WorksheetsVSEPR and Polarity Lesson
Total questions: 20
Worksheet time: 12mins
Name
Class
Date
1.
A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
2.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
3.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
4.
What molecule could this be?
a)
BF3
b)
CH4
c)
H2O
d)
CO2
5.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
6.
What molecular geometry would PH3 have?
a)
Trigonal Pyramidal
b)
Trigonal Bipyramidal
c)
Bent
d)
Linear
7.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
8.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
9.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
10.
True or False
Attractions between polar molecules are Weaker than attractions between nonpolar molecules.
a)
True
b)
False
11.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
12.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
13.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
14.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
15.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
16.
What causes a partial charge on a molecule?
a)
unequal sharing of electrons
b)
an electronegativity difference between 0.4 and 1.8.
c)
the shape of the molecule
d)
all of the above
17.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
18.
Strongest type of intermolecular force between molecules of HF...?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
19.
Strongest type of intermolecular force between molecules of C2H4...?
a)
London dispersion
b)
Dipole-dipole
c)
Hydrogen bonding
d)
Double bond
20.
Which of these is not an intermolecular force?
a)
covalent bonding
b)
hydrogen bonding
c)
London dispersion forces
d)
dipole-dipole forces
100 %
