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AP CHEMISTRY UNIT 2 REVIEW PACKET

Total questions: 100

Worksheet time: 3hrs 41mins

Name
Class
Date
1.

Why does an atom tend to chemically bond with another atom?

a)

To become more stable

b)

To remain on its present state

c)

To maintain its energy

d)

To decrease its stability

2.
Covalent bonds are between...
a)
two or more nonmetals
b)
sodium and chlorine
c)
metals and metals
d)
metals and nonmetals
3.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

4.

Which of the following best describes ionic bonds?

a)

transfer of electrons between a metal and a metal; resulting in no charges (+/-)

b)

sharing of electrons between a metal and a nonmetal

c)

transfer of electrons between a metal and a nonmetal; resulting in ions (charges +/-)

d)

sharing of electrons between nonmetals

5.

Which of the following is the correct example of a CATION?

a)

Na+

b)

Cl-

c)

Na-

d)

Cl+

6.

Which of atom is the correct ANION?

a)

Cl+

b)

Cl-

c)

Na-

d)

Na+

7.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
8.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)
HF
b)
Ne
c)
O2
d)
ICl
9.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
10.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

11.

Intermolecular forces for: NH3

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

12.

Which molecule: Br2, HCl, H2S, or NH3, will most likely have London dispersion forces as the MOST important IMF considered when determining melting/boiling points?

a)

Br2, it only has dispersion forces when interacting

b)

HCl, it can participate in dipole-dipole interactions and also dispersion forces

c)

H2S, it can participate in dipole-dipole interactions and also dispersion forces

d)

NH3, it can participate in hydrogen bonding and also dispersion forces

13.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

14.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
15.

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

16.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

17.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

18.

Carbon Monoxide containing an electronegativity difference of 1 would contain what type of intermolecular forces if any?

a)

Hydrogen Bonding

b)

Dipole-Dipole

c)

London Dispersion

d)

None

19.

What dispersion forces cause ice to have an open hexagonal structure in the solid state and float?

a)

H-bonding

b)

dispersion forces

c)

D-D interactions

d)

Ion - D interactions

20.
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.
21.
Does H2O have hydrogen bonding?
a)
yes
b)
no
22.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

23.

Which type of IMF is pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

24.

Rank these in order of strength:

covalent bond

dispersion force

hydrogen bond

dipole-dipole attraction

a)

dipole-dipole > covalent bond > hydrogen bond > dispersion

b)

dispersion > dipole-dipole > hydrogen bond > covalent bond

c)

covalent bond > hydrogen bond > dipole-dipole > dispersion

d)

hydrogen bond > dipole-dipole > dispersion > covalent bond

25.

Which molecule will have hydrogen bonds with other molecules in the sample?

a)

a) CO2

b)

b) HCN

c)

c) C2H2

d)

none of the above

26.

Crystalline solids _____

a)

have their particles arranged randomly

b)

have highly ordered structures

c)

are usually very soft

d)

exist only at high temperatures

27.

The shape of a liquid's meniscus is determined by ____.

a)

the viscosity of the liquid

b)

the type of material the container is made of

c)

the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container

d)

the amount of hydrogen bonding in the liquid

28.

Which type of solid has mobile electrons in the crystal (sea of electrons)?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

29.

Which type of solid typically has the lowest melting point of the four types of crystals?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

30.

Which is an example of an ionic crystal?

a)

SiO2

b)

NaCl

c)

SO3

d)

Li

31.

Which is an example of a molecular crystal?

a)

SiO2

b)

NaCl

c)

NH3

d)

Mg

32.

What is the name of the three-dimensional pattern that forms when ions bond?

a)

a crystal lattice

b)

a chemical compound

c)

an ionic bond

d)

an ionic chalice

33.
Which of these typically increases when IMF's increase?
a)
boiling point
b)
melting point
c)
viscosity
d)
all of these 
34.
When the atmospheric pressure equals the equilibrium vapor pressure ___ occurs.
a)
freezing
b)
melting
c)
boiling
d)
sublimation
35.

This is an example of a(n) __________.

a)

Hydrogen Bonding

b)

Dipole

c)

Nonpolar Molecule

d)

Intermolecular Force

36.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

polar covalent bonding

c)

London dispersion forces

d)

dipole-dipole interaction

37.

What kind of force is the arrow pointing to?

a)

Intramolecular Force

b)

Intermolecular Force

38.

What kind of force is the arrow pointing to?

a)

Intramolecular force

b)

Intermolecular force

39.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

40.

Which types of elements become cations?

a)

non-metals

b)

metals

c)

metalloids

41.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

A firm handshake

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

42.

Molten or dissolved compound conducts electricity.

a)

ionic compound

b)

covalent compound

43.

Diagram above shows the arrangement of atoms in brass. Which of the following could be atoms X and Y?

a)

X : Copper Y: Tin

b)

X: Zinc Y: Copper

c)

X: Iron Y: Carbon

d)

X: Copper Y: Zinc

44.

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

45.

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

46.
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
47.

Which of these pictures shows the particles in a solid, pure metal?

a)
b)
c)
d)
48.

Which structure represents that of an alloy?

a)

A

b)

B

c)

C

d)

D

49.

The diagram shows the structure of brass. Why is brass harder than pure copper?

a)

The zinc atoms form strong covalent bonds with copper atoms.

b)

The zinc atoms prevent layers of copper atoms from slipping over each other easily.

c)

The zinc atoms prevent the ‘sea of electrons’ from moving freely in the solid.

d)

Zinc atoms have more electrons than copper atoms.

50.

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

51.

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

52.

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

53.

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

a)

NF3

b)

IF3

c)

PF3

d)

SbF3

e)

SO42-

54.

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

55.

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

56.

Bond enthalpy is __________.

a)

always negative

b)

always positive

c)

sometimes positive and sometimes negative

d)

always zero

e)

unpredictable

57.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
58.

Which of these bonds takes the most energy to break?

a)

single

b)

double

c)

triple

d)

quadruple

59.

The ion NO- has _____ valence electrons.

a)

10

b)

12

c)

14

d)

15

e)

16

60.

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

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

61.

Choose the correct shape for H2S

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Trigonal planar

62.
The following molecules all contain polar bonds however only one is a polar molecule.  Which one?
a)
CCl4
b)
CO2
c)
NH3
d)
CH4
63.
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 
64.
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
65.

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

66.
What is the VSPER shape of PCl5
a)
See-saw
b)
trigonal planar
c)
octahedral
d)
trigonal bipyramidal
67.
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
68.
Of the following molecules, which has the largest dipole moment?
a)
CO
b)
CO2
c)
O2
d)
HF
69.
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
70.
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
71.

Arrange these elements in order of increasing electronegativity: antimony, fluorine, indium, selenium

a)

antimony, fluorine, indium, selenium

b)

indium, selenium, antimony, fluorine,

c)

indium, fluorine, selenium antimony

d)

indium, antimony, selenium, fluorine

72.

Calculate ΔEN for Pb-S

a)

1.1

b)

-0.1

c)

0.6

d)

3.7

73.

Calculate ΔEN for Na-Br

a)

1.9

b)

0.9

c)

2.8

d)

1.0

74.

Which type of bond is created between Na-I?

a)

Polar Covalent

b)

Non-polar Covalent

c)

Ionic

d)

Metallic

75.

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

76.

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

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

77.

Choose the correct shape for H2S

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Trigonal planar

78.
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
79.
What is the VSPER shape of PCl5
a)
See-saw
b)
trigonal planar
c)
octahedral
d)
trigonal bipyramidal
80.
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
81.

The molecular geometry of this molecular compound is ...

a)

Trigonal planar

b)

Tetrahedral bent

c)

Linear

d)

Tetrahedral tetrahedral

82.

The bond angle of the central atom in this molecular compound is ...

a)

109.5

b)

90

c)

90, 120

d)

180

83.

What is the molecular geometry of this molecular compound?

a)

Trigonal bypyramidal

b)

Tetrahedral

c)

Trigonal planar

d)

linear

84.

What is the hybridization of the central atom in this molecular compound?

a)

sp2

b)

sp3d5

c)

s

d)

sp3

85.

Ionic substances typically have high conductivities in which of the following state(s) of matter?

a)

Solids

b)

Molten liquids

c)

Aqueous liquids

86.

Which property of metals means that metal atoms can easily be drawn into a wire without breaking?

a)

Alloy

b)

Conductive

c)

Ductile

d)

Malleable

87.

Which of these alloys is a substitutional alloy?

a)

Bronze

b)

Steel

88.
How many are shared in a double bond?
a)
2
b)
4 pairs
c)
6
d)
4
89.
What is the the shape of this molecule according to VSPER theory?
a)
Linear
b)
Tetrahedral
c)
Trigonal Planar
d)
Trigonal pyramidal
90.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
91.

Draw the Lewis Dot structure for ICl2- and determine its predicted molecular geometry.

a)

see-saw

b)

trigonal bipyramidal

c)

linear

d)

bent

92.

Draw the Lewis Dot structure for PCl5 and determine the predicted molecular geometry

a)

octahedral

b)

trigonal pyramidal

c)

seesaw

d)

trigonal bipyramidal

93.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
94.
Bond angle for bent
a)
120o
b)
109.5o
c)
104.5o
d)
107o
95.
How many sigma and pi bonds does this have?
a)
1 sigma and 1 pi
b)
2 sigma and 1 pi
c)
1 sigma and 2 pi
d)
2 sigma and 2 pi
96.
This structure is called...
a)
tetrahedral
b)
Trigonal pyramidal
c)
Seesaw
d)
Bent/Angular
97.
Carbon atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
98.
Nitrogen atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
99.
Xe atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)

sp3d hybridization

100.

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

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