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AP Chem Unit 4: Review

Total questions: 100

Worksheet time: 2hrs 40mins

Name
Class
Date
1.

Which of the following represents the net ionic equation for the precipitation reaction between sodium carbonate and magnesium sulfate?

a)

Na2CO3 + MgSO4 --> MgCO3 + Na2SO4

b)

2Na+ + CO3-2 + Mg+2 + SO4-2 --> Mg+2 + CO3-2 + 2Na+ + SO4-2

c)

2Na+ + SO4-2 --> Na2SO4

d)

CO3-2 + Mg+2 --> MgCO3

2.

Which of the following represents the net ionic equation for the precipitation reaction between sodium phosphate and lead (II) acetate?

a)

2Na3PO4+ 3Pb(C2H3O2)2 --> Pb3(PO4)2 + 6NaC2H3O2

b)

6Na+ + 2PO4-3 + 3Pb+2 + 3C2H3O2-1 --> Pb3(PO4)2 + 6NaC2H3O2

c)

2PO4-3 + 3Pb+2 --> Pb3(PO4)2

d)

Na+ + C2H3O2-1 --> NaC2H3O2

3.

Chemical or physical change? 2 H2O(l) + O2(g) → 2 H2O2(l)

a)

Chemical

b)

Physical

4.

Chemical or physical change? H2O(l) → H2O(g)

a)

Chemical

b)

Physical

5.

Physical changes occur when...

a)

bonds are broken and formed

b)

a different phase appears in the product side

6.

Chemical changes occur when...

a)

bonds are broken and formed

b)

a different phase appears in the product side

7.

Which observation suggests a physical change occurred?

a)

The shape of an object changed

b)

Color change

c)

Clear solutions turn cloudy

8.

Which observation suggests a chemical change occurred?

a)

The mass stays constant

b)

The solution stays colorless

c)

A precipitate forms

9.

Which observation suggests a chemical change occurred?

a)

Change in total volume

b)

Change in temperature

c)

Change in total pressure

10.

Boiling is an example of a __________

a)

Physical change because bonds are broken

b)

Physical change because IMFs are overcome

c)

Chemical change because bonds are broken

d)

Chemical change because IMFs are overcome

11.

What represents the net ionic equation for the reaction that occurs when the solutions of sodium carbonate and calcium nitrate are combined?

a)

Na2CO3 + Ca(NO3)2 --> 2NaNO3 + CaCO3

b)

2Na+ + CO3-2 + Ca+2 + 2NO3-1 --> 2NaNO3 + CaCO3

c)

Na+ + NO3-1 --> NaNO3

d)

CO3-2 + Ca+2 --> CaCO3

12.

A precipitation reaction must...

a)

Have a solid ionic product from aqueous reactants

b)

Have only gaseous products from gaseous reactants

c)

Have only aqueous products from aqueous reactants

13.

In order to be considered an oxidation-reduction reaction,

a)

a precipitate must form

b)

the oxidation number of two species must change

c)

the pH must change

14.

In order to be considered an acid-base reaction,

a)

a precipitate must form

b)

the oxidation number of two species must change

c)

one or more protons must be transfered

15.

In a combustion reaction,

a)

oxygen must be a reactant and carbon dioxide and water are products

b)

carbon dioxide and water are reactants and oxygen must be a product

16.

In a redox reaction, electrons are

a)

transferred from the species that's reduced to the species that's oxidized

b)

transferred from the species that's oxidized to the species that's reduced

17.

What acronym can we use to remember soluble ions?

a)

LEO says GER

b)

SPAN

c)

OIL RIG

d)

BAAD

18.

An acid is defined as a...

a)

proton donor

b)

proton acceptor

19.

An base is defined as a...

a)

proton donor

b)

proton acceptor

20.

In this example, H+ + H2O -> H3O+ the water acts as a(n)

a)

acid donating a proton

b)

acid accepting a proton

c)

base donating a proton

d)

base accepting a proton

21.

In the following example, CH3CH2COOH(aq) + H2O(l) ⇄ CH3CH2COO-(aq) + H3O+(aq) what would be considered a conjugate acid-base pair?

a)

CH3CH2COOH(aq) and H2O(l)

b)

CH3CH2COO-(aq) and H3O+(aq)

c)

CH3CH2COO-(aq) and CH3CH2COOH(aq)

d)

CH3CH2COOH(aq) and H3O+(aq)

22.

Which of the following represent a Brønsted-Lowry conjugate acid-base pair?

a)

HF and H2O

b)

NaOH and H2O

c)

HF and NaOH

d)

HF and F-

23.

Which of the following represent a Brønsted-Lowry conjugate acid-base pair

a)

HCN and H2O

b)

H3O+ and CN-

c)

CN- and H+

d)

HCN and CN-

24.

Given this general acid-base reaction HA + B- --> A- + HB, if K>0, which acid is stronger?

a)

HA

b)

HB

25.

Given this general acid-base reaction HA + B- --> A- + HB, if K<0, which base is stronger?

a)

A-

b)

B-

26.

Given the following: NH3(aq) + HCl(aq) ⇄ NH4+(aq) + Cl-(aq)

The Brønsted-Lowry acids in the reaction represented above are

a)

NH3(aq) and NH4+(aq)

b)

HCl(aq) and NH4+(aq)

c)

HCl(aq) and Cl-(aq)

d)

NH3(aq) and HCl(aq)

27.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
28.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
29.
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)
30.
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) →
31.
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
32.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
33.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
34.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
35.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
36.
Which statement is true:
Mg → Mg2+ + 2e–
a)
Mg gains 2 electrons
b)
Mg2+ loses 2 electrons
c)
Mg loses 1 electron
d)
Mg loses 2 electrons
37.

What is the oxidation number assigned to manganese in KMnO4?

a)

+7

b)

+2

c)

+4

d)

+3

38.

- What is the oxidation number of chromium in K2Cr2O7

a)

+6

b)

+3

c)

+5

d)

+2

39.

Which half-reaction correctly represents reduction?

a)

S2– → S + 2e–

b)

Mn7+ → Mn4+ + 3e–

c)

Mn7+ + 3e– → Mn4+

d)

S2– + 2e– → S

40.

Chemical or physical change? 2 H2O(l) + O2(g) → 2 H2O2(l)

a)

Chemical

b)

Physical

41.

Chemical or physical change? H2O(l) → H2O(g)

a)

Chemical

b)

Physical

42.

Which observation suggests a chemical change occurred?

a)

The mass stays constant

b)

The solution stays colorless

c)

A precipitate forms

43.

In order to be considered an oxidation-reduction reaction,

a)

a precipitate must form

b)

the oxidation number of two species must change

c)

the pH must change

44.

In order to be considered an acid-base reaction,

a)

a precipitate must form

b)

the oxidation number of two species must change

c)

one or more protons must be transfered

45.

An acid is defined as a...

a)

proton donor

b)

proton acceptor

46.

An base is defined as a...

a)

proton donor

b)

proton acceptor

47.

In this example, H+ + H2O -> H3O+ the water acts as a(n)

a)

acid donating a proton

b)

acid accepting a proton

c)

base donating a proton

d)

base accepting a proton

48.

Given the following: NH3(aq) + HCl(aq) ⇄ NH4+(aq) + Cl-(aq)

The Brønsted-Lowry acids in the reaction represented above are

a)

NH3(aq) and NH4+(aq)

b)

HCl(aq) and NH4+(aq)

c)

HCl(aq) and Cl-(aq)

d)

NH3(aq) and HCl(aq)

49.

Balance this equation:


____ Zn + _____HCl → _____ ZnCl2 + _______H2

a)

1,2,1,2

b)

2,1,1,2

c)

1,2,1,1

d)

1,3,1,2

50.

____ Zn + _____HCl → _____ ZnCl2 + _______H2


If 70.50 g of Zn and 71.65 g of HCl are combined, what is the limiting reactant?

a)

Zn limits

b)

HCl limits

c)

ZnCl2 limits

d)

H2 limits

51.

____ Zn + _____HCl → _____ ZnCl2 + _______H2


If 70.50 g of Zn and 71.65 g of HCl are combined, what is the maximum mass of zinc chloride that can be produced?

a)

133.9 g ZnCl2

b)

131.8 g ZnCl2

c)

146.9 g ZnCl2

d)

267.83 g ZnCl2

52.

____ Zn + _____HCl → _____ ZnCl2 + _______H2


If the reaction is done in a lab and 125.6 g of zinc chloride are produced, what is the percent yield?

a)

85.50%

b)

93.80%

c)

95.29%

d)

46.90%

53.

____ Zn + _____HCl → _____ ZnCl2 + _______H2


If 70.50 g of Zn and 71.65 g of HCl are combined, how many moles of the excess reactant are left over?

a)

0.3251 mol H2

b)

0.9826 mol Zn

c)

1.078 mol Zn

d)

0.095 mol Zn

54.

_____HCl + ____ Mg → _____ MgCl2 + _______H2

If 69.75 g of Mg and 70.25 g of HCl are combined, what is the limiting reactant?

a)

HCl limits

b)

Mg limits

c)

MgCl2 limits

d)

H2 limits

55.

_____HCl + ____ Mg → _____ MgCl2 + _______H2

If 69.75 g of Mg and 70.25 g of HCl are combined, what is the maximum mass of magnesium chloride that can be produced?

a)

273.2 g MgCl2

b)

91.72 g MgCl2

c)

183.4 g MgCl2

d)

136.6 g MgCl2

56.

_____HCl + ____ Mg → _____ MgCl2 + _______H2

If the reaction is done in a lab and 84.6 g of magnesium chloride is produced, what is the percent yield?

a)

30.97%

b)

46.13%

c)

92.24%

d)

61.93%

57.

_____HCl + ____ Mg → _____ MgCl2 + _______H2

If 69.75 g of Mg and 70.25 g of HCl are combined, how many moles of the excess reactant are left over?

a)

2.869 mol Mg

b)

1.906 mol Mg

c)

0.9634 mol HCl

d)

1.927 mol HCl

58.

Balance this equation:


_____HCl + ____ Mg → _____ MgCl2 + _______H2

a)

2,1,1,1

b)

2,2,1,1

c)

2,4,1,2

d)

1,2,1,3

59.
Oxygen always has an oxidation number of...
a)
-1
b)
1
c)
2
d)
-2
60.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
61.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
62.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
63.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
64.
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)
65.
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) →
66.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
67.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
68.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
69.
Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
a)
Fe
b)
S
c)
FeS
d)
none 
70.
Which problem is balanced?
(Check ALL answers)
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
71.
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 
72.
Which of the following equations are correctly balanced?
a)
12CO2 +H2O --> C6H12O6 + O2
b)
CO2 + 9H2O --> C6H12O6 + O2
c)
CO2 + H2O --> 3C6H12O6 + O2
d)
6CO2 + 6H2O --> C6H12O6 + 6O2
73.

Balance the following:

____ H2SO4 + ____ NaNO2 → ____ HNO2 + ____ Na2SO4

a)
1,1,2,1
b)
1,2,2,1
c)
2,3,3,2
d)
4,3,2,1
74.

Which type of reaction is:

2 NaBr + Ca(OH)2 → CaBr2 + 2 NaOH

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
75.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
76.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

77.

What is the limiting reactant if 10 moles of NH3 react with 30.0 moles of NO?

4NH3+ 6NO --> 5N2 + 6H2O

a)

NH3

b)

NO

c)

N2

d)

water

78.

Balance the reaction: _AlBr3 + _K2SO4 → _KBr + _Al2(SO4)3

a)

6 AlBr3 + 1 K2SO4 → 6 KBr + 1 Al2(SO4)3

b)

2 AlBr3 + 3 K2SO4 → 6 KBr + 1 Al2(SO4)3

c)

1 AlBr3 + 1 K2SO4 → 2 KBr + 3 Al2(SO4)3

d)

2 AlBr3 + 3 K2SO4 → 1 KBr + 2 Al2(SO4)3

79.

What is the percent yield of the following reaction if 145g of P2O5 reacts with 40 grams of water, but you only collect 112 grams of phosphoric acid?

3 H2O + P2O5 -> 2H3PO4

a)

80%

b)

85%

c)

77%

d)

58%

80.

B2H6 + 3O2 -->2 HBO2 + 2 H2O

What mass of O2 will be needed to burn 36.1 g of B2H6?

a)

13.8 g

b)

3.86 g

c)

124 g

d)

198.3 g

81.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
82.
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
83.

What is the oxidation number of N in NO2-1?

a)

-3

b)

+4

c)

-2

d)

+3

84.

How many moles of glucose, C6H12O6, can be "burned" biologically when 10.0 mol of oxygen is available?


C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)

a)

A. 0.938 mol

b)

B. 1.67 mol

c)

C. 53.3 mol

d)

D. 60.0 mol

85.

How many moles of hydrogen gas are needed to react completely with two moles of nitrogen gas?


3 H2 + N2 → 2 NH3

a)

A. 3 mol

b)

B. 6 mol

c)

C. 9 mol

d)

D. 12 mol

86.

How many grams of calcium chloride are required to make 20 grams of calcium hydroxide?

CaCl2 + 2 NaOH → Ca(OH)2 + 2 NaCl

a)

20 grams

b)

25 grams

c)

30 grams

d)

35 grams

87.

How many liters of NH are needed to react completely with 30.0 L of NO (at STP)?

4NH3(g) + 6NO(g) 5N2(g) + 6H2O(g)

a)

5 L

b)

20.0 L

c)

7.5 L

d)

120 L

88.

Epinephrine (adrenaline) is a hormone secreted into the bloodstream in times of stress. It contains 59.0% C, 7.15% H, 7.65% N, and 26.20% O and has a molar mass of 183 g/mol. What is its molecular formula?

a)

C8H12NO2

b)

C9H13NO3

c)

C7H9N2O

d)

C5H11N2O3

89.

For the reaction 2Na + Cl2 → 2NaCl, calculate the percent yield if 200. g of chlorine react with excess sodium to produce 240. g of sodium chloride?

a)

61.2%

b)

88.4%

c)

83.4%

d)

72.8%

90.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
91.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
92.
What is a Limiting Reagent?
a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
93.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
94.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
95.

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

96.

What is the molar mass of table salt (NaCl)?

a)

116.89 g/mol

b)

35.45 g/mol

c)

22.99 g/mol

d)

58.44 g/mol

97.

I use 6.02 x 1023 when the problem gives me molecules?

a)

True

b)

False

98.

I use molar mass when the problem gives me grams?

a)

False

b)

True

99.

How many liters are in 1 mole at STP?

a)

15.9

b)

22.4

c)

33.3

d)

40.0

100.
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

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