wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Final Review

Total questions: 120

Worksheet time: 30hrs 0mins

Name
Class
Date
1.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
2.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
3.

__ Al + __ FeO → Al2O2 + __ Fe

a)

1, 1, 2

b)

2,1,2

c)

2, 2, 2

d)

2,4,2

4.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
5.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
6.
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
7.
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
8.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
9.
What is the mole ratio in the following reaction:
2CO  +  O2  → 2CO2
a)
2:1:2
b)
1:1:1
c)
1:2:1
d)
Have no clue what a mole ratios is!!
10.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron (Fe) can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
11.

In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen (aluminum is asked for, oxygen is given)?

a)

10/6

b)

3/4

c)

4/3

d)

2/3

12.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
13.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
14.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
d)
None
15.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

16.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

17.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

18.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

19.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
20.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

21.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
22.

As one moves down the pH scale from 14 to 1, what happens to the concentration of H+ in the solution?

a)

concentration of H+ decreases

b)

concentration of H+ increases

c)

concentration of H+ stays the same

23.

If pure water is added to an acid with a pH of 3, what happens to the pH of the solution?

a)

the pH increases to above 3

b)

the pH decreases to below 3

c)

the pH stays the same at 3

24.

For a solution at 25oC, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

25.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

26.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

27.

If a nitrogen gas occupies a volume of 500 mL at a pressure of 0.971 atm. What volume will the gas occupy at a pressure of 1.50 atm, assuming the temperature remains constant?

a)

323.6 mL

b)

728.25 mL

c)

772.39 mL

d)

0.002 mL

28.

According to Boyle's law, at constant temperature, as the pressure of a given sample of gas is increased, the volume will –

a)

Increase

b)

Decrease

c)

Remains the same

d)

They are not related

29.
What is the equation for Charles' Law?
a)
P1V1=P2V2
b)
V1/T1=V2/T2
c)
V1/n1=V2/n2
d)
P1/T1=P2/T2
30.
What is the equation for Boyle's Law?
a)
P1V1=P2V2
b)
V1/T1=V2/T2
c)
V1/n1=V2/n2
d)
P1/T1=P2/T2
31.
If 200 mL of a gas at 27°C is cooled to -33°C at a constant pressure, the volume will be
a)
250 mL
b)
204 mL
c)
196 mL
d)
160 mL
32.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
33.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

34.

A scientist needs to store 28.0 moles of xenon gas at STP in the lab. What size gas tank will he need?

a)

628 L

b)

473 L

c)

219 L

d)

376 L

35.

A water bottle at STP is cooled to -155°C. What is the new pressure?

a)

3.2 atm

b)

0.43 atm

c)

1.8 atm

d)

0.27 atm

36.

The pressure of a 6.5 L sample of oxygen gas is measured to be 3.8 atm. If the gas is transferred into a 12 L tank, what is the new pressure?

a)

6.6 atm

b)

3.9 atm

c)

4.5 atm

d)

2.1 atm

37.
In a lab, a scientist calculates that he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
38.
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
39.
Find the percentage composition of Mg in Mg3(PO4)2.
   

a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
40.
What is the percentage of chromium in K2Cr2O7?
a)
38.1%
b)
27.2%
c)
34.7%
d)
100%
41.
Which of the following would decrease the rate of solution when dissolving a solid in water?
a)
Raise the temperature of the solution
b)
Crush the solid before mixing
c)
Stir the solution after mixing
d)
Use a single cube of solid
42.
What will allow more solute to be dissolved in a solvent.
a)
adding more solute
b)
stiring
c)
cooling solution
d)
heat
43.

Stirring the solution increases the rate of dissolution (rate of dissolving).

a)

True

b)

False

44.

The smaller the particle size the faster the rate of dissolution (rate of dissolving).

a)

True

b)

False

45.

Which will dissolve faster? Crushed table salt or a cube of table salt. Assume they have an equal mass.

a)

crushed table salt

b)

crystal of table salt

46.

When no more solute dissolves the solution is _________

a)

supersaturated

b)

unsaturated

c)

saturated

d)

extra saturated

47.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q = m Cp ∆T
b)
Q = m Cp
c)
Q =  ½ m v
d)
m = Q Cp
48.
If the specific heat of water is 4,186 J/kg∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? 
a)
-80,371.2 J
b)
44,938.6 J
c)
80,371.2 J
d)
112,575.9 K
49.
Water has a specific heat of 4184 J/KgºC.  Wood has a specific heat of 1760 J/KgºC.  What material needs more energy to raise the temperature 1ºC
a)
Wood
b)
Water
c)
Both are the same
50.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
51.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
52.

What is the molar mass of Sr(NO3)2?

a)

211.64 g/mol

b)

163.64 g/mol

c)

149.63 g/mol

d)

197.63 g/mol

53.

How many octane molecules would be in 8.4 moles of octane (C8H18)?

a)

959.8

b)

5.06 x 1024

c)

5.06

54.

The symbol represents a(n) ___ particle.

a)

positron

b)

beta

c)

gamma

d)

alpha

55.

In ___ decay, an neutron is changed into an electron and a proton.

a)

alpha

b)

beta

c)

gamma

d)

positron

56.

A(n) ___ particle consists of 2 protons and 2 neutrons.

a)

alpha

b)

beta

c)

gamma

d)

positron

57.

When a proton decays into a neutron and a(n) ___, this is called ___ decay.

a)

electron, beta minus

b)

electron, beta plus

c)

positron, beta minus

d)

positron, beta plus

58.

The time it takes for half of a sample of radioactive particles to decay is called ___.

a)

decay time

b)

half-life

c)

one life

d)

years

59.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
60.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
61.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
62.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
63.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
64.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
65.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
66.
What is the shape of this molecule?
a)
bent
b)
linear
c)
trigonal pyramidal
d)
tetrahedral
67.
What is the shape of this molecule?
a)
Linear
b)
bent
c)
tetrahedral
d)
trigonal planar
68.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Pyramidal
69.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Pyramidal
70.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
71.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
72.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
73.
K20 - name?
a)
potassium dioxide
b)
potassium oxide
c)
potassium oxygen
d)
dipotassium dioxide
74.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
75.

MgO- name?

a)

oxygen magnesium

b)

magnesium oxide

c)

magnesium oxate

d)

magnesium oxygenate

76.
What is the chemical formula for phosphorus triiodide?
a)
P3I
b)
PI
c)
P3I3
d)
PI3
77.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
78.
Name the acid: H3PO3
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
79.

Name the following ionic compound: Cr(NO3)3

a)

chromium III nitride

b)

chromium II nitride

c)

chromium II nitrate

d)

chromium III nitrate

80.

Name the following ionic compound: MgSO4

a)

magnesium (II) sulfide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium (II) sulfate

81.

How many protons are in the nucleus of the element shown?

a)

19

b)

9

c)

10

d)

28

82.

What is the mass number of the element shown?

a)

15

b)

7

c)

8

d)

0

83.

How many protons and neutrons are in the nucleus of the atom shown?

a)

9 protons and 19 neutrons

b)

19 protons and 9 neutrons

c)

10 protons and 9 neutrons

d)

9 protons and 10 neutrons

84.

Which name is correct for the atom shown?

a)

Carbon-6

b)

Carbon-14

c)

Carbon-8

d)

Carbon-0-

85.

An atom has 12 protons and 13 neutrons in its nucleus. Which is the correct symbol?

a)
b)
c)
d)
86.

An atom has 9 protons and 10 neutrons in its nucleus. Which is the correct symbol?

a)
b)
c)
d)
87.

If you need to know what something smells like you will

a)

never put the chemical directly near your face

b)

Waft the air above it

c)

sniff directly

d)

never smell in the lab , always cover your nose

88.

What should you not do in the lab?

a)

follow directions

b)

run

c)

prank

d)

walk

e)

push/shove

89.
What should you do if you break glass in the lab?
a)
Tell the teacher.
b)
Sweep up the glass.
c)
Pick up the glass with your hands.
d)
Ignore it; the teacher will clean it up when she sees it later.
90.
Elements in the same ____________ tend to have similar properties
a)
group
b)
period
91.
The density of pyrite is 5g/cm3 . This is an example of 
a)
physical intensive property
b)
physical extensive property
c)
chemical change
d)
chemical property
92.
Wood burning is an example of _______
a)
physical intensive property
b)
physical extensive property
c)
chemical change
d)
Physical change
93.
Physical properties of a substance include _________
a)
color and odor
b)
melting and boiling points
c)
density 
d)
all of the choices are correct
94.
The mass of a lead cube is 64 grams. This is an example of 
a)
physical intensive property
b)
physical extensive property
c)
chemical change
d)
physical change
95.
Which of the following is a chemical property of milk?
a)
it is white
b)
it has fats
c)
it has turns sour if left out of the refridgerator
d)
it is soluble in water
96.
What kind of properties can only be observed when a substance changes into a different substance?
a)
physical properties
b)
chemical properties
c)
liquid properties
d)
real properties
97.
Which of the phases have particles that have a fixed volume but not a fixed shape? 
a)
solid
b)
liquid
c)
gas
d)
plasma
98.
Which phase has a constant volume and a constant shape? 
a)
solid
b)
liquid
c)
gas
d)
plasma
99.
What is the right part of a chemical equation called?
H2 + O → H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
100.
What are the products of the chemical reaction pictured?
a)
CH4 and CO2
b)
CH4 and O2
c)
CO2 and H2O
d)
O2 and H2O
101.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
102.
DIFFERENT kinds of atoms chemically combined to form a substance are
a)
Mixture
b)
Element
c)
Compound
d)
Substance
103.
A ____________ mixture has different concentrations of particles throughout. 
a)
Homogeneous
b)
Heterogeneous
c)
Solid
d)
Liquid
104.
DIFFERENT kinds of atoms chemically combined to form a substance are
a)
Mixture
b)
Element
c)
Compound
d)
Substance
105.
Italian Salad Dressing is a . . .
a)
heterogeneous mixture
b)
homogeneous mixture
c)
Pure Substance
d)
Compound
106.

The law that states that the repeating chemical and physical properties of elements relate to and depend on the elements' atomic numbers is _______.

a)
periodic
b)
period
c)
periodic table of the elements
d)
periodic law
107.

How was Dmitri Mendeleev's periodic table organized?

a)

atomic number

b)

atomic mass

c)

it wasn't organized

d)

nuetrons

108.

  Why were there blank spaces left in Mendeleev's periodic table?

a)

 He didn't know what to put there.

b)

  Undiscovered elements not yet known.

c)

Multiple elements could have fit

d)

He forgot to add the elements in

109.

______arranged elements in a periodic table according to the increasing order of atomic number

a)

John Newlands

b)

Dimitri Mendeleev

c)

Henry Moseley

d)

Lothar Mayer

110.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
111.
Which of the following is the most reactive in water?
a)
Lithium
b)
Sodium
c)
Potassium
112.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

113.

As you move down the group, halogens' reactivity...

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

114.

Which halogen is the most reactive?

a)

iodine

b)

chlorine

c)

bromine

d)

fluorine

115.

Which halogen is the least reactive?

a)

iodine

b)

chlorine

c)

bromine

d)

fluorine

116.

Classify:

2H2 + O2 ---->2H2O

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

117.

Classify:

2KClO3 ---->2KCl + 3Os

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

118.

Classify:

Mg + 2HCl ----> MgCl2 + H2

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

119.

Classify:

2HCl + 2NaOH -----> NaCl + H2O

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

120.

Classify:

CH4 + O2 → CO2 + H2O

a)

single replacement

b)

double replacement

c)

synthesis

d)

combustion

Similar Resources on Wayground

Periodic Table

122 questions

Periodic Table

quiz

Worksheet

•

9th Grade

IPC Semester 2 Exam Review

120 questions

IPC Semester 2 Exam Review

quiz

Worksheet

•

10th Grade

ôn tập học kì 1 lớp 11

117 questions

ôn tập học kì 1 lớp 11

quiz

Worksheet

•

11th Grade

Matter and Measurement

122 questions

Matter and Measurement

quiz

Worksheet

•

10th - 12th Grade

Periodic Table & Trends

122 questions

Periodic Table & Trends

quiz

Worksheet

•

10th Grade

Physical Science Unit 3 Test Review

125 questions

Physical Science Unit 3 Test Review

quiz

Worksheet

•

9th - 12th Grade

GRADE 10- ARYABHATTA

120 questions

GRADE 10- ARYABHATTA

quiz

Worksheet

•

10th Grade