wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Final Review

Total questions: 106

Worksheet time: 3hrs 55mins

Name
Class
Date
1.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

2.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

3.

Shivani measures out 6.0 moles of epsom salt (MgSO4) to put in her bath. How many grams of MgSO4 went in the bath?

a)

3.6 x 1024 g

b)

720 g

c)

0.050 g

d)

340 g

4.

Which of the following dimensional analysis setups will correctly convert 27.76 g of Li to atoms of Li?

a)

A

b)

B

c)

C

d)

D

5.

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%

6.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
7.

Which equation is balanced?

a)

PbO2 + 2H2

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

8.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
9.

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

10.

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

11.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
12.
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
13.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
14.
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
15.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
16.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
17.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)
Synthesis
b)
Decomposition
c)
Single Replacement Replacement
d)
Double Replacement Replacement
18.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
19.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
20.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
21.

What is the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure? (Round your answer to the ones place, ex. 111)

22.

A quantity of gas has a volume of 250 L, at 290 K and 304 kPa of pressure. What volume must the gas be for the gas to be at 273 K and 101 kPa? (Round your answer to the ones place, ex. 111)

23.

What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20⁰C and 1.2 atm? (Round your answer to the ones place, ex. 11)

24.

What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 40⁰C? (Round your answer to the hundredths place, ex. 0.11)

25.

A gas at 1.10 atm was measured at 295 K and 326 mL. What will the temperature be if the gas is moved to a container that is 168 mL and the pressure is adjusted to 1.90 atm? (Round your answer to the ones place, ex. 111)

26.

What is the pressure change when a constant volume of gas at 1.00 atm is heated from 20.0 °C to 30.0 °C? (Round your answer to the hundredths place, example: 1.23)

27.

A sample of gas has a pressure of 700 mmHg and 30.0 degrees C. At what temperature, would the pressure be 600 mmHg if the volume remains constant? (Give your answer in Kelvin, and round to the ones place, example: 123)

28.

You have 600 mL of air at 20 degrees Celcius. It's volume is compressed to 400 mL. What is the new temperature of the gas? (Give your answer in Kelvin and round your answer to the ones place, example: 123).

29.

A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be? (Round to the nearest tenth, example 0.1).

30.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

31.
Which of the following word pairs correctly completes the sentence below?
_______ are corrosive substances characterized as having a strong smell, a sour taste, and a _______.
a)
Acids; pH less than 7
b)
Acids; pH greater than 7
c)
Bases; pH greater than 7
d)
Bases; pH less than 7
32.
Which of the following is a base?
a)
orange juice
b)
water
c)
vinegar
d)
dishwashing detergent
33.
 Which of the following is an acid?
a)
shampoo
b)
baking soda
c)
orange juice
d)
water
34.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
35.
On the pH scale what numbers are bases?
a)
8-14
b)
0-7
c)
7
d)
1
36.
On the pH scale what numbers are acids?
a)
8-14
b)
0-7
c)
7
d)
1
37.

What type of radioactive decay is this example?

a)

Alpha

b)

Negative Beta

c)

Positive Beta

d)

Gamma

38.

How is the alpha particle written in a nuclear equation?

a)

42He

b)

24He

c)

0-1e

d)

00γ

39.

How is the negative beta particle written in a nuclear equation?

a)

42He

b)

0+1e

c)

0-1e

d)

00γ

40.

If we start off with element 5024X after an gamma decay we get another element that looks like

a)

5124X

b)

5023X

c)

5024X

d)

5125X

41.

22087Fr —› 42He + ____

a)

22089Ac

b)

22490Th

c)

21685At

d)

21688Ra

42.

146C —› 0-1e + ____

a)

126C

b)

147N

c)

148O

d)

145B

43.
Has the highest penetrating power.  Can penetrate our body.  Even several cm thick of lead or several meters thick of concrete cannot stop all of it.
a)
Alpha
b)
Beta
c)
Gamma
44.
Has the lowest penetrating power.  Can only penetrate 0.05 mm into the body and can be stopped by a piece of paper or clothing.
a)
Alpha
b)
Beta
c)
Gamma
45.
The process of nuclear change in an atom of radioactive material is called... 
a)
nuclear decay
b)
nuclear mass
c)
isotopes
d)
radon
46.

He discovered a very dense, very small, positive nucleus inside atoms.

a)

John Dalton

b)

J. J. Thomson

c)

Ernest Rutherford

d)

Neils Bohr

47.

He discovered negative particles inside neutral atoms.

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

48.

Man who discovered neutrons.

a)

John Dalton

b)

J. J. Thomson

c)

Ernest Rutherford

d)

James Chadwick

49.

He did the gold foil experiment.

a)

J. J. Thomson

b)

Ernest Rutherford

c)

Neils Bohr

d)

Werner Heisenberg

50.

He hypothesized that electrons can only orbit at certain distances from the nucleus.

a)

Democritus

b)

J.J. Thomson

c)

Ernest Rutherford

d)

Neils Bohr

51.

He made observations of colors given off by excited electrons.

a)

Jonn Dalton

b)

J.J. Thomson

c)

Ernest Rutherford

d)

Neils Bohr

52.

He proposed the Plum Pudding Model of the atom.

a)

John Dalton

b)

J. J. Thomson

c)

Earnest Rutherford

d)

Neils Bohr

53.

He proposed the "solar system" or "planetary" model of the atom.

a)

John Dalton

b)

J. J. Thomson

c)

Neils Bohr

d)

James Chadwick

54.

On the periodic table, the PERIODS are

a)

the rows that go left to right.

b)

the columns that got top to bottom.

c)

the little spot at the end of a sentence.

55.

On the periodic table, the GROUP or FAMILY are

a)

the rows that go left to right.

b)

the columns that got top to bottom.

c)

your people that you have a lot in common with.

56.

Metals are MOSTLY _____ at room temperature.

a)

solid

b)

liquid

c)

gas

57.

Nonmetals are MOSTLY _____ at room temperature.

a)

solid

b)

liquid

c)

gas

58.

How are the elements on the periodic table arranged?

a)

Atomic mass

b)

Atomic number

c)

State of matter

d)

Type of element (metal, nonmetal, metalloid)

59.

Valence electrons are

a)

the number of electrons in the outer most energy shell.

b)

the number of protons in the nucleus.

c)

the atomic mass.

d)

total number of electrons.

60.

How many valence electrons does phosphorus (P).

a)

3

b)

5

c)

15

d)

31

61.

Which of the following elements has 7 valence electrons?

a)

Sodium (Na)

b)

Aluminum (Al)

c)

Fluorine (Fl)

d)

Calcium (Ca)

62.

Which of the following is a metal?

a)

Calcium (Ca)

b)

Neon (Ne)

c)

Oxygen (O)

d)

Sulfur (S)

63.

Nitrogen is a

a)

metal.

b)

nonmetal.

c)

metalloid.

64.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
65.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
66.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
67.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
68.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
69.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)
beryllium, Be
b)
potassium, K
c)
titanium, Ti
d)
yttrium, Y
70.
What is the family name of this group of elements? 
a)
Alkali metals 
b)
Halogens 
c)
Noble Gases 
d)
Alkali Earth Metals 
71.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
72.

Match the following

a)

Na2O2Na_2O_2

1.

Sodium peroxide

b)

KCl

2.

Potasium chloride

c)

FeCl2FeCl_2

3.

Iron (II) chloride

d)

N2O4N_2O_4

4.

Dinitrogen Tetroxide

e)

SCl6SCl_6

5.

sulfur hexachloride

73.
What would be the proper chemical formula for combining Al3+ and l- :
a)
Al l3
b)
Al3l
c)
Al l
d)
Al3 l3
74.

What is the name of the following compound: CuBr2

a)

copper bromine

b)

copper bromide

c)

copper(I) bromide

d)

copper(II) bromide

75.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
76.

The correct name for SiO2 is:

a)

Silicon dioxide

b)

Silicon oxide

c)

Sulfur dioxide

d)

Silicon oxygen

77.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

78.

How many valence electrons does Hydrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

79.

How many valence electrons does Helium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

80.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

81.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
82.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
83.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
84.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
85.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
86.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
87.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
88.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
89.

The freezing point of a solution is ______ the freezing point of the pure solvent.

a)

higher than

b)

the same as

c)

lower than

d)

higher or lower than

90.

In a sugar and water solution, some sugar remains undissolved in the water. Which term best describes the solution?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

None of these

91.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
92.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
93.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)
94.

H2O has how many covalent bonds?

a)

0

b)

1

c)

2

d)

3

95.

Match the following

a)

Covalent Bond

1.

Formed between two nonmetals

b)

Ionic Bond

2.

Formed between metal and nonmetal

c)

Lone Pair

3.

2 electrons not shared by atoms in a covalent compound

d)

Line

4.

How 2 bonding electrons are shown in a dot diagram

e)

Dots

5.

How lone pair electrons are shown in a dot diagram

96.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
97.
The total energy of all the particles in a substance is called: 
a)
temperature
b)
thermal energy
c)
degrees
d)
mass
98.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

99.

For a skillet, used for cooking, do you want a high or low specific heat

a)

High, so that it will need more energy to heat up

b)

Low, so that it will change temperature quickly

100.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)
a)
25g
b)
30g
c)
20g
d)
50g
101.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?
a)
Exothermic
b)
Endothermic
102.

What is happening to the particles in the substance between points D and E?

a)

Melting

b)

Freezing

c)

Vaporizing

d)

Sublimating

103.

The melting point of the sample is

a)

-60 ºC

b)

-100 ºC

c)

60 ºC

d)

100 ºC

104.

Given the heating curve of a solid being heated at a constant rate, what is the boiling point of this substance?

a)

20°C

b)

50°C

c)

110°C

d)

170°C

105.

What phase of matter exists in part C of the graph?

a)

Gas

b)

Liquid

c)

Solid

d)

Plasma

106.

What phase of matter exists in part E of the graph?

a)

Gas

b)

Liquid

c)

Solid

d)

Plasma

Similar Resources on Wayground

Regents Chemistry Midterm Review #1

105 questions

Regents Chemistry Midterm Review #1

quiz

Worksheet

•

10th - 12th Grade

Periodic Table Quiz Review

103 questions

Periodic Table Quiz Review

quiz

Worksheet

•

10th - 12th Grade

SAE Practice 1

109 questions

SAE Practice 1

quiz

Worksheet

•

9th - 12th Grade

Combined PSAT review and Chemistry LBC L11-12 parts of atom, mass, charge

101 questions

Combined PSAT review and Chemistry LBC L11-12 parts of atom, mass, charge

quiz

Worksheet

•

9th - 12th Grade

19.3 Acid-Base Nomenclature

106 questions

19.3 Acid-Base Nomenclature

quiz

Worksheet

•

10th - 12th Grade

Assessment - Fall semester (long)

110 questions

Assessment - Fall semester (long)

quiz

Worksheet

•

10th - 12th Grade

End of Year Review

102 questions

End of Year Review

quiz

Worksheet

•

9th - 12th Grade

Concept 3 Review

102 questions

Concept 3 Review

quiz

Worksheet

•

9th - 12th Grade