Chemistry Final Exam Review

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1 Chemistry Final Exam Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. All of the following are physical properties of matter EXCEPT. a. mass c. melting point b. color d. ability to rust 2. Which state of matter has a definite volume and takes the shape of its container? a. solid c. gas b. liquid d. both b and c 3. Which of the following is a heterogeneous mixture? a. air c. steel b. salt water d. soil 4. Which of the following is a heterogeneous mixture? a. vinegar in water c. oil and vinegar b. milk d. air 5. A substance that can be separated into two or more substances only by a chemical change is a(n). a. solution c. mixture b. element d. compound 6. Which of the following is a chemical property? a. color c. freezing point b. hardness d. ability to react with oxygen 7. The closeness of a measurement to its true value is a measure of its. a. precision c. reproducibility b. accuracy d. usefulness 8. If the temperature changes by 100 K, by how much does it change in C? a. 0 C c. 100 C b. 37 C d. 273 C 9. The particles that are found in the nucleus of an atom are. a. neutrons and electrons c. protons and neutrons b. electrons only d. protons and electrons 10. The atomic number of an element is the total number of which particles in the nucleus? a. neutrons c. electrons b. protons d. protons and electrons

2 11. An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are. a. 152 protons and 76 electrons c. 38 protons and 38 electrons b. 76 protons and 0 electrons d. 76 protons and 76 electrons 12. The sum of the protons and neutrons in an atom equals the. a. atomic number c. atomic mass b. nucleus number d. mass number 13. What does the number 84 in the name krypton-84 represent? a. the atomic number c. the sum of the protons and electrons b. the mass number d. twice the number of protons 14. All atoms of the same element have the same. a. number of neutrons c. mass numbers b. number of protons d. mass 15. Isotopes of the same element have different. a. numbers of neutrons c. numbers of electrons b. numbers of protons d. atomic numbers 16. Which of the following sets of symbols represents isotopes of the same element? a. J J J c. M M M b. L L L d. Q Q Q 17. In which of the following is the number of neutrons correctly represented? a. F has 0 neutrons. c. Mg has 24 neutrons. b. As has 108 neutrons. d. U has 146 neutrons. 18. How does the energy of an electron change when the electron moves closer to the nucleus? a. It decreases. c. It stays the same. b. It increases. d. It doubles. 19. What is the shape of the 3p atomic orbital? a. sphere c. bar b. dumbbell d. two perpendicular dumbbells 20. How many energy sublevels are in the second principal energy level? a. 1 c. 3 b. 2 d The shape (not the size) of an electron cloud is determined by the electron's. a. energy sublevel c. speed b. position d. principal quantum number 22. The letter "p" in the symbol 4p indicates the. a. spin of an electron c. principle energy level b. orbital shape d. speed of an electron

3 23. According to the aufbau principle,. a. an orbital may be occupied by only two electrons b. electrons in the same orbital must have opposite spins c. electrons enter orbitals of highest energy first d. electrons enter orbitals of lowest energy first 24. What is the electron configuration of potassium? a. 1s 2s 2p 3s 3p 4s c. 1s 2s 3s 3p 3d b. 1s 2s 2p 3s 3p d. 1s 2s 2p 3s 3p 4s 25. How many unpaired electrons are in a sulfur atom (atomic number 16)? a. 0 c. 2 b. 1 d How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum? a. The speed of visible light is greater. b. The speed of gamma rays is greater. c. The speeds are the same. d. No answer can be determined from the information given. 27. Which color of visible light has the shortest wavelength? a. yellow c. blue b. green d. violet 28. The light given off by an electric discharge through sodium vapor is. a. a continuous spectrum c. of a single wavelength b. an emission spectrum d. white light 29. To what category of elements does an element belong if it is a poor conductor of electricity? a. transition elements c. nonmetals b. metalloids d. metals 30. What element has the electron configuration 1s 2s 2p 3s 3p? a. nitrogen c. silicon b. selenium d. silver 31. Atomic size generally. a. increases as you move from left to right across a period b. decreases as you move from top to bottom within a group c. remains constant within a period d. decreases as you move from left to right across a period 32. What element in the second period has the largest atomic radius? a. carbon c. potassium b. lithium d. neon

4 33. The metals in Groups 1A, 2A, and 3A. a. gain electrons when they form ions c. all have ions with a 1 charge b. all form ions with a negative charge d. lose electrons when they form ions 34. What is the element with the highest electronegativity value? a. cesium c. calcium b. helium d. fluorine 35. Which of the following statements correctly compares the relative size of an ion to its neutral atom? a. The radius of an anion is greater than the radius of its neutral atom. b. The radius of an anion is identical to the radius of its neutral atom. c. The radius of a cation is greater than the radius of its neutral atom. d. The radius of a cation is identical to the radius of its neutral atom. 36. How many valence electrons are in an atom of phosphorus? a. 2 c. 4 b. 3 d What is the formula unit of aluminum oxide? a. AlO c. AlO b. Al O d. Al O 38. Which of the following is NOT a characteristic of most ionic compounds? a. They are solids. b. They have low melting points. c. When melted, they conduct an electric current. d. They are composed of metallic and nonmetallic elements. 39. Which of these elements does not exist as a diatomic molecule? a. Ne c. H b. F d. I 40. Why do atoms share electrons in covalent bonds? a. to become ions and attract each other b. to attain a noble-gas electron configuration c. to become more polar d. to increase their atomic numbers 41. Which of the following diatomic molecules is joined by a double covalent bond? a. c. b. d. 42. A bond formed between a silicon atom and an oxygen atom is likely to be. a. ionic c. polar covalent b. coordinate covalent d. nonpolar covalent 43. Which of the following covalent bonds is the most polar? a. H F c. H H b. H C d. H N

5 44. When placed between oppositely charged metal plates, the region of a water molecule attracted to the negative plate is the. a. hydrogen region of the molecule c. H O H plane of the molecule b. geometric center of the molecule d. oxygen region of the molecule 45. What type of ions have names ending in -ide? a. only cations c. only metal ions b. only anions d. only gaseous ions 46. When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a. a. prefix c. Roman numeral following the name b. suffix d. superscript after the name 47. Which of the following compounds contains the Mn ion? a. MnS c. Mn O b. MnBr d. MnO 48. Which element, when combined with fluorine, would most likely form an ionic compound? a. lithium c. phosphorus b. carbon d. chlorine 49. What is the correct formula for potassium sulfite? a. KHSO c. K SO b. KHSO d. K SO 50. What is the formula for phosphoric acid? a. H PO c. HPO b. H PO d. HPO 51. What does an -ite or -ate ending in a polyatomic ion mean? a. Oxygen is in the formula. c. Nitrogen is in the formula. b. Sulfur is in the formula. d. Bromine is in the formula. 52. Avogadro's number of representative particles is equal to one. a. kilogram c. kelvin b. gram d. mole 53. How many molecules are in 2.10 mol CO? a molecules c molecules b molecules d molecules 54. What is the mass in grams of 5.90 mol C H? a g c. 389 g b g d. 673 g

6 55. What is the volume, in liters, of mol of C H gas at STP? a L c L b L d L 56. What is the percent by mass of carbon in acetone, C H O? a. 20.7% c. 1.61% b. 62.1% d. 30.0% 57. What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight? a. SO c. SO b. SO d. S O 58. What are the coefficients that will balance the skeleton equation below? AlCl + NaOH Al(OH) NaCl a. 1, 3, 1, 3 c. 1, 1, 1, 3 b. 3, 1, 3, 1 d. 1, 3, 3, What are the missing coefficients for the skeleton equation below? Al (SO ) (aq) KOH(aq) Al(OH) (aq) K SO (aq) a. 1, 3, 2, 3 c. 4, 6, 2, 3 b. 2, 12, 4, 6 d. 1, 6, 2, The type of reaction that takes place when one element reacts with a compound to form a new compound and a different element is a. a. combination reaction c. single-replacement reaction b. decomposition reaction d. double-replacement reaction 61. Which of the following is a balanced equation representing the decomposition of lead(iv) oxide? a. PbO Pb 2O c. Pb O 2Pb O b. PbO Pb O d. PbO Pb O 62. In the activity series of metals, which metal(s) will displace hydrogen from an acid? a. only metals above hydrogen c. any metal b. only metals below hydrogen d. only metals from Li to Na 63. If a combination reaction takes place between rubidium and bromine, the chemical formula for the product is. a. RuBr c. RbBr b. Rb Br d. RbBr 64. The calculation of quantities in chemical equations is called. a. stoichiometry c. percent composition b. dimensional analysis d. percent yield 65. How many moles of aluminum are needed to react completely with 1.2 mol of FeO? 2Al(s) + 3FeO(s) 3Fe(s) + Al O (s)

7 a. 1.2 mol c. 1.6 mol b. 0.8 mol d. 2.4 mol 66. Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum? 2Al(s) + 3H SO (aq) Al (SO ) (aq) + 3H (g) a mol c mol b mol d mol 67. How many grams of chromium are needed to react with an excess of CuSO to produce 27.0 g Cu? 2Cr(s) + 3CuSO (aq) Cr (SO ) (aq) + 3Cu(s) a g c g b g d g 68. When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the. a. actual yield c. theoretical yield b. percent yield d. minimum yield 69. A gas occupies a volume of 2.4 L at 14.1 kpa. What volume will the gas occupy at 84.6 kpa? a. 497 L c. 14 L b. 2.5 L d L 70. At high pressures, how does the volume of a real gas compare with the volume of an ideal gas under the same conditions? a. It is much greater. c. There is no difference. b. It is much less. d. It depends on the type of gas. 71. Which of the following gases will effuse the most rapidly? a. bromine c. ammonia b. chlorine d. hydrogen 72. If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was. a. unsaturated c. an emulsion b. saturated d. supersaturated 73. What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution? a. 6M c. 7M b. 12M d. 3M 74. If an atom is reduced in a redox reaction, what must happen to another atom in the system? a. It must be oxidized. b. It must be reduced. c. It must be neutralized. d. Nothing needs to happen to another atom in the system. 75. What is another name for an oxidation-reduction reaction? a. O-reaction c. redox reaction b. R-reaction d. oxred reaction

8 76. In which of the following types of reaction are electrons gained? a. decomposition c. neutralization b. oxidation d. reduction 77. Oxidation is. a. a loss of oxygen c. a loss of electrons b. a gain of electrons d. a gain of hydrogen 78. Cu Cu + 2 e- The equation above represents the type of reaction called. a. redox c. reduction b. hydrolysis d. oxidation 79. The oxidation number of magnesium in magnesium chloride is. a. 1 c. +1 b. 0 d The oxidation number of hydrogen when it is in a compound other than a hydride is. a. 2 c. 0 b. 1 d The oxidation number of bromime in bromime gas is. a. 2 c. 0 b. 1 d. +1

9 Chemistry Final Exam Review Answer Section MULTIPLE CHOICE 1. ANS: D DIF: L1 REF: p. 40 OBJ: ANS: B DIF: L1 REF: p. 41 OBJ: ANS: D DIF: L1 REF: p. 45 OBJ: ANS: C DIF: L1 REF: p. 45 OBJ: ANS: D DIF: L2 REF: p. 48 OBJ: ANS: D DIF: L1 REF: p. 53 OBJ: ANS: B DIF: L1 REF: p. 64 OBJ: ANS: C DIF: L1 REF: p. 77, p. 78 OBJ: ANS: C DIF: L2 REF: p. 106, p. 107 OBJ: 4.2.1, ANS: B DIF: L1 REF: p. 110 OBJ: ANS: D DIF: L1 REF: p. 110 OBJ: ANS: D DIF: L1 REF: p. 111 OBJ: ANS: B DIF: L1 REF: p. 111 OBJ: ANS: B DIF: L1 REF: p. 110 OBJ: ANS: A DIF: L1 REF: p. 112, p. 113 OBJ: ANS: C DIF: L3 REF: p. 112, p. 113 OBJ: ANS: D DIF: L2 REF: p. 112, p. 113 OBJ: ANS: A DIF: L2 REF: p. 128 OBJ: ANS: B DIF: L2 REF: p. 131 OBJ: ANS: B DIF: L2 REF: p. 131 OBJ: ANS: A DIF: L2 REF: p. 131 OBJ: ANS: B DIF: L2 REF: p. 131 OBJ: ANS: D DIF: L2 REF: p. 133 OBJ: ANS: D DIF: L2 REF: p. 133, p. 134, p. 135 OBJ: ANS: C DIF: L3 REF: p. 133, p. 134 OBJ: ANS: C DIF: L2 REF: p. 139 OBJ: ANS: D DIF: L2 REF: p. 139 OBJ: ANS: B DIF: L2 REF: p. 141 OBJ: ANS: C DIF: L3 REF: p. 160 OBJ: ANS: C DIF: L2 REF: p. 164 OBJ: ANS: D DIF: L2 REF: p. 171 OBJ: ANS: B DIF: L2 REF: p. 171 OBJ: ANS: D DIF: L2 REF: p. 162, p. 163, p. 172, p. 176

10 34. ANS: D DIF: L1 REF: p. 177 OBJ: ANS: A DIF: L2 REF: p. 172, p. 176 OBJ: ANS: D DIF: L1 REF: p. 187 OBJ: ANS: D DIF: L2 REF: p. 195 OBJ: ANS: B DIF: L1 REF: p. 196, p. 198 OBJ: ANS: A DIF: L1 REF: p. 217 OBJ: ANS: B DIF: L2 REF: p. 217 OBJ: ANS: A DIF: L2 REF: p. 221 OBJ: ANS: C DIF: L2 REF: p. 238, p. 239 OBJ: 8.1.1, ANS: A DIF: L3 REF: p. 238, p. 239 OBJ: ANS: A DIF: L3 REF: p. 239 OBJ: ANS: B DIF: L1 REF: p. 254 OBJ: ANS: C DIF: L1 REF: p. 254, p. 255 OBJ: ANS: C DIF: L1 REF: p. 262, p. 263 OBJ: ANS: A DIF: L2 REF: p. 253, p. 254, p. 262 OBJ: ANS: C DIF: L2 REF: p. 257, p. 261, p. 262 OBJ: ANS: B DIF: L2 REF: p. 272 OBJ: ANS: A DIF: L1 REF: p. 257, p. 278 OBJ: 9.1.3, ANS: D DIF: L1 REF: p. 290 OBJ: ANS: D DIF: L2 REF: p. 291, p ANS: D DIF: L2 REF: p. 297, p. 298 OBJ: ANS: B DIF: L2 REF: p. 301 OBJ: ANS: B DIF: L2 REF: p. 307 OBJ: ANS: C DIF: L2 REF: p. 310 OBJ: ANS: A DIF: L1 REF: p. 324, p. 325 OBJ: ANS: D DIF: L2 REF: p. 324, p. 327 OBJ: ANS: C DIF: L1 REF: p. 333 OBJ: ANS: B DIF: L2 REF: p. 332 OBJ: ANS: A DIF: L2 REF: p. 333 OBJ: ANS: D DIF: L2 REF: p. 330, p. 337 OBJ: ANS: A DIF: L1 REF: p. 354 OBJ: ANS: B DIF: L1 REF: p. 359, p. 360

11 OBJ: ANS: D DIF: L2 REF: p. 359, p. 360 OBJ: ANS: A DIF: L2 REF: p. 371 OBJ: ANS: C DIF: L1 REF: p. 372 OBJ: ANS: D DIF: L2 REF: p. 419 OBJ: ANS: A DIF: L2 REF: p. 428 OBJ: ANS: D DIF: L2 REF: p. 436 OBJ: ANS: D DIF: L2 REF: p. 474 OBJ: ANS: D DIF: L1 REF: p. 481 OBJ: ANS: A DIF: L1 REF: p. 632 OBJ: ANS: C DIF: L1 REF: p. 632 OBJ: ANS: D DIF: L1 REF: p. 633 OBJ: ANS: C DIF: L1 REF: p. 633 OBJ: ANS: D DIF: L1 REF: p. 634 OBJ: ANS: D DIF: L1 REF: p. 639 OBJ: ANS: D DIF: L1 REF: p. 639 OBJ: ANS: C DIF: L1 REF: p. 639 OBJ:

b. Na. d. So. 1 A basketball has more mass than a golf ball because:

b. Na. d. So. 1 A basketball has more mass than a golf ball because: Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the