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Semester 2 H. Chem Final Exam Review 2021/22

Total questions: 85

Worksheet time: 21hrs 15mins

Name
Class
Date
1.
The name of Al₂(SO₄)₃ is
a)
aluminum sulfur oxide
b)
aluminum sulfate
c)
aluminum trisulfate
d)
aluminum (III) sulfate
2.
The name of Fe(OH)₂ is
a)
iron oxide
b)
iron hydroxide
c)
iron (II) hydroxide
d)
iron dihydroxide
3.
The chemical formula of sodium sulfate is
a)
S₂SO₄
b)
NaSO₂
c)
NaSO₄
d)
Na₂SO₄
4.

What is the formula for magnesium carbonate?

a)
MgCO3
b)
Mg(CO3)2
c)
Mg2CO6
d)
Mg2CO3
5.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
6.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
7.

What is the formula for tricarbon octahydride?

a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
8.

The formula for phosphorous trichloride is

a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
9.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

10.

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

11.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

12.

In water, the __ is negative since it ________.

a)

Hydrogen ; has a large gravitational pull

b)

Hydrogen ; out numbers the oxygen

c)

Oxygen ; has the greatest electronegativity

d)

Oxygen ; has the greatest gravitational pull

13.
Which molecule contains bonds of GREATER polarity?
a)

H2O

b)

OF2

14.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Nonpolar

c)

Ionic

15.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Nonpolar

c)

Ionic

16.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

17.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
18.

What is the correct Lewis Structure for ammonia NH3?

a)
b)
c)
d)
19.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

20.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

21.

What two types of atoms that make up a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

22.

Compounds composed of a ______________ and _____________ like the compound CaCl2 , are ionic compounds.

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

23.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
24.

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

25.

What explains the very high melting and boiling point of water?

a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
26.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

27.

Which of the following molecules does NOT have a linear shape?

a)

CS2

b)

HCN

c)

OF2

d)

BeF2

28.

What is the shape of a CH2Cl2 molecule?

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Octahedral

29.

What shape is this molecule, and what bond angle?

a)

linear, 180o

b)

bent, 120o

c)

bent, 109o

d)

trigonal planar, 120o

30.

What shape is this molecule, and what bond angle?

a)

bent, 120o

b)

bent, 109o

c)

trigonal planar, 1200

d)

trigonal pyramid, 109o

31.

The pH value of an acid is

a)

Less than 7

b)

Equal to 7

c)

More than 7

d)

Either less than 7 or more than 7

32.

One property of sodium hydroxide is that it

a)

Turns blue litmus paper red

b)

Turns red litmus paper blue

c)

reacts with metals to produce H2 gas

d)

does not conduct electricity

33.

When an indicator is added to solutions of different pH values, it should show a change in

a)

Color

b)

Volume

c)

State

d)

Smell

34.

When phenolphthalein is added to an alkaline (or basic) solution , it turns

a)

White

b)

Colorless

c)

Pink

d)

Green

35.

A neutralization reaction will produce...

a)

water & a salt

b)
water
c)

a salt

d)
water & carbon
36.

Which of these formulas represents an acid?

a)

HNO3

b)

Ba(OH)2

c)

H2O

d)

Ba(NO3)2

37.

Which of the following correctly describes an ACID?

a)

feels slippery

b)

contains a hydroxide ion(OH-)

c)

has a bitter taste

d)

forms hydrogen ions when dissolved in water (H+)

38.

Conducts electricity (has electrolytes)

a)

acid

b)

base

c)

both an acid and a base

39.

According to Arrhenius, what is the definition of an ACID?

a)

a substance that contains hydroxide and ionizes to produce OH-

b)

a substance that contains hydrogen and ionizes to produce H+

c)

a substance that contains hydrogen and ionizes to produce OH-

d)

a substance that contains hydroxide and ionizes to produce H+

40.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

41.
A hydrogen ion, H+, is the same as a(n):
a)

neutron

b)

electron

c)

proton

d)

hydroxide ion

42.

A Bronsted Lowry acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

43.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

44.

In the equation below, what is the Bronsted Lowry acid?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

45.

In the equation below, what is the Bronsted Lowry base?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

46.

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

47.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
48.
The conjugate acid of HCO3- is ___ and the conjugate base of HCO3- is ___.  (remember that H+ ion? well, follow it!!)
a)
H2CO3; CO3-2
b)
CO3-2; CO3-2
c)
H2CO3; H2O
d)
H2O; H2CO3
49.
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
50.
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
51.
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
52.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
53.
How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 
a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
54.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

55.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
56.
Identify the products of the chemical equation
3 LiOH + H3PO4 →
a)
Li3PO4 + 3 H2O
b)
LiPO4 + 3 H2O
c)
Li(PO4)3 + 3 H2O
d)
BOY + La + N2
57.

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

58.

If the [H+] 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

59.

If the [H+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

60.

If a solution has a pOH of 3.7 the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

61.

Oranges have a [H+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

62.

Which of the following would result in being able to dissolve a greater amount of gas in a solution? (CHOOSE ALL THAT APPLY)

a)

Lower the temperature

b)

Decrease the pressure

c)

Stir the solution.

d)

Increase the pressure.

63.

What are the factors that increase solubility of solid particles in liquid?

a)

increased rate of stirring

b)

smaller particle size

c)

higher temperature

d)

all of these

64.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
65.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
66.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
67.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
68.

Solution is a/an __________________.

a)

Compound

b)

Heterogeneous Mixture

c)

Element

d)

Homogeneous Mixture

69.

Which of the following types of solutions is likely to produce crystals if disturbed?

a)

Supersaturated

b)

Unsaturated

c)

Solubility

d)

Saturated

70.

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

71.

5.11 x 1023 atoms of lithium (Li) is equal to how many moles?

a)

1.18 moles

b)

0.351 moles

c)

1.34 moles

d)

0.849 moles

72.

How many atoms are present in 5.00 g of Fe?

a)

0.0895 atoms

b)

3.36×10183.36\times10^{18} atoms

c)

1.88×10211.88\times10^{21} atoms

d)

5.39×10225.39\times10^{22} atoms

73.

What is the percent composition of benzene, C6H6?

a)

C = 50.%

H = 50.%

b)

C = 85.7 %

H = 14.3%

c)

C = 92.2%

H = 7.8%

d)

C = 71.9%

H = 28.1%

74.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
75.

4NH3 + 5O2-->4NO + 6H2O

What is the mole ratio of H2O to NH3?

a)

3:1

b)

3:2

c)

2:1

d)

1:3

76.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
77.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
125.2 g O2
78.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
79.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
80.

3NH4NO3 + Na3PO4 --> (NH4)3PO4 + 3 NaNO3

Assuming we start with 30 g of NH4NO3 and 50 g of Na3PO4, identify the limiting reactant. (HINT: solve for one of the products to compare answers)

a)

ammonium phosphate

b)

sodium phosphate

c)

ammonium nitrate

d)

sodium nitrate

81.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

82.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
83.

Using the balanced chemical equation:

4NH3 + 3O2 --> 2N2 + 6H2O


Determine the amount of grams of N2 is produced if 4.03 moles of NH3 react?

a)

28.0 g N2

b)

56.4 g N2

c)

2.02 g N2

84.
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
85.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
a)
15
b)
18
c)
20
d)
24

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