1) There are ______paired and ______unpaired electrons in the Lewis symbol for a phosphorus atom.
A) 4, 2
B) 2, 4
C) 2, 3
D) 4, 3
E) 0, 3
Answer: C
Diff: 1
Page Ref: Sec. 8.1
3) Based on the octet rule, magnesium most likely forms a ______ion.
A)
B)
C)
D)
E)
Answer: A
Diff: 1
Page Ref: Sec. 8.1
10) The halogens, alkali metals, and alkaline earth metals have ______valence electrons, respectively.
A) 7, 4, and 6
B) 1, 5, and 7
C) 8, 2, and 3
D) 7, 1, and 2
E) 2, 7, and 4
Answer: D
Diff: 2
Page Ref: Sec. 8.1
14) For a given arrangement of ions, the lattice energy increases as ionic radius ______and as ionic charge ______.
A) decreases, increases
B) increases, decreases
C) increases, increases
D) decreases, decreases
E) This cannot be predicted.
Answer: A
Diff: 1
Page Ref: Sec. 8.2
24) A ______covalent bond between the same two atoms is the longest.
A) single
B) double
C) triple
D) They are all the same length.
E) strong
Answer: A
Diff: 1
Page Ref: Sec. 8.3
23) How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell?
A) 3
B) 4
C) 1
D) 2
E) 0
Answer: B
Diff: 1
Page Ref: Sec. 8.3
26) A double bond consists of ______pairs of electrons shared between two atoms.
A) 1
B) 2
C) 3
D) 4
E) 6
Answer: B
Diff: 2
Page Ref: Sec. 8.3
27) What is the maximum number of double bonds that a hydrogen atom can form?
A) 0
B) 1
C) 2
D) 3
E) 4
Answer: A
Diff: 1
Page Ref: Sec. 8.3
29) In the molecule below, which atom has the largest partial negative charge ______?
A) Cl
B) F
C) Br
D) I
E) C
Answer: B
Diff: 1
Page Ref: Sec. 8.4
30) The ability of an atom in a molecule to attract electrons is best quantified by the ______.
A) paramagnetism
B) diamagnetism
C) electronegativity
D) electron change-to-mass ratio
E) first ionization potential
Answer: C
Diff: 1
Page Ref: Sec. 8.4
31) Given the electronegativities below, which covalent single bond is most polar?
Element: H C N O
Electronegativity:2.1 2.5 3.0 3.5
A) C-H
B) N-H
C) O-H
D) O-C
E) O-N
Answer: C
Diff: 1
Page Ref: Sec. 8.4
32) Electronegativity ______from left to right within a period and ______from top to bottom within a group.
A) decreases, increases
B) increases, increases
C) increases, decreases
D) stays the same, increases
E) increases, stays the same
Answer: C
Diff: 1
Page Ref: Sec. 8.4
38) The Lewis structure of HCN (H bonded to C) shows that ______has ______nonbonding electron pairs.
A) C, 1
B) N, 1
C) H, 1
D) N, 2
E) C, 2
Answer: B
Diff: 2
Page Ref: Sec. 8.5
39) The formal charge on carbon in the molecule below is ______.
A) 0
B) +1
C) +2
D) +3
E) -1
Answer: A
Diff: 1
Page Ref: Sec. 8.5
43) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ______.
A) 0
B) +1
C) -1
D) +2
E) -2
Answer: B
Diff: 1
Page Ref: Sec. 8.6
44) How many equivalent resonance forms can be drawn for - (carbon is the central atom)?
A) 1
B) 2
C) 3
D) 4
E) 0
Answer: C
Diff: 1
Page Ref: Sec. 8.6
47) How many different types of resonance structures can be drawn for the ion where all atoms satisfy the octet rule?
A) 1
B) 2
C) 3
D) 4
E) 5
Answer: A
Diff: 2
Page Ref: Sec. 8.6
48) Using the table of average bond energies below, the for the reaction is ______kJ.
Bond: C≡CC-CH-IC-IC-H
D (kJ/mol): 839348299 240413
A) +160
B) -160
C) -217
D) -63
E) +63
Answer: C
Diff: 1
Page Ref: Sec. 8.8
51) Using the table of bond dissociation energies, the for the following gas-phase reaction is ______kJ.
A) -44
B) 38
C) 304
D) 2134
E) -38
Answer: A
Diff: 1
Page Ref: Sec. 8.8
4) Which of the following does not have eight valence electrons?
A)
B)
C) Xe
D)
E) All of the above have eight valence electrons.
Answer: A
Diff: 3
Page Ref: Sec. 8.1
7) In ionic bond formation, the lattice energy of ions ______as the magnitude of the ion charges ______and the radii ______.
A) increases, decrease, increase
B) increases, increase, increase
C) decreases, increase, increase
D) increases, increase, decrease
E) increases, decrease, decrease
Answer: D
Diff: 3
Page Ref: Sec. 8.2
5) The chloride of which of the following metals should have the greatest lattice energy?
A) potassium
B) rubidium
C) sodium
D) lithium
E) cesium
Answer: D
Diff: 2
Page Ref: Sec. 8.2
10) The electron configuration [Kr]4d10 represents ______.
A) Sr+2
B) Sn+2
C) Te+2
D) Ag+1
E) Rb+1
Answer: D
Diff: 3
Page Ref: Sec. 8.2
13) The type of compound that is most likely to contain a covalent bond is ______.
A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table
B) a solid metal
C) one that is composed of only nonmetals
D) held together by the electrostatic forces between oppositely charged ions
E) There is no general rule to predict covalency in bonds.
Answer: C
Diff: 1
Page Ref: Sec. 8.3
14) In which of the molecules below is the carbon-carbon distance the shortest?
A)
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 8.3
15) Of the atoms below, ______is the most electronegative.
A) Br
B) O
C) Cl
D) N
E) F
Answer: E
Diff: 1
Page Ref: Sec. 8.4
21) Which of the following has the bonds correctly arranged in order of increasing polarity?
A)
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 8.4
23) The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e) of the negative charge on I in HI?
(; ;)
A)
B) 0.057
C) 9.1
D) 1
E) 0.22
Answer: B
Diff: 5
Page Ref: Sec. 8.4
26) The Lewis structure of shows ______.
A) a nitrogen-nitrogen triple bond
B) a nitrogen-nitrogen single bond
C) each nitrogen has one nonbonding electron pair
D) each nitrogen has two nonbonding electron pairs
E) each hydrogen has one nonbonding electron pair
Answer: C
Diff: 2
Page Ref: Sec. 8.5
29) The Lewis structure of the ion is ______.
A)
B)
C)
D)
E)
Answer: A
Diff: 2
Page Ref: Sec. 8.5
31) Resonance structures differ by ______.
A) number and placement of electrons
B) number of electrons only
C) placement of atoms only
D) number of atoms only
E) placement of electrons only
Answer: E
Diff: 1
Page Ref: Sec. 8.6
33) To convert from one resonance structure to another, ______.
A) only atoms can be moved
B) electrons and atoms can both be moved
C) only electrons can be moved
D) neither electrons nor atoms can be moved
E) electrons must be added
Answer: C
Diff: 1
Page Ref: Sec. 8.6
For the questions that follow, consider the BEST Lewis structures of the following oxyanions:
(i)(ii)(iii)(iv)(v)
35) There can be four equivalent best resonance structures of ______.
A) (ii)
B) (iii)
C) (i)
D) (iv)
E) (v)
Answer: D
Diff: 2
Page Ref: Sec. 8.5-8.7
45) A valid Lewis structure of ______cannot be drawn without violating the octet rule.
A)
B)
C)
D)
E)
Answer: C
Diff: 1
Page Ref: Sec. 8.7
1) Using the VSEPR model, the electron-domain geometry of the central atom in is ______.
A) linear
B) trigonal planar
C) tetrahedral
D) trigonal bipyramidal
E) octahedral
Answer: B
Diff: 1
Page Ref: Sec. 9.2
8) Using the VSEPR model, the molecular geometry of the central atom in is ______.
A) linear
B) trigonal planar
C) tetrahedral
D) bent
E) trigonal pyramidal
Answer: D
Diff: 1
Page Ref: Sec. 9.2
1) What is the molecular geometry of a molecule that has three bonding and two non-bonding domains?
Answer: T-shaped
Diff: 4
Page Ref: Sec. 9.2
2) In the valence shell of an atom there are six electron domains. They will be arranged in a (an) ______geometry.
Answer: octahedral
Diff: 5
Page Ref: Sec. 9.2
3) What are the three bond angles in the trigonal bipyramidal structure?
Answer: 90 °, 120 °, 180 °
Diff: 4
Page Ref: Sec. 9.2
4) Three molecules have similar electron domains, but different molecular shapes. Why?
Answer: different numbers of non-bonding domains
Diff: 4
Page Ref: Sec. 9.2
5) The 1s hydrogen orbital overlaps with the ______iodine orbital in HI.
Answer: 5p
Diff: 2
Page Ref: Sec 9.5
6) A covalent bond in which overlap regions lie above and below an internuclear axis is called a(n) ______.
Answer: π bond
Diff: 2
Page Ref: Sec 9.6
Multiple choice
1) The basis of the VSEPR model of molecular bonding is ______.
A) regions of electron density on an atom will organize themselves so as to maximize s-character
B) regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap
C) atomic orbitals of the bonding atoms must overlap for a bond to form
D) electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions
E) hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry
Answer: D
Diff: 1
Page Ref: Sec. 9.2
4) The electron domain and molecular geometry of is ______.
A) tetrahedral, trigonal planar
B) trigonal planar, trigonal planar
C) trigonal pyramidal, linear
D) tetrahedral, bent
E) trigonal pyramidal, seesaw
Answer: D
Diff: 4
Page Ref: Sec. 9.2
7) The bond angle in the ion is approximately ______.
A) 90 °
B) 109.5 °
C) 120 °
D) 180 °
E) 60 °
Answer: C
Diff: 2
Page Ref: Sec. 9.2
9) The molecular geometry of the ion is ______.
A) trigonal pyramidal
B) trigonal planar
C) bent
D) tetrahedral
E) T-shaped
Answer: A
Diff: 2
Page Ref: Sec. 9.2
10) The molecular geometry of the left-most carbon atom in the molecule below is ______.
A) trigonal planar
B) trigonal bipyramidal
C) tetrahedral
D) octahedral
E) T-shaped
Answer: C
Diff: 1
Page Ref: Sec. 9.2
12) The bond angles marked a, b, and c in the molecule below are about ______, ______, and ______, respectively.
A) 90 °, 90 °, 90 °
B) 120 °, 120 °, 90 °
C) 120 °, 120 °, 109.5 °
D) 109.5 °, 120 °, 109.5 °
E) 109.5 °, 90 °, 120 °
Answer: D
Diff: 2
Page Ref: Sec. 9.2
15) The central iodine atom in the ion has ______nonbonded electron pairs and ______bonded electron pairs in its valence shell.
A) 2, 2
B) 3, 4
C) 1, 3
D) 3, 2
E) 2, 4
Answer: E
Diff: 1
Page Ref: Sec. 9.2
16) The central iodine atom in has ______unbonded electron pairs and ______bonded electron pairs in its valence shell.
A) 1, 5
B) 0, 5
C) 5, 1
D) 4, 1
E) 1, 4
Answer: A
Diff: 1
Page Ref: Sec. 9.2
18) An electron domain consists of ______.
a) a nonbonding pair of electrons
b) a single bond
c) a multiple bond
A) a only
B) b only
C) c only
D) a, b, and c
E) b and c
Answer: D
Diff: 1
Page Ref: Sec. 9.2
27) For molecules of the general formula n can be greater than four ______.
A) for any element A
B) only when A is an element from the third period or below the third period
C) only when A is boron or beryllium
D) only when A is carbon
E) only when A is Xe
Answer: B
Diff: 2
Page Ref: Sec. 9.2
29) Of the molecules below, only ______is polar.
A)
B)
C)
D)
E)
Answer: B
Diff: 2
Page Ref: Sec. 9.3
34) The molecular geometry of the molecule is ______, and this molecule is ______.
A) linear, nonpolar
B) linear, polar
C) bent, nonpolar
D) bent, polar
E) trigonal planar, polar
Answer: A
Diff: 1
Page Ref: Sec. 9.3
41) According to valence bond theory, which orbitals overlap in the formation of the bond in
A) 1s on H and 4p on Br
B) 1s on H and 4s on Br
C) 1s on H and 3p on Br
D) 2s on H and 4p on Br
E) 2s on H and 3p on Br
Answer: A
Diff: 1
Page Ref: Sec. 9.4
44) The electron-domain geometry of a carbon-centered compound is tetrahedral. The hybridization of the central carbon atom is ______.
A) sp
B)
C)
D)
E)
Answer: C
Diff: 2
Page Ref: Sec. 9.5
45) Of the following, only ______has hybridization of the central atom.
A)
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 9.5
46) Of the following, the central atom is hybridized only in ______.
A)
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 9.5
50) The hybridizations of iodine in and are ______and ______, respectively.
A) ,
B) ,
C) ,
D) ,
E) ,
Answer: B
Diff: 1
Page Ref: Sec. 9.5
51) The hybridizations of bromine in and of arsenic in are ______and ______, respectively.
A) ,
B) ,
C) ,
D) ,
E) ,
Answer: D
Diff: 1
Page Ref: Sec. 9.5
52) The hybrid orbitals used for bonding by the sulfur atom in the molecule are ______orbitals.
A) sp
B)
C)
D)
E)
Answer: D
Diff: 1
Page Ref: Sec. 9.5
61) When three atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed?
A) one
B) six
C) three
D) four
E) five
Answer: C
Diff: 1
Page Ref: Sec. 9.5
62) The blending of one s atomic orbital and two p atomic orbitals produces ______.
A) three sp hybrid orbitals
B) two hybrid orbitals
C) three hybrid orbitals
D) two hybrid orbitals
E) three hybrid orbitals
Answer: E
Diff: 1
Page Ref: Sec. 9.5
68) There are ______σ bonds and ______π bonds in .
A) 14, 2
B) 10, 3
C) 12, 2
D) 13, 2
E) 16, 3
Answer: E
Diff: 4
Page Ref: Sec. 9.6
69) Which of the following molecules or ions will exhibit delocalized bonding?
A) , , and
B) only
C) and
D) and
E) None of the above will exhibit delocalized bonding.
Answer: C
Diff: 1
Page Ref: Sec. 9.6
73) The carbon-carbon σ bond in ethylene, , results from the overlap of ______.
A) sp hybrid orbitals
B) hybrid orbitals
C) hybrid orbitals
D) s atomic orbitals
E) p atomic orbitals
Answer: C
Diff: 1
Page Ref: Sec. 9.6
74) The π bond in ethylene, , results from the overlap of ______.
A)hybrid orbitals
B) s atomic orbitals
C) sp hybrid orbitals
D)hybrid orbitals
E) p atomic orbitals
Answer: E
Diff: 1
Page Ref: Sec. 9.6
78) The hybridization of nitrogen in the molecule is ______.
A) sp
B)
C)
D)
E)
Answer: A
Diff: 1
Page Ref: Sec. 9.6
80) The hybridization of the oxygen atom labeled x in the structure below is ______.
A) sp
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 9.6
81) The Lewis structure of carbon dioxide is given below. The hybridization of the carbon atom in carbon dioxide is ______.
A)
B)
C) sp
D)
E)
Answer: C
Diff: 2
Page Ref: Sec. 9.6
82) Electrons in ______bonds remain localized between two atoms. Electrons in ______bonds can become delocalized between more than two atoms.
A) pi, sigma
B) sigma, pi
C) pi, pi
D) sigma, sigma
E) ionic, sigma
Answer: B
Diff: 2
Page Ref: Sec. 9.6
86) In molecular orbital theory, the orbital is ______and the orbital is ______in the molecule.
A) filled, filled
B) filled, empty
C) filled, half-filled
D) half-filled, filled
E) empty, filled
Answer: B
Diff: 4
Page Ref: Sec. 9.7
88) Based on molecular orbital theory, the bond order of the bond in the ion is ______.
A) 0
B) 1/2
C) 1
D) 3/2
E) 2
Answer: B
Diff: 4
Page Ref: Sec. 9.7
89) An antibonding π orbital contains a maximum of ______electrons.
A) 1
B) 2
C) 4
D) 6
E) 8
Answer: B
Diff: 3
Page Ref: Sec. 9.7
94) Based on molecular orbital theory, the only molecule in the list below that has unpaired electrons is ______.
A)
B)
C)
D)
E)
Answer: D
Diff: 3
99) Based on molecular orbital theory, the bond order of the bond in the molecule is ______.
A) 0
B) 1
C) 2
D) 3
E) 4
Answer: C
Diff: 4
Page Ref: Sec. 9.8
102) According to MO theory, overlap of two p atomic orbitals produces ______.
A) two bonding molecular orbitals
B) one bonding molecular orbital and one antibonding molecular orbital
C) two bonding molecular orbitals and two antibonding molecular orbitals
D) two bonding molecular orbitals and one antibonding molecular orbital
E) three bonding molecular orbitals and three antibonding molecular orbitals
Answer: B
Diff: 3
Page Ref: Sec. 9.8
103) According to MO theory, overlap of two p atomic orbitals produces ______.
A) one π MO and one MO
B) one π MO and one σ MO
C) one π MO and one MO or one σ MO and one MO
D) one MO and one MO
E) two π MOs, two MOs, one σ MO, and one MO
Answer: C
Diff: 3
Page Ref: Sec. 9.8
106) The bond order of a homonuclear diatomic molecule can be decreased by ______.
A) removing electrons from a bonding MO or adding electrons to an antibonding MO
B) adding electrons to a bonding MO or removing electrons from an antibonding MO
C) adding electrons to any MO
D) removing electrons from any MO
E) The bond order of a homonuclear diatomic molecule cannot be decreased by any means.
Answer: A
Diff: 4
Page Ref: Sec. 9.8
107) The order of MO energies in, , and, is different from the order in, , and This is due to ______.
A) less effective overlap of p orbitals in, F2, and
B) the more metallic character of boron, carbon and nitrogen as compared to oxygen, fluorine, and neon
C) greater 2s-2p interaction in, , and
D) greater 2s-2p interaction in , and
E) less effective overlap of p orbitals in, , and
Answer: D
Diff: 5
Page Ref: Sec. 9.8