University:
Winston-Salem Forsyth County Schools
Course:
AP Physics C: Elec & Mag
Academic year:

2014
Views:

380

Pages:

9
Author:

Hugo Sweeney

Chapter 7-9 and 11 Test Review Hopefully enough stuff Answer Section MATCHING 1. ANS: E 2. ANS: B 3. ANS: D DIF: L1 DIF: L1 DIF: L1 REF: p. 187 REF: p. 188 REF: p. 188 OBJ: 7.1.1 OBJ: 7.1.2 OBJ: 7.1.4 4. ANS: A 5. ANS: E DIF: L1 DIF: L1 REF: p. 223 REF: p. 238 OBJ: 8.2.4 OBJ: 8.4.1 DIF: DIF: DIF: DIF: L1 L1 L1 L2 REF: REF: REF: REF: p. 187 OBJ: 7.1.1 p. 188 OBJ: 7.1.1 p. 188 OBJ: 7.1.1 p. 188, p. 189 DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: L2 L1 L1 L1 L1 L2 L2 L2 REF: REF: REF: REF: REF: REF: REF: REF: p. 188 p. 191 p. 192 p. 194 p. 194 p. 195 p. 195 p. 192, p. 195 MULTIPLE CHOICE 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. ANS: ANS: ANS: ANS: OBJ: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: OBJ: ANS: OBJ: ANS: OBJ: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: OBJ: ANS: ANS: ANS: D D B A 7.1.1 A A B C D C D B 7.2.1 B 7.2.1 A 7.2.1 A A B A D C A A D A 8.4.1 B B C DIF: L2 REF: p. 192, p. 195 DIF: L2 REF: p. 192, p. 194 DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: REF: REF: REF: REF: REF: REF: REF: REF: REF: REF: L1 L1 L2 L2 L2 L1 L1 L1 L2 L3 DIF: L1 DIF: L1 DIF: L1 p. 201 p. 217 p. 217 p. 221 p. 229 p. 230 p. 232 p. 232 p. 235 p. 238, p. 239 REF: p. 243 REF: p. 254 REF: p. 254 OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: 7.1.2 7.1.4 7.1.4 7.2.1 7.2.1 7.2.1 7.2.1 OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: 7.3.1 8.2.1 8.2.1 8.2.3 8.2.7 8.3.1 8.3.2 8.3.2 8.3.3 OBJ: 8.4.4 OBJ: 9.1.1 OBJ: 9.1.1 33. ANS: OBJ: 34. ANS: OBJ: 35. ANS: OBJ: 36. ANS: OBJ: 37. ANS: OBJ: 38. ANS: 39. ANS: 40. ANS: OBJ: 41. ANS: 42. ANS: 43. ANS: 44. ANS: 45. ANS: 46. ANS: OBJ: 47. ANS: OBJ: 48. ANS: 49. ANS: 50. ANS: 51. ANS: 52. ANS: 53. ANS: 54. ANS: OBJ: 55. ANS: 56. ANS: OBJ: 57. ANS: OBJ: 58. ANS: OBJ: 59. ANS: 60. ANS: 61. ANS: OBJ: 62. ANS: 63. ANS: 64. ANS: Matching B 9.1.1, 9.1.2 C 9.2.1 D 9.2.1 C 9.2.2 C 9.2.2 C C A 9.2.1, 9.3.2 B C C B D D 9.2.1, 9.5.2 B 9.3.2, 9.5.3 C C A C B C C 11.1.3 C D 11.2.1 C 11.2.1 D 11.2.1 C D C 11.3.2 C A B DIF: L1 REF: p. 254, p. 255, p. 257 DIF: L1 REF: p. 262, p. 263 DIF: L2 REF: p. 262, p. 263 DIF: L2 REF: p. 257, p. 261, p. 262 DIF: L2 REF: p. 264, p. 277 DIF: L2 DIF: L1 DIF: L1 REF: p. 268 OBJ: 9.3.1 REF: p. 268 OBJ: 9.3.1, 9.3.2 REF: p. 261, p. 269 DIF: DIF: DIF: DIF: DIF: DIF: REF: REF: REF: REF: REF: REF: L2 L2 L1 L2 L3 L2 p. 268 OBJ: p. 269 OBJ: p. 271 OBJ: p. 272 OBJ: p. 272 OBJ: p. 261, p. 262, p. 277 DIF: L2 REF: p. 269, p. 277 DIF: DIF: DIF: DIF: DIF: DIF: DIF: REF: REF: REF: REF: REF: REF: REF: L1 L1 L1 L1 L1 L1 L2 p. 232 p. 232 p. 232 p. 232 p. 232 p. 325 p. 324, p. 325 OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: 9.3.2 9.3.2 9.4.1 9.4.2 9.4.2 8.3.2 8.3.2 8.3.2 8.3.2 8.3.2 11.1.3 DIF: L1 DIF: L1 REF: p. 336 OBJ: 11.2.1 REF: p. 336, p. 337 DIF: L2 REF: p. 334, p. 335 DIF: L2 REF: p. 333, p. 334 DIF: L1 REF: p. 356 DIF: L2 REF: p. 334, p. 344 DIF: L2 DIF: L2 DIF: L1 REF: p. 327 REF: p. 233 REF: p. 240 OBJ: 12.1.2 OBJ: 11.1.3 OBJ: 8.3.2 OBJ: 8.4.3 Match each item with the correct statement below. a. halide ion e. valence electron b. octet rule f. coordination number c. ionic bond g. metallic bond d. electron dot structure ____ ____ ____ 1. an electron in the highest occupied energy level of an atom 2. Atoms react so as to acquire the stable electron structure of a noble gas. 3. a depiction of valence electrons around the symbol of an element Match each item with the correct statement below. a. coordinate covalent bond d. single covalent bond b. double covalent bond e. polar bond c. structural formula f. hydrogen bond ____ ____ 4. a covalent bond in which the shared electron pair comes from only one of the atoms 5. a covalent bond between two atoms of significantly different electronegativities Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. ____ ____ ____ ____ ____ ____ 6. How many valence electrons are in an atom of phosphorus? a. 2 c. 4 b. 3 d. 5 7. How many valence electrons are in an ion of magnesium? a. 2 c. 6 b. 4 d. 8 8. How does calcium obey the octet rule when reacting to form compounds? a. It gains electrons. b. It gives up electrons. c. It does not change its number of electrons. d. Calcium does not obey the octet rule. 9. What is the electron configuration of the calcium ion? a. 1s 2s 2p 3s 3p c. 1s 2s 2p 3s 3p 4s b. 1s 2s 2p 3s 3p 4s d. 1s 2s 2p 3s 10. The octet rule states that, in chemical compounds, atoms tend to have ____. a. the electron configuration of a noble gas b. more protons than electrons c. eight electrons in their principal energy level d. more electrons than protons 11. How does oxygen obey the octet rule when reacting to form compounds? a. It gains electrons. b. It gives up electrons. c. It does not change its number of electrons. d. Oxygen does not obey the octet rule. ____ 12. The electron configuration of a fluoride ion, F , is ____. a. 1s 2s 2p c. 1s 2s 2p 3s b. the same as that of a neon atom d. the same as that of a potassium ion ____ 13. What is the net charge of the ionic compound calcium fluoride? a. 2– c. 0 b. 1– d. 1 ____ 14. A compound held together by ionic bonds is called a ____. a. diatomic molecule c. covalent molecule b. polar compound d. salt ____ 15. What is the formula unit of sodium nitride? a. NaN c. Na N b. Na N d. NaN ____ 16. What is the formula unit of aluminum oxide? a. AlO b. Al O c. AlO d. Al O ____ 17. What is the name of the ionic compound formed from lithium and bromine? a. lithium bromine c. lithium bromium b. lithium bromide d. lithium bromate ____ 18. What is the formula for sodium sulfate? a. NaSO c. Na(SO ) b. Na SO d. Na (SO ) ____ 19. Which of the following compounds has the formula KNO ? a. potassium nitrate c. potassium nitrite b. potassium nitride d. potassium nitrogen oxide ____ 20. What characteristic of metals makes them good electrical conductors? a. They have mobile valence electrons. b. They have mobile protons. c. They have mobile cations. d. Their crystal structures can be rearranged easily. ____ 21. Which of these elements does not exist as a diatomic molecule? a. Ne d. I b. F e. C c. H ____ 22. 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 ____ 23. Which of the following diatomic molecules is joined by a double covalent bond? a. c. b. d. ____ 24. In which of the following compounds is the octet expanded to include 12 electrons? a. H S c. PCl b. PCl d. SF ____ 25. How many electrons can occupy a single molecular orbital? a. 0 c. 2 b. 1 d. 4 ____ 26. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible? ____ 27. ____ 28. ____ 29. ____ 30. ____ 31. a. pairs of valence electrons c. mobile electrons b. inner shell electrons d. the electrons closest to the nuclei The shape of the methane molecule is called ____. a. tetrahedral c. four-cornered b. square d. planar What is the shape of a molecule with a triple bond? a. tetrahedral c. bent b. pyramidal d. linear Which of the following covalent bonds is the most polar? a. H—F c. H—H b. H—C d. H—N Which type of solid has the highest melting point? a. ionic solid c. metal b. network solid d. nonmetallic solid What type of ions have names ending in -ide? a. only cations c. only metal ions b. only anions d. only gaseous ions ____ 32. What is the correct name for the N ion? a. nitrate ion b. nitrogen ion ____ 33. Which of the following is NOT a cation? a. iron(III) ion b. sulfate c. nitride ion d. nitrite ion c. Ca d. mercurous ion ____ 34. Which of the following compounds contains the Mn ion? a. MnS c. Mn O b. MnBr d. MnO ____ 35. In which of the following is the name and formula given correctly? a. sodium oxide, NaO c. cobaltous chloride, CoCl b. barium nitride, BaN d. stannic fluoride, SnF ____ 36. What is the correct formula for potassium sulfite? a. KHSO c. K SO b. KHSO d. K SO ____ 37. What type of compound is CuSO ? a. monotomic ionic c. polyatomic ionic b. polyatomic covalent d. binary molecular ____ 38. Sulfur hexafluoride is an example of a ____. a. monatomic ion c. binary compound b. polyatomic ion d. polyatomic compound ____ 39. Molecular compounds are usually ____. a. composed of two or more transition elements b. composed of positive and negative ions c. composed of two or more nonmetallic elements d. exceptions to the law of definite proportions ____ 40. What is the ending for the names of all binary compounds, both ionic and molecular? a. -ide c. -ade b. -ite d. -ate ____ 41. Which of the following is a binary molecular compound? a. BeHCO c. AgI b. PCl d. MgS ____ 42. Which of the following formulas represents a molecular compound? a. ZnO c. SO b. Xe d. BeF ____ 43. When dissolved in water, acids produce ____. a. negative ions b. polyatomic ions ____ 44. What is the formula for phosphoric acid? a. H PO b. H PO ____ 45. What is the formula for hydrosulfuric acid? a. H S b. H SO c. hydrogen ions d. oxide ions c. HPO d. HPO c. HSO d. H S ____ 46. What is the correct name for the compound CoCl ? a. cobalt(I) chlorate c. cobalt(II) chlorate b. cobalt(I) chloride d. cobalt(II) chloride ____ 47. Which of the following is the correct name for N O ? a. nitrous oxide c. nitrogen dioxide b. dinitrogen pentoxide d. nitrate oxide ____ 48. The shape of a carbon dioxide molecule is called ____. a. tetrahedral c. linear b. square d. planar ____ 49. The shape of the BI3 molecule is called ____. a. tetrahedral c. pyramidal b. square d. planar ____ 50. What causes the difference in shape between BH3 and NH3____. Make sure you can draw differences a. lone pair of electrons c. molecular geometry b. electronegativity differences d. division of sixes ____ 51. The angle between bonds of carbon tetrachloride molecule is ____. a. 105 d. 120 b. 107 e. 180 c. 109.5 ____ 52. The angle between bonds of boron trifluoride molecule is ____. a. 105 d. 120 b. 107 e. 180 c. 109.5 ____ 53. Chemical equations must be balanced to satisfy ____. a. the law of definite proportions c. the law of conservation of mass b. the law of multiple proportions d. Avogadro’s principle ____ 54. What are the missing coefficients for the equation below? Cr(s) Fe(NO ) (aq) Fe(s) Cr(NO ) (aq) a. 4, 6, 6, 2 c. 2, 3, 3, 2 b. 2, 3, 2, 3 d. 1, 3, 3, 1 ____ 55. In a combustion reaction, one of the reactants is ____. a. hydrogen c. oxygen b. nitrogen d. a metal ____ 56. The products of a combustion reaction do NOT include ____. a. water c. carbon monoxide b. carbon dioxide d. hydrogen ____ 57. What are the correct formulas and coefficients for the products of the following double-replacement reaction? RbOH H PO a. Rb(PO ) H O c. Rb PO 3H O b. RbPO 2H O d. H Rb PO OH ____ 58. Use the activity series of metals to complete a balanced chemical equation for the following single replacement reaction. Ag(s) KNO (aq) a. AgNO K b. AgK NO c. AgKNO d. No reaction takes place because silver is less reactive than potassium. ____ 59. In a chemical reaction, the mass of the products ____. a. is less than the mass of the reactants b. is greater than the mass of the reactants c. is equal to the mass of the reactants d. has no relationship to the mass of the reactants ____ 60. What is the correct net ionic equation for the following. Na2SO4 + Pb(NO3)2  a. Na+1 + SO4-2  Na2SO4 c. Na+1 + NO3-1 NaNO3 +2 -1 b. Pb + 2NO3 Pb(NO3)2 d. Pb+2 + SO4-2  PbSO4 ____ 61. What is the precipitate in the following reaction? Ni(NO ) (aq) K S(aq) a. Hydrogen gas c. Nickel (II) sulfide b. Nickel (II) nitrate d. Potassium nitrate ____ 62. When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is ____. Also, write the net ionic equation above. a. KH BaCl KCl BaH b. KOH BaCl KCl BaOH c. 2KOH BaCl d. KOH BaCl 2KCl Ba(OH) KCl BaOH ____ 63. What causes water molecules to have a bent shape, according to VSEPR theory? a. repulsive forces between unshared pairs of electrons b. interaction between the fixed orbitals of the unshared pairs of oxygen c. ionic attraction and repulsion d. the unusual location of the free electrons ____ 64. Which of the forces of molecular attraction is the weakest? a. dipole interaction c. hydrogen bond b. dispersion d. single covalent bond Chapter 7-9 and 11 Test Review Hopefully enough stuff Answer Section MATCHING 1. ANS: E 2. ANS: B 3. ANS: D DIF: L1 DIF: L1 DIF: L1 REF: p. 187 REF: p. 188 REF: p. 188 OBJ: 7.1.1 OBJ: 7.1.2 OBJ: 7.1.4 4. ANS: A 5. ANS: E DIF: L1 DIF: L1 REF: p. 223 REF: p. 238 OBJ: 8.2.4 OBJ: 8.4.1 DIF: DIF: DIF: DIF: L1 L1 L1 L2 REF: REF: REF: REF: p. 187 OBJ: 7.1.1 p. 188 OBJ: 7.1.1 p. 188 OBJ: 7.1.1 p. 188, p. 189 DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: L2 L1 L1 L1 L1 L2 L2 L2 REF: REF: REF: REF: REF: REF: REF: REF: p. 188 p. 191 p. 192 p. 194 p. 194 p. 195 p. 195 p. 192, p. 195 MULTIPLE CHOICE 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. ANS: ANS: ANS: ANS: OBJ: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: OBJ: ANS: OBJ: ANS: OBJ: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: OBJ: ANS: ANS: ANS: D D B A 7.1.1 A A B C D C D B 7.2.1 B 7.2.1 A 7.2.1 A A B A D C A A D A 8.4.1 B B C DIF: L2 REF: p. 192, p. 195 DIF: L2 REF: p. 192, p. 194 DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: DIF: REF: REF: REF: REF: REF: REF: REF: REF: REF: REF: L1 L1 L2 L2 L2 L1 L1 L1 L2 L3 DIF: L1 DIF: L1 DIF: L1 p. 201 p. 217 p. 217 p. 221 p. 229 p. 230 p. 232 p. 232 p. 235 p. 238, p. 239 REF: p. 243 REF: p. 254 REF: p. 254 OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: 7.1.2 7.1.4 7.1.4 7.2.1 7.2.1 7.2.1 7.2.1 OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: 7.3.1 8.2.1 8.2.1 8.2.3 8.2.7 8.3.1 8.3.2 8.3.2 8.3.3 OBJ: 8.4.4 OBJ: 9.1.1 OBJ: 9.1.1 33. ANS: OBJ: 34. ANS: OBJ: 35. ANS: OBJ: 36. ANS: OBJ: 37. ANS: OBJ: 38. ANS: 39. ANS: 40. ANS: OBJ: 41. ANS: 42. ANS: 43. ANS: 44. ANS: 45. ANS: 46. ANS: OBJ: 47. ANS: OBJ: 48. ANS: 49. ANS: 50. ANS: 51. ANS: 52. ANS: 53. ANS: 54. ANS: OBJ: 55. ANS: 56. ANS: OBJ: 57. ANS: OBJ: 58. ANS: OBJ: 59. ANS: 60. ANS: 61. ANS: OBJ: 62. ANS: 63. ANS: 64. ANS: B 9.1.1, 9.1.2 C 9.2.1 D 9.2.1 C 9.2.2 C 9.2.2 C C A 9.2.1, 9.3.2 B C C B D D 9.2.1, 9.5.2 B 9.3.2, 9.5.3 C C A C B C C 11.1.3 C D 11.2.1 C 11.2.1 D 11.2.1 C D C 11.3.2 C A B DIF: L1 REF: p. 254, p. 255, p. 257 DIF: L1 REF: p. 262, p. 263 DIF: L2 REF: p. 262, p. 263 DIF: L2 REF: p. 257, p. 261, p. 262 DIF: L2 REF: p. 264, p. 277 DIF: L2 DIF: L1 DIF: L1 REF: p. 268 OBJ: 9.3.1 REF: p. 268 OBJ: 9.3.1, 9.3.2 REF: p. 261, p. 269 DIF: DIF: DIF: DIF: DIF: DIF: REF: REF: REF: REF: REF: REF: L2 L2 L1 L2 L3 L2 p. 268 OBJ: p. 269 OBJ: p. 271 OBJ: p. 272 OBJ: p. 272 OBJ: p. 261, p. 262, p. 277 DIF: L2 REF: p. 269, p. 277 DIF: DIF: DIF: DIF: DIF: DIF: DIF: REF: REF: REF: REF: REF: REF: REF: L1 L1 L1 L1 L1 L1 L2 p. 232 p. 232 p. 232 p. 232 p. 232 p. 325 p. 324, p. 325 OBJ: OBJ: OBJ: OBJ: OBJ: OBJ: 9.3.2 9.3.2 9.4.1 9.4.2 9.4.2 8.3.2 8.3.2 8.3.2 8.3.2 8.3.2 11.1.3 DIF: L1 DIF: L1 REF: p. 336 OBJ: 11.2.1 REF: p. 336, p. 337 DIF: L2 REF: p. 334, p. 335 DIF: L2 REF: p. 333, p. 334 DIF: L1 REF: p. 356 DIF: L2 REF: p. 334, p. 344 DIF: L2 DIF: L2 DIF: L1 REF: p. 327 REF: p. 233 REF: p. 240 OBJ: 12.1.2 OBJ: 11.1.3 OBJ: 8.3.2 OBJ: 8.4.3