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AP Chemistry

Total questions: 25

Worksheet time: 27mins

Name
Class
Date
1.

The Lewis structure of N2H2 shows __________.

a)

a nitrogen-nitrogen triple bond

b)

a nitrogen-nitrogen single bond

c)

each nitrogen has one lone pair

d)

each nitrogen has two lone pairs

e)

each hydrogen has one lone pair

2.

In the nitrite ion (NO2-), __________.

a)

both bonds are single bonds

b)

both bonds are double bonds

c)

both bonds are the same because of resonance

d)

there are 20 valence electrons

e)

there is one single and one double bond

3.

The ability of an atom in a molecule to attract electrons is best quantified by the ______.

a)

electronegativity

b)

paramagnetism

c)

diamagnetism

d)

electron change-to-mass ratio

e)

first ionization energy

4.

A valid Lewis structure of _______ cannot be drawn without violating the octet rule.

a)

NF3

b)

IF3

c)

PF3

d)

SbF3

e)

SO42-

5.

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

a)

N

b)

C

c)

H

d)

O

e)

B

6.

In the resonance form of ozone shown, the formal charge on the central oxygen atom is _______.

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

7.

Bond enthalpy is __________.

a)

always negative

b)

always positive

c)

sometimes positive and sometimes negative

d)

always zero

e)

unpredictable

8.

As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

e)

is unpredictable

9.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
10.

Which of these bonds takes the most energy to break?

a)

single

b)

double

c)

triple

d)

quadruple

11.

The ion NO- has _____ valence electrons.

a)

10

b)

12

c)

14

d)

15

e)

16

12.

Potassium iodide, KI,has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

13.

The formal charge on carbon in the molecule shown is _______.

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

14.

Choose the correct shape for H2S

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Trigonal planar

15.
The electronegativity of C is 2.5, F is 4.0.  predict the character of a C-F bond.
a)
polar covalent
b)
nonpolar covalent
c)
ionic
d)
metallic
16.
The following molecules all contain polar bonds however only one is a polar molecule.  Which one?
a)
CCl4
b)
CO2
c)
NH3
d)
CH4
17.
 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
18.
How are compounds with metallic bonds similar to ionic compounds? 
a)
Both tend to have double and triple bonds
b)
Both tend to have low boiling points 
c)
Both tend to have poor conductivity
d)
Both tend to have high melting points 
19.
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
20.

How many sigma and pi bonds are there in C2H2? (the structure will be ordered HCCH)

a)

1 sigma and 1 pi

b)

3 sigma and 1 pi

c)

3 sigma and 2 pi

d)

2 sigma and 3 pi

21.
What is the VSPER shape of PCl5
a)
See-saw
b)
trigonal planar
c)
octahedral
d)
trigonal bipyramidal
22.
The interaction energy of two hydrogen atoms is shown on the graph above. Which of the answer choices displayed on the graph best represents the bond length of the H2 molecule?
a)
A
b)
B
c)
C
d)
D
23.
Of the following molecules, which has the largest dipole moment?
a)
CO
b)
CO2
c)
O2
d)
HF
24.
CCl4, CO2, PCl3, PCl5, SF6
Which of the following does not describe any of the molecules above?
a)
Trigonal pyramidal
b)
Octahedral
c)
Square planar
d)
Tetrahedral
25.
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

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