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Spring Midterm Exam Review 2021-2022

Total questions: 151

Worksheet time: 2hrs 28mins

Name
Class
Date
1.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
2.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
3.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
4.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
5.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
6.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
7.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
8.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
9.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
10.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
11.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
12.
*
a)
bent or angular
b)
trigonal pyramid
c)
linear
d)
tetrahedral
13.
*
a)
tetrahedral
b)
trigonal pyramid
c)
angular or bent
d)
trigonal plane
14.
Which of the following most likely represents the molecular geometry of water?
a)
A
b)
B
c)
C
d)
D
15.
A molecule consists of four bonds and no lone pairs. What is its structure? 
a)
square planar
b)
tetrahedral
c)
linear
d)
square pyramidal 
16.
The molecular geometry of boron trichloride is...
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
17.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
18.
SiCl4 has what shape?
a)
square planar
b)
square pyramidal
c)
tetrahedral
d)
octahedral
19.
Which of the following is octahedral?
a)
SCl6
b)
XeI4
c)
NBr5
d)
CH4
20.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
21.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
22.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
23.
How many lone pairs are in this molecule's structure?
a)
6
b)
2
c)
0
d)
4
24.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
25.
What kind of bond occurs between the carbons in C2H2?
a)
single
b)
double
c)
triple
d)
quadruple
26.
What is the name of pairs of electrons that do not participate in bonding? 
a)
outer pair
b)
unvalenced pair
c)
lone pair
d)
inner pair
27.
What kind of chemical bond forms between a metal and a nonmetal?
a)
Covalent bond
b)
Ionic bond
c)
Can be either covalent or ionic
d)
Hydrogen bond
28.
What is this molecule?
a)
CH4
b)
NaCl3
c)
SK4
d)
S4K2
29.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
30.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
31.

Which of the following is a strong acid?

a)

HF

b)

KOH

c)

HClO4

d)

HClO

32.

All of the following are weak acids except

a)

HCNO

b)

HBr

c)

HF

d)

HCN

33.

Which of the following is NOT a strong base?

a)

KOH

b)

Ca(OH)2

c)

LiOH

d)

Al(OH)3

34.

A solid acid HX is mixed with water. Two possible solutions can be obtained. Which of the following is true?

a)

In case I, HX is acting like a weak acid, and in case II, HX is acting like a strong acid.

b)

In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak acid.

c)

In both cases, HX is acting like a strong acid.

d)

In both cases, HX is acting like a weak acid.

35.

An acid is a substance that produces OH1- ions in water.

a)

True

b)

False

36.

Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct?

a)

Both NaCl and CuS precipitate from solution

b)

No reaction will occur

c)

CuS will precipitate from solution.

d)

NaCl will precipitate from solution.

37.

Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct?

a)

Both KNO3 and (NH4)2SO4 precipitate from solution

b)

A gas is released.

c)

KNO3 will precipitate from solution

d)

No reaction will occur

38.

Which of the following salts is insoluble in water?

a)

Na2S

b)

K2CO3

c)

Pb(NO3)2

d)

All of these are soluble in water.

39.

Which of the following ions is most likely to form an insoluble sulfate?

a)

K1+

b)

Li1+

c)

S2-

d)

Ca2+

40.

Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?

a)

Al3+, S2–

b)

Pb2+, Cl–

c)

Mg2+, SO42–

d)

Ba2+, PO43–

41.

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced molecular equation contains which one of the following terms?

a)

AgCl (s)

b)

2AgCl (s)

c)

2Ba(NO3)2 (aq)

d)

BaNO3 (aq)

42.

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced complete ionic equation contains which of the following terms?

a)

2Ba2+(aq)

b)

Cl–(aq)

c)

2Ag+(aq)

d)

AgCl(aq)

43.

When sodium chloride and lead(II) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation?

a)

PbCl(s)

b)

Pb2Cl(s)

c)

NaNO3(aq)

d)

2NaNO3(aq)

44.
KBr
a)
Soluble
b)
Insoluble
45.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
46.
Silver Iodide
a)
Soluble 
b)
Insoluble 
47.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
48.
KOH
a)
Soluble 
b)
Insoluble
49.
Silver acetate
a)
Soluble 
b)
Insoluble
50.
NiCl2
a)
Soluble 
b)
Insoluble
51.
PbI2
a)
Soluble
b)
Insoluble
52.
NaC2H3O2
a)
soluble
b)
insoluble
53.
K2CO3
a)
soluble
b)
insoluble
54.
CaCO3
a)
soluble
b)
insoluble
55.
BaSO4
a)
soluble
b)
insoluble
56.
Ca(OH)2
a)
soluble
b)
insoluble
57.
FeS
a)
soluble
b)
insoluble
58.
K2SO4
a)
soluble
b)
insoluble
59.
AgCl
a)
soluble
b)
insoluble
60.
NH4NO3
a)
soluble
b)
insoluble
61.
What are always soluble?
a)
Nitrates
b)
Phosphates
c)
Carbonates
d)
Hydroxides
62.
BaCl2
a)
soluble
b)
insoluble
63.
Fe(C2H3O2)3
a)
soluble
b)
insoluble
64.
Which pairs, below, form a precipitate when mixed together?
a)
sodium chloride, lead(II) nitrate
b)
calcium nitrate, potassium iodide
c)
lithium phosphate, ammonium nitrate
d)
potassium chloride, barium nitrate
65.
Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct?
a)
Both NaCl and CuS precipitate from solution.
b)
No reaction will occur.
c)
CuS will precipitate from solution.
d)
NaCl will precipitate from solution.
66.
How many of the following salts are expected to be insoluble in water?
sodium sulfide 
barium nitrate
ammonium sulfate  
potassium phosphate
a)
0
b)
1
c)
2
d)
3
67.
Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?
a)
Al3+, S2–
b)
Pb2+, Cl–
c)
Mg2+, SO42–
d)
Ba2+, PO43–
68.
Which of the following compounds is soluble in water?
a)
Ni(OH)2
b)
K3PO4
c)
BaSO4
d)
CoCO3
69.
A decomposition reaction is a reaction between at least two reactants in which
a)
one breaks down into at least two products.
b)
a compound is decomposed by an electric current.
c)
a compound burns in the presence of oxygen.
d)
a new, more complex compound is formed.
70.
A chemical equation is balanced by changing or adding
a)
chemical symbols.
b)
subscripts
c)
coefficients.
d)
reactants.
71.
A chemical reaction in which the energy is absorbed primarily in the form of heat is ______.
a)
flammable
b)
exothermic
c)
endothermic
d)
endergonic
72.
A substance that speeds up a chemical reaction without undergoing permanent change itself is a(n) 
a)
inhibitor
b)
coefficient
c)
reactant
d)
catalyst
73.
The breaking down of a substance into two or more substances is ______________.
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
74.
If energy in the form of heat is given off when a chemical reaction takes place, the reaction is 
a)
exothermic
b)
exerrgonic
c)
cooled
d)
endothermic
75.
What type of chemical reaction is shown in the equation AgNO3 + KCl     〉 AgCl + KNO3?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
76.
A _________ chemical equation has the same number of atoms of each element on both sides of the equation.
a)
simple
b)
balanced
c)
unbalanced
d)
complex
77.
When you activate a hand warmers pack, water mixes with a chemical and the pack gets very warm. This is an example of:
a)
an endothermic reaction.
b)
an exothermic reaction.
c)
a combustion reaction
d)
a physical change.
78.
Which of the following could represent a synthesis reaction?
a)
element + element = compound
b)
compound = element + element
c)
element + compound = element + compound
d)
compound + compound = compound + compound
79.
Which of the following reactions produces water and CO2
a)
synthesis
b)
decomposition
c)
combustion
d)
double displacement
80.
What is wrong with the following chemical equation?
N2 + O2 > N2O
a)
too many oxygen atoms on the reactants side
b)
too many nitrogen atoms on the products side
c)
too many nitrogen atoms on the reactants side
d)
too many oxygen atoms on the products side
81.

What should be done to balance the following equation?

N2 + O2 > N2O

a)

Put a 2 in front of O2 and a 2 in front of N2O

b)

Put 3 in front of N2O

c)

put a 2 in front of N2 and a 2 in front of N2O

d)

put a 2 in front of N2

82.

How many hydrogen atoms are on the product side of the following chemical equation?

N2 + 3H2 > 2 NH3

a)

3

b)

5

c)

2

d)

6

83.
The idea that the matter can neither be created nor destroyed but can rearrange to made different substances is 
a)
The Law of Conservation of Mass
b)
Newton's 3rd Law
c)
The Law of Conservation of Energy
d)
none of the above
84.
The product of bubbles is a sign that
a)
a chemical change is taking place
b)
a physical change is taking place
c)
oxygen is present
d)
organic chemicals are present
85.
What type of reaction is shown in the chemical equation Mg + 2HCl  -->  MgCl2 + H2?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
86.
What type of reaction is shown in the chemical equation 2Na + Cl2 >  2NaCl?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
87.
What type of reaction is shown in the chemical equation 2Al2O3 --> 4Al + 3O2?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
88.
What type of reaction is shown in the chemical equation Pb(NO3)2 + 2NaCl --> 2NaNO3 + PbCl2?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
89.
What type of reaction is shown in the chemical equation S8 + 12O2 --> 8SO3?
a)
synthesis
b)
decomposition
c)
single-displacement
d)
double-displacement
90.
Which type of chemical reaction produces water and CO2 when a hydrocarbon is burned?
a)
synthesis
b)
decomposition
c)
combustion
d)
double displacement
91.
Which element cannot be replaced by sodium in a single-replacement reaction?
a)
Pb
b)
Fe
c)
Ca
d)
Ag
92.
Is the following chemical equation balanced?
Na + I2 > NaI
a)
yes
b)
no
c)
maybe
d)
all of the above
93.
Which element cannot be replaced by iron in a single-replacement reaction?
a)
Pb
b)
Co
c)
Cu
d)
Zn
94.

When the equation Fe3O4 + Al --> Fe + Al2O3 is correctly balanced, what is the coefficient of Al?

a)

3

b)

4

c)

6

d)

8

95.
Which element can be replaced by lead in a single-replacement reaction?
a)
Na
b)
Mg
c)
Cr
d)
Cu
96.
What is the small whole number that appears behind a chemical symbol in a formula in a chemical equation?
a)
a subscript
b)
a superscript
c)
a ratio
d)
a coefficient
97.
What are the correct coefficients when this equation is balanced?
Sb + O2 --> Sb4O6 
a)
1,2,10
b)
4,6,1
c)
4,3,1
d)
10,5,1
98.

KBr

a)

soluble

b)

insoluble

99.

zinc hydroxide

a)

soluble

b)

insoluble

100.

silver iodide

a)

soluble

b)

insoluble

101.

CaCO3

a)

soluble

b)

insoluble

102.

silver acetate

a)

soluble

b)

insoluble

103.

Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct?

a)

Both NaCl and CuS precipitate from solution.

b)

No reaction will occur.

c)

CuS will precipitate from solution.

d)

NaCl will precipitate from solution.

104.

Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?

a)

Al3+, S2–

b)

Pb2+, Cl–

c)

Mg2+, SO42–

d)

Ba2+, PO43–

105.

Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. What is the formula of the solid formed in the reaction?

a)

Ca(PO4)2

b)

CaPO4

c)

Ca3(PO4)2

d)

Ca3(PO3)2

106.

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced molecular equation contains which one of the following terms?

a)

AgCl (s)

b)

2AgCl (s)

c)

2Ba(NO3)2 (aq)

d)

BaNO3 (aq)

107.

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced complete ionic equation contains which of the following terms?

a)

2Ba2+(aq)

b)

Cl–(aq)

c)

2Ag+(aq)

d)

NO3– (aq)

108.

The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species?

a)

2Br–(aq)

b)

PO43–(aq)

c)

2Ca3(PO4)2(s)

d)

3Ca2+(aq)

109.

When solutions of phosphoric acid and iron(III) nitrate react, which of the following terms will be present in the balanced molecular equation?

a)

HNO3(aq)

b)

3HNO3(aq)

c)

2FePO4(s)

d)

3FePO4(s)

110.

The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species?

a)

3Al3+(aq)

b)

OH–(aq)

c)

3OH–(aq)

d)

2Al(OH)3(s)

111.

All of the following are in aqueous solution. Which is incorrectly named?

a)

H2SO4, sulfuric acid

b)

H2CO3, carbonic acid

c)

H3PO4, phosphoric acid

d)

HCN, cyanic acid

112.

All of the following are in aqueous solution. Which is incorrectly named?

a)

HC2H3O2, acetic acid

b)

HBr, bromic acid

c)

H2SO3, sulfurous acid

d)

HNO2, nitrous acid

113.

Rewrite the following word equation as a balanced chemical equation. What is the coefficient and symbol for fluorine? 
nitrogen trifluoride →\rightarrow nitrogen + fluorine 

a)

6F2

b)

F3

c)

6F

d)

3F2

114.

In order for the reaction 2Al + 6HCl →\rightarrow   2AlCl3 + 3H2 to occur, which of the following must be true?

a)

Al must be above Cl on the activity series.

b)

Al must be above H on the activity series.

c)

Heat must be supplied for the reaction.

d)

A precipitate must be formed.

115.

A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of the products of this reaction is

a)

Co(OH)3.

b)

Co(OH)2.

c)

LiCo3.

d)

LiCl3.

116.

What is the driving force in the following reaction?  Ni(NO3)2(aq)+K2S(aq)→Ni\left(NO_3\right)_2\left(aq\right)+K_2S\left(aq\right)\rightarrow  

a)

A gas is formed.

b)

A precipitate is formed.

c)

Ionic compounds are reactants.

d)

Ionic compounds are products.

117.

Use the activity series of metals to complete a balanced chemical equation for the following single replacement reaction.  Ag(s)+KNO3(aq)→Ag\left(s\right)+KNO_3\left(aq\right)\rightarrow  

a)

AgNO3+KAgNO_3+K  

b)

AgK+NO3AgK+NO_3  

c)

AgKNO3AgKNO_3  

d)

No reaction takes place because silver is less reactive than potassium.

118.
What is the molar mass of carbon?
a)
6.0 g/mol
b)
12.0 g/mol
c)
22.4 g/mol
d)
6.02 x 1023 g/mol
119.
What is the molar mass of CO2?
a)
22.0 g/mol
b)
28.0 g/mol
c)
44.0 g/mol
d)
56.0 g/mol
120.
A mole of Neon contains
6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
121.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.0500 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
122.

A mole of potassium chloride, an ionic compound, contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

123.

How many molecules are in 2.00 moles of H2O?

a)

124x1024 molecules of H2O

b)

1.20x1023 molecules of H2O

c)

12.04 x1023 molecules H2O

d)

124

124.
How many atoms are in 1.50 moles of Hg?
a)
9.03x1023 atoms Hg
b)
9.03x1024 atoms Hg
c)
903 atoms of Hg
d)
9.03 atoms of Hg
125.

88.0 grams of CO2 is about _____________. [Select 2 answers.]

a)

1 mole of CO2

b)

2 moles of CO2

c)

6.02 x 1023 molecules of CO2

d)

two times 6.02 x 1023 molecules of CO2

126.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
127.

What is the molar mass of NaCl?

a)

58 g/mol

b)

28 g/mol

c)

12 g/mol

d)

6.02 x 1023

128.
We use the periodic table to calculate...
a)
mass
b)
molar mass
c)
moles
129.

Which one has the most molecules or formula units?

a)

1 mole H2O

b)

1 mole Al(OH)3

c)

1 mole NaCl

d)

They are all the same

130.

What is the molar mass of one molecule of Nitrogen N2?

a)

14 amu (atomic mass units)

b)

14 g

c)

28 g

d)

28 amu

131.

The molar mass of an element is the mass of one ____ of the element, with numbers taken from the mass number on the periodic table.

a)

atom

b)

molecule

c)

mole

d)

gram

132.
Which has more molecules?
a)
1 mole CO2
b)
1 mole of N2O4
c)
1 mole of H2O
d)
They are all the same
133.
If I have 6.02 x1023 molecules of CO2, what is the mass?
a)
44.0 g
b)
2.65 x1023 g
c)
1.37 x1022 g
d)
96.0 g
134.

The sum of the percent by mass of each element in a compound must equal 100%.

a)

True

b)

False

135.

To find the percent by mass of a compound if you are given the formula, divide the molar mass of that element in one mole of the compound by the total molar mass of the compound.

a)

True

b)

False

136.

An element’s molar mass is equivalent to the atomic number of the element.

a)

True

b)

False

137.

Which element has a molar mass of 30.974 g/mol?

a)

potassium

b)

phosphorus

c)

gallium

d)

palladium

138.

Which is the correct molar mass for the compound FeSO4?

a)

103.85 g/mol

b)

151.85 g/mol

c)

415.4 g/mol

d)

247.85 g/mol

139.

How many formula units are in 3.6 grams of NaCl?

a)

0.06

b)

1.0x1021

c)

1.3x1026

d)

3.7x1022

140.

Which is the percent composition of phosphorus in Zn3(PO4)2?

a)

16.1%

b)

9.66%

c)

50.1%

d)

24.01%

141.

How many grams of phosphorus are in 500.0 grams of calcium phosphide?

a)

49.92 g

b)

99.84 g

c)

310.2 g

d)

130.1 g

142.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
143.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
144.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
145.
What is the percent by mass of chlorine in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
146.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
147.
What is the percent by mass of calcium in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
148.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
149.
What is the percent composition by mass of magnesium in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
150.
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%
151.
In which compound is the percent composition by mass of Cl equal to 42%?
a)
HClO (gram formula mass = 52 g/mol)
b)
HClO2 (gram formula mass = 68 g/mol)
c)
HClO3 (gram formula mass = 84 g/mol)
d)
HClO4 (gram formula mass = 100 g/mol)

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