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Chem 2 Q1

Total questions: 154

Worksheet time: 2hrs 13mins

Name
Class
Date
1.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

2.

Which states of matter are fluid?

a)

gases and liquids

b)

liquids and solids

c)

gases only

d)

liquids only

3.
The movement of gas molecules is greatly affected by _________.
a)
the shape of the container
b)
size of the container
c)
temperature of the container
4.
The energy of an object as it is in motion is defined as
a)
Kinetic Theory
b)
Kinetic energy
c)
Potential energy
d)
Electric energy
5.
Gas molecules can easily be compressed  because ___________. 
a)
gas molecules are soft
b)
gas molecules are far apart
c)
gas molecules follow the shape of the container
6.

The kinetic theory states

a)

Particles won't move if you don't apply energy to it.

b)

Particles only move in liquids and gases.

c)

Particles are always in motion.

d)

At the same temperature the object that has the most mass heats quicker.

7.

If you spray air freshener on side of the room, why is there a delay for the smell to reach the other side of the room? 

a)
Attractive forces between air and air freshener particles
b)
Not enough air freshener particles
c)
Because the particles like where they are at
d)
Collisions between air and air freshener particles
8.
If you place a balloon in a freezer what happens to the size of the balloon?
a)
Doubles
b)
increases
c)
decreases
d)
stays still
9.
In which state of matter are the particles moving the least random
a)
Gas
b)
Liquid
c)
Solid
d)
Plasma
10.
In which state of matter are the particles only vibrating?
a)
Gas
b)
Liquid
c)
Solid
d)
Plasma
11.
a)
Gases do not move in straight line
b)
Most of the volume of gas is empty space
c)
Gas particles are not in constant random motion
d)
Gas particles attract each other
12.
The slower the particles in a substance move,
a)
the colder it is.
b)
the warmer it is.
c)
the more energy it has.
d)
the less energy it has.
13.
Which is NOT an assumption made by the kinetic molecular theory of gases?
a)
Gas particles are small and take up little volume
b)
Particles travel in constant, random, straight-line motion until colliding
c)
When particles collide, their total kinetic energy is decreased
d)
Particles do not attract or repel each other
14.
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
15.
Of these three states of matter, which one has the most kinetic energy? 
a)
Solid 
b)
Liquid 
c)
Gas
16.

What intermolecular force present in a sample of pure HCl?

a)

dipole-dipole attraction

b)

H-bonds

c)

London dispersion forces 

d)

molecule-ion attraction

17.

 Intermolecular forces are the forces that exist

a)

within molecules

b)

between molecules

18.

Which of these is not an intermolecular force?

a)

covalent bonding

b)

London dispersion forces

c)

hydrogen bonding

d)

dipole-dipole forces

19.

Which are the strongest intermolecular forces?

a)

hydrogen bonds

b)

London dispersion forces

c)

dipole-dipole forces

d)

molecule-ion attractions

20.

Hydrogen bonding is a special type of what force?

a)

London dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

covalent force

21.

What type of intermolecular force is present in all substances, regardless of polarity?

a)

London dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

22.

What explains the very high melting and boiling point of water?

a)

Dipole-dipole forces between water molecules

b)

London dispersion forces between water molecules

c)

Hydrogen bonds between water molecules

d)

Molecule-ion attractions between water molecules

23.

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

a)

Higher

b)

The same

c)

Lower

24.

Which is the second strongest intermolecular force, after hydrogen bonding?

a)

dipole-dipole attraction

b)

London forces

25.

What are intermolecular forces?

a)

forces of attraction or repulsion which act between neighboring particles

b)

forces which keep a molecule together.

26.

Which is NOT an intramolecular force?

a)

Polar Covalent Bond

b)

Nonpolar Covalent Bond

c)

London Dispersion Force

d)

Ionic Bond

27.

Electrons that are free to move in metals are

a)

delocalized electrons

b)

oxidation number

c)

chemical bond

d)

salts

28.

Which has the strongest forces between particles (usually)?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

29.

Which has the weakest forces between particles (usually)?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

30.

Which structure consists of a giant lattice of cations and anions held together by strong electrostatic forces of attraction?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

31.

Which occurs between metal and non-metals?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

32.

Which structure consists of a giant lattice of regularly arranged cations surrounded by a sea of delocalized electrons.

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

33.

Which of the following types of bonding results in materials which are malleable and ductile?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

34.

Which of the following types of bonding results in materials which are generally insoluble in water?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

35.

Which of the following types of bonding results in materials which have the highest melting and boiling points?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

36.

Which of the following types of bonding results in materials which have the lowest melting and boiling points?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

37.

In the case of metallic bonding, the greater the number of delocalized electrons, the ________ the metallic bond strength.

a)

weaker

b)

stronger

38.

Which occurs between metals and metals?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

39.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

covalent bonding

40.

Which intermolecular force is characterized by partially oppositely charged ions?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

41.
Which of the following molecules has hydrogen bonding?
a)
HCl
b)
HI
c)
HF
d)
HBr
42.
Which of the following molecules contains only London dispersion forces?
a)
CF4
b)
HCl
c)
H2O
d)
MgO(aq)
43.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)
HF
b)
Ne
c)
O2
d)
ICl
44.
Which of the following molecules would have the lowest boiling point?
a)
CH4
b)
C2H6
c)
C3H8
d)
C4H10
45.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
46.
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
47.
Does H2O have hydrogen bonding?
a)
yes
b)
no
48.
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.
49.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
50.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
51.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

52.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

53.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

54.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
55.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
56.
If fluorine is stronger then carbon, what charge will the fluorine receive?
a)
negative
b)
slight negative
c)
positive
d)
slight positive
57.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
58.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
59.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
60.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
61.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
62.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
63.

the interactive force that exist between water molecules and sides of a graduated cylinder is______.

a)

adhesion

b)

capillarity

c)

cohesion

d)

IMF

64.

The temperature at which its vapor pressure equals atmospheric pressure.

a)

specific heat

b)

vapor pressure

c)

molar heat of fusion

d)

boiling point

65.

The ascension of liquids through slim tube, cylinder or permeable substance due to adhesive and cohesive forces interacting between the liquid and the surface is called_____.

a)

surface tension

b)

cohesion

c)

capillarity

d)

adhesion

66.

Cohesive forces

a)

Are the attraction of molecules within a liquid

b)

Are only present when the liquid is exposed to glue

c)

Are the attraction of molecules to the container walls

d)

Are important for upward movement in capillary action

67.

Capillary action is

a)

Caused by cohesive and adhesive forces

b)

Not observed in liquid mercury

c)

Allows some liquids to 'flow' vertically up a thin tube

d)

All of the above

68.

A substance with a high vapor pressure have _______ intermolecular forces?

a)

strong

b)

weak

69.

A substance with a high amount of intermolecular forces will have a ______ vapour pressure.

a)

high

b)

low

70.

Water droplets are mainly formed by what force?

a)

Viscosity

b)

Van der Waals forces

c)

Hydrogen Bonding

d)

Dipole-Dipole interactions

71.

As the temperature of a liquid increases, the viscosity

a)

Increases

b)

Decreases

c)

Doesn't change

d)

Not enough information

72.

Which of the following is NOT a property of a liquid

a)

surface tension

b)

capillary action

c)

viscosity

d)

polar

73.

This type of solid forms a regular repeating

three-dimensional structure called a crystal lattice. What type of solid is this?

a)

amorphous

b)

crystalline

c)

glass

d)

diamond

74.

In amorphous solids, the atoms or molecules are held together in a completely random formation.

a)

true

b)

false

75.

Which of the following is not true about crystalline solids?

a)

Have a sharp melting point

b)

Crystalline solids are anisotropic in nature

c)

Cannot be cleaved along a definite plane

d)

They are considered as true solids

76.

Which of the following is true of solids?

a)

Solids maintain a defined shape and size under all conditions.

b)

All solids have a crystalline structure.

c)

All solids maintain a defined shape and size if conditions remain constant.

d)

All solids have a lattice structure at the atomic level.

77.

One major difference between crystalline and amorphous solids is that

a)

crystalline solids have a precise melting point.

b)

amorphous solids have a lattice structure.

c)

amorphous solids always behave consistently and uniformly.

d)

crystalline solids break unpredictably and can produce curved fragments.

78.

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

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

79.

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

80.

Which is an example of an ionic crystal?

a)

Quartz

b)

NaCl

c)

Ammonia

d)

Iron

81.

Which is an example of a metallic crystal?

a)

Quartz

b)

NaCl

c)

Ammonia

d)

Iron

82.

A friend in your chemistry class is struggling to understand why crystalline solids are grouped into four main types: network, molecular, ionic, and metallic. Which explanation below will BEST help him begin to understand why chemists might have these groups?

a)

Crystalline solids all share a lattice structure, but have different densities. Chemists use the groups to organize the solids by density.

b)

Crystalline solids all share a lattice structure and the same types of bonds, but are composed of different elements. These elements affect the way the solid conducts heat and electricity.

c)

Crystalline solids all share a lattice structure, but behave differently under similar conditions.

d)

Crystalline solids all share a lattice structure, but the bonds that hold them together at the atomic level differ. The elements that make up the solids also differ. These differences affect how a solid conducts heat and electricity.

83.

Solids have many different properties. ___________ solids are known for their ability to be flattened into a sheet, stretched into a wire, and to conduct energy well.

a)

Molecular

b)

Metallic

c)

Covalent Network

d)

Ionic

84.

It is possible to tell the difference between a solid with a crystalline structure and one with an amorphous structure just by looking at it.

a)

True

b)

False

85.

An engineer is designing an electrical system and is looking for a material to transmit energy. She has four solids available, each made with different materials. To conduct energy most efficiently and effectively, she should use material

a)

whose electron are held with ionic bonds.

b)

whose electron are held with covalent bonds.

c)

whose electrons are held with metallic bonds.

d)

that is an electrical insulator.

86.

Which statement is true about the properties of solids?

a)

Metallic solids have a high melting point.

b)

Network solids are generally not soluble in water.

c)

Molecular solids do not dissolve easily in water.

d)

All ionic solids are similar in density.

87.

Which one of the following diagrams best represents a sematic A liquid crystal phase?

a)

A

b)

B

c)

C

d)

D

e)

E

88.

Which letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

89.

Which letter on the diagram represents a liquid?

a)

A

b)

B

c)

C

d)

D

90.

What does point B represent?

a)

Triple point

b)

Critical point

c)

Equilibrium point

d)

Normal melting point

91.

Which letter on the diagram represents a solid?

a)

A

b)

B

c)

C

d)

D

92.

The temperature and pressure conditions at which the solid, liquid, and gas phases of a substance exist at the same time is called the

a)

Critical point

b)

Triple point

c)

Melting point

d)

Boiling point

93.

What is the normal melting point of this substance?

a)

150°C

b)

100°C

c)

-50°C

d)

0°C

94.

Which letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

95.

What is true regarding CO2 for temperatures above 31°C?

a)

It does not exist

b)

It decomposes

c)

It cannot be condensed back into a liquid

d)

It is a plasma

96.

What is the normal melting point of this substance?

a)

40°C

b)

60°C

c)

100°C

d)

110°C

97.

What phase change occurs from F to E?

a)

Sublimation

b)

Deposition

c)

Melting

d)

Condensation

98.

The temperature and pressure at which the gas and liquid states of a substance become identical and form one phase is called the

a)

Critical point

b)

Triple point

c)

Melting point

d)

Boiling point

99.

What is the normal boiling point of this substance?

a)

40°C

b)

60°C

c)

100°C

d)

110°C

100.

What phase change occurs from C to D?

a)

Condensation

b)

Vaporization

c)

Melting

d)

Sublimation

101.

What phase would this substance be in at 0.5 atm of pressure and 100°C?

a)

Solid

b)

Liquid

c)

Gas

102.

What phase change occurs from E to C?

a)

Sublimation

b)

Freezing

c)

Melting

d)

Vaporization

103.

What phase would this substance be in at 1 atm of pressure and 80°C?

a)

Solid

b)

Liquid

c)

Gas

104.

Normal freezing/melting and boiling points occur at standard pressure, which is

a)

1 atm

b)

5 atm

c)

10 atm

d)

15 atm

105.

What is the normal boiling point of this substance?

a)

0°C

b)

100 °C

c)

-50°C

d)

150°C

106.

Which state of matter is shown?

a)

solid

b)

liquid

c)

gas

107.

What phase change is happening? (hint: solid to liquid)

a)

freezing

b)

condensation

c)

melting

d)

sublimation

108.

What phase change happens when dew forms on leaves? (hint: gas to liquid)

a)

freezing

b)

melting

c)

deposition

d)

condensation

109.

The phase change from liquid to gas is _________

a)

Melting

b)

Evaporation

c)

Deposition

d)

Condensation

110.

Phase change from liquid to solid is ___________.

a)

Freezing

b)

Melting

c)

Sublimation

d)

Condensation

111.

All phase changes need energy added or taken away.

a)

True

b)

False

112.

What happens to particles when they are heated?

a)

They stop moving

b)

They move closer together and compress

c)

They speed up and spread around

d)

They slow down and get closer

113.

Which points are the phase changes?

a)

A,C and E

b)

B and D

c)

A and C

d)

B and E

114.

At what point is the substance liquid?

a)

B

b)

A

c)

C

d)

D

115.

Which point shows evaporation or condensation driving a phase change?

a)

B

b)

E

c)

D

d)

A

116.

What does point B show?

a)

Melting and Freezing

b)

Condensation and Evaporation

c)

Sublimation

d)

Deposition

117.

The particles that make up a solid move _________________ than particle that make up a gas.

a)

More quickly

b)

More slowly

c)

Farther away

d)

In the same way

118.

During a phase change the temperature of a substance __________

a)

Stays constant

b)

Increases

c)

Decreases

d)

Vanishes

119.
In which region(s) does temperature remain constant?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
120.
In which region(s) does temperature increase?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
121.
In which region(s) of the graph does a phase change occur?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
122.
In which region(s) of the graph would the substance only be in one phase?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
123.
Describe the substance between letters C and D. 
a)
Gas
b)
Liquid
c)
Melting
d)
Evaporating
124.
Between which points is the substance changing its state of matter?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
125.

Thermal energy always moves:

a)

From a high temperature object to a lower temperature object.

b)

From a lower temperature object to a higher temperature object.

c)

From an object with lower kinetic energy to an object with higher kinetic energy.

d)

From an object of higher mass to an object of lower mass.

126.
The freezing and melting points of water are the same.
a)
True
b)
False
127.
What is water's freezing point?
a)
0 F
b)
32 C
c)
50 C
d)
0 C
128.
To determine the freezing and melting points use a 
a)
thermometer
b)
scale
c)
balance
129.
When does condensation happen?
a)
solid to liquid
b)
liquid to gas
c)
gas to liquid
d)
solid to gas
130.

Given the heating curve of a solid being heated at a constant rate, what is the boiling point of this substance?

a)

20°C

b)

50°C

c)

110°C

d)

170°C

131.

The melting point of the sample is

a)

-60 ºC

b)

-100 ºC

c)

60 ºC

d)

100 ºC

132.

NaCl(s) was heated up starting at an initial temperature of 0°C. The heating curve is shown in the picture. What is the melting point of this substance?

a)

0°C

b)

801°C

c)

1000°C

d)

1465°C

133.

Given the heating curve of water, what is happening to potential and kinetic energy during segment CD?

a)

the potential energy and kinetic energy both increase

b)

the potential energy increases while the kinetic energy decreases

c)

the potential energy is constant while the kinetic energy increases

d)

the potential energy increases while the kinetic energy is constant

134.

It is a type of homogeneous mixture that is made up of two or more substances.

a)

Solution

b)

Emulsion

c)

Suspension

d)

Colloid

135.

A __________mixture is a type of mixture with a uniform composition.

a)

homogenous

b)

heterogenous

c)

hypotonic

d)

hypertonic

136.

This is the substance that makes up the minority of the solution, or this is the part that is dissolved.

a)

SOLUTION

b)

SOLUTE

c)

SOLVENT

d)

SUSPENSION

137.

This is the substance that makes up the majority of the solution. This is the part where the solute is dissolved.

a)

SOLUTION

b)

SOLUTE

c)

SOLVENT

d)

SUSPENSION

138.

It is a type of solution into which gases can spontaneously mix in any proportion.

a)

SOLID SOLUTION

b)

LIQUID SOLUTION

c)

GASEOUS SOLUTION

d)

AQUEOUS SOLUTION

139.

It is a type of solution which are generally called alloys, where two or more metals are present.

a)

SOLID SOLUTION

b)

LIQUID SOLUTION

c)

GASEOUS SOLUTION

d)

AQUEOUS SOLUTION

140.

It is the most common and it can be obtained by the dissolution of a gaseous, liquid, or solid solute.

a)

SOLID SOLUTION

b)

LIQUID SOLUTION

c)

GASEOUS SOLUTION

d)

AQUEOUS SOLUTION

141.

#1

a)

Unsaturated

b)

Saturated

c)

Supersaturated

142.

#2

a)

Unsaturated

b)

Saturated

c)

Supersaturated

143.

#3

a)

Unsaturated

b)

Saturated

c)

Supersaturated

144.

When CH3OH is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

3

c)

4

d)

5

e)

6

145.

When KCl (potassium chloride) is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

6

146.
Which technique could increase or speed up the rate of dissolving?
a)
Allowing the mixture to settle
b)
Stirring the mixture
c)
Adding more powder
d)
Adding more water
147.
Colligative properties depend on the _________ of the solute but not the __________ of the solute.
a)
 concentration; identity
b)
identity; concentration
c)
reactivity; nature
d)
nature; reactivity
148.
When the temperature of matter 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
149.

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

a)

higher

b)

lower

150.
What is happening at the boiling point?
a)
liquid to gas
b)
gas to liquid
c)
solid to liquid
d)
liquid to solid
151.
When a solid reaches the temperatures of its ___, it can become a liquid.
a)
melting point
b)
freezing point
c)
boiling point
d)
density
152.

A substance has a melting point of -125 oC and a boiling point of -35 oC. What state is it at 15oC?

a)

Solid

b)

Liquid

c)

Gas

153.

Freezing point

a)

The classification of matter as a solid, a liquid, or a gas

b)

Physical change in matter from a gas to a liquid

c)

The temperature at which a substance changes states from a solid to a liquid

d)

The temperature at which a substance changes from a liquid to a solid

154.

The freezing point of water is...

a)

100oC

b)

0oC

c)

-10oC

d)

150oC

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