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Test Bank General Chemistry, 10th edition 1
Chapter 9 - Ionic and Covalent Bonding
1. In which pair do both compounds exhibit predominantly ionic bonding?
A)
RbCl and CaO
B)
PCl5 and HF
C)
KI and O3
D)
Na2SO3 and BH3
E)
NaF and H2O
2. The following representation of an atom is called
A)
a Lewis dot structure.
B)
an ion.
C)
a structural formula.
D)
an electrostatic potential map.
E)
an ionic bond.
3. Which of the following concerning Coulomb’s law is/are correct?
1.
The energy of an ionic bond is proportional to the size of the ion charges.
2.
The energy of an ionic bond is inversely proportional to the distance between
the charges.
3.
The size of an ion is not important in determining the energy of an ionic bond.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
4. When the cations Na+, K+, Rb+, Cs+ are combined with chloride ion in the gas phase to form
ion pairs, which pair formation releases the greatest amount of energy?
A)
KCl
B)
All release the same amount of energy.
C)
RbCl
D)
NaCl
E)
CsCl
5. Which one of the following has an enthalpy change that is equal to the lattice energy of
?
A)
B)
C)
D)
E)
6. Which of the following statements concerning lattice energy is false?
A)
MgO has a larger lattice energy than NaF.
B)
The lattice energy for a solid with 2+ and 2– ions should be two times that for a
solid with 1+ and 1– ions.
C)
MgO has a larger lattice energy than LiF.
D)
Lattice energy is often defined as the change in energy that occurs when an ionic
solid is separated into isolated ions in the gas phase.
E)
All of these are true.
7. Which of the following is a correct description of lattice energy?
A)
The energy change that occurs when electrons are removed from a lattice.
B)
The energy change that occurs when a gas condenses to a liquid.
C)
The energy change that occurs when a liquid freezes.
D)
The energy change that occurs when an ionic solid is separated into its ions in the
gas phase.
E)
The lattice energy of a substance is identical to the ionic bond energy determined
from coulombs law.
Test Bank General Chemistry, 10th edition 3
8. In the Born–Haber cycle for , which of the following processes corresponds to the
first ionization energy of Na?
A)
B)
C)
D)
E)
9. In the Born–Haber cycle for , which of the following processes corresponds to the
enthalpy of formation of ?
A)
B)
C)
D)
E)
10. In the Born–Haber cycle for , which of the following processes corresponds to the
electron affinity of F?
A)
B)
C)
D)
E)
11. Which of the following processes is not exothermic?
A)
B)
C)
D)
E)
12. Calculate the lattice energy for LiF(s) given the following:
sublimation energy for Li(s)
+166 kJ/mol
Hf for F(g)
+77 kJ/mol
first ionization energy of Li(g)
+520. kJ/mol
electron affinity of F(g)
–328 kJ/mol
enthalpy of formation of LiF(s)
–617 kJ/mol
A)
1052 kJ/mol
B)
285 kJ/mol
C)
–650. kJ/mol
D)
800. kJ/mol
E)
none of these
13. Which of the following compounds has the most ionic bonding (has the highest percentage
of ionic character)?
A)
CaF2
B)
LiI
C)
OF2
D)
CsF
E)
LiF
14. Which of the following compounds would be expected to have the lowest melting point?
A)
AlF3
B)
RbF
C)
NaF
D)
MgF2
E)
CaF2
Test Bank General Chemistry, 10th edition 5
15. Which of the following compounds would be expected to have the highest melting point?
A)
CsF
B)
LiCl
C)
LiF
D)
NaBr
E)
CsI
16. Which of the following compounds would be expected to have the highest melting point?
A)
NCl3
B)
OCl2
C)
MgCl2
D)
LiCl
E)
CCl4
17. Atoms of an element X have the ground-state electron configuration 1s22s22p63s23p4. What
type of ion is X most likely to form?
A)
X6+
B)
X3–
C)
X4+
D)
X–
E)
X2–
18. Which of the following is the Lewis dot structure for the rubidium ion?
A)
B)
C)
Test Bank General Chemistry, 10th edition 6
D)
E)
19. Which of the following is the Lewis dot structure for the bromide ion?
A)
B)
C)
D)
E)
20. Which of the following is the Lewis dot structure for one formula unit of magnesium
sulfide?
A)
B)
C)
D)
E)
21. All of the following species have ground-state noble-gas electron configurations except
A)
Ge4+
B)
K+
C)
Kr
D)
I–
E)
P3–
22. Which of the following concerning the formation of ions is/are correct?
1.
Elements with large electron affinities tend to form monoatomic anions.
2.
No ionic compounds are found with positive ions having charges greater than
the element group number.
3.
Group 1A and 2A metals always have a positive charge equal to their group
number in their ionic compounds.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
23. Which of the following concerning the formation of ions is/are correct?
1.
Compounds of +4 ions are rare because of the large amount of energy
required to form a +4 ion.
2.
Some main group metals may have more than one possible positive charge
because of the different energies required to remove s versus p valence
electrons.
3.
The nonmetals closest to the noble gases (Group 6A and 7A) tend to form
monatomic anions with noble gas configurations.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
24. All of the following have ground-state noble-gas electron configurations except
A)
Ar
B)
N3–
C)
P3+
D)
Mg2+
E)
Cl–
25. The formation of which monatomic ion of sulfur is the most energetically favorable?
A)
B)
C)
D)
E)
Test Bank General Chemistry, 10th edition 9
26. What is the ground-state electron configuration of the ion?
A)
B)
C)
D)
E)
27. What is the ground-state electron configuration of the sulfide ion?
A)
B)
C)
D)
E)
28. What is the electron configuration for ?
A)
B)
C)
D)
E)
29. The Cr2+ ion would be expected to have ____ unpaired electrons.
A)
4
B)
2
C)
3
D)
0
E)
1
30. What is the electron configuration of ?
A)
B)
C)
D)
E)
31. What is the ground-state electron configuration of ?
A)
B)
C)
D)
E)
32. What is the ground-state electron configuration of ?
A)
B)
C)
D)
E)
33. What is the ground-state electron configuration of the copper(I) ion, ?
A)
B)
C)
D)
E)
34. What is the ground-state electron configuration of ?
A)
B)
C)
D)
E)
35. All of the following ions have the ground-state electron configuration of a noble gas except
which one?
A)
Ca2+
B)
Cl–
C)
Ga3+
D)
Al3+
E)
H–
36. Which set of ions are isoelectronic in their ground-state electron configurations?
A)
N, O, F, Ne
B)
Na+, K+, Rb+, Cs+
C)
F–, Cl–, Br–, I–
D)
Mg2+, Ca2+, Sr2+, Ba2+
E)
N3–, O2–, Mg2+, Al3+
Test Bank General Chemistry, 10th edition 12
37. Which of the following species is isoelectronic with Kr?
A)
B)
C)
D)
E)
Ar
38. All of the following species are isoelectronic except
A)
Ar.
B)
Ca2+.
C)
Mg2+.
D)
Cl–.
E)
S2–.
39. Which pair of species is isoelectronic?
A)
Na+ and K+
B)
K+ and Cl–
C)
Be2+ and Na+
D)
Ne and Ar
E)
Li+ and Ne
40. Which two species are isoelectronic?
A)
Na+ and K+
B)
Al3+ and Ne
C)
P– and Ca+
D)
Cl– and F–
E)
Ca2+ and Mg2+
41. All of the following species are isoelectronic except
A)
S2–
B)
K+
C)
Na+
D)
Ar
E)
Cl–
Test Bank General Chemistry, 10th edition 13
42. All of the following species are isoelectronic except
A)
O–
B)
Ne
C)
N3–
D)
Mg2+
E)
F–
43. The following species, , , and , all have the same number of
A)
electrons.
B)
nucleons.
C)
neutrons.
D)
protons.
E)
isotopes.
44. Rank the following ions in order of decreasing atomic radii: Mo4+, Mo5+, Mo6+.
A)
Mo4+ > Mo5+ > Mo6+
B)
Mo6+ > Mo5+ > Mo4+
C)
Mo5+ > Mo4+ > Mo6+
D)
Mo6+ > Mo4+ > Mo5+
E)
Mo4+ > Mo6+ > Mo5+
45. Rank the following ions in order of decreasing atomic radii: Te2−, Te4+, Te6+.
A)
Te2− > Te4+ > Te6+
B)
Te6+ > Te4+ > Te2−
C)
Te4+ > Te2− > Te6+
D)
Te2− > Te6+ > Te4+
E)
Te4+ > Te6+ > Te2−
Test Bank General Chemistry, 10th edition 14
46. Which of the following species would you expect to have the largest radius?
A)
B)
F
C)
D)
E)
47. In which of the following lists do the ions not appear in order of increasing ionic radius?
A)
S2– < Cl– < K+
B)
Na+ < F– < O2–
C)
Cl– < Br– < I–
D)
Li+ < Na+ < K+
E)
Al3+ < Mg2+ < Na+
48. Rank the following ions in order of decreasing ionic radius: S2–, O2–, F–, Na+, Mg2+.
A)
S2–, O2–, F–, Na+, Mg2+
B)
O2–, F–, Na+, Mg2+, S2–
C)
O2–, S2–, F–, Na+, Mg2+
D)
Mg2+, Na+, F–, O2–, S2–
E)
Mg2+, S2–, Na+, F–, O2–
49. Rank the following species in order of decreasing radii: K+, Cl-, Se2-, Br-.
A)
Br- > Se2- > Cl- > K+
B)
Se2- > Br- > Cl- > K+
C)
K+> Cl- > Se2- > Br-
D)
Br- > Cl- > Se2- > K+
E)
Cl- > Se2- > K+ > Br-
50. For which of the following pairs of species is the difference in radius the greatest?
A)
C and F
B)
K+ and Br–
C)
Li+ and I–
D)
Na and Mg
E)
O2– and F–
51. Which of the following is the best explanation for a covalent bond?
A)
electrons simultaneously attracted by more than one nucleus
B)
an interaction between outer electrons
C)
the overlapping of unoccupied orbitals of two or more atoms
D)
the overlapping of two electron-filled orbitals having different energies
E)
a positive ion attracting negative ions
52. The formulas of many binary covalent compounds can be predicted on the basis
A)
that a bond is formed by the overlapping of two filled orbitals.
B)
that the number of bonds an atom can have is equal to the number of empty
valence orbitals it has.
C)
that a bond is formed by the overlapping of atomic orbitals.
D)
that the number of bonds an atom can have is equal to the number of half-filled
valence orbitals it can have.
E)
that bonding electrons are simultaneously attracted by more than one nucleus.
53. During the formation of a chemical bond between two hydrogen atoms, which of the
following statements is always true?
A)
Energy is released during the formation of the bond.
B)
A polar covalent bond is formed.
C)
Electrons always are between the nuclei of the atoms.
D)
One of the hydrogen atoms is ionized.
E)
Resonance stabilizes the bond.
Test Bank General Chemistry, 10th edition 16
54. A bond in which both electrons of the bond are donated by one atom is called ____.
A)
a coordinate covalent bond
B)
a polar covalent bond
C)
an ionic bond
D)
a double bond
E)
a triple bond
55. A bond in which an electron pair is unequally shared by two atoms is
A)
polar covalent.
B)
coordinate covalent.
C)
ionic.
D)
nonpolar covalent.
E)
metallic.
56. The measure of the attraction that an atom has for the electrons in a chemical bond is called
A)
electronegativity.
B)
lattice energy.
C)
resonance energy.
D)
ionization energy.
E)
electron affinity.
57. Which of the following atoms is the most electronegative?
A)
B
B)
N
C)
Al
D)
Cs
E)
Na
58. An atom of which of the following elements has the highest electronegativity?
A)
K
B)
As
C)
Ba
D)
Si
E)
Br
59. Which of the following concerning electronegativity is/are correct?
1.
Differences in element electronegativities may be used to predict the type of
bonding, ionic or covalent, in a substance.
2.
The larger the differences in electronegativity between two bonded atoms the
more polar the bond.
3.
The electrons in a polar bond tend to spend more time around the least
electronegative element.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
60. Which pair of elements would form a covalent bond that is the least polar?
A)
S and Li
B)
Al and N
C)
O and H
D)
O and F
E)
S and Cs
61. Rank the following covalent bonds in order of decreasing polarity: C-H, N-H, O-H, F-H.
A)
F-H, O-H, N-H, C-H
B)
O-H, F-H, N-H, C-H
C)
N-H, F-H, O-H, C-H
D)
C-H, N-H, O-H, F-H
E)
C-H, F-H, O-H, N-H
Test Bank General Chemistry, 10th edition 18
62. Which of the following bonds would be the least polar yet still be considered polar
covalent?
A)
Mg-O
B)
C-O
C)
Si-O
D)
O-O
E)
N-O
63. In which of the following species is there the greatest unequal sharing of the bonding
electrons?
A)
SO3
B)
SO32–
C)
H2S
D)
H2O
E)
NH4+
64. The Lewis formula for phosphine, PH3, has
A)
four lone pairs.
B)
four bonding pairs.
C)
two bonding pairs and two lone pairs.
D)
three bonding pairs and one lone pair.
E)
one bonding pair and three lone pairs.
65. Which of the following concerning Lewis electron-dot formulae is/are correct?
1.
A Lewis electron-dot formula (Lewis structure) is identical to a structural
formula.
2.
The skeleton of a molecule need not be known to draw the correct Lewis
electron-dot structure.
3.
Lewis electron-dot formulae show the location of bonding and nonbonding
electrons in three dimensional space.
Test Bank General Chemistry, 10th edition 19
A)
1 only
B)
2 only
C)
3 only
D)
1, 2, and 3
E)
none of the above
66. What is the total number of valence electrons in N2O4?
A)
34
B)
11
C)
16
D)
17
E)
46
67. In the Lewis formula for difluorodiazine, N2F2, the total number of lone electron pairs
around the two nitrogen atoms is
A)
4.
B)
0.
C)
3.
D)
1.
E)
2.
68. Which of the following Lewis formulas is incorrect?
A)
B)
C)
D)
E)
69. Which of the following is a correct Lewis electron-dot formula for H2SO4?
A)
B)
C)
D)
E)
70. Which of the following is a correct Lewis electron-dot formula for CO?
A)
B)
C)
D)
E)
