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2nd Semester Chemistry Review

Total questions: 112

Worksheet time: 2hrs 14mins

Name
Class
Date
1.

Identify the Reactants in this equation.

a)

A

b)

B

2.

What state of matter is this substance?

a)

solid

b)

liquid

c)

gas

d)

aqueous

3.

Identify the number in blue.

a)

Product

b)

Reactant

c)

Coefficient

d)

Subscript

4.

In what state is this substance?

a)

solid precipitate

b)

dissolved in water

c)

released as a gas

d)

liquid

5.

How many atoms of nitrogen are in the compound shown above?

a)

1

b)

2

c)

3

d)

4

6.

What are the blue numbers called?

a)

oxidation numbers

b)

subscripts

c)

group numbers

d)

product numbers

7.

How many atoms of nitrogen are present in this molecule?

a)

1

b)

2

c)

3

d)

4

8.

What does the symbol inside the circle mean?

a)

"yields, or produces"

b)

"dissolved in water"

c)

"forms a precipitate"

d)

"released as a gas"

9.

How many atoms of oxygen are represented in the picture?

a)

2

b)

3

c)

5

d)

6

10.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
11.
O2 + CS2 --> CO2 + SO2
What coefficient would go in front of the O2?
a)
1
b)
2
c)
3
d)
4
12.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
13.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
14.
True or False. You must convert grams to moles to do stoichiometry.
a)
True
b)
False
15.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
16.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
17.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
18.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
19.
The Formula to make S'mores is:
2C + 1M + G2 → C2MG2. If you have 5 Marshmallows (M), 9 Chocolate Pieces (C), and 9 Graham Cracker Halves (G), how many S'mores can you make?
a)
5
b)
4
c)
8
d)
42
20.
100 degrees Celsius is equal to _______ Kelvin. 
a)
0 K
b)
273 K
c)
173 K
d)
373 K
21.

What will happen to the volume of a balloon if you put it into hot water?

a)

Volume will increase

b)

Volume will decrease

c)

Volume will not change

22.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
23.

If the temperature of a gas decreases, the pressure...

a)

Decreases

b)

Increases

c)

Does not change

24.
Which container will have lower pressure?
a)
left
b)
right
c)
they both have the same pressure
25.
Gas laws involve what three variables?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
26.
When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the
a)
air molecules hit the walls of the tire less frequently
b)
rubber in the tires reacts with oxygen in the atmosphere
c)
air molecules speed up and collide with the tire walls more often
d)
air molecules diffuse rapidly through the walls of the tire.
27.

The kinetic molecular theory of matter states that all of the particles that make up matter are constantly

a)

growing

b)

shrinking

c)

crying

d)

moving

28.
At higher temperatures...
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
29.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

30.

When the temperature of a gas increases the particles...

a)

speed up and move closer

b)

speed up and move farther apart

c)

slow down and move closer together

d)

slow down and move farther apart

31.
True or False: Gases can be compressed. 
a)
True
b)
False
32.

When volume increases, pressure must...

a)

Increase

b)

Decrease

33.
Pressure is caused by ______.
a)
gravity.
b)
gas molecules colliding with each other.
c)
gas molecules colliding with surfaces of the container.
d)
gas molecules reacting with each other.
34.

What will happen to the size of a balloon if you take it outside in the winter?

a)

Volume will increase

b)

Volume will decrease

c)

Volume will not change

35.

In an "inverse relationship", such as Boyle's Law, when one variable shows an increase the other variable...

a)

increases as well

b)

remains constant

c)

shows a flat line on a graph

d)

decreases

36.
Gas pressure is caused by
a)
gas molecules colliding with surfaces
b)
gas molecules condensing to a liquid
c)
gas molecules hitting other gas molecule
d)
barometers
37.
a)
Flask 1 contain the most molecules
b)
Flask 2 contain the most molecules
c)
Flask 3 contain the most molecules
d)
Flask 4 contain the most molecules
38.
Of these three states of matter, which one has the most kinetic energy? 
a)
Solid 
b)
Liquid 
c)
Gas
39.

A balloon is filled with 35.0 L of helium in the morning when the temperature is 20.0 0C. By noon the temperature has risen to 45.0 0C. What is the new volume of the balloon?

a)

380 L

b)

38.0 L

c)

3.0 L

d)

8.0 L

40.

A 35 L tank of oxygen is at 315 K with an internal pressure of 190 atmospheres. How many moles of gas does the tank contain?

a)

26 moles of gas

b)

60 moles of gas

c)

20 moles of gas

d)

260 moles of gas

41.

A balloon that can hold 85 L of air is inflated with 3.5 moles of gas at a pressure of 1.0 atmosphere. What is the temperature in Celcius (0C) of the balloon?

a)

296 K = 230 C

b)

212 K = -61 C

c)

0 K = -273 C

d)

296 K = 23 C

42.

There are 135 L of gas in a container at a temperature of 260 0C. If the gas was cooled until the volume decreased to 75 L, what would the temperature of the gas be?

a)

26 K

b)

96 K

c)

496 K

d)

296 K

43.

A 75 L container holds 62 moles of gas at a temperature of 215 0C. What is the pressure in atmospheres inside the container?

a)

33 atm

b)

3 atm

c)

330 atm

d)

13 atm

44.

A weather balloon has a volume of 35 L at sea level (1.0 atm). After the balloon is released it rises to where the air pressure is 0.75 atm. What will the new volume of the weather balloon be?

a)

7 L

b)

47 L

c)

87 L

d)

11L

45.

A water molecule has the chemical formula H2O. This means that the water molecule is made up of

a)

Two hydrogen atoms and one oxygen atom

b)

Two oxygen atoms and one hydrogen atom

c)

Two hydrogen atoms and two oxygen atoms

d)

Two molecules of water

46.

The atoms in a water molecule are held together by covalent bonds. This means that the bonded atoms

a)

Lose protons

b)

Lose electrons

c)

Share electrons

d)

Switch neutrons

47.

The water molecule is a polar molecule. A water molecule is polar because

a)

The electrons are shared equally

b)

Oxygen has a stronger attraction for electrons than hydrogen

c)

It is very cold

d)

Hydrogen atoms have a stronger attraction for electrons than oxygen

48.

The water molecule is

a)

Slightly negative near the hydrogen atoms and slightly positive near the oxygen atom

b)

Slightly positive in all areas of the molecule

c)

Slightly negative near the oxygen atom and slightly positive near the hydrogen atoms

d)

The same charge in all areas of the molecule

49.

Water molecules are attracted to each other because

a)

They are all positively charged

b)

Each water molecule has the same number of protons as electrons

c)

The positive area of one water molecule is attracted to the negative area of another

d)

All water molecules are neutral

50.

A paper clip can stay on the surface of a sample of water because of water’s strong surface tension. Water’s surface tension is mostly a result of

a)

Water’s temperature

b)

The motion of water molecules

c)

The attraction of water molecules

d)

The impurities in the water

51.

Water is able to dissolve sodium chloride because

a)

The polar areas of water molecules attract the oppositely charged ions of sodium chloride

b)

The shape of the water molecules pushes the sodium and chloride ions apart

c)

The oxygen in the water molecules reacts with the sodium and chloride ions

d)

Water molecules and sodium chloride are covalently bonded

52.

Polar liquids, like water, dissolve other liquids which are polar or somewhat polar

a)

True

b)

False

53.

The attraction that causes water and other liquids to form drops on thin films is called ________________. This is also water's ability to be attraction to other water molecules.

a)

Adhesion

b)

Cohesion

c)

Surface Tension

d)

Capillary Action

54.

Ice freezes at the top of a pond and protects the aquatic life underneath. What property of water is KEY in this situation?

a)

Cohesion

b)

Adhesion

c)

Ice is less dense than liquid water

d)

The top of a pond is always the coldest part

55.

What property of water helps to moderate earth's temperature?

a)

Heat Capacity

b)

Capillary Action

c)

Cohesion

d)

Cooler Effect

56.

What atoms make up a water molecule?

a)

2 Hydrogen and 2 Oxygen

b)

3 Hydrogen and 1 Oxygen

c)

1 Oxygen and 2 Hydrogen

d)

3 Gold and 1 Silver

57.

Capillary Action is key for

a)

Water moving from roots to leaves in plants

b)

Air moving from mouth to lungs

c)

Ice floating on water

d)

Water moving to lower areas

58.

When you mix oil and water they immediately separate because

a)

Water is too good for oil

b)

Oil is dirty and water is clean

c)

Both oil and water are polar

d)

Water is polar and oils are non polar

59.

Plants use this to "drink" water and to "defy" gravity.

a)

capillary action

b)

muscles

c)

suction

d)

straw

60.

Since more substances can be dissolved in water than any other substance on Earth, it is called the

a)

universal solvent

b)

ultimate solution

c)

united states

d)

untied shoes

61.

Solid water (ice) is ____ dense than liquid water and therefore it floats.

a)

MORE

b)

LESS

62.
Why can water have no net charge but have slight charges in different parts of the molecule?
a)
The oxygen end is slightly negative and the hydrogen end is slightly positive
b)
The hydrogen end is slightly negative and the oxygen end is slightly positive
c)
The hydrogen and oxygen ends change in polarity
d)
Because it is hydrophobic
63.
Pure water has a
a)
Neutral pH 
b)
Negative pH
c)
Positive pH
d)
Both Negative and Positive pH
64.

A new dish soap claims that it is able to remove grease from pots and pans while still fully dissolving in the dishwasher water.

Which of the following best explains the ideal structure of the dish soap molecule?

a)

The dish soap molecule must be polar at one end to dissolve grease, and nonpolar at the other end so it can dissolve in water.

b)

The dish soap molecule must be nonpolar so that it can dissolve in both grease and water.

c)

The dish soap molecule must be polar so that it can dissolve both grease and water.

d)

The dish soap molecule must be nonpolar at one end to dissolve grease, and polar at the other end so it can dissolve in water.

65.
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
a)
60 ºC
b)
30 ºC
c)
50 ºC
d)
83 ºC
66.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
67.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
68.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
69.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
70.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
71.

A paper clip can stay on the surface of a sample of water because of water’s strong surface tension. Water’s surface tension is mostly a result of

a)

Water’s temperature

b)

The motion of water molecules

c)

The attraction of water molecules

d)

The impurities in the water

72.

The attraction that causes water and other liquids to form drops on thin films is called ________________. This is also water's ability to be attraction to other water molecules.

a)

Adhesion

b)

Cohesion

c)

Surface Tension

d)

Capillary Action

73.

When you mix oil and water they immediately separate because

a)

Water is too good for oil

b)

Oil is dirty and water is clean

c)

Both oil and water are polar

d)

Water is polar and oils are non polar

74.

Since more substances can be dissolved in water than any other substance on Earth, it is called the

a)

universal solvent

b)

ultimate solution

c)

united states

d)

untied shoes

75.

Plants use this to "drink" water and to "defy" gravity.

a)

capillary action

b)

muscles

c)

suction

d)

straw

76.
NaCl
a)
soluble
b)
insoluble
77.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
78.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
79.

What is a solvent

a)

A liquid that will dissolve a solid solute

b)

Another word for solution

c)

A thing that make drinks change colour

d)

Usually the solid about to be dissolved

80.

The ___ is the thing being dissolved.

a)

solute

b)

solvent

c)

mixture

d)

solution

81.

The substance in which a solute is dissolved is a?

a)

solution

b)

solvent

c)

alloy

d)

mixture

82.
Solutions are composed of __________ .
a)
salts and solutes
b)
solvents and salts
c)
solutes and alloys
d)
solutes and solvents
83.
If I dissolve sugar in water, what is the solute?
a)
Water
b)
Hydrogen
c)
Sugar
d)
Carbon
84.

If I dissolve carbon dioxide in water, what is the solvent?

a)

Carbon Dioxide

b)

There is no solvent

c)

Oxygen

d)

Water

85.

Define the term soluble.

a)

Can dissolve in water

b)

Cannot dissolve in water

c)

Partially dissolves in water

86.

Define the term insoluble.

a)

Can dissolve in water.

b)

Cannot dissolve in water.

c)

Partially dissolves in water.

87.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

88.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

89.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

90.
The concentration of a mixture can be increased in which of the following ways?
a)
Heating the mixture
b)
Adding more water “solvent”
c)
Adding more powder “solute”
d)
Stirring the mixture
91.

Electrolytes

a)

don't conduct electricity

b)

conduct electricity

92.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

93.

Bases have a pH of

a)

7

b)

Less than 7

c)

More than 7

94.

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

95.

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

96.

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

97.

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

98.

Water can act as both an acid and a base according to the bronsted lowry model. This means water is

a)

neutral

b)

conjugate

c)

ionic

d)

amphoteric

99.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
100.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
101.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
102.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
103.

Which of the following is the strongest acid?

a)

1

b)

5

c)

3

d)

8

104.

Which of the following is a characteristic of an acid?

a)

bitter

b)

slippery

c)

sour

d)

releases hydroxide ions in water

105.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
106.

In a test of pH levels, a baking soda has a pH of 9 and bleach has a pH of 12. What is true about there relationship?

a)

Both of the solution are Bases

b)

Both of the solution are Acids

c)

The Baking soda is an acid and the Bleach is a base

d)

The baking soda is a base and the Bleach is an Acid.

107.
A solution has a pH of 7.0.  What would happen to the pH if OH ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
108.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

109.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

110.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

111.

If a solution has a pOH of 3.7 the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

112.

Ammonia has a pOH of 2. Ammonia is a(n) __________.

a)

acid

b)

base

c)

neutral

d)

metal

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