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Chem Unit 8 Review

Total questions: 40

Worksheet time: 45mins

Name
Class
Date
1.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

2.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

3.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

4.

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

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

5.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

6.

Intermolecular forces for: NH3

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

7.

Viscosity is

a)

the resistance to flow

b)

the resistance to spread out

c)

the ability to make sheets of metal

d)

the ability to make wire

8.

A weak IMF will result in a

a)

high melting point

b)

high viscosity

c)

high surface tension

d)

low surface tension

9.

Surface tension is the property of water in which...

a)

water molecules at the surface tend to stick together.

b)

water spills easily.

c)

water tends to be see-through.

10.

Molecules with strong attraction between themselves require __________ to separate than weakly attracted molecules.

a)

More energy

b)

Less energy

c)

No energy

d)

Nuclear energy

11.

the spontaneous rising of a liquid in a narrow tube

a)

Surface Tension

b)

Capillary Action

c)

Viscosity

d)

None of the above

e)

All of the above

12.

A hydrogen bond is a covalent bond. True or False

a)

True

b)

False, because it is ionic

c)

False because it has an intramolecular force

d)

False because it has an intermolecular force

13.
What is the formula for molarity?
a)
moles/grams
b)
moles/kilograms
c)
moles/milliliters
d)
moles/liters
14.
The ___ is the thing being dissolved
a)
solute
b)
solvent
15.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)

2 L

b)

3 L

c)

4 L

d)

6 L

16.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
17.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
18.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

19.

The part of the solution that is present in the greater amount and does the dissolving

a)

Solute

b)

Solvent

c)

Solution

d)

Solubility

20.

Able to be dissolved

a)

dissolvability

b)

Insoluble

c)

Soluble

d)

Unsaturated

21.

Unable to be dissolved

a)

dissolvability

b)

Insoluble

c)

Soluble

d)

Unsaturated

22.

A measure of the maximum amount of solute that will dissolve in a certain amount of solvent at a certain temperature and pressure

a)

Solution

b)

Solute

c)

Solvent

d)

Solubility

23.

When a solution can hold more solute because it currently contains less than the maximum amount for the solvent available.

a)

Concentration

b)

Saturated

c)

Supersaturated

d)

Unsaturated

24.

When a solution cannot hold anymore solute in a solvent at a given temperature and pressure

a)

Concentration

b)

Saturated

c)

Supersaturated

d)

Unsaturated

25.
Salt dissolves in water because
a)
The water molecules wiggle between the Na and Cl atoms
b)
Water gets warm and moves around too much
c)
The polar areas of water molecules stick to the Na and CL ions
26.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
27.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
28.

How does a solution become supersaturated?

a)

Vigorous stirring to dissolve more solute than usual.

b)

Heat the solution to increase the solute then let it cool.

c)

Add more solvent to lower the concentration.

d)

Keep pouring solute in the solvent until it goes in.

29.
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
30.

What happens along the AC line?

a)

Melting/Freezing

b)

Vaporizing/Condensing

c)

Vaporizing/melting

d)

freezing/condensing

31.

What happens along the BC line?

a)

Melting/Freezing

b)

Vaporizing/Condensing

c)

Vaporizing/melting

d)

freezing/condensing

32.

What is being measured on the y axis?

a)

Pressure

b)

Temperature

c)

Energy

d)

Mass

33.

What is being measured on the x axis?

a)

Pressure

b)

Temperature

c)

Energy

d)

Mass

34.

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

35.

What is the vaporization point of this substance at 1 atm?

a)

40°C

b)

60°C

c)

100°C

d)

110°C

36.

Which end of the water molecule would surround a Cl- ion in a solution

a)

the Oxygen end

b)

the Hydrogen end

c)

neither end

d)

they don't surround the ion

37.

When water molecules completely surround ions or covalent molecules, they form what around them to keep them apart?

a)

hydration shells

b)

a polar bond

c)

an invisible force field

d)

a hydrogen bond

38.

Determine if the compound is soluble or insoluble:

NaOH

a)

Soluble

b)

Insoluble

39.

Determine if the compound is soluble or insoluble:

Hg2SO4

a)

Soluble

b)

Insoluble

40.

In the following equation, determine which compound is insoluble:

CdSO4        + K2S        → K2SO4        + CdS

a)

CdSO4 (s)

b)

K2S (s)

c)

K2SO4 (s)

d)

CdS (s)

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