Final Exam Study Guide and Review

1. Final Exam Study Guide and Review

2. The abbreviation for atomic mass unit is a. amu. b. mu. c. a. d. µ.

3. The carbon-12 atom is assigned a relative mass of exactly a. 1 amu. b.6 amu. c. 12 amu. d. 100 amu.

4. Which is the ground-state electron configuration for ? a. [Ar] 4s23d4 b. [Ar] 4s13d5 c. [Ar] 4s33d3 d. [Ar] 4s43d2

5. The letter designations for the first four sublevels, with the number of electrons that can be accommodated in each sublevel are a. s: 1, p: 3, d: 10, and f: 14. b. s: 1, p: 3, d: 5, and f: 7. c. s: 2, p: 6, d: 10, and f: 14. d. s: 1, p: 2, d: 3, and f: 4.

6. Most of the volume of an atom is occupied by the a. nucleus. b. nuclides. c. electron cloud. d. protons.

7. Isotopes of an element contain different numbers of a. electrons. b. protons. c. neutrons. d. nuclides.

8. Isotopes are atoms of the same element that have different a. principal chemical properties. b. masses. c. numbers of protons. d. numbers of electrons.

9. An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is a. 13. b. 14. c. 27. d. 40.

10. What is the name of Sn3(PO4)4? a. stannous phosphate b. tin(IV) phosphate c. tin(III) phosphate d. tin(II) phosphate

11. Name the compound CuCO3. a. Copper(I) carbonate b. cupric trioxycarbide c. cuprous carbide d. copper(II) carbonate

12. Name the compound Fe(NO2)2. a. iron(II) nitrate b. iron(II) nitrite c. ferric nitrate d. ferrous nitride

13. Name the compound KClO3. a. potassium chloride b. potassium trioxychlorite c. potassium chlorate d. hypochlorite

14. Name the compound Hg2(NO3)2. a. mercury(II) nitrate b. dimercury dinitrate c. mercury(I) nitrate d. mercuric nitrate

15. Name the compound Zn3(PO4)2. a. zinc potassium oxide b. trizinc polyoxide c. zinc phosphate d. zinc phosphite

16. Name the compound Ni(ClO3)2. a. nickel chlorate b. nickel chloride c. nickel chlorite d. nickel peroxide

17. What is the formula for the compound formed by the barium ion, Ba2+, and the hydroxide ion, OH–? a. BaOH b. BaOH2 c. Ba(OH)2 d. Ba(OH)

18. What is the formula for the compound formed by tin(IV) and the chromate ion, CrO42–? a. Sn(CrO4)4 b. Sn2(CrO4)2 c. Sn2(CrO4)4 d. Sn(CrO4)2

19. What is the formula for the compound formed by aluminum(III) and the sulfate ion, SO42–? a. AlSO4 b. Al2SO4 c. Al2(SO4)3 d. Al(SO4)3

20. What is the formula for the compound formed by lead(II) ions and chromate ions, CrO42–? a. PbCrO4 c. Pb2(CrO4)3 b. Pb2CrO4 d. Pb(CrO4)2

21. A comparison of calcium sulfate and calcium sulfite shows that a. both have a monatomic cation and a polyatomic anion. b. calcium sulfite has more oxygen atoms than calcium sulfate. c. only calcium sulfite contains a polyatomic anion. d. only calcium sulfate is arranged in a crystal lattice pattern.

22. The symbol HCO3– represents a a. monatomic ion. b. stable compound c. polyatomic ion. d. salt.

23. The chemical formula for an ionic compound represents the a. number of atoms in each molecule. b. number of ions in each molecule. c. simplest ratio of ions that results in an electrically neutral compound. d. total number of ions in the crystal lattice.

24. What is the formula for the compound formed by calcium ions, Ca2+, and chloride ions, Cl–? a. CaCl b. Ca2Cl c. CaCl3 d. CaCl2

25. What is the metallic ion in the compound CuCl2? a. Cu2– b. Cu– c. Cu+ d. Cu2+

26. The indium(II) ion and indium(III) ion a. have the same charge. b. are polyatomic ions. c. have charges of 1+ and 2+, respectively. d. have charges of 2+ and 3+, respectively.

27. What is the ratio of cations to anions in a compound composed of sodium ions, Na+, and carbonate ions, ? a. 1 to 1 b. 1 to 2 c. 2 to 1 d. 3 to 1

28. A compound that has the same number of positive and negative charges is said to be a. cationic. b. anionic. c. electroneutral. d. isoelectronic.

29. An ion and its parent atom have the same a. electron configuration. b. number of charges c. atomic number. d. chemical reactivity.

30. Once an atom has full s and p orbitals in its outermost energy level, a. it is highly reactive only with alkali metals. b. it is highly reactive only with halogens. c. it can be combined with most elements. d. it has a stable octet and is unreactive.

31. The elements of the _____ group satisfy the octet rule without forming compounds. a. halide b. noble gas c. alkali metal d. alkaline-earth metal

32. An anion a. is an ion with a negative charge. b. attracts ions with negative charges. c. results when an alkaline-earth metal loses one of its two outermost electrons. d. has more protons than electrons.

33. Atoms of copper and iron a. generally form stable bonds with transition elements. b. have stable electron configurations. c. tend to form cations. d. tend to form anions.

34. The electron configuration of nitrogen is 1s22s22p3. How many more electrons does nitrogen need to have an electron configuration similar to neon? a. 1 b. 3 c. 5 d. 8

35. In the compound sodium fluoride, NaF, the sodium atom loses one electron and the fluorine atom gains one electron to form ions that have electron configurations similar to a. helium. b. oxygen. c. neon. d. calcium.

36. Which of the following electron configurations belongs to an element that is NOT chemically reactive? a. 1s22s22p3 b. 1s22s22p63s23p6 c. 1s22s22p5 d. 1s22s22p63s23p64s1

37. Manganese has the electron configuration, 1s2 2s2 2p6 3s2 3p6 4s2 3d5. Which of the following forms is most likely that of the ion? a. Mn5_ b. Mn2_ c. Mn2+ d. Mn6_

38. According to the octet rule, a calcium atom has a tendency to a. lose one electron. b. lose two electrons. c. gain one electron. d. gain two electrons.

39. The correct name for the salt with the formula CaI2 is a. calcium diodide. b. calcium iodine. c. calcium iodide. d. dicalcium iodine.

40. The pair of ions listed below with similar chemical properties is a. F- and Cl-. b. F- and Li+. c. Na+ and Cl-. d. Na+ and F-.

41. How many electrons does Barium have in its outermost shell? a. 1 b. 2 c. 3 d. 4

42. Which of the following elements is a transition metal? a. calcium b. iron c. sodium d. sulfur

43. The alkali metal elements are found in of the periodic table. a. Group 1 b. Group 2 c. Period 1 d. Period 2

44. How many electrons does carbon have in its outermost shell? a. 1 b. 2 c. 3 d. 4

45. A covalent bond is formed when two atoms a. share an electron with each other. b. share one or more pairs of electrons with each other. c. gain electrons. d. gain and lose electrons

46. A polyatomic anion consists of a. a single atom with a negative charge. b. a single atom with a positive charge. c. multiple atoms with an overall negative charge. d. multiple atoms with an overall positive charge

47. In the word equation sodium chloride → chlorine gas + sodium a. sodium is a product. b. chlorine gas is a reactant. c. sodium chloride is a product. d. None of the above

48. The formation of a solid product in a chemical reaction is represented by the symbol a. (aq). b. (g). c. (l). d. (s).

49. An atom of potassium has 19 protons and 20 neutrons. Its mass number is a. 9. b. 19. c. 20. d. 39.

50. The electron configuration in Figure 1 violates ↑↓ 1s ↑↓ 2s 2p ↑↓↑ __ Figure 1 a. the Pauli exclusion principle. b. the aufbau principle. c. Hund’s rule. d. Both (a) and (c)