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chem finals

Total questions: 97

Worksheet time: 2hrs 39mins

Name
Class
Date
1.

Metals and nonmetals form (a)   bonds

2.

Nonmetals combine to form molecular compounds with (a)   bonds

3.

A charged particle consisting of nonmetals covalently bonded together is known as a/an

(a)  

4.

What is the formula for Calcium Sulfide?

a)

CaS2

b)

CaS

c)

CaSO4

d)

SCa

5.

What is the name of the following compound?

MgBr2

a)

magnesium bromide

b)

magnesium bromine

c)

magnesium dibromide

d)

bromine magnesium

6.

What is the correct name for the following compound?

Ca(NO2)2

a)

Calcium nitroxide

b)

calcium nitrite

c)

calcium nitrate

d)

calcium nitro dioxided

7.

What is the correct formula for Lithium dichromate?

a)

LiCr2O7

b)

LiCrO4

c)

Li2Cr2O7

d)

Li2CrO4

8.

Which is the correct formula for Aluminum perchlorate?

a)

Al(ClO)3

b)

Al(ClO2)3

c)

Al(ClO3)3

d)

Al(ClO4)3

9.

What is the formula for tetraphosphorous decasulfide?

a)

PS10

b)

P10S4

c)

P4S10

d)

P6S5

10.

What is the name of N2O?

a)

nitrogen oxide

b)

dinitrogen monoxide

c)

nitrogen monoxide

d)

dinitrogen oxide

11.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
12.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
13.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
14.

Is this the correct structure for CH2O?

a)

Yes

b)

No

15.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
16.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
17.
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
18.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
19.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
20.

Which of the following compounds has only single bonds?

a)

I only

b)

II only

c)

III only

d)

I and III

e)

III and IV

21.

What is the correct structure for BF3?

a)

Option A.

b)

Option B.

c)

Option C.

d)

Option D.

22.

By replacing the element symbol, this could be a diagram of which element?

a)

Li

b)

Al

c)

C

d)

Be

23.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
24.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
25.

Which image could be a representation of NH3?

a)

A

b)

B

c)

C

26.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

27.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

28.

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

a)

Single

b)

Double

c)

Triple

29.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

30.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

31.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

32.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

33.
Which molecule contains bonds of GREATER polarity?
a)
H2O
b)
OF2
34.

Polar or non polar? H2S

a)

polar

b)

nonpolar

35.

Polar or nonpolar? PH3

a)

polar

b)

nonpolar

36.
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.
37.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
38.
Does H2O have hydrogen bonding?
a)
yes
b)
no
39.
Does HF have hydrogen bonding?
a)
yes
b)
no
40.
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
41.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

42.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

43.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

44.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
45.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)
HF
b)
Ne
c)
O2
d)
ICl
46.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

47.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

48.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

49.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

50.
Which molecule contains bonds of GREATER polarity?
a)
H2O
b)
OF2
51.

Polar or non polar? H2S

a)

polar

b)

nonpolar

52.

Polar or nonpolar? PH3

a)

polar

b)

nonpolar

53.
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.
54.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
55.
Does H2O have hydrogen bonding?
a)
yes
b)
no
56.
Does HF have hydrogen bonding?
a)
yes
b)
no
57.
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
58.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

59.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

60.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

61.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
62.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)
HF
b)
Ne
c)
O2
d)
ICl
63.

The red numbers in the image below represent ________

a)

subscripts

b)

coefficients

c)

oxidation numbers

d)

None of the answers are correct

64.

The blue numbers in the image below represent ________

a)

oxidation numbers

b)

coefficients

c)

subscripts

d)

none of the answers are correct

65.

The original substances before a chemical reaction are called the ____

a)

product

b)

yield

c)

chemical symbol

d)

reactants

66.

In the equation, 2Mg + O2 ---> 2MgO, which are the reactants?

a)

Mg and O2

b)

MgO

c)

Mg and MgO

d)

O2 and MgO

67.

In a chemical reaction, the new substances formed are called ______________.

a)

Products

b)

Yields

c)

Molecules

d)

Reactants

68.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
69.

What type of reaction is the following equation?

Fe + S --> FeS

a)

combination

b)

decomposition

c)

single replacement

d)

double replacement

70.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
71.

How many total H atoms are in 3 (NH₄)₂CrO₄

a)

4

b)

2

c)

8

d)

24

72.

Which is the meaning of the Law of Conservation of Mass ?

a)

Matter cannot be gained or lost in a chemical reaction.

b)

Matter can only be lost in a chemical reaction.

c)

Matter can only be gained in a chemical reaction.

d)

Matter can be gained and lost in a chemical reaction.

73.

Balance this equation...

Sb2S3 + O2 --> Sb + SO2

a)

It is balanced

b)

Sb2S3 + 3O2 --> 2Sb + 3SO2

c)

Sb2S3 + O2 --> 2Sb + SO2

d)

Sb2S3 + O2 --> 2Sb + 3SO2

74.

Name this reaction type, Cl2 + 2KI --> I2 + 2KCl

a)

Combination

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

75.

Name this reaction type, CO2 + H2O --> H2CO3

a)

Decomposition

b)

Single Replacement

c)

Combination

d)

Combustion

76.

What does (aq) mean after a formula?

a)

solid

b)

liquid

c)

gas

d)

dissolved in water

77.

When an element exists as two bonded atoms as opposed to a single atom, it is referred to as

a)

duo

b)

diatomic

c)

duet

d)

double

78.

What type of reaction is this?

2 C6H14 + 19 O2 → 12 CO2 + 14 H2O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

79.

What will K kick out in this Single Replacement reaction:

K + HCl →

a)

H

b)

Cl

c)

HCl

d)

K

80.

Which elements would form from the decomposition of Al2O3 ?

a)

Al + O2

b)

AlO

c)

Fe + S

d)

Al + O

81.

Which statement is true regarding endothermic reactions?

a)

a) The substances release energy and decrease disorder.

b)

b) The substances release energy and increase disorder.

c)

c) The substances absorb energy and increase disorder.

d)

d) The substances absorb energy and decrease disorder.

82.

Based on the graph, which statement is correct?

a)

The products are more stable than the reactants.

b)

The products have gained energy after reacting.

c)

The reactants are more stable than the products.

d)

The reactants have gained energy after reacting.

83.

The compound with a pink square is known as a ___.

a)

Reactant

b)

Product

84.

In order for this equation to be balanced, what number must be written as a coefficient for the substance in the blue box?

a)

1

b)

2

c)

4

d)

0

85.

Which type of reaction is shown?

a)

Combustion

b)

single replacement

c)

double replacement

d)

decomposition

86.

What must be done to this equation for it to be balanced?

a)

change the subscript to 3 in the reactants

b)

change the subscript to 3 in the products

c)

no change; it's balanced as is

d)

change the coefficients to 2

87.

What type of reaction is shown?

a)

Decomposition

b)

Single replacement

c)

Combustion

d)

Combination (or Synthesis)

88.

To balance this equation, what coefficient belongs in the red box?

a)

3

b)

2

c)

1

d)

0

89.

What type of reaction is this?

a)

Combination (or Synthesis)

b)

Single replacement

c)

Double replacement

d)

Decomposition

90.

To balance this equation, what coefficient must be written in the yellow box?

a)

0

b)

1

c)

2

d)

3

91.

Which type of reaction is shown?

a)

Combustion

b)

Combination (or Synthesis)

c)

Decomposition

d)

Double replacement

92.

To balance this equation, what coefficient must be written in the blue box?

a)

1

b)

2

c)

3

d)

4

93.

Which type of chemical reaction involves the production of a single complex compound from several simpler reactants?

a)

Decomposition

b)

Combustion

c)

Combination (or Synthesis)

d)

Single replacement

94.

What are the products of a combustion reaction?

a)

a single complex compound

b)

several simpler elements

c)

carbon dioxide and water

d)

carbon dioxide and hydrogen

95.

Which element is always present in the reactants of a combustion reaction?

a)

oxygen

b)

hydrogen

c)

carbon

d)

water

96.

Which type of reaction is shown?

a)

Single replacement

b)

Double replacement

c)

Combustion

d)

Decomposition

97.

To balance this equation, what coefficient must be written in the red box?

a)

1

b)

2

c)

4

d)

5

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