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WorksheetsMore VSEPR
Total questions: 15
Worksheet time: 28mins
Name
Class
Date
1.
Boron, an exception when it comes to stability, only needs to be surrounded by ____ valence electrons.
a)
2
b)
4
c)
6
d)
8
2.
True or False: The Lewis Dot diagram for CATIONS show a complete octet of valence electrons.
a)
True
b)
False
3.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
4.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
5.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
6.
What is the molecular shape of a silicon dioxide molecule?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
7.
Determine the molecular shape of carbon tetrafluoride.
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
8.
Determine the molecular geometry of ammonia (NH3).
a)
trigonal pyramidal
b)
trigonal planar
c)
bent
d)
tetrahedral
9.
What molecular shape is the structure shown here? (BeCl2)
a)
linear
b)
bent
c)
trigonal planar
d)
tetrahedral
10.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
11.
VSEPR is used to predict the shape of individual molecules based to the extent to which valence electrons...
a)
attract each other
b)
repel each other
c)
bond with each other
d)
mock each other
12.
True or False: You can use Lewis Dot structures to diagram elements, ions, ionic compounds, molecular compounds, and polyatomic ions.
a)
True
b)
False
13.
True or False: Lewis Dot diagrams (or structures) show ALL electrons for each atom.
a)
True
b)
False
14.
To determine the SHAPE of a molecular compound you assess the number of bonding groups and unshared electron pairs...
a)
on the central atom only
b)
on all elements in the compound
c)
on the cations only
d)
on the anions only
15.
There are _____ sigma bond(s) and _____ pi bond(s) in 1 molecule of H2CO (formaldehyde).
a)
1, 2
b)
2, 3
c)
3, 1
d)
4, 0
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