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Bonding
Bonding Test
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
1. In the compound sodium fluoride, NaF, the sodium atom loses one electron and the fluorine atom gains one
electron to form ions that are isoelectric with
a. helium.
c. neon.
b. oxygen.
d. calcium.
2. 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.
3. 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.
4. The elements of the ____ group satisfy the octet rule without forming compounds.
a. main
c. alkali metal
b. noble gas
d. alkaline-earth metal
5. Once an atom has a full 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.
6. What principle states that atoms tend to form compounds so that each atom can have eight electrons in its
outermost energy level?
a. rule of eights
c. configuration rule
b. Avogadro's principle
d. octet rule
7. How many sodium ions, Na+, are needed to make a carbonate ion, CO32– electrically neutral?
a. 1
c. 3
b. 2
d. 4
8. An ion of bromine with a single negative charge has the symbol and name
a. Br+, bromide ion.
c. Br+, bromium ion.
–
b. Br , bromide ion.
d. Br–, bromium ion.
9. Lead(II) ion and lead(IV) ion
a. have the same charge.
b. are polyatomic ions.
c. have charges of 2+ and 4+ respectively.
d. have charges of 1+ and 3+ respectively.
10. What is the metallic ion in the compound copper(II) chloride?
a. Co2+
c. Cu2+
–
b. Cl2
d. Cl–
11. The chemical formula for an ionic compound represents the
a.
b.
c.
d.
number of atoms in each molecule.
number of ions in each molecule.
simplest ratio of ions that results in an electrically neutral compound.
total number of ions in the crystal lattice.
12. A formula that shows the types and numbers of ions combined in a single compound is called a(n)
a. molecular formula.
c. Lewis structure.
b. ionic formula.
d. covalent formula.
13. What is the formula for the compound formed by zinc ions, Zn2+, and fluoride ions, F–?
a. ZnF
c. Zn2F
b. ZnF2
d. Zn2F3
14. What is the formula for the compound formed by calcium ions, Ca2+, and chloride ions, Cl–?
a. CaCl
c. CaCl3
b. Ca2Cl
d. CaCl2
15. Binary compounds
a. are not ionic compounds.
b. are named with the cation first.
c. are named with the anion first.
d. generally have a charge of 2+.
16. An ionic compound is not represented by a molecular formula because an ionic compound
a. does not contain bonds.
c. lacks molecules.
b. does not have charged particles.
d. always has a positive charge.
17. Which of the following is NOT a property of an ionic compound?
a. low boiling point
b. brittleness
c. hardness
d. molten compound conducts electricity
18. Because the particles in ionic compounds are more strongly attracted than in molecular compounds, the
melting points of ionic compounds are
a. equal for all ionic compounds.
b. lower than melting points of molecular compounds.
c. higher than melting points of molecular compounds.
d. approximately equal to room temperature.
19. The symbol HCO3– represents a
a. monatomic ion.
b. stable compound.
c. polyatomic ion.
d. salt.
20. Sodium bicarbonate, NaHCO3,
a. contains four different ions.
b. contains a polyatomic cation.
c. is not a salt.
d. contains a monatomic cation and a polyatomic anion.
21. 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
22. What is the formula for the compound formed by aluminum(III) and the sulfate ion, SO42–?
a. AlSO4
c. Al2(SO4)3
b. Al2SO4
d. Al(SO4)3
23. What is the formula for the compound formed by tin(IV) and the chromate ion, CrO42–?
a. Sn(CrO4)4
c. Sn2(CrO4)4
b. Sn2(CrO4)2
d. Sn(CrO4)2
24. What is the formula for the compound formed by the barium ion, Ba2+, and the hydroxide ion, OH–?
a. BaOH
c. Ba(OH)2
b. BaOH2
d. Ba(OH)
25. Name the compound Ni(ClO3)2.
a. nickel chlorate
b. nickel chloride
c. nickel chlorite
d. nickel peroxide
26. Name the compound Zn3(PO4)2.
a. zinc potassium oxide
b. trizinc polyoxide
c. zinc phosphate
d. zinc phosphite
27. Name the compound KClO3.
a. potassium chloride
b. potassium trioxychlorite
c. potassium chlorate
d. hypochlorite
28. Name the compound Fe(NO2)2.
a. iron(II) nitrate
b. iron(II) nitrite
c. ferric nitrate
d. ferrous nitride
29. Name the compound CuCO3.
a. copper(I) carbonate
b. cupric trioxycarbide
c. cuprous carbide
d. copper(II) carbonate
30. What is the name of Sn3(PO4)4?
a. stannous phosphate
b. tin(IV) phosphate
c. tin(III) phosphate
d. tin(II) phosphate
31. The oxidation number of fluorine is
a. always 0.
b. –1 in all compounds.
c. +1 in all compounds.
d. equal to the positive charge of all the metal ions in a compound.
32. What is the oxidation number of oxygen in most compounds?
a. –8
c. 0
b. –2
d. +1
33. In a compound, the algebraic sum of the oxidation numbers of all atoms equals
a. 0.
c. 8.
b. 1.
d. the charge on the compound.
34. The formula Na2CO3  10H2O shows that
a. Na2CO3 cannot trap water.
b. there are 10 units of water present for every unit of Na2CO3.
c. there are 10 units of Na2CO3 present for every unit of water.
d. the compound cannot exist.
35. A covalent bond results from the mutual attraction of the nuclei of atoms and
a. electrons.
c. neutrons.
b. protons.
d. dipoles.
36. A neutral group of atoms held together by covalent bonds is a
a. molecular formula.
c. compound.
b. chemical formula.
d. molecule.
37. A molecule is a
a. negatively charged group of atoms held together by covalent bonds.
b. positively charged group of atoms held together by covalent bonds.
c. neutral group of atoms held together by covalent bonds.
d. neutral group of atoms held together by ionic bonds.
38. All of the following are true statements about a molecule EXCEPT
a. it is capable of existing on its own.
b. it may consist of two or more atoms of the same type.
c. it must be part of a molecular compound.
d. it may consist of two or more atoms of different types.
39. A(n) ____ shows the types and numbers of atoms joined in a single molecule of a molecular compound.
a. molecular formula
c. covalent bond
b. chemical formula
d. ionic bond
40. Which of the following is NOT an example of a molecular formula?
a. H2O
c. NH3
b. B
d. O2
41. Atoms are ____ when they are combined.
a. more stable
b. less stable
c. not bound together
d. at a high potential energy
42. Atoms naturally move
a. toward high potential energy.
b. toward low potential energy.
c. toward less stability.
d. away from each other.
43. The chemical bond formed when two atoms share electrons is called a(n)
a. ionic bond.
c. Lewis structure.
b. orbital bond.
d. covalent bond.
44. If two covalently bonded atoms are identical, the bond is
a. nonpolar covalent.
c. nonionic.
b. polar covalent.
d. coordinate covalent.
45. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called
a. nonpolar.
c. ionic.
b. polar.
d. dipolar.
46. A chemical bond resulting from the attraction between positive and negative ions is called a(n)
a. covalent bond.
c. charged bond.
b. ionic bond.
d. dipole bond.
47. Most chemical bonds are
a. purely ionic.
b. purely covalent.
c. partly ionic and partly covalent.
d. metallic.
48. The Mg—F bond in MgF2 (electronegativity for Mg is 1.3; electronegativity for F is 4.0) is
a. polar covalent.
c. nonpolar covalent.
b. ionic.
d. pure covalent.
49. The C—F bond (electronegativity for C is 2.5; electronegativity for F is 4.0) in CF4 is
a. polar covalent.
b. ionic.
c. nonpolar covalent.
d. pure covalent.
50. The type of bond in Br2 (electronegativity for Br is 2.8) is
a. nonpolar covalent.
c. pure covalent.
b. polar covalent.
d. pure ionic.
51. The type of bond in LiCl (electronegativity for Li is 1.0; electronegativity for Cl is 3.2) is
a. pure ionic.
c. nonpolar covalent.
b. polar covalent.
d. ionic.
52. In which of these compounds is the bond between the atoms NOT a nonpolar covalent bond?
a. Cl2
c. HCl
b. H2
d. O2
53. To draw a Lewis structure, it is NOT necessary to know
a. bond energies.
b. the types of atoms in the molecule.
c. the number of valence electrons for each atom.
d. the number of atoms in the molecule.
54. In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by
a. 2 electrons.
c. 8 electrons.
b. 4 electrons.
d. 10 electrons.
55. If, after drawing a Lewis structure, too many valence electrons have been used, the molecule probably
contains
a. too many atoms.
b. one or more multiple covalent bonds.
c. too many unshared pairs of electrons.
d. an ionic bond.
56. Multiple covalent bonds may occur in atoms that contain carbon, nitrogen, or
a. chlorine.
c. oxygen.
b. hydrogen.
d. helium.
57. The substance whose Lewis structure shows three covalent bonds is
a. H2O.
c. NH3.
b. CH2Cl2.
d. CCl4.
58. How many double bonds are in the Lewis structure for hydrogen fluoride, HF?
a. none
c. two
b. one
d. three
59. The chemical formula for water, a covalent compound, is H2O. This formula is an example of a(n)
a. formula unit.
c. ionic formula.
b. Lewis structure.
d. molecular formula.
60. Which formula does NOT represent a molecule?
a. H2O (water)
c. CO2 (carbon dioxide)
b. NH3 (ammonia)
d. NaCl (table salt)
61. Name the compound CF4.
a. calcium fluoride
b. carbon fluoride
c. carbon tetrafluoride
d. monocarbon quadrafluoride
62. Name the compound SiO2.
a. silver oxide
b. silicon oxide
c. silicon dioxide
d. monosilicon dioxide
63. Name the compound N2O4.
a. sodium tetroxide
b. dinitrogen tetroxide
c. nitrous oxide
d. binitrogen oxide
64. Name the compound SO3.
a. sulfur trioxide
b. silver trioxide
c. selenium trioxide
d. sodium trioxide
65. Name the compound N2O5.
a. dinickel pentoxide
b. dinitrogen pentoxide
c. neon oxide
d. nitric oxide
66. Name the compound N2O3.
a. dinitrogen oxide
b. nitrogen trioxide
c. nitric oxide
d. dinitrogen trioxide
67. Name the compound PBr5.
a. potassium hexabromide
b. phosphorus(V) bromide
c. phosphorus pentabromide
d. phosphoric acid
68. According to VSEPR theory, the shape of the ammonia molecule, NH3, is
a. linear.
c. trigonal pyramidal.
b. bent.
d. tetrahedral.
69. Use VSEPR theory to predict the shape of the hydrogen chloride molecule, HCl.
a. tetrahedral
c. bent
b. linear
d. trigonal planar
70. Use VSEPR theory to predict the shape of the water molecule, H2O.
a. tetrahedral
c. bent
b. linear
d. octahedral
71. Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.
a. tetrahedral
c. bent
b. linear
d. trigonal planar
72. The following molecules contain polar bonds. The only polar molecule is
a. CCl4.
c. NH3.
b. CO2.
d. CH4.
73. The following molecules contain polar bonds. The only nonpolar molecule is
a. HCl.
c. CO2.
b. H2O.
d. NH3.
74. A polar molecule contains
a. ions.
b. a region of positive charge and a region of negative charge.
c. only London forces.
d. no bonds.
75.A molecule of hydrogen chloride is polar because
a. it is composed of ions.
b. it is magnetic.
c. it contains metallic bonds.
d. the chlorine attracts the shared electrons more strongly than does the hydrogen.
Bonding Test
Answer Section
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