Molecular Shape, Polarity, and Intermolecular Forces Practice Test
Part 1: True False. Read the statement and decide it if it true or false. Mark “A” for true
and “B” for false.
1. Ionic bonds are stronger than hydrogen bonds.
2. All molecules that contain hydrogen experience hydrogen bonding with other
molecules.
3. Molecules “stick” to other molecules via dipole-dipole interactions, London
dispersion forces or hydrogen bonds.
4. According to VSEPR theory, electrons in a molecule want to be as far from each
other as possible.
5. Intermolecular forces would not affect whether substances are soluble in each
other.
6. Stronger intermolecular forces result in lower boiling points.
7. A non-polar molecule can never become polar.
8. A molecule with three atoms bonded to the central atom will always be polar.
Multiple Choice: Choose the best answer.
9. Which of the following would be the correct Lewis Dot Structure for SO2 (Ignoring
outside atom valence electrons)?
a. O=S-O
b. S=O-S
c. O-S-O
d. O=S=O
10.
Which of the following would be the correct polarity of the bonds in SO2?
a. The bonds are polar, with the oxygen ends being slightly negative.
b. The bonds are polar, with the oxygen ends being slightly positive.
c. The bonds are non-polar
11.
a.
b.
c.
d.
SO2 is:
Polar covalent
Non-polar covalent
Ionic
Metallic
12. What would be the intermolecular force that SO2 would experience with other
SO2 molecules?
a. London dispersion forces
b. Dipole-Dipole forces
c. Hydrogen bonding
d. No intermolecular forces would be experienced
13.
SO2 and NH3 would form what type of intermolecular force between them?
a. Hydrogen bond
b. Dipole-Dipole force
c. London dispersion forces
d. Covalent bond
14.
What is the bond angle on CH4?
a. 109.5o
b. 120o
c. 107o
d. 90o
15.
Which would evaporate faster, NH3 or SO2?
a. NH3
b. SO2
c. They would evaporate at the same rate
d. There is no way of knowing
16.
Based on intermolecular forces, which of the following should have the
highest boiling point?
a. CCl4
b. CHBr3
c. H2O
d. CS2
17.
Of the molecules below, only __________ is nonpolar.
a. CO2
b. H 2 O
c. NH3
d. HCl
e. TeCl2
18.
Of the molecules below, only __________ is polar.
a. SbF5
b. AsH 3
c. I 2
d. SF6
e. CH4
19.
The molecular geometry of the CHF3 molecule is __________, and the
molecule is __________.
a. trigonal pyramidal, polar
b. tetrahedral, nonpolar
c. tetrahedral, polar
Use the following diagrams to answer questions 20-25.
20.
a.
b.
c.
d.
e.
What do the arrows over the bonds indicate?
The bonds are polar
The bonds are non-polar
The bonds are ionic
The bonds are metallic
That they are hydrogen bonds
21.
a.
b.
c.
d.
For compound X3Y, what is the charge on Y?
Partially positive
Partially negative
Completely positive
Completely negative
22.
a.
b.
c.
d.
For compound XZ2 , what is the charge on the X?
Partially positive
Partially negative
Completely positive
Completely negative
23. For compound XZ2, which atom is attracting the electrons more in the
bond between X & Z?
a. X
b. Z
c. Y
d. Neither, the bond is non-polar
24. Toward what atom do the arrow-type symbols in the diagrams always
point?
a. The atom of lower reactivity
b. The less electronegative atom
c. The atom of higher mass
d. The more electronegative atom
25.
a.
b.
c.
d.
e.
Which of the molecules would be considered non-polar?
X3Y
X3Y and XYZ
X3Y and XZ2
XYZ and XZ2
X3Y, XZ2, and XYZ
26. The molecular geometry of the CS 2 molecule is __________.
A) linear
B) bent
C) tetrahedral
D) trigonal planar
E) T-shaped
27. 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
28. According to VSEPR theory, if there is one lone pair of electrons and three
atoms bonded to the central atom, they will be arranged in a(n) __________ geometry.
A) octahedral
B) linear
C) tetrahedral
D) trigonal planar
E) trigonal pyramidal
29. CO2 has linear geometry. There are __________ lone electron pairs on the central
atom in this molecule.
A) 0
B) 1
C) 2
D) 3
E) 4