WorksheetsVSEPR
Total questions: 16
Worksheet time: 17mins
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 of the following shapes has an unshared pairs of electrons on the central atom?
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
4.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
5.
What molecule could this be?
a)
BF3
b)
CH4
c)
H2O
d)
CO2
6.
What molecule could this be?
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
7.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
8.
Who could this be?
a)
CO2
b)
NH3
c)
H2S
d)
CH4
9.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
10.
What molecular geometry would PH3 have?
a)
Trigonal Pyramidal
b)
Trigonal Bipyramidal
c)
Bent
d)
Linear
11.
A molecule with a lone pair on the central atom would have the same electron and molecular geometry
a)
True
b)
False
12.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
13.
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .
a)
eg = tetrahedral, mg = tetrahedral
b)
eg = linear, mg = linear
c)
eg = octahedral, mg = square planar
d)
eg = trigonal bipyramidal, mg = tetrahedral
14.
Consider the molecule below. 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
15.
Is this molecule polar?
a)
Yes
b)
No
16.
Is this molecule polar?
a)
No
b)
Yes
100 %
