Ch08_Testbank
8.1 Multiple-Choice and Bimodal Questions
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
2) In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons.
A) 4, 2
B) 4,1
C) 2, 5
D) 6, 1
E) 0, 5
Answer: D
Diff: 1
Page Ref: Sec. 8.1
3) Based on the octet rule, magnesium most likely forms a __________ ion.
A) 2
Mg+
B) 2
Mg-
C) 6
Mg-
D) 6
Mg+
E) _
Mg
Answer: A
Diff: 1
Page Ref: Sec. 8.1
4) Based on the octet rule, phosphorus most likely forms a __________ ion.
A) 3P+
B) 3P-
C) 5P+
D) 5P-
E) +P
Answer: B
Diff: 1
Page Ref: Sec. 8.1
5) Based on the octet rule, iodine most likely forms an __________ ion.
A) 2I+
B) 4I+
C) 4I-
D) I+
E) I-
Answer: E
Diff: 1
Page Ref: Sec. 8.1
6) There are __________ unpaired electrons in the Lewis symbol for an oxygen atom.
A) 0
B) 1
C) 2
D) 4
E) 3
Answer: C
Diff: 1
Page Ref: Sec. 8.1
7) How many unpaired electrons are there in the Lewis structures of a 3N-ion?
A) 0
B) 1
C) 2
D) 3
E) This cannot be predicted.
Answer: A
Diff: 1
Page Ref: Sec. 8.1
8) How many unpaired electrons are there in an 2
O-ion?
A) 0
B) 1
C) 2
D) 3
E) This cannot be predicted.
Answer: A
Diff: 1
Page Ref: Sec. 8.1
9) The electron configuration of the phosphide ion (3P-) is __________.
A) 2
[Ne]3S
B) 21
[Ne]3S3P
C) 23
[Ne]3S3P
D) 2
[Ne]3P
E) 26
[Ne]3S3P
Answer: E
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
11) The only noble gas without eight valence electrons is __________.
A) Ar
B) Ne
C) He
D) Kr
E) All noble gases have eight valence electrons.
Answer: C
Diff: 1
Page Ref: Sec. 8.1
12) Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration?
O Sr Na Se Br
A) O, Se
B) Sr
C) Na
D) Br
E) Sr, O, Se
Answer: B
Diff: 1
Page Ref: Sec. 8.1
13) Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration?
O Sr Na Se Br
A) Br
B) Sr
C) Na
D) O, Se
E) Sr, O, Se
Answer: D
Diff: 1
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
15) The electron configuration of the 2S-ion is __________.
A) 26
[Ar]3S3p
B) 22
[Ar]3S3p
C) 22
[Ne]3S3p
D) 26
[Ne]3S3p
E) 26
[Kr]3S2p-
Answer: D
Diff: 1
Page Ref: Sec. 8.2
16) The principal quantum number of the electrons that are lost when tungsten forms a cation is __________.
A) 6
B) 5
C) 4
D) 3
E) 2
Answer: A
Diff: 1
Page Ref: Sec. 8.2
17) Which one of the following species has the electron configuration4
[Ar]3d?
A) 2
Mn+
B) 2
Cr+
C) 3V+
D) 3
Fe+
E) K+
Answer: B
Diff: 1
Page Ref: Sec. 8.2
18) What is the electron configuration for the 2
Co+ion?
A) 16
[Ar]4S3d
B) 07
[Ar]4S3d
C) 05
[Ar]4S3d
D) 29
[Ar]4S3d
E) 210
[Ne]3S3p
Answer: B
Diff: 1
Page Ref: Sec. 8.2
19) What is the electron configuration for the 2
Fe ion?
A) 06
[Ar]4S3d
B) 24
[Ar]4S3d
C) 08
[Ar]4S3d
D) 28
[Ar]4S3d
E) 62
[Ar]4S3d
Answer: A
Diff: 1
Page Ref: Sec. 8.2
20) The formula of palladium(IV) sulfide is __________.
A)
Pd S
24
B)
PdS
4
C)
Pd S
4
D)
PdS
2
E)
Pd S
22
Answer: D
Diff: 1
Page Ref: Sec. 8.2
21) Elements from opposite sides of the periodic table tend to form __________.
A) covalent compounds
B) ionic compounds
C) compounds that are gaseous at room temperature
D) homonuclear diatomic compounds
E) covalent compounds that are gaseous at room temperature
Answer: B
Diff: 1
Page Ref: Sec. 8.2
22) Determining lattice energy from Born-Haber cycle data requires the use of
__________.
A) the octet rule
B) Coulomb's law
C) Periodic law
D) Hess's law
E) Avogadro's number
Answer: D
Diff: 2
Page Ref: Sec. 8.2
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
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
25) How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?
A) 1
B) 2
C) 3
D) 4
E) 5
Answer: D
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
28) What is the maximum number of double bonds that a carbon atom can form?
A) 4
B) 1
C) 0
D) 2
E) 3
Answer: D
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
33) A nonpolar bond will form between two __________ atoms of __________ electronegativity.
A) different, opposite
B) identical, different
C) different, different
D) similar, different
E) identical, equal
Answer: E
Diff: 1
Page Ref: Sec. 8.4
34) The ion
ICI-has __________ valence electrons.
4
A) 34
B) 35
C) 36
D) 28
E) 8
Answer: C
Diff: 1
Page Ref: Sec. 8.5
35) The ion NO-has __________ valence electrons.
A) 15
B) 14
C) 16
D) 10
E) 12
Answer: E
Diff: 1
Page Ref: Sec. 8.5
AsH shows __________ nonbonding electron pair(s) on As.
36) The Lewis structure of
3
A) 0
B) 1
C) 2
D) 3
E) This cannot be determined from the data given.
Answer: B
Diff: 1
Page Ref: Sec. 8.5
37) The Lewis structure of
PF shows that the central phosphorus atom has __________
3
nonbonding and __________ bonding electron pairs.
A) 2, 2
B) 1, 3
C) 3, 1
D) 1, 2
E) 3, 3
Answer: B
Diff: 1
Page Ref: Sec. 8.5
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
40) The formal charge on nitrogen in
NO-is __________.
3
A) -1
B) 0
C) +1
D) +2
E) -2
Answer: C
Diff: 2
Page Ref: Sec. 8.5
41) The formal charge on sulfur in 2
SO-is __________, where the Lewis structure of
4
the ion is:
A) -2
B) 0
C) +2
D) +4
E) -4
Answer: B
Diff: 2
Page Ref: Sec. 8.5
42) In the Lewis structure of ClF, the formal charge on Cl is __________ and the formal charge on F is __________.
A) -1, -1
B) 0, 0
C) 0, -1
D) +1, -1
E) -1, +1
Answer: B
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 2
CO - (carbon is the
3
central atom)?
A) 1
B) 2
C) 3
D) 4
E) 0
Answer: C
Diff: 1
Page Ref: Sec. 8.6
45) How many equivalent resonance forms can be drawn for
SO without expanding
2
octet on the sulfur atom (sulfur is the central atom)?
A) 0
B) 2
C) 3
D) 4
E) 1
Answer: B
Diff: 1
Page Ref: Sec. 8.6
46) How many equivalent resonance structures can be drawn for the molecule of
SO without having to violate the octet rule on the sulfur atom?
3
A) 5
B) 2
C) 1
D) 4
E) 3
Answer: E
Diff: 1
Page Ref: Sec. 8.6
47) How many different types of resonance structures can be drawn for the ion
2
SO where all atoms satisfy the octet rule?
3
A) 1
B) 2
C) 3
D) 4
E) 5
Answer: A
Diff: 2
Page Ref: Sec. 8.6
__________ kJ.
Bond: C≡C C-C H-I C-I C-H
D (kJ/mol): 839 348 299 240 413
A) +160
B) -160
C) -217
D) -63
E) +63
Answer: C
Diff: 1
Page Ref: Sec. 8.8
49) Using the table of average bond energies below, the H ?for the reaction is __________ kJ.
2H C C H (g) + H I (g)H C CHI (g)-≡--→=
Bond: C≡C C=C H-I C-I C-H
D (kJ/mol): 839 614 299 240 413
A) +506
B) -931
C) -506
D) -129
E) +129
Answer: D
Diff: 1
Page Ref: Sec. 8.8
__________ kJ.
23C O (g)+2H (g)H C O H (g) ≡→--
Bond: C-O C=O C≡O C-H H-H O-H
D (kJ/mol): 358 799 1072 413 436 463
A) +276
B) -276
C) +735
D) -735
E) -116
Answer: E
Diff: 1
Page Ref: Sec. 8.8
51) Using the table of bond dissociation energies, the H ? 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
reaction is __________ kJ.
A) 291
B) 2017
C) -57
D) -356
E) -291
Answer: C
Diff: 1
Page Ref: Sec. 8.8
__________ kJ.
222HCl (g)F (g)2HF (g)Cl (g)+→+
A) -359
B) -223
C) 359
D) 223
E) 208
Answer: A
Diff: 1
Page Ref: Sec. 8.8
8.2 Multiple-Choice Questions
1) Which ion below has a noble gas electron configuration?
A) 2Li +
B) 2Be +
C) 2B +
D) 2C +
E) 2N -
Answer: B
Diff: 1
Page Ref: Sec. 8.1