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Chemistry 2nd Semester Final Review

Total questions: 95

Worksheet time: 3hrs 44mins

Name
Class
Date
1.

Why do all bonds form?

a)

to fill the outermost energy level

b)

so an atom can be unstable

c)

so the number of protons and electrons can equal.

d)

so they can gain neutrons.

2.

How do covalent bonds form?

a)

by sharing electrons between atoms

b)

by donating or receiving electrons

3.

What two types of atoms make a covalent bond?

a)

2 nonmetals

b)

2 metals

c)

1 metal and 1 nonmetal`

4.

Ionic bonds are between

a)

metals and nonmetals

b)

2 metals

c)

2 nonmetals

5.

How are ionic bonds formed?

a)

transfer of electrons

b)

sharing of electrons

6.

Covalent compounds can have

a)

Single Bonds

b)

Double Bonds

c)

Triple Bonds

d)

Quadruple Bonds

7.

What kind of bond will form between Hydrogen and Oxygen?

a)

ionic

b)

covalent

c)

metallic

d)

no bond

8.

Electrons are involved in chemical reactions, not protons or neutrons.

a)

true

b)

false

9.
Ionic or covalent?
C  O
a)
Ionic
b)
Covalent
10.
Ionic or covalent?
Na  Br
a)
Ionic
b)
Covalent
11.
Ionic or covalent?
K  Br
a)
Ionic
b)
Covalent
12.
Ionic or covalent?
H  O
a)
Ionic
b)
Covalent
13.
Ionic or covalent?
C  H
a)
Ionic
b)
Covalent
14.
Ionic or covalent?
Na  Cl
a)
Ionic
b)
Covalent
15.
Ionic or covalent?
Na  F
a)
Ionic
b)
Covalent
16.
Ionic or covalent?
N  H
a)
Ionic
b)
Covalent
17.
Ionic or covalent?
Ca  Cl
a)
Ionic
b)
Covalent
18.
Ionic or covalent?
H  H
a)
Ionic
b)
Covalent
19.
What is the rule for figuring out if it is ionic or covalent?
a)
Covalent bonds form between two metals.
b)
Ionic bonds form between two metals.
c)
Covalent bonds form between a metal and a non-metal.
d)
Ionic bonds form between a metal and a non-metal.
20.

Which type of compounds conduct electricity when melted or dissolved?

a)

covalent compounds

b)

ionic compounds

c)

both

d)

neither

21.

Which type of bonds form neutral compounds?

a)

ionic

b)

covalent

c)

both

d)

neither

22.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
23.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
24.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

25.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

26.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
27.

In stoichiometry problems, usually the first thing you do when starting the calculations is

a)

convert given quantities to masses

b)

convert given quantities to volumes

c)

convert given quantities to moles

d)

convert to wanted moles using mole ratio

28.

Which of the following is the correct, balanced equation for the decomposition of Calcium Oxide into its elements?

a)

Ca2O(s) → Ca(s) + O2(g)

b)

2CaO(s) → 2Ca(s) + O2(g)

c)

CaO2(s) → Ca(s) + O2(g)

d)

CaO(s) → Ca(s) + O2(g)

29.

Which of the following is correct for iron(III) is placed in copper(II) chloride?

a)

Fe(s) + CuCl2(aq) → Cu(s) + FeCl2(aq)

b)

Fe(s) + 2CuCl(aq) → 2Cu(s) + FeCl2(aq)

c)

2Fe(s) + 3CuCl2(aq) → 3Cu(s) + 2FeCl3(aq)

d)

3Fe(s) + 2CuCl2(aq) → 2Cu(s) + 3FeCl3(aq)

30.

The reason chemical equations are balanced is

a)

to satisfy the Law of Conservation of Mass.

b)

to satisfy the Law of Definite Proportions.

c)

to be prepared for stoichiometry.

d)

to satisfy the Law of Multiple Proportions.

31.

Which of the following is NOT true about limiting and excess reagents?

a)

Some of the excess reagent is left over after the reaction is complete.

b)

A balanced equation is necessary to determine which reactant is the limiting reagent.

c)

The amount of product obtained is determined by the limiting reagent.

d)

The reactant that has the smallest given mass is the limiting reagent.

32.

C2H4 + O2 → CO2 + H2O

What type of reaction is shown in the skeleton equation above?

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

e)

combustion

33.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
34.

When 12 moles of O2 reacts with 1.1 mole of C10H8, what is the limiting reactant? C10H8 + 12 O2 --> 10 CO2 + 4 H2O

a)

Oxygen

b)

C10H8

c)

Water

d)

Carbon Dioxide

35.

4NH3 + 5O2 --> 4NO + 6H2O

How many grams of NO are formed if 0.765 g of ammonia (NH3) react with excess oxygen?

a)

0.37g

b)

0.045g

c)

1.35g

d)

11.1g

36.

How many moles of water are produced when 3.75 moles of oxygen reacts with excess hydrogen? 2 H2 + O2 → 2 H2O

a)

16.0 moles H2O

b)

7.5 moles H2O

c)

5.75 moles H2O

d)

2 moles H2O

37.

What mass of hydrogen is required to produce 25.0 moles of water?

2H2 + O2 → 2H2O

a)

25 g H2

b)

50 g H2

c)

75 g H2

d)

100 g H2

38.

What type of reaction occurs between an element and a compound such as the one shown below?

Zn + 2HCl --> ZnCl2 + H2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

39.

What type of reaction is shown below?

4Fe + 3O2 → 2Fe2O3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

40.

What type of reaction is shown below?

2H2O2 →2 H2O + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

Double replacement

41.

What type of reaction is shown below?

AgNO3 + NaCl → AgCl + NaNO3

a)

Single Replacement

b)

Double Replacement

c)

Decomposition

d)

Combustion

e)

Synthesis

42.

What type of reaction is shown below?

CaCO3 + Ag2SO4 → CaSO4 + Ag2CO3

a)

Decomposition

b)

Single Replacement

c)

Double Replacement

d)

Combustion

e)

Synthesis

43.

Balance this equation:

_Al +_HCl --> _H2 +_AlCl3

a)

2, 6, 3, 2

b)

it is already balanced

c)

4, 12, 3, 4

d)

2, 1, 4, 5

44.

Balance this equation:

__P4 + __O2 --> __P2O3

a)

it is already balanced

b)

2, 1, 3

c)

1, 2, 3

d)

1, 3, 2

45.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
46.
Balance this equation.
_SnO2 +_H2-->_Sn +_H2O
a)
1,1,2,1
b)
1,2,1,1
c)
1,2,1,2
d)
1,2,2,1
47.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

48.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
49.

What are the three main statements of the kinetic molecular theory?

a)

All matter is made up of tiny particles that are constantly moving so they expand and contract.

b)

All matter is made up of tiny particles that move and cause the objects to collide.

c)

All matter is made up of tiny particles that are constantly moving and colliding with each other and the edges/container.

d)

All matter is made up of large segments that can be moved and rearranged to make space for other objects.

50.

For a fixed amount of gas at a constant temperature, the volume increases as the pressure...

a)

remains steady.

b)

increases.

c)

decreases.

d)

fluctuates.

51.

Which statement is not a key point of the particle theory of matter?

a)

The particles of matter are in constant motion

b)

All matter is made up of particles

c)

Particles naturally repel one another

d)

There are spaces between particles

52.

When any kind of gas such, as nitrogen or carbon dioxide, is heated, it

a)

sublimates.

b)

evaporates

c)

explodes

d)

expands

53.

What happens to particles when energy is added (heated)?

a)

They speed up and spread out

b)

They slow down and compress

c)

They stop moving

d)

They move closer together and speed up

54.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

55.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

56.

The pressure of a 6.5 L sample of oxygen gas is measured to be 3.8 atm. If the gas is transferred into a 12 L tank, what is the new pressure?

a)

6.6 atm

b)

3.9 atm

c)

4.5 atm

d)

2.1 atm

57.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

58.

A sample of gas containing 9.2 moles is transferred from an 13 L tank to a 23 L tank. What is the new number of moles that can be stored in the tank?

a)

10.2 mol

b)

13.7 mol

c)

19.1 mol

d)

16.3 mol

59.

What is the volume of a balloon that contains 3.7 moles of helium at 75°C and 5.1 atm?

a)

37 L

b)

13 L

c)

45 L

d)

21 L

60.
If the pressure exerted by a gas at 25 degrees C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a)
.002766 mole
b)
.0069 mol
c)
2.766 mol
d)
9.887 mol
61.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
62.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
63.
What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT
a)
14.19 atm
b)
16.53 atm
c)
18.42 atm
d)
22.54 atm
64.

What would be considered the weakest base?

a)

8

b)

7.8

c)

11.6

d)

14

65.

Pure water has a pH of 7. Pure water _______.

a)

is a base

b)

is a neutral substance

c)

could be either an acid or a base

d)

is an acid

66.

pH is the measure of the concentration of ______.

a)

Acids

b)

H+ ion

c)

OH- ion

d)

Base

67.

If a solution is basic which ion will be more present?

a)

H+

b)

K+

c)

OH-

d)

H-

68.

Stronger acids have a pH closer to...

a)

7

b)

14

c)

0

d)

9

69.

Weaker bases have a pH closer to...

a)

8

b)

14

c)

0

d)

4

70.

Neutralization is the process of an acid and a base reacting to form what? Select all that apply

a)

An ionic salt

b)

Hydronium ions

c)

NaCl

d)

Water

71.

An arrhenius acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

72.

An arrhenius base

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

73.

A bronsted lowry base

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

74.

A bronsted lowry acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

75.

Identify the true statement about the following reaction:

F- + H2O --> HF +OH-

a)

H2O is a bronsted lowry base

b)

H2O is not an acid or base according to either model

c)

H2O is a bronsted lowry acid

d)

H2O is an arrhenius acid

76.

Is the following compound an acid or a base?


HCl

a)

Acid

b)

Base

77.

Is the following compound an acid or a base?


NH4OH

a)

acid

b)

base

78.

Is the following compound an acid or a base?


HI

a)

acid

b)

base

79.

Is the following compound an acid or a base?


H3PO4

a)

acid

b)

base

80.

In the following chemical equation, which compound is the acid?


HCl + NH3 → NH4+ + Cl−

a)

HCl

b)

NH3

c)

NH4+

d)

Cl−

81.

In the following chemical equation, which compound is the base?


HCl + NH3 → NH4+ + Cl−

a)

HCl

b)

NH3

c)

NH4+

d)

Cl−

82.
Acid + Metal --> ?
a)
Salt + Water
b)
Salt + Hydrogen
c)
Salt
d)
Hydrogen
83.

Which of the following metals do not react with acid?

a)

copper

b)

silver

c)

gold

d)

magnesium

84.
An acid reacts with metal to produce 
a)
Carbon dioxide 
b)
Hydrogen gas
c)
Hydrogen gas and water 
d)
Salt and hydrogen gas 
85.
A neutralisation reaction produces 
a)
An acid 
b)
A neutral substance 
c)
Only water 
d)
Salt and water 
86.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
87.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

88.

Complete the following reaction:

H3PO4 + NaOH -->

a)

Na3PO4 + H2O

b)

Na +H2O

c)

Na3PO4 + H2

d)

Na3PO4 + H2O + CO2

89.

Complete the following reaction:

HNO3 + Ca(OH)2 -->

a)

Ca(NO3)2 + H2O

b)

Ca +H2O

c)

Ca(NO3)2 + H2

d)

Ca(NO3)2 + H2O + CO2

90.

What is the concentration of hidroxide ions in a solution with a pH = 7.65?

a)

2.24x10-8

b)

2.5x10-7

c)

4.47x10-7

d)

1.8x10-8

91.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

92.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

93.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
94.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
95.
if the [H+] of a solution is 8.4 x 10-3 mol/L the pOH of the solution will be
a)
2.08
b)
11.92
c)
1.02
d)
12.98

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