Honors Chemistry
Chapter 10 Take-Home Quiz
1) Give the approximate bond angle for a molecule with a trigonal planar shape.
A) 109.5°
C) 120°
B) 180°
D) 105°
E) 90°
2) Determine the electron geometry (eg) and molecular geometry (mg) of BCl3.
A) eg=trigonal planar, mg=trigonal planar
D) eg=trigonal planar, mg=bent
B) eg=tetrahedral, mg=trigonal planar
E) eg=trigonal bipyramidal, mg= trigonal
C) eg=tetrahedral, mg=trigonal pyramidal
bipyramidal
3) Determine the electron geometry (eg) and molecular geometry (mg) of CH 3+1.
A) eg=tetrahedral, mg=tetrahedral
D) eg=trigonal planar, mg=trigonal planar
B) eg=tetrahedral, mg=trigonal pyramidal
E) eg=tetrahedral, mg=trigonal planar
C) eg=trigonal planar, mg=bent
4) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined atom
CH3OCH3.
A) eg=tetrahedral, mg=tetrahedral
D) eg=trigonal bipyramidal,
B) eg=linear, eg=linear
mg=tetrahedral
C) eg=tetrahedral, mg=bent
E) eg=octahedral, mg=square planar
5) Consider the molecule at right. Determine the molecular
geometry at each of the 2 labeled carbons.
A) C1 = tetrahedral, C2 = linear
B) C1 = trigonal planar, C2= bent
C) C1 = bent, C2 = trigonal planar
D) C1 = trigonal planar, C2 = tetrahedral
E) C1 = trigonal pyramidal, C2 = see-saw
6) Consider the molecule at right. Determine the molecular geometry at
each of the 3 labeled atoms.
A) 1=trigonal planar, 2=tetrahedral, 3=trigonal pyramidal
B) 1=tetrahedral, 2=tetrahedral, 3=tetrahedral
C) 1=trigonal planar, 2=tetrahedral, 3=tetrahedral
D) 1=tetrahedral, 2=tetrahedral, 3=trigonal planar
E) 1=trigonal planar, 2=trigonal pyramidal, 3=trigonal pyramidal
7) Place the following in order of increasing X-Se-X bond angle, where
X represents the outer atoms in each molecule.
SeO2
SeCl6
SeF2
SeCl
<
SeF
<
SeO
A)
6
2
2
D) SeO2 < SeF2 < SeCl6
B) SeF2 < SeO2 < SeCl6
E) SeCl6 < SeO2 < SeF2
SeF
<
SeCl
<
SeO
C)
2
6
2
8) A pilot checks for water in the gas before flying a small airplane. How does she do it?
A) Drain a little bit of gas from the bottom and look for two layers.
B) Smell it.
C) Shake the wings.
D) Pipet the liquid from the top of the tank and look for two layers.
E) Check the gas gauge.
9) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO 3.
A) eg=tetrahedral, mg=trigonal pyramidal, polar
B) eg=tetrahedral, mg=tetrahedral, nonpolar
C) eg=trigonal planar, mg=trigonal planar, nonpolar
D) eg= trigonal bipyramidal, mg=trigonal planar, polar
E) eg=trigonal pyramidal, mg=bent, nonpolar
10) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO 2.
A) eg=tetrahedral, mg=bent, polar
B) eg=trigonal planar, mg=bent, polar
C) eg=linear, mg=linear, nonpolar
D) eg=tetrahedral, mg=tetrahedral, nonpolar
E) eg=trigonal pyramidal, mg=trigonal pyramidal, polar
11) Choose the compound below that contains at least one polar covalent bond, but is nonpolar.
A) HCN
D) ICl3
E) Both B and C are nonpolar and contain
B) CF4
SeBr
a polar covalent bond.
C)
4
12) Place the following in order of increasing dipole moment.
I. BCl3
II. BIF2
III. BClF2
A) I < II = III
D) II < I < III
B) II < III < I
E) I < III < II
C) I < II < III
13) Describe a pi bond.
A) side by side overlap of p orbitals
B) end to end overlap of p orbitals
C) s orbital overlapping with the
end of a p orbital
D) overlap of two s orbitals
E) p orbital overlapping with a d
orbital
14) Describe a sigma bond.
A) side by side overlap of p orbitals
B) end to end overlap of p orbitals
C) s orbital overlapping with the
side of a p orbital
D) overlap of two s orbitals
E) p orbital overlapping with a d
orbital
15) A molecule containing a central atom with sp hybridization has a(n) __________ electron
geometry.
A) linear
D) tetrahedral
B) trigonal bipyramidal
E) bent
C) trigonal planar
16) Identify the number of electron groups around a molecule with sp hybridization.
A) 1
D) 4
B) 2
E) 5
C) 3
17) A molecule containing a central atom with sp2 hybridization has a(n) __________ electron
geometry.
A) linear
D) tetrahedral
B) trigonal bipyramidal
E) bent
C) trigonal planar
2
18) Identify the number of electron groups around a molecule with sp2 hybridization.
A) 1
B) 2
C) 3
D) 4
E) 5
19) A molecule containing a central atom with sp3 hybridization has a(n) __________ electron
geometry.
A) linear
D) tetrahedral
B) trigonal bipyramidal
E) bent
C) octahedral
20) Identify the number of electron groups around a molecule with a tetrahedral shape.
A) 1
B) 2
C) 3
D) 4
21) Identify the number of electron groups around a molecule with a trigonal bipyramidal shape.
A) 1
D) 4
B) 2
E) 5
C) 3
22) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in
CH3CN.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, mg=trigonal planar
C) eg=trigonal planar, mg=bent
D) eg=linear, mg=linear
E) eg=trigonal planar, mg=trigonal planar
23) Determine the electron geometry (eg) and molecular geometry (mg) of H 2CO.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, mg=trigonal planar
C) eg=trigonal planar, mg=bent
D) eg=linear, mg=linear
E) eg=trigonal planar, mg=trigonal planar
24) Draw the Lewis structure for OF2. What is the hybridization on the O atom?
A) sp
C) sp2
B) sp3
D) sp3d
E) sp3d2
25) Draw the Lewis structure for H3O+. What is the hybridization on the O atom?
A) sp
C) sp2
B) sp3
D) sp3d
E) sp3d2
26) Consider the molecule at right. Determine the hybridization at each
of the 2 labeled carbons.
D) C1 = sp3d, C2 = sp3d2
A) C1 = sp3, C2 = sp3d
B) C1 = sp, C2 = sp2
E) C1 = sp2, C2 = sp3
C) C1 = sp2, C2 = sp3d
27) Consider the molecule at right. Determine the hybridization at each of
the 3 labeled atoms.
A) 1=sp2, 2=sp3, 3=sp2
D) 1=sp3, 2=sp3, 3=sp2
B) 1=sp2, 2=sp3, 3=sp3
E) 1=sp, 2=sp2, 3=sp2
C) 1=sp3, 2=sp3, 3=sp3
3
E) 5
28) How many of the following molecules have sp hybridization on the central atom?
C2Cl2
CO2
O3
H2O
A) 0
B) 1
C) 2
D) 3
E) 4
29) How many of the following molecules have sp 2 hybridization on the central atom?
HCN
SO2
OCl2
XeCl2
A) 4
B) 3
C) 2
D) 1
E) 0
30) List the number of sigma bonds and pi bonds in a single bond.
A) 1 sigma, 0 pi
C) 1 sigma, 1 pi
B) 0 sigma, 1 pi
D) 1 sigma, 2 pi
31) List the number of sigma bonds and pi bonds in a double bond.
A) 1 sigma, 1 pi
C) 2 sigma, 2 pi
B) 2 sigma, 1 pi
D) 1 sigma, 2 pi
32) List the number of sigma bonds and pi bonds in a triple bond.
A) 1 sigma, 1 pi
C) 2 sigma, 2 pi
B) 2 sigma, 1 pi
D) 1 sigma, 2 pi
33) Draw the Lewis structure for the molecule C3H4. How many sigma and pi bonds does it contain?
A) 7 sigma, 1 pi
D) 10 sigma, 0 pi
B) 8 sigma, 0 pi
E) 8 sigma, 2 pi
C) 6 sigma, 2 pi
34) Which of the following statements is TRUE?
A) The total number of molecular orbitals formed doesn't always equal the number of atomic
orbitals in the set.
B) A bond order of 0 represents a stable chemical bond.
C) When two atomic orbitals come together to form two molecular orbitals, one molecular
orbital will be lower in energy than the two separate atomic orbitals and one molecular
orbital will be higher in energy than the separate atomic orbitals.
D) Electrons placed in antibonding orbitals stabilize the ion/molecule.
E) All of the above are true.
35) Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your
answer and give an example.
36) Explain why oil and water do not mix.
37) Determine the molecular geometry about each interior atom in CH2CHCCCH3. Sketch the threedimensional structure and label the interior atoms with the corresponding molecular geometry.
Determine the hybridization about each interior atom in the following structure.
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