a. adhesion. c. cohesion. b. surface tension. d. capillary action. I can explain forces and energy changes involved in changes of state. 34. A liquid becomes a gas during. a. evaporation c. sublimation b. condensation d. deposition I can describe dipole-dipole forces. 35. As dipole-dipole forces increase, melting points. a. increase. c. remain the same. b. decrease. d. cannot be predicted. I can relate water s physical properties to its intermolecular forces. 36. Water s relatively high boiling point is the result of. a. covalent bonding. c. ionic bonding. b. hydrogen bonding. d. London forces. I can interpret a phase diagram including triple point, boiling point, melting point, and type of phase change given specific parameters. Answer questions 37-41 using this phase diagram. 37. At a pressure of 30 atm, the boiling point of this substance is. a. -105 C c. 200 C b. -15 C d. 50 C 38. The area on the graph that represents the solid phase is. a. A c. C b. B d. none of the above 39. The triple point on this graph occurs at. a. 200 ºC and 300 atmospheres c. -15 ºC and 1 atmosphere b. -15 ºC and 6 atmospheres d. 0 ºC and 6 atmospheres 40. The phase change from B to A is known as a. freezing c. evaporation e. melting b. condensation d. sublimation 41. The phase change from A to C is known as a. freezing c. evaporation e. deposition b. condensation d. sublimation

Chapter 12 - Gas Laws I can manipulate the combined gas law to explain the relationship between volume, pressure, and temperature. 42. A sample of a gas occupies a volume of 1384mL at 25 C. What volume will the gas occupy if the temperature increases to 50 C, if the pressure remains constant? a. 376mL c. 815mL b. 694mL d. 1500mL 43. A sample of a gas has a pressure of 2.52atm at 25 C. What would the gas pressure be at 52 C, if the volume remains constant? a. 1.44atm c. 3.27atm b. 2.75atm d. 6.24atm 44. The volume of a gas is 400.0mL when the pressure is 1.00atm. At the same temperature, what is the pressure at which the volume of the gas is 2.0L? a. 8.00atm c. 0.20atm b. 1.500atm d. 2.0atm 45. A sample of oxygen occupies 560mL when the pressure is 800.00mmHg. At constant temperature, what volume does the gas occupy when pressure falls to 700.00mmHg? a. 640mL c. 250mL b. 500mL d. 490mL 46. The volume of a gas is 5.0L when the temperature is 5.0 C. If the temperature is increased by 10.0 C without changing the pressure, what is the new volume? a. 6.2L c. 7.25L b. 4.82L d. 5.09L I can manipulate the ideal gas law to find the number of particles in a gas. 47. When pressure, volume, and temperature are known, the ideal gas law can be used to calculate a. The chemical formula c. molar amount b. The ideal gas constant d. compressibility 48. Calculate the approximate volume of a 0.600 mol sample of gas at 15 C and a pressure of 1.10atm. a. 12.9L c. 24.6L b. 22.4L d. 129L 49. For a constant number of moles of a gas, pressure varies a. Directly with temperature and inversely with volume b. Inversely with temperature and directly with volume c. Directly with temperature and directly with volume d. Inversely with temperature and inversely with volume 50. Calculate the approximate volume of a 1.00 mol sample of gas at STP. a. 12.9 L c. 24.6 L b. 22.4 L d. 129 L I can distinguish between the following gas pressures: atmospheres, mm of Hg, torr, kilopascals, and pounds per square inch. 51. The SI unit for measuring pressure is. a. newton c. pascal b. mm Hg d. liter 52. Standard temperature and pressure are. a. 32 F and 10 atm c. 10 K and 1 atm b. 0 C and 1 atm d. 0 F and 1 atm

53. A pressure of 760.0 mm Hg is equal to. a. 1.000 atm c. 100.0 atm b. 10.00 atm d. 7.600 atm 54. A pressure of 20 torr is equal to. a. 133.322 Pa c. 20 mm Hg b. 20 Pa d. 1 mm Hg I can solve stoichiometric problems involving gases using the ideal gas law. 55. For the given unbalanced reaction, H 2 S + SO 2 H 2 O + S If 6.00 L of H 2 S gas at 750. torr produced 3.20 g of sulfur, calculate the temperature in C. a. 1085 C c. 811 C b. 1410 C d. 400 C Chapter 13 - Solutions I can calculate concentration of molarity, molality, percent concentration, and parts per million. 56. Which number is the closest to the number of moles of KNO 3 in 100.0mL of a 0.10M solution? a. 10.0 c. 0.0010 e. 0.010 b. 1.0 d. 0.10 57. Which number is closest to the number of ml of water needed to be added to make a 1.0M solution, using 100.0g of KNO 3? a. 100.0mL c. 1000.0mL e. 2000.0mL b. 500.0mL d. 1500.0mL 58. Which number is closest to the concentration of a solution that contains 100.0g of KNO 3 in 100.0mL of water? a. 0.010M c. 1.0M e. 100.0M b. 0.10M d. 10.0M 59. Which number is closest to the concentration of a solution that contains 2.0 moles of NaCl in 1000.0mL of water? a. 0.020M c. 2.0M e. 1.0M b. 0.20M d. 20.0M 60. There are 3.4 mg of lead present in 2,000 g of a water sample. What is the concentration of lead in ppm? a. 1.7 ppm c. 3.4 ppm b. 1.7 x 10 3 ppm d. 3.4 x 10 3 ppm I can differentiate between a solute, solvent, and solution. 61. Carbon dioxide in air is an example of which solute-solvent combination? a. gas-liquid c. liquid-liquid b. liquid-gas d. gas-gas I can distinguish between a suspension, colloid, and solution. 62. Which of the following is a colloid? a. water c. soil b. milk d. concrete 63. A mixture that appears to be uniform while being stirred but separates into different phases when agitation ceases is a. a. solvent c. suspension b. colloid. d. solute

I can identify an unsaturated, saturated, and supersaturated solution via a solubility curve. 64. All of the KBr that will dissolve in a solution has dissolved, and several undissolved crystals remain on the bottom. The solution is. a. saturated. c. unsaturated. b. supersaturated. d. at the incorrect pressure to dissolve the solid. I can solve stoichiometric problems involving solutions. 65. How many ml of 0.715 M HCl is required to neutralize 2.50 grams of sodium carbonate? HCl (aq) + Na 2 CO 3(s) NaCl (aq) + H 2 CO 3(aq) a. 66.0 ml c. 23.6 ml b. 47.1 ml d. 1.79 ml I can describe the effect of solutes on a given solution relating to boiling point elevation and freezing point depression. 66. Which of the following would have the biggest effect on boiling point elevation (BPE) and freezing point depression (FPD)? a. NaCl c. AlCl 3 b. MgCl 2 d. C 6 H 12 O 6 For questions 67-71 use the given solubility chart. 67. If a saturated solution of NH 4 Cl in 100.0g of water is cooled from 70 C to 30 C, how many grams of NH 4 Cl would precipitate? a. 40.0g c. 20.0g e. 10.0g b. 60.0g d. 80.0g 68. Which substance on the graph is the most soluble at 10 C in 1000.0g of water? a. NaCl c. KNO 3 e. KClO 3 b. NH 3 d. KI 69. Which number is closest to the number of grams of potassium nitrate that will dissolve in 100.0g of water at 40 C? a. 25.0g c. 45.0g e. 60.0g b. 35.0g d. 55.0g 70. Which number is closest to the temperature at which 40g of KCl will form a saturated solution in 100.0g of water? a. 10.0 C c. 30.0 C e. 50.0 C b. 20.0 C d. 40.0 C 71. How many grams of KNO 3 will dissolve in 300.0g of water at 40 C? a. 60.0g c. 180.0g e. 100.0g b. 120.0 d. 30.0g

Chapter 15 - Acids and Bases I can name acids and bases. 72. Name the acid H 2 SO 4 a. sulfate acid c. hydrosulfuric acid b. sulfuric acid d. hyposulfuric acid 73. Name the acid H 3 P a. phosphate acid c. hydrophosphoric acid b. phosphoric acid d. hyprophosphoric acid 74. Name the base LiOH a. ammonia c. lithium hydroxide b. lithium oxide d. lithium oxhydride I can write formulas for acids and bases. 75. Write the formula for barium hydroxide a. BaOH c. BOH b. BaOH 2 d. Ba(OH) 2 76. Write the formula for nitrous acid a. H 3 N c. HNO 2 b. HN d. HNO 3 I can differentiate between acids and bases by their properties. 77. In the reaction, HC 2 H 3 O 2 + OH - - C 2 H 3 O 2 + H 2 O, which species is the a Bronsted-Lowry acid? a. OH - - c. C 2 H 3 O 2 b. HC 2 H 3 O 2 d. None of the above 78. In the reaction, HBr + H 2 O H 3 O + + Br -, which species is a Bronsted-Lowry base? a. HBr c. Br - b. H 2 O d. None of the above 79. In the reaction HS - + H 2 O H 3 O + + S 2-, a conjugate acid-base pair is a. HS - and H 2 O c. HS - and H 3 O + b. S 2- and H 3 O + d. HS - and S 2- I can complete an acid-base reaction. 80. The substances produced when, HC 2 H 3 O 2 neutralizes NH 4 OH are a. HNH 3 and C 2 H 3 O 3 OH c. HNH 4 C 2 H 3 O 2 and OH - b. H 3 O + and NH 3 C 2 H 3 O 2 d. H 2 O and NH 4 C 2 H 3 O 2 81. The substances produced when LiOH neutralizes HNO 2 are a. LiH and NO 2 OH c. HLiO and NOOH b. LiNO 2 and H 2 O d. H 3 O and NOLi 82. The substances produced when NaOH neutralizes HClO 3 are a. ClOH and NaO 3 H c. NaHO 3 - and ClO b. H 2 O and NaClO 3 d. HO 3 OH and NaCl I can calculate ph, [H + ], [OH - ], and poh of any acidic or basic solution. I can use the ph scale. I can identify a basic, neutral, and acidic solution by using the ph scale. 83. What is the [OH - ] in a sample of blood with a poh of 6.6? a. 1 x 10-2 M c. 1 x 10-10 M b. 2.5 x 10-7 M d. 3.98 x 10-8 M

84. What is the [H + ] in a sample of orange juice with a ph of 3.6? a. 1 x 10-7 M c. 3 x 10-10 M b. 2.5 x 10-4 M d. 10.4M 85. Is the solution from #84 an acid, base, or neutral solution? a. acid c. neutral b. base 86. What is the [OH - ] in a sample of NaOH solution with a ph of 13.00? a. 1 x 10-13 M c. 1 x 10-1 M b. 3.1 x 10-11 M d. 3 x 10-11 M 87. Is the solution from #86 an acid, base, or neutral solution? a. acid c. neutral b. base 88. What is the ph in a sample of soft drink with a [H + ] = 3.2 x 10-4 M? a. 3.5 c. 10.5 b. 3.1 x 10-11 M d. 3 x 10-11 M 89. What is the poh in a sample of household cleaner with a [OH - ] = 6.3 x 10-12 M? a. 2.8 c. 11.2 b. 1.6 x 10-3 M d. 1 x 10-12 M I can solve problems using the titration process. 90. If 10.0mL of a KOH solution were neutralized by 26.5mL of a 0.122M HBr solution, what is the molarity of the base? a. 0.0460 M c. 3.09 M b. 0.323 M d. 0.483 M 91. Calculate the volume of a 0.10M NaOH solution necessary to neutralize 25.0mL of a 0.20M HCl solution. a. 25. ml c. 90. ml b. 13 ml d. 50. ml Chapter 18 - Nuclear Chemistry I can identify nuclear particles. 92. What does the 4 in 4 2He represent? a. The mass number c. the number of protons b. The atomic number d. the number of neutrons 93. Which of the following lists rank nuclear radiation from most massive to least massive? a. Alpha, beta, gamma c. gamma, alpha, beta b. Beta, gamma, alpha d. gamma, beta, alpha I can determine if nuclear isotopes are stable. 94. Among atoms with low atomic numbers, what is the neutron-proton ratio of the most stable nuclei? a. 1.8 c. 1.0 b. 1.5 d. 0.5 I can calculate half-life problems. 95. What is the half-life of an isotope if 62.5g of a 500g sample of the isotope remains after 3.0 years? a. 1.5 years c. 1.0 years b. 2.5 years d. 4.5 years 96. How many half-lives are required for 15/16 of the nuclei of an isotope in a sample to decay? a. 3 c. 2 b. 4 d. 5

I can balance nuclear reactions. 97. Balance the following equation: 226 88Ra 222 86Rn +? a. 4 2He c. 1 1H b. 1 0n d. 0-1e I can identify nuclear types of reactions. For each of the following nuclear equations, identify the type of decay represented. a. positron emission d. fusion b. beta decay e. alpha decay c. electron capture 98. 59 26Fe 59 27Co + 0-1e 99. 118 54Xe 118 53I + 0 +1e 100. 185 79Au 181 77Ir + 4 2He