Free Printable Unit 3 Exam 2 & 1

1.

When two samples of ideal gases have the same

______, their molecules must have the same ______.

(a)

2.

KMT

a)

Gases are all hard spheres

b)

They are small relative to size of system volume

c)

They undergo elastic collisions and don’t stick or react

d)

They have a T equal system T that gives all of them the same Ek

e)

They all have the same Ek, but Ek = 1⁄2 mv2 so they have different velocity as inverse square of mass

3.

$m_1v_1^2=m_2v_2^2$

(a)

4.

Ideal conditions:

a)

P is low so don't collide

b)

V is large so don't collide

c)

n is small so don’t collide

d)

T is large so don’t stick

e)

gases are small and nonpolar so don’t stick

5.

Van der Whalls equation for non-ideality

(no spaces inbetween)

(a)

6.

Gas X has a larger value than gas Y for the Van der

Waals constant "a". This indicates that

a)

1. The molecules of X have stronger

intermolecular attractions for each other than

the molecules of Y have for each other

b)

2. The molecules of X are larger than the

molecules of Y

c)

3. The molecules of gas X have a higher velocity

than the molecules of gas Y

d)

4. The molecules of has X repel other X

molecules

7.

a corrects

a)

stickiness

b)

size

c)

polarity

8.

b corrects

a)

stickiness

b)

size

c)

polarity

9.

Ideal Gases

a)

He

b)

H2

c)

H2O

d)

NH3

10.

Ideal Gases

a)

nonpolar

b)

small

c)

large

d)

polar

11.

Non-Ideal Gases

a)

He

b)

H2O

c)

NH3

d)

H

12.

Non-Ideal Gases

a)

large IMF (like H-bonding)

b)

non-polar

c)

large gases

d)

small

13.

Which of the following molecules would have the

largest a and b terms, respectively, in the Van der

Waals equation?

Kr, CCl4, C2H4 C3H8, C4H10

a)

1. CCl4 , C4H10

b)

2. C4H10, CCl4

c)

3. C4H10, Kr

d)

4. Kr, C3H8,

e)

5. CCl4, CCl4

14.

Inter-Molecular Forces

a)

dispersion

b)

covalent single

c)

dipole

d)

h-bonding

e)

covalent triple

15.

Intra-Molecular Forces

a)

dispersion

b)

covalent single

c)

dipole

d)

h-bonding

e)

covalent triple

16.

Which of the following molecules have

the largest intermolecular and

intramolecular forces, respectively?

C2H5OH, C2H4, C2H2, CHCl3

a)

1. C2H2, C2H2

b)

2. CHCl3, C2H4

c)

3. C2H5OH, CHCl3

d)

4. C2H5OH, C2H2

17.

Dispersion Force

a)

1

b)

5

c)

20

d)

400

18.

Dipole-Dipole

a)

1

b)

5

c)

20

d)

400

19.

H-Bond

a)

1

b)

5

c)

20

d)

400

20.

Single Covalent

a)

400

b)

600

c)

800

d)

20

21.

Double Covalent

a)

200

b)

400

c)

500

d)

600

22.

Triple Covalent

a)

800

b)

300

c)

600

d)

200

23.

occur from the instantaneous dipoles formed by

asymmetrically distributed electrons.

a)

Dipole-Dipole

b)

Dispersion

24.

occurs in all compounds but is the dominant force in

non-polar (symmetrical) molecules.

a)

dispersion

b)

h-bond

c)

dipole-dipole

25.

As molecules increase in size,

(a) forces can grow to allow liquids and solids to be formed.

26.

occur in molecules that have permanent

dipoles (polar compounds). The magnitude of these forces is related to the size of the permanent dipole ∑ ΔEN.

a)

Dispersion

b)

dipole-dipole

c)

h-bond

d)

ionic bond

27.

Dispersion (London) forces result from...

a)

1. The formation of a loose covalent linkage

between a hydrogen atom connected to a

very electronegative atom in a neighboring

molecule.

b)

2. Distortion of the electron cloud of an atom

or molecule by the presence of nearby

atoms or molecules

c)

3. Attraction between molecules in a liquid

and molecules or atoms in a solid surface

with which the liquid is in contact.

d)

4. Attractive forces between a molecule at the

surface of the liquid and those beneath it

which are not balanced by corresponding

forces from above.

e)

5. The balance of attractive and repulsive

forces between two polar molecules.

28.

In ranking : NH3, H2O, HF, the order is:

a)

NH3 < HF < H2O

b)

HF < NH3 < H2O

c)

H2O < HF < NH3

d)

NH3 < H2O < HF

29.

___ is the only __ bond. In contrast, OH shows up as multiple H-bonds in sugars which is why they are so sticky

(a)

30.

Down periodic table, larger compounds and more (a)

31.

Identify the dominant intermolecular force in the following species,

respectively: RbCl, C6H6 (benzene), HI, Fe2O3, CH2NH.

a) ionic forced

b) hydrogen bonding

c) dipole-dipole

d) instantaneous dipoles

a)

1. a, c, c, d, b

b)

2. c, d, a, a, b

c)

3. a, b, c, b, a

d)

4. a, b, d, a, c

e)

5. a, d, c, a, b

32.

(a)

33.

(a)

34.

(a)

35.

(a)

36.

Surface tension describes

a)

1. The inward forces that must be overcome in order to expand the surface area of a liquid.

b)

2. The forces of attraction between surface molecules of a solvent and the solute molecules.

c)

3. Adhesive forces between molecules.

d)

4. The forces of attraction between the surface of a liquid and the air above it

37.

A bulk phenomenon in which gas bubbles from

the vapor of the liquid form and the escape became the vapor

pressure of bubble > atm. pressure

a)

Boiling Point

b)

Surface Tension

c)

viscosity

d)

Vapor pressure

e)

Evaporation rate

38.

A surface phenomenon in which an inward

force reduces the surface area of liquid. This is why liquids like

H2O bead up on windrows in the rain.

a)

Boiling Point

b)

Surface Tension

c)

viscosity

d)

Vapor pressure

e)

Evaporation rate

39.

Surface phenomenon in which the liquid

climbs the walls of the container because of IMF.

a)

Capillary Action

b)

Surface Tension

c)

viscosity

d)

Vapor pressure

e)

Evaporation rate

40.

The tendency of a liquid to resist pouring because of

IMF attraction to bulk solution.

a)

Capillary Action

b)

Surface Tension

c)

viscosity

d)

Vapor pressure

e)

Evaporation rate

41.

The energy in IMF that must be overcome for a liquid on

the surface to vaporize.

a)

Capillary Action

b)

Surface Tension

c)

ΔHvap

d)

Vapor pressure

e)

Evaporation rate

42.

The pressure of the vapor above the surface

and is inversely related to IMF

a)

Capillary Action

b)

Surface Tension

c)

ΔHvap

d)

Vapor pressure

e)

Evaporation rate

43.

How quickly a liquid will vaporize. Increases

at IMF decreases.

a)

Boiling Point

b)

Surface Tension

c)

viscosity

d)

Vapor pressure

e)

Evaporation rate

44.

Rank the following compounds by boiling point, from lowest

to highest: HF, CH3F, H2O, NH3.

a)

1. CH3F < NH3 < HF < H2O

b)

2. HF < H2O < CH3F < NH3

c)

3. H2O < CH3F < NH3 < HF

d)

4. H2O < NH3 < CH3F < HF

45.

as MW increases, (a) increases

46.

ΔEN increases, IMF increases (ranking within buckets)

(a)

47.

follow charge density rules: NaCl < CaO < MgO (within bucket rankings)

(a)

48.

a)

Increases with IMF

b)

Decreases with IMF

49.

Decreases with IMF

a)

evaporation rate

b)

viscosity

c)

vapor pressure

d)

non-ideality

50.

Arrange

Al2O3, Nb, I2, C (s) (diamond)

In the order metallic solid, covalent network, covalent solid, ionic solid.

a)

1. Nb; C (s) diamond; I2; Al2O3

b)

2. Al2O3; C (s) (diamond); I2; Nb

c)

3. C (s) (diamond); Nb; Al2O3; I2

d)

4. Nb; I2; C (s) (diamond); Al2O3

51.

Cation

a)

positively charged

b)

negatively charged

52.

Anion

a)

positively charged

b)

negatively charged

53.

Elements found down and to the left on

table.

a)

Metal Solids

b)

Ionic Solids

c)

Covalent Network Solids

d)

Molecular Solids

54.

Combination of metal cation and nonmetal

anion to make a salt.

a)

Metal Solids

b)

Ionic Solids

c)

Covalent Network Solids

d)

Molecular Solids

55.

Found on right side of table. Long

chains of covalent bonded atoms:

a)

Metal Solids

b)

Ionic Solids

c)

Covalent Network Solids

d)

Molecular Solids

56.

Solids from IMF forming at low temperature.

These are the molecules you drew in unit 2

a)

Metal Solids

b)

Ionic Solids

c)

Covalent Network Solids

d)

Molecular Solids

57.

Solid Metals

a)

Fe

b)

Pb

c)

Na

d)

NaCl

e)

H2O

58.

Solid Ionic

a)

Fe

b)

CaO

c)

Na

d)

NaCl

e)

H2O

59.

Solid Covalent Network

a)

graphite

b)

cellouse

c)

Na

d)

Diamond

e)

H2O

60.

Solid Covalent Molecular

a)

graphite

b)

cellouse

c)

Frozen CO2

d)

Frozen H2O

e)

Pb

61.

Put the following compounds

LiF, HF, F2, NF3

In order of increasing melting points.

a)

F2, HF, NF3, LiF

b)

LiF, HF, NF3 , F2

c)

NF3 HF, F2 , LiF

d)

F2, NF3, HF, LiF

e)

LiF , NF3 HF, F2

62.

At a temperature of 300 K, all gases (like He, Ar, Kr)have ? average kinetic energies and they have ?

a)

different; the same diffusion rates

b)

different; different average velocities

c)

the same; the same diffusion rates 𝜈

d)

the same; the same average velocities

e)

the same; different average velocities

63.

At ___, gas molecules don't get to their speed invacuum because of ______.

(a)

64.

Typical values for gas _____ in a vacuum atroom temperature are ___ s of m/s

(a)

65.

a)

Will collide and result in small velocities

b)

Will collide and result in high velocity

c)

Will not collide

66.

a)

Will collide and result in small velocities

b)

Will collide and result in high velocity

c)

Will not collide

67.

a)

a) C

b)

b) Cannot be determined

c)

c) A

d)

d) B

68.

Which has the greatest mass?

a)

A

b)

B

c)

C

69.

Which has the smallest mass?

a)

A

b)

B

c)

C

70.

Inversely Related To Size

a)

speed

b)

effusion rate

c)

diffusion rate

d)

polarity

71.

Calculate the ratio of the rate of effusion of He to that of CO2 (at the same temperatures).

a)

1: $\sqrt{11}$

b)

11: 1

c)

$\sqrt{11}$ : 1

d)

1: $11^2$

e)

1:1

72.

The ratio of the rate is (a) to the masses.

73.

If the ratio is A to B

a)

$\left(\frac{B}{A}\right)^{\frac{1}{2}}$

b)

$\left(\frac{A}{B}\right)^{\frac{1}{2}}$

74.

If the ratio is B to A

a)

$\left(\frac{B}{A}\right)^{\frac{1}{2}}$

b)

$\left(\frac{A}{B}\right)^{\frac{1}{2}}$

75.

A gas has a volume of 9.0 L at a pressure of 1520 torr. If the pressure is decreases to 380 torr, what will be the new volume? (Assume the temperature remains constant.)

a)

2.3 L

b)

4.6 L

c)

0.28 L

d)

36 L

76.

Boyles Law

a)

P_1V_1=P_2V_2

b)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

c)

$P_1+P_2+P_3....$

77.

Charles Law

a)

P_1V_1=P_2V_2

b)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

c)

$P_1+P_2+P_3....$

78.

Daltons Law

a)

P_1V_1=P_2V_2

b)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

c)

$P_1+P_2+P_3....$

79.

A gas mixture is found to be 4 parts nitrogen, 1 part carbon dioxide, and 1 part oxygen. If the total system pressure is 2 atm, what is the partial pressure of nitrogen?

a)

4 atm

b)

0.33 atm

c)

0.66 atm

d)

1.33 atm

80.

Combined Gas Law

a)

P_1V_1=P_2V_2

b)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

c)

$P_1+P_2+P_3....$

d)

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

81.

What volume will 40.0 L of Heat 50.00°C and 1201 torr occupy at STP?

a)

2) 12.8 L

b)

3) 53.4 L

c)

4) 26.7 L

d)

5) 31.1 L

e)

1) 18.6

82.

Ideal Gas Law

a)

P_1V_1=P_2V_2

b)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

c)

$P_1+P_2+P_3....$

d)

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

e)

$\frac{PMW}{RT}$

83.

Molecular Weight

a)

P_1V_1=P_2V_2

b)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

c)

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

d)

$\frac{PMW}{RT}$

e)

$\frac{gRT}{PV}$

84.

The balanced reaction for the combustion of ethanol (MW = 46 g/mol) is: C2H5OH(g) + 3O2 (g) --> 2CO2 (g) + 3H2O(g) 92 grams of ethanol reacts to completion with 96 grams of oxygen at STP. What is the volume of the system after reaction?

a)

200 L

b)

66 L

c)

134 L

d)

112 L

85.

a)

a) 90 atm

b)

b) 6 atm

c)

c) 30 atm

d)

d) 3 atm

Unit 3 Exam 2 & 1

Total questions: 85

Worksheet time: 54mins

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