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Quarterly Exam #3

Total questions: 50

Worksheet time: 45mins

Name
Class
Date
1.

According to Table G, which substance forms an unsaturated solution when 80. grams of the substance are stirred into 100. grams of H2O at 10.°C?

a)

KNO3

b)

KI

c)

NH3

d)

NaCl

2.

Which compound becomes less soluble in water as the temperature of the solution is increased?

a)

HCl

b)

KCl

c)

NaCl

d)

NH4Cl

3.

An unsaturated aqueous solution of NH3 is at 90°C in 100. grams of water. According to Reference Table G, how many grams of NH3 could this unsaturated solution contain?

a)

5 g

b)

10 g

c)

15 g

d)

20 g

4.

When 5 grams of KCl are dissolved in 50. grams of water at 25°C, the resulting mixture can be described as

a)

heterogeneous and unsaturated

b)

heterogeneous and supersaturated

c)

homogeneous and unsaturated 

d)

homogeneous and supersaturated

5.

A solution contains 35 grams of KNO3 dissolved in 100 grams of water at 40°C. How much more KNO3 would have to be added to make it a saturated solution?

a)

29 g

b)

24 g

c)

12 g

d)

4 g

6.

A saturated solution of NaNO3 is prepared at 60.ºC using 100. grams of water. As this solution is cooled to 10.ºC, NaNO3 precipitates (settles) out of the solution. The resulting solution is saturated. Approximately how many grams of NaNO3 settled out of the original solution?

a)

46 g

b)

61 g

c)

85 g

d)

126 g

7.

According to Reference Table G, which solution is saturated at 30°C?

a)

12 grams of KClO3 in 100 grams of water

b)

12 grams of KClO3 in 200 grams of water

c)

30 grams of KClO3 in 200 grams of water

d)

30 grams of KClO3 in 100 grams of water

8.

A solution is formed by dissolving 45 grams of NH4Cl in 100 grams of H2O at 70ºC. Which statement correctly describes this solution?

a)

NH4Cl is the solute, and the solution is saturated.

b)

NH4Cl is the solute, and the solution is unsaturated.

c)

NH4Cl is the solvent, and the solution is saturated.

d)

NH4Cl is the solvent, and the solution is unsaturated.

9.

How many grams of KCl must be dissolved in 200 grams of water to make a saturated solution at 60°C?

a)

30 g

b)

45 g

c)

56 g

d)

90 g

10.

Which compound is insoluble in water?

a)

KOH

b)

NH4Cl

c)

Na3PO4

d)

PbSO4

11.

According to Table F, which substance is most soluble in water?

a)

AgCl

b)

CaCO3

c)

Na2CO3

d)

SrSO4

12.

According to Table F which compound is soluble in water?

a)

barium phosphate

b)

calcium sulfate

c)

silver iodide

d)

sodium perchlorate

13.

According to Table F, which of these salts is least soluble in water?

a)

LiCl

b)

RbCl

c)

FeCl2

d)

PbCl2

14.

According to your Reference Tables, which of these compounds is the least soluble in water?

a)

K2CO3

b)

KC2H3O2

c)

Ca3(PO4)2

d)

Ca(NO3)2

15.

According to your Reference Tables, which substance forms an saturated solution when 80 grams of the substance is dissolved in 100 grams of H2O at 10°C?

a)

KI

b)

NaNO3

c)

KNO3

d)

NaCl

16.

Based on Table S, an atom of which element has the strongest attraction for electrons in a chemical bond?

a)

Aluminum

b)

Chlorine

c)

Magnesium

d)

Sulfur

17.

Which diatomic molecule is formed when two atoms share six electrons?

a)

H2

b)

O2

c)

N2

d)

F2

18.

Based on Table S, an atom of which element has the strongest attraction for electrons in a chemical bond?

a)

Aluminum

b)

Chlorine

c)

Magnesium

d)

Sulfur

19.

Which symbol represents an atom in the ground state with the most stable electron configuration?

a)

B

b)

O

c)

Li

d)

Ne

20.

Which compound has the least ionic character?

a)

KBr

b)

HF

c)

MgO

d)

BrCl

21.

The bonds in BaO are best described as

a)

covalent, because valence electrons are shared

b)

covalent, because electrons are transferred

c)

ionic, because valence electrons are shared

d)

ionic because electrons are transferred

22.

Which property best accounts for the conductivity of metals?

a)

the relatively high first ionization energy

b)

the malleability of most metals

c)

the free electrons in the valence energy levels

d)

the filled inner electron energy levels

23.

The results of these tests suggest that

a)

both solids contain only ionic bonds

b)

both solids contain only covalent bonds

c)

Solid A contains only covalent bonds and solid B contains only ionic bonds

d)

Solid A contains only ionic bonds and solid B contains only covalent bonds

24.

Which phrase describes the distribution of charge and the polarity of a CH4 molecule?

a)

symmetrical and polar

b)

symmetrical and nonpolar

c)

asymmetrical and polar

d)

asymmetrical and nonpolar

25.

Based on bond type, which compound has the highest melting point?

a)

CH3OH

b)

C6H14

c)

CaCl2

d)

CCl4

26.

The liquids hexane and water are placed in a test tube. The test tube is stoppered, shaken, and placed in a test tube rack. The liquids separate into two distinct layers because hexane and water have different

a)

formula masses

b)

molecular polarities

c)

pH values

d)

specific heats

27.

What is the chemical formula for ammonium sulfide?

a)

(NH4)2S

b)

(NH4)2SO3

c)

(NH4)2SO4

d)

(NH4)2S2O3

28.

What is the name of PbO2

a)

Lead Oxide

b)

Lead (II) Oxide

c)

Lead (IV) Oxide

d)

Lead Hydroxide

29.

Which element consists of positive ions immersed in a "sea" of mobile electrons?

a)

Sulfur

b)

Nitrogen

c)

Calcium

d)

Chlorine

30.
2 CO (g) + O2(g) → 2 CO2 (g)
In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?
a)
0.178 L
b)
358.4 Liters
c)
704 grams
d)
0.36 grams
31.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
32.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
33.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
34.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
35.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
36.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
37.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
38.

Which of the following is an intramolecular force?

a)

hydrogen bonding

b)

covalent bonding

39.

Which intramolecular force has the greatest strength?

a)

ionic bond

b)

nonpolar covalent

c)

polar covalent

d)

metallic

40.

Which of these is the weakest intermolecular force?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

41.

Which intermolecular force do all molecules have?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

42.

Which intermolecular force requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

43.

Water's boiling point is significantly elevated due to this intermolecular force.

a)

hydrogen bonding

b)

ionic bonding

c)

covalent bonding

44.

Which type of intermolecular force does this molecular drawing best represent?

a)

dipole-dipole

b)

hydrogen bonding

c)

London dispersion forces

45.

Determine whether Al(OH)3 is soluble using Table F

a)

Soluble

b)

Insoluble

46.

Determine whether Na2SO4 is soluble or insoluble using Table F

a)

Soluble

b)

Insoluble

47.

Which substance is most soluble at 40 degrees Celsius?

a)

KCl

b)

KNO3

c)

NaCl

d)

NH3

48.
How many moles of HNO3 are needed to prepare 5L of a 2M solution? 
a)
10 mol
b)
2.5 mol
c)
0.4 mol 
d)
100 mol 
49.
This solution would be considered
a)
Unsaturated
b)
Supersaturated
c)
Saturated
d)
Undefined
50.

Based on Reference Table F, which of the following saturated solutions would be the least concentrated?

a)

sodium sulfate

b)

potassium sulfate

c)

copper (II) sulfate

d)

barium sulfate

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