Name: ________________________ Class: ___________________ Date: __________ ID: A Chapter 8 and 9 Test Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. ____ ____ ____ ____ ____ 1. What type of ions have names ending in -ide? a. only cations c. only metal ions b. only anions d. only gaseous ions 2. When Group 2A elements form ions, they ____. a. lose two protons c. lose two electrons b. gain two protons d. gain two electrons 3. 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 4. Aluminum is a group 3A metal. Which ion does A1 typically form? c. Al 5 − a. Al 3 − b. Al 3 + d. Al 5 + 5. Which of the following compounds contains the Mn 3 + ion? a. MnS c. Mn 2 O 3 b. ____ ____ ____ d. MnO 6. How are chemical formulas of binary ionic compounds generally written? a. cation on left, anion on right b. anion on left, cation on right c. Roman numeral first, then anion, then cation d. subscripts first, then ions 7. Which of the following formulas represents an ionic compound? a. CS 2 c. N 2 O 4 b. ____ MnBr 2 BaI 2 d. PCl 3 8. Which element, when combined with fluorine, would most likely form an ionic compound? a. lithium c. phosphorus b. carbon d. chlorine 9. Which of the following shows correctly an ion pair and the ionic compound the two ions form? a. Sn 4 + , N 3 − ; Sn 4 N 3 c. Cr 3 + , I − ; CrI b. Cu 2 + , O 2 − ; Cu 2 O 2 d. Fe 3 + , O 2 − ; Fe 2 O 3 ____ 10. In which of the following is the name and formula given correctly? a. sodium oxide, NaO c. cobaltous chloride, CoCl 3 b. barium nitride, BaN d. stannic fluoride, SnF 4 ____ 11. Which of the following compounds contains the lead(II) ion? a. PbO c. Pb2O b. PbCl4 d. Pb2S 1 Name: ________________________ ID: A ____ 12. 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 ____ 13. Which of the following correctly shows a prefix used in naming binary molecular compounds with its corresponding number? a. deca-, 7 c. hexa-, 8 b. nona-, 9 d. octa-, 4 ____ 14. Which of the following formulas represents a molecular compound? a. ZnO c. SO 2 b. Xe d. BeF 2 ____ 15. When naming acids, the prefix hydro- is used when the name of the acid anion ends in ____. a. -ide c. -ate b. -ite d. -ic ____ 16. Which of the following shows both the correct formula and correct name of an acid? c. H 3 PO 4 , phosphoric acid a. HClO 2 , chloric acid b. HNO 2 , hydronitrous acid ____ 17. What is the formula for sulfurous acid? a. H 2 SO 4 b. H 2 SO 3 d. HI, iodic acid c. H 2 SO 2 d. H2 S ____ 18. How are bases named? a. like monatomic elements c. b. like polyatomic ions d. ____ 19. Select the correct formula for sulfur hexafluoride. c. a. S 2 F 6 b. F 6 SO 3 d. like ionic compounds like molecular compounds F6 S2 SF 6 ____ 20. Which of the following is the correct name for N 2 O 5 ? a. nitrous oxide b. dinitrogen pentoxide ____ 21. What is the correct name for Sn 3 (PO 4 ) 2 ? c. d. nitrogen dioxide nitrate oxide a. tritin diphosphate c. tin(III) phosphate b. tin(II) phosphate d. tin(IV) phosphate ____ 22. Which is a typical characteristic of an ionic compound? a. Electron pairs are shared among atoms. b. The ionic compound has a low solubility in water. c. The ionic compound is described as a molecule. d. The ionic compound has a high melting point. ____ 23. Which of these elements does not exist as a diatomic molecule? a. Ne c. H b. F d. I 2 Name: ________________________ ID: A ____ 24. How do atoms achieve noble-gas electron configurations in single covalent bonds? a. One atom completely loses two electrons to the other atom in the bond. b. Two atoms share two pairs of electrons. c. Two atoms share two electrons. d. Two atoms share one electron. ____ 25. Which of the following diatomic molecules is joined by a double covalent bond? c. N 2 a. O 2 d. He 2 ____ 26. A molecule with a single covalent bond is ____. c. a. CO 2 CO b. b. Cl2 Cl 2 d. N2 ____ 27. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible? a. pairs of valence electrons c. mobile electrons b. inner shell electrons d. the electrons closest to the nuclei ____ 28. The shape of the methane (CH4) molecule is called ____. a. tetrahedral c. four-cornered b. square d. planar ____ 29. 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 ____ 30. Which of the following covalent bonds is the most polar? a. H—F c. H—H b. H—C d. H—N Short Answer 31. Draw the Lewis Dot Diagram for H2O. . 32. Draw the Lewis Dot Diagram for CF4. . 33. Draw the Lewis Dot Diagram for N2O4. . 3 Name: ________________________ ID: A 34. Draw two resonance structures for (CO3)-2. . 4 ID: A Chapter 8 and 9 Test Answer Section MULTIPLE CHOICE 1. ANS: STO: 2. ANS: STO: 3. ANS: OBJ: 4. ANS: STO: 5. ANS: OBJ: 6. ANS: STO: 7. ANS: STO: 8. ANS: OBJ: 9. ANS: STO: 10. ANS: OBJ: 11. ANS: OBJ: 12. ANS: STO: 13. ANS: STO: 14. ANS: STO: 15. ANS: STO: 16. ANS: STO: 17. ANS: STO: 18. ANS: STO: 19. ANS: OBJ: 20. ANS: OBJ: B C.1.33 C C.1.7 C 9.1.1 B C.1.33 C 9.2.1 A C.1.6 B C.1.6 A 9.2.1 D C.1.6 D 9.2.1 A 9.2.1 C C.1.36 B C.1.36, C.1.6 C C.1.36, C.1.6 A C.1.8 C C.1.8 B C.1.8 C C.1.8 D 9.3.2, 9.5.2 B 9.3.2, 9.5.3 DIF: L1 REF: p. 254 OBJ: 9.1.1 DIF: L1 REF: p. 254 OBJ: 9.1.1 DIF: L1 STO: C.1.6 DIF: L1 REF: p. 254, p. 255 DIF: L1 STO: C.1.7, C.1.6 DIF: L1 REF: p. 262, p. 263 REF: p. 261 OBJ: 9.2.1 DIF: REF: p. 262 OBJ: 9.2.1 L2 REF: p. 253 OBJ: 9.1.1 DIF: L2 STO: C.1.36 DIF: L2 REF: p. 253, p. 254, p. 262 DIF: STO: DIF: STO: DIF: L2 C.1.6 L2 C.1.6 L1 REF: p. 262, p. 263 REF: p. 268 OBJ: 9.3.1, 9.3.2 DIF: L2 REF: p. 269 OBJ: 9.3.2 DIF: L2 REF: p. 269 OBJ: 9.3.2 DIF: L2 REF: p. 272 OBJ: 9.4.1 DIF: L2 REF: p. 272 OBJ: 9.4.1 DIF: L2 REF: p. 272 OBJ: 9.4.2 DIF: L1 REF: p. 273 OBJ: 9.4.3 DIF: STO: DIF: STO: L2 C.1.8 L2 C.1.7 REF: p. 270, p. 278 REF: p. 262 OBJ: 9.2.1 REF: p. 262, p. 263 REF: p. 269, p. 277 1 ID: A 21. ANS: OBJ: 22. ANS: STO: 23. ANS: STO: 24. ANS: STO: 25. ANS: STO: 26. ANS: STO: 27. ANS: STO: 28. ANS: STO: 29. ANS: OBJ: 30. ANS: OBJ: B 9.5.3 D C.1.36 A C.1.36 C C.1.36 A C.1.36 B C.1.36 A C.1.36 A C.1.36 C 8.1.1, 8.4.1 A 8.4.1 DIF: L3 STO: C.1.7 DIF: L2 REF: p. 264, p. 277 REF: p. 244 OBJ: 8.1.1 DIF: L1 REF: p. 217 OBJ: 8.2.1 DIF: L2 REF: p. 217 OBJ: 8.2.1 DIF: L2 REF: p. 221 OBJ: 8.2.3 DIF: L2 REF: p. 222 OBJ: 8.2.1, 8.2.4 DIF: L1 REF: p. 232 OBJ: 8.3.2 DIF: L1 REF: p. 232 OBJ: 8.3.2 DIF: STO: DIF: STO: L2 C.1.36 L3 C.1.36 REF: p. 238, p. 239 REF: p. 238, p. 239 SHORT ANSWER 31. ANS: See Drawing Key 32. ANS: See drawing key 33. ANS: See drawing key 34. ANS: See drawing key 2