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AP Chemistry Unit 2 Molecular & Ionic Cmpd Structure & Prop

Total questions: 29

Worksheet time: 25mins

Name
Class
Date
1.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
2.

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

3.

Resonance structures differ by __________.

a)

number and placement of electrons

b)

number of electrons only

c)

placement of atoms only

d)

number of atoms only

e)

placement of electrons only

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.

Bond enthalpy is __________.

a)

always negative

b)

always positive

c)

sometimes positive and sometimes negative

d)

always zero

e)

unpredictable

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.

Of the possible bonds between carbon atoms (single, double, and triple), _____.

a)

a triple bond is longer than a single bond

b)

a double bond is stronger than a triple bond

c)

a single bond is stronger than a triple bond

d)

a double bond is longer than a triple bond

e)

a single bond is stronger than a double bond

10.

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

11.

The ion NO- has _____ valence electrons.

a)

10

b)

12

c)

14

d)

15

e)

16

12.

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

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

13.

In the Lewis structure of ClF, the formal charge on Cl is _______ and the formal charge on F is _______.

a)

0,0

b)

-1, -1

c)

0, -1

d)

-1, 0

e)

+1, -1

14.

Using the table of average bond energies below, the ΔH for the reaction is _____ kJ.

a)

+160

b)

-160

c)

-217

d)

+217

e)

-63

15.

Which of these bonds takes the most energy to break?

a)

single

b)

double

c)

triple

d)

quadruple

16.

Potassium iodide, KI,has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

17.

Choose the correct shape for H2S

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Trigonal planar

18.
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
19.
The following molecules all contain polar bonds however only one is a polar molecule.  Which one?
a)
CCl4
b)
CO2
c)
NH3
d)
CH4
20.
 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
21.
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 
22.
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
23.

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

24.
What is the VSPER shape of PCl5
a)
See-saw
b)
trigonal planar
c)
octahedral
d)
trigonal bipyramidal
25.
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
26.
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
27.
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
28.

How many peaks should oxygen have in it's PES diagram?

a)

1

b)

2

c)

3

d)

4

29.

Given the peaks of a PES diagram of oxygen, the peaks of fluorine would be

a)

shifted to the right (assuming binding energy goes from highest energy to lowest energy on the x axis)

b)

shifted to the left (assuming binding energy goes from highest energy to lowest energy on the x axis)

c)

be in the same position, just higher (assuming binding energy goes from highest energy to lowest energy on the x axis)

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