Chemistry 1B Winter 2016 MWF 9:30
Midterm 2
Test Form A
For all Lewis structures, be sure to minimize the distribution of formal charge.
1.
Predict the formula of an ionic compound formed by strontium and iodine
A) SrI
B) Sr2I
C) SrI2
D) Sr2I3
E) Sr3I2
2.
Predict the formula of an ionic compound formed by antimony (Sb) and oxygen
A) SbO
B) Sb2O
C) SbO 2
D) Sb2O 3
E) Sb3O 2
3.
For the elements Rb, F, and O, the order of increasing electronegativity is
A) Rb < F < O
B) Rb < O < F
C) O < F < Rb
D) F < Rb < O
E) none of these
4.
Which of the following bonds is the least polar? The electronegativity of H is lower than that of C.
A) H–F
B) H–N
C) H–O
D) H–C
E) All are the same.
5.
Which of the following elements forms the most ionic bond with chlorine?
A) Cs
B) Ga
C) P
D) Ar
E) I
6.
The nitrate ion NO 3 has ___ total electrons and ___ valence electrons.
A) 24, 24
B) 31, 23
C) 32, 32
D) 32, 24
E) 33, 25
7.
Among the following molecules, which has no dipole moment?
A) CO 2
B) H 2O
C) SF2
D) NCl3
E) ICl3
8.
How many electrons are in the Lewis structure for NO 2–?
A) 16
B) 30
C) 32
D) 20
E) 18
-
9.
As indicated by Lewis structures, which of the following species would not exist as a stable
molecule?
A) NH 3
B) N 2H 2
C) N 2H 6
D) N 2H 4
E) N 2O 4
10.
In the Lewis structure for Br3 , there are ____ lone pairs around the central bromine atom.
A) 1
B) 2
C) 3
D) 5
E) 6
11.
Which species has a single unpaired electron?
A) N 2
B) NO
C) CO
D) OH –
E) none of these
12.
Which molecule or ion is an exception to the octet rule?
A) I3–
B) NO 3–
C) PF3
D) H 2O
E) none of these
13.
In the Lewis structure for BF3
A) one F forms a double bond with B
B) there are three lone pairs on each F, and one lone pair on B
C) there are three equivalent resonance structures
D) the formal charge on each F is -1
E) there are three equivalent single bonds to the B
14.
Select the correct molecular structure for Br3–.
A) linear
B) bent
C) pyramidal
D) tetrahedral
E) T-shape
15.
VSEPR theory predicts that the bond angles about the carbon atom in the molecule,
Cl2C =O, are about
A) 120°
B) 60°
C) 109°
D) 180°
E) 90°
16.
What type of structure does the XeOF2 molecule have?
A) trigonal pyramid
B) tetrahedral
C) T-shaped
D) trigonal planar
E) octahedral
–
17.
Select the correct molecular structure for NO 3–.
A) trigonal pyramid
B) tetrahedral
C) square planar
D) octahedral
E) trigonal planar
18.
Select the correct molecular structure for PO 43–.
A) pyramidal
B) tetrahedral
C) square planar
D) octahedral
E) none of these
19.
In the molecule SF6, the formal charge on sulfur atom is
A) 0
B) 1
C) 2
D) 6
E) none of these
20.
The molecule ozone, O 3, has a bent structure. The formal charge on the central oxygen atom is
A) -1
B) 0
C) +1
D) +2
E) cannot be determined
21.
What is the hybridization of S in the molecule H 2S?
A) sp
B) sp2
C) sp3
D) dsp3
E) d2sp3
22.
What is the hybridization of I in the molecule IF 3?
A) sp
B) sp2
C) sp3
D) dsp3
E) d2sp3
23.
Elements from the second row of the periodic table, when sp3 hybridized, are capable
of forming ____ pi bond(s).
A) 0
B) 1
C) 2
D) 3
E) 4
24.
What is the hybridization of the central atom in PCl4+?
A) sp
B) sp2
C) sp3
D) dsp3
E) d2sp3
25.
What is the hybridization of the carbon atom in CO 2?
A) sp
B) sp2
C) sp3
D) dsp3
E) d2sp3
26.
Consider the following molecule. (Lone pairs are not drawn in.)
H
C
H
C
C2
C1
O
H
C
C
C4
C3
H
C
N
C5
H
Specify the hybridization of each carbon atom (in numeric order: C1 C2
A) sp2 sp2 sp2 sp3
sp
B) sp2 sp2 sp2
sp3 sp3
C) sp2 sp2 sp3
sp3 sp
2
2
3
D) sp
sp
sp
sp3
sp3
2
E) sp
sp
sp
sp
sp
27.
Which of the following has two pi bonds?
A) C 2H 6
B) C 2H 4
C) C 2H 2
D) at least two of these
E) none of these
28.
This molecule has
C3 C4 C5).
H
H
C
C
N
H
A) 7 sigma and 0 pi bonds
B) 6 sigma and 1 pi bonds
C) 5 sigma and 1 pi bonds
D) 4 sigma and 3 pi bonds
E) 5 sigma and 2 pi bonds
29.
BF3 reacts with NH3 to form F3B-NH 3. Upon forming this product, the B atom
A) remains with sp2 hybridization
B) changes hybridization from sp 2 to sp3
C) changes hybridization from sp 3 to sp2
D) atoms never change hybridization during a reaction
E) remains with sp3 hybridization
30.
This doubly charged anion to the right has, in total
A) no resonance structures
B) two resonance structures
C) three resonance structures
D) four resonance structures
E) five resonance structures
31.
O
O
C
C
O
Of these molecules, CH 4, NH 3 and H 2O, which has the smallest H-X-H bond?
A) CH 4
B) NH 3
C) H 2O
D) all are sp3 hybridized and therefore have the same bond angle
E) cannot determine from the information given
O
2-
-
32.
Because of the resonance structures in the nitrate ion, NO3 , each bond between the nitrogen and
oxygen can be considered
A) strictly a single bond
B) strictly a double bond
C) a pi bond
D) a sigma bond
E) a bond with both single and double bond character
33.
The methylene radical CH 2 is paramagnetic and has an approximate bond angle of 120˚. From these
data we can postulate
A) the molecule has sp2 hybridization with a lone pair in an sp2 orbital
B) the molecule has sp2 hybridization with one electron in an sp2 orbital and the other in a p orbital
C) the molecule has sp3 hybridization with two orbitals each containing a single electron
D) the molecule has sp3 hybridization with a lone pair in an sp3 orbital
E) the carbon atom has unhybridized orbitals
34.
A pi bond is distinct from a sigma bond because
A) a pi bond has no wavefunction density on the axis between the two atoms
B) a pi bond hinders rotation between the bonding atoms
C) a pi bond has maximum and equal wavefunction density above and below the bonding plane
D) a pi bond typically requires overlap of p orbitals
E) all of the above
35.
The Lewis structure for BeH 2 suggests
A) the Be atom has two unfilled 2p orbitals
B) the molecule has a bent structure
C) has an octet around the Be atom
D) has resonance structures
E) has a dipole moment
36.
For fluoromethane, shown in the orientation to the right, what is the direction of the dipole moment?
A) "
F
B) f
C) #
C
D) i
H
H
E) has no dipole moment
H
37.
The Lewis structure of the perchlorate ion ClO 4 results in ___ double bonds to the Cl atom.
A) 0
B) 1
C) 2
D) 3
E) 4
38.
What is the formal charge on the phosphorus atom in tetramethylphosphonium cation P(CH 3)4 ?
A) 0
B) +1
C) -1
D) +2
E) cannot be determined
-
+
39.
Molecular orbital theory applied to the diatomic molecule OF uses the following energy level
ordering
(σ2s) (σ2s*) (σ2p) (π2p) (π2p*) (σ2p*)
From this, we find that OF has
A) one unpaired electron, and a bond order of 3/2
B) one unpaired electron, and a bond order of 2
C) no unpaired electrons, and a bond order of 3/2
D) one unpaired electron, and a bond order of 1/2
E) none of these
40.
Molecular orbital theory applied to HeH predicts this species will
A) be unstable
B) be stable and paramagnetic
C) be stable with a bond order of 1/2
D) be stable with a bond order of 1
E) be stable with a bond order of 3/2
+