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Worksheets

Fall Semester Chemistry Review

Total questions: 157

Worksheet time: 6hrs 46mins

Name
Class
Date
1.

What should be done with chemical waste after completing an experiment?

a)

Leave it at your station

b)

Dispose of it properly

c)

Dump it in the trash

d)

Pour it down the sink

2.

What should you do if a piece of equipment breaks?

a)

Keep it to yourself

b)

Tell your lab partner

c)

Notify your instructor

d)

Clean it up by yourself

3.

What should you do if you do not understand part of the lab instructions?

a)

Ask your instructor for help

b)

Skip that part of the lab

c)

Ask your lab partner

d)

Figure it out during the lab

4.

What should you do if you are injured during a lab?

a)

See the school nurse after class

b)

See a doctor after school

c)

Attempt first aid on your own

d)

Notify your instructor immediately

5.

What should you do after completing a lab in which chemicals or biological specimens were used?

a)

Wipe your hands on your clothing

b)

Wash your hands with soap and water

c)

Wipe your hands with a paper towel

d)

Rub some skin lotion on your hands

6.

What should be done with long hair before starting a lab?

a)

Do nothing, let it hang freely

b)

Hold it back with your hand

c)

Tie it back out of the way

d)

Use a hat to hold it back

7.

What type of footwear would be best worn in a laboratory?

a)

High Heels

b)

Sandals

c)

Sneakers

d)

Flip-Flops

8.

When is horseplay, or goofing around, acceptable in a laboratory?

a)

Always

b)

Sometimes

c)

Never

d)

Depends

9.

What is the safest way to smell a substance during a lab?

a)

Lean over and smell it directly

b)

Put it on your hand and smell it

c)

Waft the air towards your face

d)

Lift the substance to your nose

10.

Why are food and drink not permitted during an experiment?

a)

They could make your lab partner hungry

b)

They could attract ants and other insects

c)

They could make your instructor hungry

d)

They could contaminate the experiment

11.

What should you do with your station after completing the lab?

a)

Clean it up properly

b)

Leave it for someone else

c)

Throw everything away

d)

Push everything to one side

12.

What are the consequences of ignoring lab safety?

a)

You get hurt

b)

You fail the lab

c)

You lose lab privileges

d)

You bring about the zombie apocalypse

13.

Which metal is found in period 3 and group 2?

a)

Boron

b)

Magnesium

c)

Aluminum

d)

Neon

14.

Which noble gas has 18 protons?

a)

Helium

b)

Hydrogen

c)

Argon

d)

Calcium

15.

Group 17 is known as the

a)

Halogens

b)

Noble Gases

c)

Alkaline Earth Metals

d)

Alkali Metals

16.

Which group of elements have full energy levels and are considered stable?

a)

Halogens

b)

Alkaline Earth Metals

c)

Alkali Metals

d)

Noble gases

17.

Elements that share common traits of both metals and non-metals are referred to as

a)

metals

b)

non-metals

c)

halogens

d)

metalloids

18.

Which element has 87 protons and is considered the most reactive metal?

a)

Francium

b)

Fluorine

c)

Calcium

d)

Hydrogen

19.

Which element is found in group 17 and is the most reactive non-metal?

a)

Chlorine

b)

Argon

c)

Fluorine

d)

Magnesium

20.

Which alkaline earth metal is found in period 2 and group 2?

a)

Sodium

b)

Beryllium

c)

Aluminum

d)

Carbon

21.

Which metalloid has an atomic number of 32?

a)

Antimony

b)

Calcium

c)

Bromine

d)

Germanium

22.

What are the elements called in groups 3-12

a)

Metalloids

b)

Transition Metals

c)

Alkali Metals

d)

Halogens

23.

Which noble gas is found in period 4?

a)

Helium

b)

Krypton

c)

Argon

d)

Neon

24.

Calcium is a

a)

metal

b)

non-metal

c)

metalloid

25.

Chlorine is a

a)

metal

b)

non-metal

c)

metalloid

26.

Boron is a

a)

metal

b)

non-metal

c)

metalloid

27.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
28.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
29.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
30.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
31.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
32.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
33.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
34.
Isotopes are atoms of the same element with different #’s of __________ & therefore different __________.
a)
n0 ;  atomic #’s
b)
p+ ; atomic #’s
c)
e- ; atomic masses
d)
n0 ; atomic masses
35.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
36.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
37.
How many neutrons does an atom of the isotope Neon-22 have?
a)
12
b)
10
c)
22
d)
20
38.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
39.
An atom is electrically neutral when
a)
protons and neutrons are the same
b)
protons and electrons are the same
c)
neutrons and electrons are the same
d)
neutrons balance the protons and electrons
40.
Two isotopes of carbon are carbon-12 and carbon-14.  These isotopes differ from one another by two protons.
a)
true
b)
false
41.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

42.

Bromine-80 has how many neutrons?

a)

41

b)

42

c)

44

d)

45

43.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

44.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
45.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
46.
When an atom gains a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
47.
If an element has 3 valence electrons, what charge will likely form on its ion ?  Hint:  It will lose those electrons.  What happens to the charge when it loses 3 electrons?
a)
+3
b)
+5
c)
-3
d)
-5
48.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
49.
Ionic bonds form between two ions that have 
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges 
50.
Atoms that gain & lose electrons are called _________
a)
ions
b)
isotopes
c)
radioactive
d)
corrosive
51.
Atoms are most stable when their outer shell is filled with electrons.
a)
true
b)
false
52.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
53.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
54.
NH4+
a)
nitrogen hydride
b)
ammonium
55.
OH-
a)
hydronium
b)
hydroxide
56.
NO3-
a)
nitrate
b)
nitrite
57.
SO42-
a)
sulfate
b)
sulfite
58.
PO43-
a)
phosphate
b)
phosphorus oxide
59.
CO32-
a)
carbon oxide
b)
carbonate
60.
C2H3O2-
a)
acetate
b)
carbon hydroxide
61.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
62.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
63.
Ammonium
a)
NH4+
b)
NO3-
c)
NO2-
d)
MnO4-
64.
Hydroxide
a)
Cr2O4-2
b)
Cr2O4-2
c)
O3-2
d)
OH-
65.
What is the name of this polyatomic ion?  CO3-2
a)
Carbonate
b)
Chromate
c)
Carbonite
d)
Chlorate
66.
acetate
a)
C2H3O21-
b)
C3H2O31-
c)
C2H2O31-
d)
C3H3O21-
67.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

68.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

69.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

70.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

71.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

72.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

73.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

74.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

75.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

76.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

77.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

78.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

79.

If I gain electrons I become

a)

Positive because I've added to my atom

b)

negative because I've added electrons

c)

same because i'm balanced

d)

equal because now I have electrons

80.

1 mole of hydrogren has a mass of (a)   g.

81.

The molar mass of oxygen is (a)   g.

82.

Reorder the following in order from greatest mass to lowest mass.

a)

1 mole of Copper

b)

1 mole of Calcium

c)

1 mole of Oxygen

d)

1 mole of Carbon

e)

1 mole of Hydrogen

1)
2)
3)
4)
5)
83.

Calculate the molar mass of water (H2O).

a)

10 g/mol

b)

17 g/mol

c)

18 g/mol

d)

34 g/mol

84.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

85.

What is the molar mass of the diatomic element nitrogen?

a)

7 g/mol

b)

14 g/mol

c)

28 g/mol

86.

Calculate the molar mass of Cu2O.

a)

37 g/mol

b)

45 g/mol

c)

79.5 g/mol

d)

143 g/mol

87.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

88.

Calculate the molar mass of CO2.

a)

14 g/mol

b)

28 g/mol

c)

36 g/mol

d)

44 g/mol

89.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
90.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
91.
Avogadro's number of representative particles is equal to one_____.
a)
kilogram
b)
gram
c)
kelvin
d)
mole
92.
What can be determined from a balanced chemical equation?
a)
Mole ratio of any two substances in the reaction
b)
Energy released in the reaction.
c)
Electron configuration of all elements in the reaction. 
d)
Mechanism involved in the reaction. 
93.
Which is Chemical Equation is Balanced?
a)
CH₄+O₂------CO₂+2H₂O
b)
H₂+O₂-----2H₂O₄
c)
4Al+3O₂-----2Al₂O₃
94.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
95.
In this image, what are the information in red is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
96.

How many moles are in 16.94 g of water? (hint: do you know the formula for water?)

a)

16.94 moles

b)

0.9403 mole

c)

305.2 moles

d)

1.063 moles

97.

How many water molecules are in 5.2 moles of water?

a)

6.0 x 1023 molecules

b)

5.2 molecules

c)

3.1 x 1024 molecules

d)

8.6 x 10-24 molecules

98.

If you want 1.55 moles of nitrogen trichloride, how many grams should you measure out?

a)

0.0129 g

b)

120. g

c)

187 g

d)

9.33 g

99.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
100.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
101.
How many atoms of carbon are in 6.00g of carbon?
a)
1.20x1024atoms C
b)
6.02x1023atoms C
c)
3.01x1023atoms C
d)
1.50x1023atoms C
102.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
103.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
104.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
105.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
106.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
107.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
108.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
109.
The name of SO₃ compound is
a)
sulfate
b)
sulfur oxide
c)
sulfur trioxide
d)
monosulfur trioxide
110.

The compound with a pink square is known as a ___.

a)

Reactant

b)

Product

111.

Which type of reaction is shown?

a)

Combustion

b)

single replacement

c)

double replacement

d)

decomposition

112.

What type of reaction is shown?

a)

Decomposition

b)

Single replacement

c)

Combustion

d)

Combination (or Synthesis)

113.

What type of reaction is this?

a)

Combination (or Synthesis)

b)

Single replacement

c)

Double replacement

d)

Decomposition

114.

Which type of reaction is shown?

a)

Combustion

b)

Combination (or Synthesis)

c)

Decomposition

d)

Double replacement

115.

Which type of chemical reaction involves the production of a single complex compound from several simpler reactants?

a)

Decomposition

b)

Combustion

c)

Combination (or Synthesis)

d)

Single replacement

116.

Which type of reaction is shown?

a)

Single replacement

b)

Double replacement

c)

Combustion

d)

Decomposition

117.
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
118.
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
119.
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
120.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
121.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
122.

How many HCl molecules do you need to balance this equation?

2Mg + ​ (a)   HCl ---> 2MgCl2 + 2H2

Choose from the below words
4
1
2
3
123.

What coefficient should be used to make the following equation balanced?

N2+O2--> __?__NO

a)

1

b)

2

c)

3

d)

4

124.

Drag and drop the coefficients that balance this equation 2 FeFe   + ​ (a)   Cl2Cl_2  ---->  ​ (b)     FeCl3FeCl_3  

Choose from the below words
3
2
125.

Balance this equation. _CF4 + _Br2 → _CBr4 + _F2

a)

3,1,2,1

b)

1,2,1,2

c)

2,2,2,2

126.
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

127.

Determine the coefficients to make the following equation balanced?

__N2 + __O2--> __NO

a)

1, 1, 1

b)

1, 1, 2

c)

2, 2, 2

d)

1, 2, 2

128.
CH4 + O2 --> CO2 + H2O 
a)
single replacement
b)
double replacement
c)
acid base
d)
combustion
129.
Mg + HCl --> MgCl2 + H2
a)
combustion
b)
synthesis
c)
decomposition
d)
single replacement
130.
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
131.

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

a)

#1 represents the enthalpy change for this exothermic reaction.

b)

#2 represents the enthalpy change for this endothermic reaction.

c)

#3 represents the enthalpy change for this endothermic reaction.

d)

#4 represents the enthalpy change for this exothermic reaction.

132.

During an exothermic reaction, heat content in the surroundings increases because

a)

heat energy is destroyed during reactions

b)

the reaction absorbs heat energy

c)

the energy contained in the reactants is lower then the products

d)

the energy contained in the products is lower than the reactants

133.

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)

134.

The graph represents the uniform heating of a substance, starting with the substance as a solid below its melting point. Which line segment listed below represents an increase in potential energy and no change in average kinetic energy?

a)

Line segment AB

b)

Line segment BC

c)

Line segment CD

d)

Line segment EF

135.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 oC from a room temperature of 22.0 oC. It is known that 1.58 x 105 J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

136.

Releasing heat into the surroundings occurs during an ___________________ reaction.

a)

Exothermic

b)

Endothermic

c)

Kinetic Energy

d)

Thermal Energy

137.

A sample of iron receives 50 J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

138.

If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal?

a)

2.34 J/g°C

b)

0.472 J/g°C

c)

6.13 J/g°C

d)

0.163 J/g°C

139.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
140.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
141.
How does a solution become supersaturated?
a)
dissolve lots of solute in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
142.
What is a solvent
a)
the liquid in which a solute is dissolved to form a solution.
b)
Another word for solution
c)
A thing that make drinks turn colors
d)
Its a metal molecole
143.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
144.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
145.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
146.
mixture of two or more substances; dissolved particles are spread evenly throughout the mixture
a)
solvent
b)
solute
c)
mixture
d)
solution
147.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

148.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

149.

How much Ce2(SO4)3 solute is saturated at 80 degrees?

a)

20

b)

15

c)

30

d)

2

150.

How much NaBr solute is saturated at 70 degrees?

a)

110

b)

120

c)

130

d)

140

151.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

152.

At what temperature can you fully dissolve 60g of KNO3?

a)

27

b)

30

c)

37

d)

You cannot determine this

153.

Between which points is the temperature of the substance remaining constant?

a)

A-B only

b)

A-B, C-D, and E-F

c)

B-C only

d)

B-C and D-E

154.

__________ show the change in state of matter as heat is added.

a)

Phase diagrams

b)

Heating curves

c)

Density graphs

d)

Temperature plots

155.

The melting point of the sample is

a)

-60 ºC

b)

20 ºC

c)

60 ºC

d)

100 ºC

156.

Which letter indicates where water is in both the solid and liquid phase at the same time?

a)

A

b)

B

c)

C

d)

D

e)

E

157.

In which region(s) does temperature increase?

a)

Region C only

b)

Regions B and D

c)

Regions A, C, and E

d)

Regions A and B

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