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Chemistry Unit 2

Total questions: 111

Worksheet time: 2hrs 12mins

Name
Class
Date
1.

CaCO3

a)

calcium carbonate

b)

calcium carbon trioxide

c)

calcium carboxide

d)

carbon trioxide

2.

LiBr

a)

lithium bromide

b)

Monolithium bromine

c)

lithium monobromide

d)

Aluminum bromate

3.

Zn3 (PO4)2

a)

zinc (II) phosphate

b)

zinc phosphorous

c)

Trizinc diphosphate

d)

Zirconium phosphate

4.

CO2

a)

Carbon dioxide

b)

Monocarbon dioxide

c)

Carbon oxide

d)

Carbonate

5.

(NH4)2SO4

a)

Ammonium sulfide

b)

Ammonium sulfate

c)

Diammonium sulfide

d)

Nitrogen tetrahydrate sulfide tetroxide

6.

N2O3

a)

dinitrogen trioxide

b)

nitrogen trioxide

c)

nitrogen oxide

d)

nitrate

7.

CuSO4

a)

copper (II) sulfate

b)

copper (IV) sulfate

c)

copper (II) sulfide

d)

copper (II) tetrasulfide

8.

Al(OH)3

a)

aluminum hydroxide

b)

aluminum trihydroxide

c)

aluminum trioxide

d)

monaluminum hydroxide

9.

AuCl3

a)

gold (III) chloride

b)

gold chloride

c)

gold trichloride

d)

gold (III) trichloride

10.

SCl6

a)

sulfur hexachloride

b)

sulfur chloride

c)

monosulfur hexachloride

d)

sulfur chlorate

11.

sulfur trioxide

a)

SO3

b)

SO2

c)

SO4

d)

S2O3

12.

cobalt (III) sulfide

a)

Co2S3

b)

CoS3

c)

CoS

d)

Co3S3

13.

phosphorus trichloride

a)

PCl3

b)

P2Cl3

c)

PCl

d)

PClO3

14.

iron (II) sulfite

a)

FeSO3

b)

FeS3

c)

Fe(SO3)2

d)

Fe2(SO3)2

15.

zinc (II) nitride

a)

Zn3N2

b)

Zn3N

c)

ZnN2

d)

ZnN

16.

lead (IV) chromate

a)

Pb(CrO3)2

b)

PbCrO3

c)

Pb2(CrO3)4

d)

Pb2(CrO3)

17.

tin (IV) oxide

a)

SnO2

b)

Sn2O4

c)

Sn2O

d)

Sn4O2

18.

AlCl3

a)

aluminum chloride

b)

aluminum trichloride

c)

aluminum chlorate

d)

aluminum (III) chloride

19.

barium hydroxide

a)

BaOH

b)

Ba(OH)2

c)

BaOH2

d)

Ba2(OH)2

20.

CuSe

a)

copper selenide

b)

copper (II) selenide

c)

copper (I) selenide

d)

copper monoselenide

21.

radium iodide

a)

RaI2

b)

RaI

c)

Ra7I2

d)

RaI3

22.

silver (I) chloride

a)

AgCl

b)

AgClO

c)

AgCl2

d)

AgClO2

23.

KI

a)

potassium iodide

b)

potassium moniodide

c)

monopotassium iodine

d)

potassium moniodine

24.

PCl3

a)

phosphorous trichloride

b)

phosphorous chloride

c)

phosphorous trichlorate

d)

phosphorous chlorate

25.

SF6

a)

Sulfur hexafluoride

b)

Sulfur heptafluoride

c)

Sulfur pentafluoride

d)

Sulfur decafluoride

26.

N2O3

a)

dinitrogen trioxide

b)

nitrogen trioxide

c)

dinitrogen monoxide

d)

binitrogen trioxide

27.

P4O10

a)

tetraphosphorus decoxide

b)

phosphorus decoxide

c)

phosphorus oxide

d)

tetraphosphorus hexoxide

28.

diphosphorus pentoxide

a)

PO5

b)

P2O5

c)

P2O4

d)

P2O6

29.

sulfur hexachloride

a)

SCl6

b)

SCl7

c)

SCl5

d)

SCl4

30.

boron dioxide

a)

BO2

b)

BO

c)

BO3

d)

B3O2

31.

dinitrogen monoxide

a)

N2O

b)

NO

c)

NO2

d)

N3O

32.

bromine pentachloride

a)

BrCl5

b)

BrCl4

c)

BrCl

d)

Br5Cl

33.
What element do all acids contain?
a)
H
b)
O
c)
C
d)
He
34.
bromic acid
a)
HBr
b)
H2Br
c)
HBrO3
d)
HBrO4
35.
carbonic acid
a)
H2CO3
b)
H2CrO4
c)
H2C2O4
d)
HCO3
36.
chlorous acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
37.
HI
a)
iodic acid
b)
hydroiodic acid
c)
iodous acid
d)
hypoiodous acid
38.
H2SO3
a)
sulfuric acid
b)
hydrosulfuric acid
c)
sulfurous acid
d)
persulfuric acid
39.
HF
a)
flouric acid
b)
hydrofluoric acid
c)
fluorate acid
d)
hydrogen fluoridic acid
40.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
41.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
42.
What is the formula for sulfuric acid?
a)
HSO3
b)
H2SO3
c)
H2SO4
d)
H3SO4
43.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
44.
What is the formula for hydrochloric acid?
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
45.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
46.
H2C2O4
a)
carbonic acid
b)
chromic acid
c)
chloric acid
d)
oxalic acid
47.

HClO

a)

hydrochloric acid

b)

chloric acid

c)

chlorous acid

d)

hypochlorous acid

48.

If you have an oxyacid and it contains an -ate polyatomic ion, then acid's ending will change to _____.

a)

-ic

b)

-ous

c)

hydro-root-ic acid

d)

-ate

49.

What is the formula for bromic acid?

a)

HBr

b)

H2Br

c)

HBrO3

d)

HBrO4

50.

What is the name for HClO3

a)

chlorous acid

b)

chloric acid

c)

hydrochloric acid

d)

hydrogen chloride

51.

What is the name of HI?

a)

iodic acid

b)

hydroiodic acid

c)

iodous acid

d)

hypoiodous acid

52.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
53.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
54.
Name the acid: H3PO3
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
55.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

56.

When naming oxyacids, change "-ate" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

57.

Chromic acid

a)

HCrO4

b)

H4CrO

c)

H2CrO4

d)

H2CrO3

58.

How many valence electrons does Hydrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

59.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

60.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
61.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
62.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

63.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
64.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

65.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

66.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

67.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

68.

CHCl3 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

69.

CH2O has which of the following?

a)

Multiple double bonds

b)

Multiple single bonds

c)

One double bond

d)

One single bond

e)

A lone pair

70.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
71.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
72.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
73.

When drawing a Lewis Dot Structure, which atom goes in the center of the molecule?

a)

The least electronegative atom

b)

The most electronegative atom

c)

The heaviest atom

d)

The lightest atom

74.
What can be generalized about covalent bonds?
a)
Electrons will be exchanged.
b)
Electrons will be transferred.
c)
Electrons will be given and taken.
d)
Electrons will be shared.
75.
What is it called if there are three-pairs of electrons being shared?
a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
76.

What type of elements form covalent bonds?

a)

Metals

b)

Non Metals

c)

Metalloids

d)

Nobel Gas

77.

When a covalent bond forms _______________ are shared.

a)

protons

b)

nutrons

c)

valence electrons

d)

quarks

78.
Which LD Diagram is correct for chloromethane (CH3Cl)
a)
A
b)
B
c)
C
d)
D
79.

What is the molecular structure?

a)

Bent/Angular

b)

Linear

c)

Trigonal Planar

d)

Trigonal Pyramidal

80.

What is the molecular shape of the following?

a)

Bent/Angular

b)

Linear

c)

Trigonal Bipyramid

d)

Tetrahedral

81.

What is the molecular shape of the following?

a)

Bent

b)

Linear

c)

SeeSaw

d)

Octahedral

82.

What is the molecular shape of the following?

a)

Tetrahedral

b)

Linear

c)

Octahedral

d)

T-Shape

83.

What is the molecular shape of the following?

a)

Hexahedral

b)

Square Pyramid

c)

Octahedral

d)

T-Shape

84.

What is the molecular shape of the following?

a)

T-Shape

b)

See-Saw

c)

Trigonal Planar

d)

Octahedral

85.

What is the molecular shape of the following?

a)

Bent Angular

b)

Tetrahedral

c)

T-Shape

d)

Square Planar

86.

What is the molecular shape of the following?

a)

Square Planar

b)

Tetrahedral

c)

Linear

d)

Square Pyramid

87.

What is the molecular shape of the following?

a)

Tetrahdral

b)

Trigonal Bipyramid

c)

See-Saw

d)

Bent

88.

What is the molecular shape of the following?

a)

Trigonal Bipyramid

b)

Octahedral

c)

T-Shape

d)

Square Pyramid

89.

What is the molecular shape of the following?

a)

Trigonal BiPyramid

b)

Tetrahedral

c)

Trigonal Planar

d)

T-Shape

90.

What is the shape of the following molecular structure?

a)

Trigonal Pyramid

b)

Linear

c)

Tetrahedral

d)

Trigonal Bipyramid

91.

What is the shape of the following molecular structure?

a)

Trigonal Bipyramid

b)

See-Saw

c)

Trigonal Planar

d)

T-Shape

92.

What is the shape of the following molecular structure?

a)

Trigonal Pyramidal

b)

Trigonal Planar

c)

T-Shape

d)

Tetrahedral

93.
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.
94.
Does HCl have hydrogen bonding?
a)
yes
b)
no
95.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
96.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

97.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

98.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
99.

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

a)

higher

b)

lower

100.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

101.
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
102.

Intermolecular Forces are the forces that exist

a)

Between two or more molecules

b)

Within a single molecule

c)

Only in molecules containing carbon

d)

In all molecules

103.

Examples of an intermolecular force include

a)

london disperson

b)

hydrogen bonding

c)

dipole dipole

d)

all of the above

104.

For hydrogen bonding to occur, a molecule must have a hydrogen bonded to

a)

carbon

b)

another hydrogen

c)

Fluorine, Chlorine or Oxygen

d)

Fluorine, Nitrogen or Oxygen

105.

Type of intermolecular force present in I2, Br2, and Cl2.

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

106.

Does NH3 or PH3 have a higher boiling point?

(Hint: identify the types of IMF's present for each)

a)

NH3 because it has the strongest IMF's

b)

PH3 because it has the strongest IMF's

c)

NH3 because it has the weakest IMF's

d)

PH3 because it has the weakest IMF's

107.

In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces

a)

Higher

b)

Lower

c)

The same

108.

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

109.

The intermolecular force present in all matter is

a)

Hydrogen Bonding

b)

Ionic Bonding

c)

Dipole-Dipole

d)

London or Dispersion

110.

The strongest IMF is

a)

London/Dispersion

b)

Dipole-Dipole

c)

Hydrogen Bonding

111.

The weakest IMF is

a)

Dipole-Dipole

b)

Dispersion

c)

Hydrogen Bonding

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