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HPC Unit 2 Part 1 Final Review

Total questions: 131

Worksheet time: 3hrs 5mins

Name
Class
Date
1.

What below is NOT considered matter?

a)

Carbon atoms

b)

Gravity

c)

Bacteria

d)

Air

2.

Matter is anything that.....

a)

Has mass and takes up space

b)

Has mass and is visible

c)

Takes up space and has energy

d)

Has energy and is visible

3.

What particle view below is a mixture?

a)

b)

c)

d)

4.

What is the best classification for this substance?

a)

An element

b)

A compound

c)

A mixture

5.

Is this a pure substance?

a)

Yes

b)

No

6.

What is the best classification of this substance?

a)

An element

b)

A compound

c)

A mixture of 2 elements

d)

A mixture of 2 compounds

7.

What is the best classification of this substance? H2SO4

a)

An element

b)

A compound

c)

A mixture

8.

What is the best classification of this substance? CO2 & H2S

a)

An element

b)

A compound

c)

A mixture of 2 compounds

d)

A mixture of many elements

9.

How would you name this sample? T = triangle, Sq = square, C = circle.

a)

T + Sq + C

b)

TC + Sq

c)

TC4 + Sq3

d)

TCSq

10.

What is an example of a physical property?

a)

Silver is shiny

b)

Alcohols are flammable

c)

Alkali metals are reactive with water

d)

Acids are sometimes corrosive

11.

What is an example of a chemical change?

a)

Tearing paper

b)

Dissolving salt in water

c)

Melting ice

d)

Burning wood

12.

Does this particle view show an element or a compound?

a)

element

b)

compound

13.

Is this image showing a homogeneous or a heterogeneous mixture? Image: Cesar salad

a)

homogeneous

b)

heterogeneous

14.

Is this image showing a homogeneous or a heterogeneous mixture? Image: Milk

a)

homogeneous

b)

heterogeneous

15.

Does this image represent a chemical or a physical change?

a)

Chemical change

b)

Physical change

16.

Does this image represent a chemical or physical change?

a)

Chemical change

b)

Physical change

17.

Which below shows a CHEMICAL change?

a)

b)

c)

18.

How many different TYPES of ATOMS are in this image?

a)

1

b)

2

c)

3

d)

4

19.

How many TOTAL MOLECULES are in this image?

a)

4

b)

5

c)

15

d)

2

20.

How many different TYPES of MOLECULES are in this image?

a)

1

b)

2

c)

4

d)

5

21.

Suppose you have two gases numbered 1 and 2.

Which equation represents make the most sense to calculate the total pressure exerted by both gases?

a)

Multiply their pressures :

Ptotal = P1 × P2

b)

Divide their pressures :

Ptotal = P1 ÷ P2

c)

Add their pressures :

Ptotal = P1 + P2

d)

Subtract their pressures :

Ptotal = P1 – P2

e)

Average their pressure :

Ptotal = (P1 + P2)/2

22.

A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?

a)

900 atm

b)

0.90 atm

c)

9.00 atm

d)

920 atm

23.

A container holds a mixture of two different gases. The oxygen in a container exerts 80 mmHg of pressure on the inside of the container. The total pressure inside the container is 120 mmHg. What is the pressure of the other gas in the container?

a)

200 mmHg

b)

80 mmHg

c)

40 mmHg

d)

120 mmHg

24.

Three gases, Ar, N2 and H2 are mixed in a 500 L container. Ar has a pressure of 30 torr, N2 has a pressure of 40 torr and H2 has pressure of 60 torr.

What is the total pressure in the container?

(a)  

25.

A gas container contains hydrogen gas and water vapor. The pressure of the water is 20 torr. If the total pressure is measured to be 750 torr, what is the pressure of only the hydrogen gas?

a)

770 torr

b)

730 torr

c)

37.5 torr

d)

15,000 torr

26.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
27.
Three gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?
a)
483torr
b)
270torr
c)
1235torr
28.

P1 is 450mmHg and the Ptotal is 750mmHg. What is the pressure of the second gas, P2?

a)

200mmHg

b)

300mmHg

c)

450mmHg

d)

750mmHg

29.

What is the partial pressure of O2 in air at a total atmospheric pressure of 97.8 kPa, given that air is about 21% oxygen?

a)

22 kilopascals

b)

19.8 kilopascals

c)

21.5 kilopascals

d)

20.5 kilopascals

30.

What is the vapor pressure of water at 19 degrees Celsius?

a)

4.2 kilopascals

b)

1.2 kilopascals

c)

2.2 kilopascals

d)

3.2 kilopascals

31.

In a gas mixture, the partial pressure of oxygen is 15\frac{1}{5} of the total pressure which is 100 kPa. What is the partial pressure of oxygen?

a)

20 kPa

b)

50 kPa

c)

5 kPa

d)

25 kPa

32.

A mixture of nitrogen and oxygen gas has a total pressure of 4.2 atm. If 4/7 of the mixture is N2, what is the partial pressure of O2?

a)

2.4 kPa

b)

2.4 atm

c)

1.8 kPa

d)

1.8 atm

33.

A mixture of two gases with a total pressure of 520 mmHg is enclosed in a sealed container. If 70% of the mixture is NO2, what is the partial pressure of the other gas?

a)

520 mmHg

b)

364 mmHg

c)

156 mmHg

34.

A sample of four mixed gases is at 760 mmHg. The partial pressures of gases A= 14. 8% and B = 41.6%. If gases C and D have equal partial pressures, what is the partial pressure of gas C?

a)

331.36 mmHg

b)

165.68 mmHg

c)

428.64 mmHg

35.
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
36.

When collecting a gas over water, the total pressure in the column is equal to the pressure of the collected gas ___

a)

plus atmospheric pressure

b)

minus atmospheric pressure

c)

plus the vapor pressure of the water

d)

minus the vapor pressure of the water

37.

The vapor pressure of water, which is the partial pressure of water vapor in the gas above it, is dependent on ___

a)

the total pressure

b)

the molar mass of water

c)

the volume of the water

d)

the temperature of the water

38.

The ratio of moles of the individual gases in a mixture to the total number of moles is called ___

a)

fractional molarity

b)

fractional distillation

c)

the mole fraction

d)

the empirical formula

39.
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
40.

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

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

41.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

42.

Intermolecular forces for: NH3

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

43.

Intermolecular forces for: CO2

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

44.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

45.

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

a)

higher

b)

lower

46.

Which molecule: Br2, HCl, H2S, or NH3, will most likely have London dispersion forces as the MOST important IMF considered when determining melting/boiling points?

a)

Br2, it only has dispersion forces when interacting

b)

HCl, it can participate in dipole-dipole interactions and also dispersion forces

c)

H2S, it can participate in dipole-dipole interactions and also dispersion forces

d)

NH3, it can participate in hydrogen bonding and also dispersion forces

47.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

48.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
49.

Which of the following will have the lowest melting point?

a)
b)
c)
d)
50.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
51.

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

52.
Does HF have hydrogen bonding?
a)
yes
b)
no
53.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
54.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

55.

Which of these is not an intermolecular force?

a)

covalent bonding

b)

London dispersion forces

c)

hydrogen bonding

d)

dipole-dipole forces

56.

Hydrogen bonding is a special type of what force?

a)

London dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

covalent force

57.

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

58.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
59.
What will be the state of the following molecule?
a)
gas
b)
liquid
c)
solid
60.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
61.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
62.
The physical separation of mixtures into individual components is..
a)
chromatography
b)
opacity 
c)
latent
d)
trace evidence 
63.
Two or more substances that are mixed together but not chemically combined is a ___
a)
compound
b)
mixture
c)
keratin
d)
chromatography
64.
Two or more substances that are chemically combined is a ___
a)
compound
b)
mixture
c)
solvent
d)
solute
65.

Ink can be separated by a method of -----------------------------------------------

a)

distillation

b)

filtration

c)

chromatography

d)

sedimentation

66.
chromatography separates the mixture of dyes on the basis of their ----------------------------
a)
density
b)
solubility
c)
gravity
d)
boiling point
67.
On the chromatogram given -------------- is mixture.
a)
red
b)
orange
c)
green
d)
black
68.
A pure substance shows ------------------ spot on chromat gram
a)
0
b)
1
c)
2
d)
3
69.
Dyes in water soluble markers may be separated by means of..
a)
crystallization
b)
sublimation
c)
chromatography
d)
sedimentation
70.
A student extracts the colour from some green smarties and uses paper chromatography to separate components colours. She finds blue has a Rf =0.38 and yellow Rf =0.75 this suggests 
a)
the yellow is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
b)
the yellow is more strongly adsorbed onto the stationary phase and is more soluble in the mobile phase.
c)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
d)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
71.
A high Rf value indicates strong
a)
strong affinity to the stationary phase
b)
strong affinity to the mobile phase
c)
no affinity to the stationary phase
d)
 no affinity to the stationary phase
72.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3
73.
The Rf value  for the red component is 
a)
0.3
b)
0.7
c)
10
d)
7
74.
Which plant species has plant pigments most similar to those in A?
a)
B
b)
C
c)
D
75.

What is chromatography?

a)

A way to see pretty colors

b)

A laboratory technique used to separate a mixture.

c)

A form of distillation

76.
Why must the base line be drawn in pencil and not pen?
a)
a) Pencil is good at keeping substances in place.
b)
b) Pencil is soluble in water
c)
c) Pencil is insoluble in water
d)
d) Pencil is not coloured
77.

In paper chromatography, the LEAST soluble solute ____.

a)

does not move from the start point

b)

stays closest to the start point

c)

travels furthest away from the start point

d)

can be found in the middle of the chromatogram

78.
In chromatography, if a solute does not separate and remains on the start line ....
a)
the solute is insoluble in the solvent
b)
the solute is soluble in the solvent
c)
the solvent is insoluble in the solute
d)
the solvent is soluble in the solute
79.
Whose blood was found at the crime scene?
a)
John
b)
Lisa
c)
Bob
d)
Sure
80.

Here is chromatography of markers with the paper placed in water. What is true.

a)

Blue dissolves best in water.

b)

Yellow dissolves best in water.

c)

Green dissolves best in water.

d)

Pink dissolves best in water

81.

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

82.

How many valence electrons does Helium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

83.

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

84.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
85.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
86.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
87.
This is a correct dot diagram for nitrogen (N)
a)
true
b)
false
88.
This is a correct dot diagram for carbon (C)
a)
true
b)
false
89.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
90.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
91.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
92.
This is a correct dot diagram for magnesium (Mg)
a)
true
b)
false
93.

Which of these is incorrect?

a)
b)
94.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
95.

This is a Bohr Diagram of Neon. How many valence electrons does Neon have?

a)

2

b)

4

c)

6

d)

8

96.

This is a Bohr Diagram of Helium. How many valence electrons does Helium have?

a)

2

b)

4

c)

6

d)

8

97.

This is a Bohr Diagram of Aluminum. How many valence electrons does Aluminum have?

a)

3

b)

4

c)

5

98.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
99.

Which of these is correct?

a)
b)
c)
100.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
101.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
102.

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

a)

8

b)

4

c)

2

d)

3

103.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
104.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

105.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

106.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

107.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

108.

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

a)

Single

b)

Double

c)

Triple

109.

CHCl3 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

110.

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

111.

Which of the following elements are an exception to the octet rule and require less than 8 valence electrons?

a)

H

b)

Li

c)

Be

d)

B

e)

C

112.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

113.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

114.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
115.

Why is the molecule polar?

a)

There is a non bonding pair electrons on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no non bonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

116.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

117.

Classify the above molecule.

a)

Polar

b)

Non polar

118.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
119.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
120.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
121.

What is the molecular geometry for this molecule?

a)

Bent

b)

Trigonal pyramidal

c)

Trigonal planar

d)

Linear

122.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
123.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
124.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
125.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
126.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
127.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
128.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

129.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

130.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

131.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

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