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2nd Semester Final Exam Review

Total questions: 61

Worksheet time: 2hrs 3mins

Name
Class
Date
1.
How many electrons are shared between two atoms that are triple bonded?
a)
6
b)
2
c)
4
d)
8
2.
The force of attraction between nonpolar molecules:
a)
Hydrogen Bonding
b)
Dipole - Dipole Forces
c)
LDF
d)
Ionic Forces
3.

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

4.

Predict the IMF

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

5.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
6.

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

a)

8

b)

4

c)

2

d)

3

7.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

8.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
9.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
10.
How many lone pairs are in this molecule's structure?
a)
6
b)
2
c)
0
d)
4
11.

Classify the following molecule.

a)

polar

b)

nonpolar

12.

Classify the following molecule.

a)

polar

b)

nonpolar

13.

Fill in the blank. (Copper has a charge of 2+)

Cu+ AgNO3 → Ag + _____

a)

Cu(NO3)2

b)

CuNO3

c)

CuAg

d)

Cu

14.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

15.

What type of reaction is this?

2 C6H14 + 19 O2 → 12 CO2 + 14 H2O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

16.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

17.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

18.
Balance the following equation:
____MgO + ____H2O → ____Mg(OH)2
a)
1,1,1
b)
1,2,2
c)
2,3,4
d)
2,2,2
19.
__Al + __Fe3N2 -->__AlN + __Fe
a)
already balanced
b)
4,2,4,6
c)
2,1,2,3
d)
1,2,1,3
20.
__H2O + __CO2 --> __C7H8 + __O2
a)
4,7,1,9
b)
4,7,1,7
c)
2,3,1,3
d)
already balanced
21.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

22.

How many molecules are there in 31.8 moles of water?

a)

5.28 x 10-23 molecules

b)

1.91 x 1025 molecules

c)

5.28x 10-25 molecules

d)

1.91 x 1023 molecules

23.

What is the mass in grams of 5.90 mol C8H18?

a)

0.0512g

b)

19.4g

c)

389g

d)

673g

24.

What is the percent composition of barium in BaCrO4?

a)

20.5%

b)

54.2%

c)

25.26%

d)

66.88%

25.

If 60.2 grams of Mg combine with 24.0 g of Cl to form a compound, what is the percent composition of Mg?

a)

28.50%

b)

41.37%

c)

60.33%

d)

71.50%

26.

Which of the following is needed to determine the molar mass of a molecule?

a)

Types of elements in the molecule

b)

Quantity of elements in the molecule

c)

Mass of the elements in the molecule

d)

All are correct and needed.

27.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
28.

What is the molar mass of AgF?

a)

514.9 g/mol

b)

99.7 g/mol

c)

126.87 g/mol

d)

198.8 g/mol

29.

Which compound below has the smallest molar mass?

a)

CO

b)

CO2

c)

H2O

d)

H2O2

30.

What is the mass of 1 mole of calcium carbonate, CaCO3?

a)

99.01 g

b)

100.09 g

c)

216.87 g

d)

84.09 g

31.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
32.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
33.

Which element in the compound potassium cyanide, KCN, has a percent composition of 60.97%?

a)

K

b)

C

c)

N

d)

None of the above

34.

How many grams of gold can be obtained from 1.33 g of Au2O3

a)

0.532 g Au

b)

1.19 g Au

c)

0.459 g Au

d)

0.789 g Au

35.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

36.

C2H6O

Which is the correct empirical formula

a)

CHO

b)

C2H6O

c)

C4H14O2

d)

None

37.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
38.

Given the following: 5.70% H, 60.33% O, and 33.97% C, determine the empirical formula.

a)

C2H5O4

b)

C3H5O4

c)

C3H6O4

d)

C3H5O3

39.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
40.

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

41.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
42.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
43.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
44.

Benzene (C6H6) burns in air according to the following equation shown below. How many moles of O2 are required to react with 0.14 mol of C6H6? 

2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g)

a)

0.55 mol O2

b)

1.5 mol O2

c)

1.1 mol O2

d)

0.85 mol O2

45.

The balanced equation for the decomposition of TNT, C7H5(NO2)3, is 

2 C7H5(NO2)3(s) → 7 C(s) + 7 CO(g) + 3 N2(g) + 5 H2O(l)

How many moles of Water would form if 6.39 mol of C7H5(NO2)3 react?

a)

10.7 mol H2O

b)

22.4 mol H2O

c)

13.5 mol H2O

d)

16.0 mol H2O

46.

Decomposition of NI3 produces nitrogen gas and iodine. How many grams of the reactant would be required to react completely to give 5.18 g of the iodine?

a)

5.37 g NI3

b)

10.33 g NI3

c)

8.76 g NI3

d)

11.20 g NI3

47.

The production of ethanol for use as a fuel can be accomplished through fermentation of glucose, a type of sugar: 

C6H12O6(s) → 2 CH3CH2OH(l) + 2CO2(g)

What mass of ethanol can be produced from the fermentation of 7.7 kg of glucose?

a)

3.9 kg CH3CH2OH

b)

1.8 kg CH3CH2OH

c)

2000 kg CH3CH2OH

d)

1.1 kg CH3CH2OH

48.

Consider the following reaction: 3 NO2(g) + H2O(l) → 2 HNO3(l) + NO(g) How many moles of the excess reactant remain if 4.00 moles of H2O and 10.00 moles of NO2 are mixed?

a)

6.00 mol H2O

b)

2.00 mol NO2

c)

0.67 mol H2O

d)

3.33 mol H2O

49.

What mass (in grams) of SF6 should be produced by the following reaction if 7.00 g of sulfur is mixed with 9.00 g of fluorine? S + 3 F2 → SF6

a)

24.0 g

b)

6.42 g

c)

16.0 g

d)

11.1 g

50.
What mass in (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?
a)
53.6
b)
1.44
c)
1.23
d)
34.5
51.

Calcium carbonate reacts with aqueous hydrochloric acid to form calcium chloride solution, water, and carbon dioxide gas in the following equation: CaCO3 (s) + 2 HCl --> CaCl2 (aq) + H2O (l) + CO2 (g) What volume (in mL) of 1.35 M HCl will be needed to completely react with 3.82 g of solid CaCO3?

a)

56.5 mL

b)

47.2 mL

c)

61.6 mL

d)

34.7 mL

e)

124 mL

52.
18.26 mL of a 1.50M hydrochloric acid reacts with magnesium hydroxide. Calculate the mass of magnesium hydroxide needed for the reaction. 
  Mg(OH)2  +  2 HCl  ->  2 H2O + MgCl2           
a)
4.68 g Mg(OH)2
b)
0.789 g Mg(OH)2
c)
0.0274 Mg(OH)2
d)
1.07 g Mg(OH)2
53.

A solution with a pH of 8.6 would be a(n)

a)

Acid

b)

Base

c)

Neutral

d)

Acid and Base

54.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
55.

This ion is responsible for the properties of acids

a)

Sodium ion

b)

Hydrogen ion

c)

Hydroxide ion

d)

Oxide ion

56.

This ion is responsible for the properties of bases

a)

Sodium ion

b)

Hydrogen ion

c)

Hydroxide ion

d)

Oxide ion

57.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

58.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

59.

The pH of a solution is 8.43. What is the [H3O+] concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

60.

If a solution has a pOH of 1 what is the pH? Is it an acid or base? (pick 2)

a)

acid

b)

base

c)

13

d)

1

e)

neutral

61.

If the [H3O+] of a solution is 6.8 x 10-8 M, the pH is

a)

7.17

b)

3.2 x 10-5

c)

7.2

d)

7.62

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