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General Chemistry Final Review

Total questions: 139

Worksheet time: 6hrs 1mins

Name
Class
Date
1.

24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.

What is the average atomic mass of this element?

a)

74.92 amu

b)

24.97 amu

c)

75.01 amu

d)

74.51 amu

2.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
3.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
4.

What number of particles can be different in isotopes of any given element?

a)

Protons

b)

Neutrons

c)

Electrons

d)

All remain constant

5.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
6.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
7.

The frequency of violet light is 7.5x1014 Hz. What is its wavelength?

a)

4.0x10-7 m

b)

4.0x107 m

c)

2.25x1023m

d)

2.25x1023 Hz

8.

Red light has a wavelength of 675 x 10-9 m. What is its frequency?

a)

2.03x1011 m

b)

4.44x1014 Hz

c)

4.44x1014 nm

d)

2.03x1011 Hz

9.
The two elements formed in Big Bang Nucleosynthesis where __________________.
a)
hydrogen and lithium
b)
hydrogen and helium
c)
hydrogen and oxygen
d)
helium and lithium
10.

Which subatomic particle(s) is/are responsible for the identity of an element?

a)

proton

b)

neutron

c)

electron

d)

quark

11.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

12.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period and increases down a group.

b)

Electronegativity decreases across a period and decreases down a group.

c)

Ionization energy increases across a period and increases down a group.

d)

Ionic radius increases across a period and increases down a group.

13.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
14.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
15.
An electron that resides in the outermost shell, or principal quantum level, of an atom
a)
periodic trend
b)
electron shell
c)
ionic radius
d)
valence electron
16.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
17.

Vertical columns of elements on the periodic table with similar properties and valence electrons

a)

groups

b)

periods

c)

quadrants

d)

rows

18.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
19.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
20.
Identify the phosphide ion
a)
P5+
b)
P3+
c)
P3-
d)
P4-
21.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
22.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
23.
What is the formula for lead (II) carbonate?
a)
PbCO3
b)
Pb2CO3
c)
Pb(CO3)2
d)
Pb(CO)4
24.
What is the metallic ion in the compound CuCl?
a)
Cu1+
b)
Cu2+
c)
Cu1-
d)
Cu2-
25.
What is the formula for aluminum sulfite?
a)
Al3S2
b)
AlSO4
c)
Al3(SO4)2
d)
Al2(SO3)3
26.
What is the formula for tin (II) chromate 
a)
Sn2(CrO4)4
b)
Sn(CrO4)2
c)
Sn4(CrO4)2
d)
SnCrO4
27.
What is the formula for barium hydride?
a)
BaOH2
b)
Ba(OH)2
c)
BaH2
d)
BaOH
28.
Name the compound Mg3(PO4)2
a)
magnesium phosphate
b)
magnesium (III) phosphate
c)
magnesium phosphite
d)
magnesium phosphide
29.
Name the compound Fe(NO2)3
a)
iron nitrite
b)
iron (III) nitrate
c)
iron (III) nitrite
d)
ferric nitrite
30.

Name the compound SiCl4

a)

silicon tetrachloride

b)

sulfur tetrachloride

c)

silicon (IV) chloride

d)

silicon chloride

31.
Name the compound CuCO3
a)
cobalt carbonate
b)
copper (III) carbonate
c)
copper (II) carbonate
d)
copper carbonate
32.

Which type of bond has an unequal sharing of electrons between two atoms?

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

mettalic

33.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
34.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
35.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)

London dispersion

d)
metallic
36.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
37.
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
38.

2SO2(g)+O2(g)⇌2SO3(g)

Adding SO3(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase K

d)

have no change

39.
4Si + S8 --> 2Si2S4
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Double displacement
40.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single diplacement
d)
Double displacement
41.
3KOH + H3PO4 --> K3PO4 + 3H2O
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Double displacement
42.
2Pb(NO3)2 --> 2PbO + 4NO2 + O2
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Combustion
43.
3Mg + N2 --> Mg3N2
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Combustion
44.
2NO2 --> N2 + 2O2
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Combustion
45.
P4 + 3O2 --> 2P2O3
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Combustion
46.
Fe + H2SO4 --> Fe2(SO4)3 + H2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
47.
Which reaction type is the following: C5H10O4 + O2 --> CO2 + H2O
a)
Decomposition
b)
Single Replacement
c)
Combustion
d)
Double Replacement
48.
C4H12 + O2 --> CO2 + H2O
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
49.
NH3 + HCl ---> NH4Cl 
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
50.
PbCl2 + AgNO3 ---> Pb(NO3)2 + AgCl 
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
51.
Predict the products for the following reactants.
C6H12 + O2 --> 
a)
CO + H2
b)
CO2 + O2
c)
C3H6O
d)
CO2 + H2O
52.
Predict the products for the following reactants.
Mg + I2 --> 
a)
MgI
b)
MgI2
c)
Mg + I2
d)
Mg2I
53.
Predict the products for the following reactants.
Na + MgCl2 -->
a)
NaCl + Mg
b)
NaCl2 + Mg
c)
No Reaction
d)
NaMgCl2
54.
Predict the products for the following reactants.
Al + O2 --> 
a)
AlO
b)
AlO2
c)
Al2O3
d)
Al2O
55.
Predict the products for the following reactants.
AgNO3 + Na2CO3 -->
a)
Ag2CO3 + NaNO3
b)
No Reaction
c)
AgCO3 + NO3Na
d)
AgCO3 + NaNO3
56.
Predict the products for the following reactants.

Al + CuCl2 -->
a)
No Reaction
b)
CuAl + Cl2
c)
Cu + AlCl3
d)
Cu2 + AlCl2
57.
Predict the products for the following reactants.

K2CO3 + BaCl2 -->
a)
No Reaction
b)
KCl + BaCO3
c)
K2Cl + BaCO3
d)
KCl2 + BaCO3
58.
Predict the products for the following reactants.

Ag­2O -->
a)
Ag + O
b)
Ag + O2
c)
AgO
d)
Ag2 + O
59.

Predict the precipitate when you mix silver nitrate and sodium chloride:

a)

AgNO3

b)

No precipitate

c)

AgCl

d)

NaNO3

60.

When you mix barium nitrate and sodium sulfate

a)

BaSO4

b)

NaNO3

c)

No precipitate

d)

BaNO3

61.

potassium chloride and sodium nitrate

a)

KNO3

b)

No precipitate

c)

NaCl

d)

KCl

62.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

63.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

64.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

65.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

66.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

67.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
68.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
69.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

70.

1Mg + 2H2O --> Mg(OH)2 + H2

What volume of hydrogen will be produced at STP by the reaction 67.3 g of magnesium?

a)

62.0 L

b)

0.12 L

c)

2.77 L

d)

1.15 L

71.

2CO + O2 −-> 2CO2

How many liters of carbon dioxide at STP are produced from 10.0 L of carbon monoxide at STP?

a)

10.0 L

b)

20.0 L

c)

5010 L

d)

0.0199

72.
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
73.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
74.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
75.
2Fe2O3  +  C  →  Fe  +  3CO2
You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)
a)
15.8%
b)
209.2%
c)
6435%
d)
15.5
76.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
77.
Which of the following do you get through measuring its mass? (No calculations)
a)
percent yield
b)
theoretical yield
c)
actual yield
d)
limiting reagent
78.
Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?
a)
25.2 grams
b)
37.3 grams
c)
37.1 grams
d)
36.3 grams
79.

Which of the following is a neutralization reaction?

a)

2Na + Cl2 → 2NaCl

b)

CH4 + 2O2 → CO2 + 2H2O

c)

HCl + KOH → KCl + H2O

d)

CaCO3 → CO2 + CaO

80.

Acid + Base makes what?

a)

Salt

b)

saltwater

c)

an explosion

d)

Water

81.

Neutralisation reactions must make which two products?

a)

carbonate

b)

salt

c)

pepper

d)

water

82.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
83.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
84.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
85.
What is the percent by mass of chlorine in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
86.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
87.
What is the percent by mass of calcium in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
88.
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
89.

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


What is the maximum amount of each product that can be formed?

a)

18.6 g of ammonium phosphate, 31.9 of sodium nitrate

b)

54 g of ammonium phosphate, 31.9 of sodium nitrate

c)

32.4 g of ammonium nitrate, 76 g of sodium phosphate

d)

21 g of ammonium nitrate, 34 g of sodium phosphate

90.

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


How much of the excess reagent is left over after the reaction is complete?

a)

12 g of sodium phosphate

b)

29.5 g of sodium phosphate

c)

17 g of ammonium nitrate

d)

95 g of ammonium phosphate

91.

3CaCO3 + 2FePO4 --> Ca3(PO4)2 + Fe2(CO3)3


What is the maximum amount of each product that can be formed?

a)

85 g of calcium carbonate, 39 g of iron(III) phosphate

b)

12.4 g of calcium phosphate, 27 g of iron(III) carbonate

c)

37.2 g of calcium phosphate, 29.3 g of iron(III) carbonate

d)

46.3 g of calcium phosphate, 43.8 g of iron(III) carbonate

92.

CuCl2 + 2NaNO3 --> Cu(NO3)2 + 2NaCl


If 15.0 grams of CuCl2 react with 20 g of NaNO3, how much NaCl can be formed?

a)

13.0 g of NaCl

b)

98 g of NaCl

c)

26 g of NaCl

d)

17.4 of NaCl

93.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

94.

How many moles are in 19.82 g Mg?

a)

1.23 mol Mg

b)

481.70 mol Mg

c)

1.00 mol Mg

d)

0.82 mol Mg

95.

How many moles are in 3.01 x 1022 atoms of magnesium?

a)

0.05 moles

b)

1.81 x 1046 moles

c)

5.00 x 1021 moles

d)

5.00 moles

96.

How many grams are in 1.2 x 1024 atoms of C?

a)

29.34 grams

b)

23.94 grams

c)

6.02 grams

d)

1.21 grams

97.

What is the percent composition by mass of sulfur (S) in the compound MgSO4?

a)

20.22%

b)

19.85%

c)

26.64%

d)

28.64%

98.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
99.
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
100.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
101.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
102.
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
103.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
104.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
105.

The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?

a)

0.13 J/(g°C)

b)

17,000 J/(g°C)

c)

1600 J/(g°C)

d)

0.065 J/(g°C)

106.
How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0oC to 50.0oC? the specific heat of aluminum is .900J/goC
a)
450
b)
-450
c)
225
d)
-225
107.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

108.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
109.

6CO2 + 6H20 + Energy --------------- C6 H12 06 + 6O2

a)

endothermic reaction

b)

exothermic reaction

110.

02 (g)+ 2H2-------------2H20 + Energy

a)

endothermic

b)

exothermic

111.
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)
112.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
113.
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
114.

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

b)

H2

c)

N2 and H2

d)

NH3

115.

What is the effect of increasing the pressure on the following equilibrium: 2NO(g) + O2 (g) ⇌2NO2(g)?

a)

The yield of NO2 increases

b)

The yield of NO2 decreases

c)

The reaction is slower

d)

The concentration of O2 increases.

116.
What is the variable for this number 22.4 L
a)
P
b)
T
c)
n
d)
V
117.
What is the variable for this number 122 K
a)
P
b)
T
c)
n
d)
V
118.
What is the variable for this number 1.5 mol
a)
P
b)
T
c)
n
d)
V
119.
What is the variable for this number 9.10 atm
a)
P
b)
T
c)
n
d)
V
120.
What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 47 oC?
PV=nRT
a)
14.19 atm
b)
16.53 atm
c)
18.42 atm
d)
22.54 atm
121.
What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?
a)
3670 atm
b)
0.245 atm
c)
4.08 atm
d)
605 atm
122.
At 17 °C, a 0.80 mole sample of a gas exerts a pressure of 1.2 atmospheres. What is the volume of the container?
a)
22.9 Liters
b)
2355 Liters
c)
0.0630 Liters
d)
15.9 Liters
123.

Which of the following statements is true concerning acids and bases?

a)

acids and bases don't react with each other

b)

acids mixed with bases neutralize each other

c)

acids mixed with bases make stronger bases

d)

acids mixed with bases make stronger acids

124.

Which is the correct set of acid properties:

a)

sour taste, corrosive, change litmus from red to blue

b)

sour taste, corrosive, change litmus from blue to red

c)

sweet taste, slippery, change litmus from blue to red

d)

sour taste, slippery, change litmus from blue to red

125.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

126.

Which is true?

a)

pH of less than 7 is basic; pH of more than 7 is acidic

b)

pH of less than 7 is acidic; pH of more than 7 is basic

127.

The pH scale is a range from:

a)

1-7

b)

0-14

c)

1-5

d)

1-14

128.
A solution with a pH of 8.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
129.

Ammonia has a pH of 11. Ammonia is __________.

a)

an acid

b)

a base

c)

an element

d)

a metal

130.

Tastes sour

a)

acid

b)

base

c)

neutral

d)

both acids & bases

131.

Tastes bitter.

a)

Acids

b)

Bases

c)

None of the following

d)

Acids & Bases

132.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
133.
What is the endpoint of a titration
a)
Where the amount of acid and base are balanced according to the equation
b)
Where there is no base
c)
At the end
134.
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
135.
I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
136.
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
137.
What acid and what base would you choose to prepare the salt potassium chlorate?
a)
KOH and HClO3
b)
KOH and HClO2
c)
HK and OHClO3
d)
HK and OHClO2
138.
A 50.0 mL sample of Ca(OH)2 is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)2 solution.
a)
1.0 M
b)
0.50 M
c)
0.15 M 
d)
0.30 M
139.
Which of the following shows the correct conjugate acid base pair?
a)
HCI (acid) / H3O+ (conjugate base)
b)
HCI (acid) / CI- (conjugate base)
c)
HCI (base) / CI- (conjugate acid)
d)
HCI (base) / H3O+ (conjugate acid)

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