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AP Chemistry Test Practice 11/14

Total questions: 109

Worksheet time: 2hrs 5mins

Name
Class
Date
1.

The measurement, 206 cm, has how many significant (measured) digits?

a)

1

b)

2

c)

3

d)

4

e)

5

2.

The measurement, 0.0020600mole g, has how many significant digits?

a)

1

b)

2

c)

3

d)

4

e)

5

3.

The measurement, 20,600 molecules has how many significant digits?

a)

1

b)

2

c)

3

d)

4

e)

5

4.

Add the following three numbers and report your answer using significant figures:


2.5 cm + 0.50 cm + 0.055 cm = ?

a)

3.055 cm

b)

3.06 cm

c)

3.1 cm

d)

3.0 cm

e)

3 cm

5.

Multiply the following three numbers and report your answer to the correct number of significant figures:


0.020 cm x 50 cm x 11.1 cm = ?

a)

10 cm3

b)

11 cm3

c)

11. cm3

d)

11.1 cm3

e)

11.10 cm3

6.

What is the measurement to the right in the correct number of significant figures.

a)

35 mL

b)

35.0 mL

c)

35.2 mL

d)

35.00 mL

e)

35.10 mL

7.

2.00 gallons is equal to how many liters?

a)

0.1321 L

b)

0.528 L

c)

7.57 L

d)

8.45 L

e)

8.5 L

8.

What is the mass of one mole of (NH4)2CO3?

a)

144 g

b)

138 g

c)

96 g

d)

78 g

e)

43 g

9.

How many moles of carbon dioxide are there in 52.06 g of carbon dioxide?

a)

8.648 × 1023

b)

0.8452

c)

3.134 × 1025

d)

1.183

e)

6.022 × 1023

10.

There are __________ molecules of methane in 0.123 mol of methane (CH4)

a)

2.46 × 10-2

b)

7.40 × 1022

c)

5

d)

0.615

e)

2.04 × 10-25

11.

A compound contains 6.0 g of carbon and 1.0 g of hydrogen. The percent composition of the compound is:

a)

14 % hydrogen and 86 % carbon

b)

86 % hydrogen and 14 % carbon

c)

17 % hydrogen and 83 % carbon

d)

83 % hydrogen and 17 % carbon

e)

None of these answers are correct.

12.

18 L of O2 would have how many molecules?

a)

4.1 x 10 -27 molecules

b)

0.80 molecules

c)

4.8 x 10 23 molecules

d)

8.0 x 10 23 molecules

e)

2.4 x 10 26 molecules

13.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
14.
What is the percentage of iron in iron(III)oxide?
a)
30%
b)
70%
c)
40%
d)
60%
15.

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

16.

Which of the following shows a correct way to balance the chemical equation:

a)

Fe + O2 --> Fe2O3

b)

4 Fe + 3 O2 --> 2 Fe2O3

c)

2 Fe + 3 O2 --> Fe2O6

d)

4 Fe + O6 --> 2 Fe2O3

e)

2 Fe + 3/2 O2 --> Fe2O3

17.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
18.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
19.
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
20.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
21.

In the quantum-mechanical model of the atom, an orbital is defined as a

a)

region of the most probable proton location.

b)

region of the most probable electron location.

c)

circular path traveled by an electron around an orbital.

d)

circular path traveled by a proton around an orbital.

22.

Which type of orbital is shaped like a clover

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

23.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
24.

What is the electron configuration for an atom of Sodium?

a)

3s1

b)

[He] 3s1

c)

1s22s23s1

d)

1s22s22p63s1

25.

The electron configuration of Fe is __________.

a)

1s2 2s2 3s2 3p6 3d6

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

c)

1s2 2s2 2p6 3s2 3p6 4s2

d)

1s2 2s2 2p6 3s2 3p6 4s2 4d6

26.

The electron configuration of Ga is __________.

a)

1s2 2s2 3s2 3p6 3d10 4s2 4p1

b)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p1

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d1

27.

Which one of the following is the correct electron configuration for a nitrogen atom?

a)

1s↑↓ 2s↑↓ 2p↑↓ ↑

b)

1s↑↓ 2s↑↑ 2p↑ ↑ ↑

c)

1s↑↑ 2s↑↓ 2p↑ ↑ ↑

d)

1s↑↓ 2s↑↓ 2p↑ ↑ ↑

28.

The electron configuration for an ion of Ga is __________.

a)

1s2 2s2 2p6 3s2 3p6 3d10

b)

1s2 2s2 3s2 3p6 3d10 4s2 4p1

c)

1s2 2s2 2p6 3s2 3p6 4s2 4d10

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

29.

How many electrons does potassium need to gain or lose to become stable?

a)

Gain 1

b)

Gain 2

c)

Lose 1

d)

Lose 2

30.

Anions tend to be __________ and cations tend to be __________.

a)

metals, metals

b)

nonmetals, nonmetals

c)

metals, nonmetals

d)

nonmetals, metals

31.

The electron dot diagram that correctly shows the bonding in H2N2 is:

a)
b)
c)
d)
32.

The structural formula for the nitrite ion, NO3- is:

a)
b)
c)
d)
e)
33.

Electronegativity is a measure of _____.

a)

the attraction of atoms for paired electrons within a bond.

b)

the energy released when an electron is added to an atom.

c)

the energy required to remove an electron from an atom.

d)

None of the answers listed are correct.

34.

What is the formula of the compound formed between strontium ions and nitrogen ions?

a)

SrN

b)

Sr3N2

c)

Sr2N3

d)

SrN2

35.

The charge on the iron ion in the salt Fe2O3 is __________.

a)

1-

b)

2+

c)

3+

d)

5-

36.

The ions Ca2+ and PO4 3- form a salt with the formula __________.

a)

CaPO4

b)

Ca2(PO4)3

c)

Ca2PO4

d)

Ca3(PO4)2

37.

In the Lewis structures of __________ which central atoms do not have a lone pair of electrons. (select ALL possible)


(i) PCl3 (ii) CH2Cl2 (iii) HCN (iv) C2H4 (v) NH3

a)

i

b)

ii

c)

iii

d)

iv

e)

v

38.

According to VSEPR theory, if there are five electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry.

a)

octahedral

b)

linear

c)

trigonal Planar

d)

trigonal bipyramidal

e)

tetrahedral

39.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
40.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
41.
Which of the following is a polar molecule?
a)
CH4
b)
Xe
c)
H2O
d)
CO2
42.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
43.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

44.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

45.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
46.
Which has a pH below 7?
a)
Acid
b)
Base
47.
Which has a slippery texture?
a)
Acid
b)
Base
48.
Turns litmus red
a)
Acids
b)
Bases
c)
All
49.

What pH is the strongest base?

a)

1

b)

7

c)

4

d)

14

50.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
51.
Which of these pH values would indicate that a solution is a weak base?
a)
4
b)
5.6
c)
8
d)
13
52.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
53.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
54.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

55.

The pH value of an acid represents its __________ of positive ions in the solution

a)

amount

b)

concentration

c)

color

d)

charge

56.

The higher the concentration of negative (hydroxide) ions in the solution, the stronger the base is.

a)

True

b)

False

57.

If the substance is neutral, what would the pH be?11

a)

3

b)

5

c)

7

d)

9

e)

11

58.
If the [H+] of a solution is 1 x 10-2 mol/L the pH is
a)
2
b)
12
c)
-2
d)
1
59.
If the pH of a solution is 5 the [H+] is
a)
1.0 x 105  M
b)
1.0 x 109  M
c)
5.0 x 101  M
d)
1.0 x 10-5  M
60.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
61.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
62.
if the [H+] of a solution is 1.0 x 10-2 mol/L the pH is
a)
2
b)
-2
c)
1
d)
12
63.
If the [H3O+] of a solution is 1 x 10-8 mol/L the [OH-] is
a)
1.0 x 10-6
b)
1.0 x 106
c)
1.0 x 10-8
d)
1.0 x 108
64.
If the [OH-] of a solution is 2.7 x 10-4 mol/L the pOH of the solution is
a)
10.44
b)
3.56
c)
1.00
d)
-4.43
65.
A solution with a [H+] of 9.4 x 10-5 mol/L is said to be
a)
Acidic
b)
Basic
c)
Neutral
d)
negative number, no solution.
66.
If the [H+] of a solution is 6.8 x 10-9 mol/L the pH is
a)
8.17
b)
8.2
c)
9.99
d)
8.62
67.
if the [H+] of a solution is 8.4 x 10-3 mol/L the pOH of the solution will be
a)
2.08
b)
11.92
c)
1.02
d)
12.98
68.
if a solution has a pOH of 5.2 the [OH-] of the solution is
a)
6 x 10 -6 M
b)
6.3 x 10 -6 M
c)
1.58 x 10-5 M
d)
2 x 10-5 M
69.
Limes have a [H3O+] of 1.3 x 10-2 mol/L.  Their pOH is
a)
1.89
b)
12.11
c)
1.03
d)
12.97
70.

What is the conjugate base of HClO4?

a)

H+

b)

Cl-

c)

ClO3-

d)

ClO4-

71.

Which is a strong acid?

a)

12.0M HNO2

b)

10.0M H2SO3

c)

5.0M HI

d)

5.0M HF

72.

The [OH-] = 4.0 x 10-9, what is the pH of the solution?

a)

9.0

b)

5.7

c)

8.3

d)

4.3

73.

Which acid produces the strongest conjugate base?

a)

HClO4 (Ka= 1.0 x 107)

b)

HCN (Ka= 4.0 x 10-10)

c)

H3PO4 (Ka= 7.5 x 10-3)

d)

H2CO3 (Ka = 4.2 x 10-7)

74.

Which relationship relates Ka, Kb and Kw?

a)

Kw = Ka + Kb

b)

Kw = Kb/Ka

c)

Ka = Kw + Kb

d)

Kb = Kw/Ka

75.

Acetic Acid is a weak monoprotic acid. It's concentration is 0.20M and it's equilibrium concentration of H+ ions is 0.0019M. Calculate it's Ka value.

a)

1.8x10 -5

b)

1.8x10 -15

c)

.0019

d)

5.56x10 -10

76.

Formic Acid is a weak monoprotic acid. It's initial concentration is 0.10M and it's equilibrium concentration of H+ ions is 0.0042M. Calculate it's Ka value.

a)

.150

b)

12.56x10 -6

c)

1.8x10 -4

d)

None of these are correct

77.

Isobutlyamine is a weak base. It's initial concentration is 0.55M and it's equilibrium concentration of OH- ions is 0.0040M. Calculate it's Kb value.

a)

.055

b)

4.0x10 -3

c)

1.6x10 -5

d)

3.1x10 -4

78.

Gallic Acid is a weak monoprotic acid. It's concentration is 0.280M and it's equilibrium concentration of H+ ions is 0.0033M. Calculate it's pH value.

a)

3.9x10 -5

b)

4.96

c)

2.48

d)

.280

79.

Uric Acid is a weak monoprotic acid. It's initial concentration is 0.110M and it's equilibrium concentration of H+ ions is 0.034M. Calculate the final concentration of Uric acid.

a)

.011

b)

.034

c)

.076

d)

1.47

80.

Ammonia is a weak base. It's concentration is 0.150M and it's Kb value is 1.7x10 -5. Calculate it's pH value.

a)

2.80

b)

11.2

c)

Both answers are correct

d)

None of the above are correct

81.

calculate the pKb of solution with a pKa of 6.9

a)

7.1

b)

6.5

c)

14

d)

9.6

82.

calculate the Ka of a solution with a pKb of 3.38

a)

3.38x10-11

b)

6.76x10-11

c)

2.40x10-11

d)

2.39x10-11

83.

Calculate the Kb of a solution that has a pKb of 4.2

a)

0.62

b)

6.3x10-5

c)

9.8

d)

4.2

84.

What are the two factors to look for when determining if the reaction is at equilibrium?

a)

Forward reaction rate is faster than the reverse and concentrations are equal

b)

Forward and reverse reaction rates are equal and concentration is constant

c)

Forward and revers reaction rates are equal and concentration is equal

d)

Forward reaction rate is faster than the reverse and concentration is equal

85.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
86.
Which is the reactant - and why?
a)
A, as concentration decreases
b)
B, as concentration decreases
c)
A, as concentration increases
d)
B, as concentration increases
87.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
88.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
89.
For the reaction...
SO2 + O2 <=>  SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
90.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
91.
For the reaction...
N2 (g) +  3 H2 (g) <=> 2 NH3 (g)

If the pressure in the system is increased,  which substance(s) will increase in concentration?
a)
N2  (as 2 mol gas  → 4 mol gas)
b)
H2 (as 2 mol gas  → 4 mol gas)
c)
N2 and H2 (as 2 mol gas  → 4 mol gas)
d)
NH3 (as 4 mol gas  → 2 mol gas)
92.

For the endothermic reaction...

N2 + O2 <=> 2NO

If the temperature is increased the equilibrium position will shift _______.

a)

to the left

b)

to the right

c)

to the left and right

d)

neither left nor right

93.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
94.
An equilibrium constant with a large value, e.g. Kc = 1000, indicates…
a)
A very fast reaction
b)
Mostly products at equilibrium
c)
Mostly reactants at equilibrium
d)
Nothing useful at all
95.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
96.
Given: 2A(g) <=> 2B(g) + C(g). At a particular temperature, Kc = 16000.
Raising the pressure, by decreasing the volume of the container, will...
a)
cause the value of Kc to increase
b)
cause the value of Kc to decrease
c)
have no effect on the value of Kc as temperature does not change
d)
favour the forward reaction
97.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
98.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
99.
The following reaction :    
SO2 (g) +  NO2 (g) <=> SO3 (g) + NO (g)  
had reached a state of equilibrium, was found to contain  
0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,
0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.
Calculate the equilibrium constant  for this reaction. 
a)
4
b)
.42
c)
.25
d)
1
100.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)
Kc =
a)
[Fe]3 [H2O]4  / [Fe3O4] [H2]4
b)
[Fe3O4] [H2]4 /  [Fe]3 [H2O]4
c)
[H2O]4 / [H2]4
d)
[Fe] [H2O] / [Fe3O4] [H2]
101.
For the reaction...
H2 (g)  + Cl2 (g) <=>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium position will _______.
a)
shift to the left
b)
shift to the right
c)
not shift position at all as 2 mol gas <=> 2 mol gas
102.
What is the Ksp expression for dissolving magnesium chloride, MgCl2, in water, knowing that the equation is:  CaCl2(s) ↔ Ca+2(aq) + 2Cl-1(aq)
a)
Ksp = [Ca+2][Cl-1]2
b)
Ksp = [Ca][Cl]2
c)
Ksp = [Ca+2][Cl-1]2/[CaCl2]
d)
Ksp = [Ca+2] + [Cl-1]2
103.
What is the proper Keq for the following reaction? 
   2 NO(g)  +  O2(g) ⇌ 2 NO2(g)
a)
Keq = [NO2]2 / [NO]2[O2]
b)
Keq =  [NO]2[O2] / [NO2]2
c)
Keq = [NO]2[O2][NO2]2
d)
Keq = 2[NO][O2] / 2[NO2]
104.
An exothermic reaction is allowed to reach equilibrium. If heat energy is then removed, the equilibrium will shift
a)
toward the middle
b)
toward the reactant side
c)
toward the product side
d)
No shift.
105.
A mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 1.00L flask.  The equilibrium constant Keq for the reaction H2(g) + I2(g) ↔ 2HI(g) is 54.3.  What is the concentration of HI at equilibrium?
a)
0.5M
b)
1.0M
c)
0.786M
d)
3.7M
106.
What states of matter are included when calculating Keq?
a)
Solids and Liquids
b)
Aqueous and Gas
c)
Solids, Liquids, Aqueous solutions and Gases
d)
Aqueous Solutions & Liquids
107.
Which is the correct equilibrium constant expression for the reaction 
CaCO3(s) ⇋ CaO(s) + CO2(g)
a)
[CaO]/[CO2]
b)
[CO2]
c)
1/[CO2]
d)
[CO2][CaO] / [CaCO3
108.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
both left and right
d)
neither left nor right
109.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right

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•

10th - 11th Grade

Chemistry Midterm Review Game

104 questions

Chemistry Midterm Review Game

quiz

Worksheet

•

10th Grade

HC07 Predicting Products - Single Replacement Reactions

107 questions

HC07 Predicting Products - Single Replacement Reactions

quiz

Worksheet

•

9th - 12th Grade

Unit 3 Review

106 questions

Unit 3 Review

quiz

Worksheet

•

10th Grade

Density

104 questions

Density

quiz

Worksheet

•

12th Grade

Covalent Bonding Test Review

108 questions

Covalent Bonding Test Review

quiz

Worksheet

•

10th - 12th Grade

Conflict and Cans (CH 4) Test Review

106 questions

Conflict and Cans (CH 4) Test Review

quiz

Worksheet

•

12th Grade