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IB (IMF +VSEPR)

Total questions: 45

Worksheet time: 42mins

Name
Class
Date
1.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
2.
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
3.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
4.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
5.

CO2 has polar bonds but is a NON POLAR molecule. Why?

a)

it has an asymmetrical shape

b)

bond polarity or dipole moment between C and O atoms cancel

c)

there is net dipole moment between C and O atoms in molecule

d)

bond polarity does not exist between C+ and O- atoms

6.

Is this molecule polar or nonpolar?

a)

polar

b)

nonpolar

7.
 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
8.

A molecular geometry with 3 bonding pairs is

a)

Trigonal pyramidal

b)

Trigonal planar

c)

Trigonal bipyramidal

d)

Linear

9.

A molecular geometry with 2 lone pairs and 2 bonding pairs is

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Linear

10.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
11.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
12.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
13.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
14.

Which molecule would have this geometry?

a)

CO2

b)

NH3

c)

H2S

d)

CH4

15.

Is this molecule polar?

a)

Yes

b)

No

16.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
17.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
18.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
19.
SiCl4 has what shape?
a)
square planar
b)
square pyramidal
c)
tetrahedral
d)
octahedral
20.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
21.

3 atoms bonded and 1 lone pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

22.

2 shared pairs and 0 unshared pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

23.

4 shared pairs and 0 unshared pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

24.

3 shared pairs and 0 unshared pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

25.

3 shared pairs and 1 unshared pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

26.

2 shared pairs and 2 unshared pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

27.

Tetrahedral molecules are

a)

polar

b)

non-polar

28.

polar molecules

a)

share electrons equally

b)

share electrons unequally

29.

polarity of bonds is based on

a)

atomic radius of each element

b)

electronegativity of each element

c)

the protons

d)

how electrons are transferred

30.

single bonds are

a)

the shortest and strongest

b)

the longest and strongest

c)

the longest and weakest

d)

the shortest and weakest

31.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

32.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

33.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
34.
Does HCl have hydrogen bonding?
a)
yes
b)
no
35.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
36.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
37.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

38.

Which statement explains why Br2 is a liquid at STP and I2 is a solid at STP?

a)

Molecules of Br2 are polar, and molecules of I2 are nonpolar

b)

Molecules of Br2 are nonpolar, and molecules of I2 are polar

c)

Molecules of Br2 have stronger intermolecular forces than molecules of I2.

d)

Molecules of I2 have stronger intermolecular forces than molecules of Br2.

39.

The correct ranking of intermolecular forces in order of greatest to least

a)

dipole-dipole, Hydrogen bonding, van der Waal forces

b)

van der Waal forces, hydrogen bonding, dipole-dipole attraction

c)

Hydrogen bonding, dipole-dipole attraction, van der Waals forces

d)

van der waal forces, dipole-dipole attractions, Hydrogen bonding

40.

Which sample has hydrogen bonding?

a)

H2S

b)

CH4

c)

NH3

d)

HI

41.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

42.

A dipole/polar molecule is...

a)

a probability map of where an electron may be found at any one time.

b)

something that occurs when two atoms of similar electronegativities bond.

c)

the creation of opposite charges at either end of the molecule.

43.

London forces occur in all molecules, but are stronger in atoms/molecules with more electrons. Which of these has the strongest London forces?

a)

F2

b)

Br2

c)

I2

d)

Cl2

44.

________ intermolecular forces (IMFs) cause liquids to have ________ boiling points.

a)

weak; high

b)

strong; low

c)

strong; high

d)

external; cold

45.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He

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