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Science 10 Chemistry Test

Total questions: 123

Worksheet time: 3hrs 57mins

Name
Class
Date
1.

WHMIS stands for (a)   ​ (b)   ​ (c)   ​ (d)   ​ (e)  

Choose from the below words
Workplace
Hazardous
Materials
Information
System
Wholesome
Survey
Harmonious
Inclusive
Mandated
2.

Match the following

a)

1.

Biohazard

b)

2.

Flammable

c)

3.

Oxidizing

d)

4.

Explosive

e)

5.

Compressed Gas

3.

Match the following

a)

1.

Poisonous

b)

2.

Long-term health effects

c)

3.

Warning (less serious health effects)

d)

4.

Corrosive

4.

Which symbol should be on a product that could explode in heat?

a)

b)

c)

d)

5.

Which symbol should be on a product that can cause cancer if exposed to it for a long period of time?

a)

b)

c)

d)

6.

Which symbol should be on a product that could cause skin irritation?

a)

b)

c)

d)

7.

Which symbol should be on a product that could cause a fire to get worse?

a)

b)

c)

d)

8.

Which symbol should be on a product that could easily catch on fire?

a)

b)

c)

d)

9.
If you break glassware in the lab, you should...
a)
Tell the teacher
b)
Clean it up quickly before the teacher notices
c)
Scream at the top of your lungs
10.
When in the lab...
a)
long sleeves and loose clothing should be rolled up
b)
closed toe shoes should be worn
c)
long hair should be pulled back
d)
all of the above
11.
Before leaving the lab you should always wash your hands.
a)
True 
b)
False
12.

List as many unsafe lab practices as you can see in the picture.

4 lines
13.

Typically in an atom, which two subatomic particles are equal in number?

a)

protons and neutrons

b)

all subatomic particles are equal in number

c)

neutrons and electrons

d)

protons and electrons

14.

Which subatomic particle is counted to determine the type of element the atom represents?

a)

proton

b)

neutron

c)

electron

d)

boron

15.
Particles in an atom that are neutral and have no charge are 
a)
negatrons 
b)
electrons 
c)
neutrons 
d)
protons 
16.
Adding or subtracting neutrons (charge = 0, mass = 1) makes the element change into an...
a)
ion
b)
mixture
c)
isotope
d)
neutral atom
17.
The atomic mass is equal to _.
a)
the number of protons only
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons, neutrons, and electrons.
18.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
19.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
20.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

21.

What is the charge of a proton?

a)

positive

+

b)

negative

-

c)

neutral

(no charge)

22.

What is the charge of an electron?

a)

proton

+

b)

neutral

(no charge)

c)

negative

-

23.

What is the charge of a neutron?

a)

positive

+

b)

neutral

(no charge)

c)

negative

-

24.

What is the mass of a proton?

a)

0 amu

b)

1 amu

c)

2 amu

25.

What is the mass of an electron?

a)

0 amu

b)

1 amu

c)

2 amu

26.

What is the mass of a neutron?

a)

0 amu

b)

1 amu

c)

2 amu

27.

Where is a proton located in an atom?

a)

in the nucleus

b)

outside the nucleus

c)

outside the atom

28.

Where is an electron located in an atom?

a)

in the nucleus

b)

outside the nucleus

c)

outside the atom

29.

Where is a neutron located in an atom?

a)

in the nucleus

b)

outside the nucleus

c)

outside the atom

30.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

31.

Metals tend to

a)

gain electrons

b)

lose electrons

32.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
33.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
34.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
35.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
36.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
37.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
38.

When a nonmetal gains electrons, it becomes this type of ion.

a)

Anion

b)

Cation

39.

When a metal loses electrons, it becomes this type of ion.

a)

anion

b)

cation

40.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
41.
Which is the correct formula for sodium chloride?
a)
SoCl
b)
SdCl
c)
NaCl
d)
NaCl2
42.
Which of the following BEST describes ionic bonds?
a)
Bond held together by a sea of electrons
b)
Bond of two ions of opposite charges held together by electrostatic forces
c)
Bond held together by the sharing of electrons
d)
Bond between hydrogen and an anion or polyatomic ion.
43.

Is this compound ionic or covalent?

a)

Ionic

b)

Covalent

44.

Is this compound ionic or covalent?

a)

ionic

b)

covalent

45.

Check all that apply.


S2F4

disulfur tetrafluoride

a)

ionic compound

b)

contains a multivalent ion

c)

contains a polyatomic ion

d)

covalent compound

46.

Check all that apply.


Fe3(PO4)2

iron (II) phosphate

a)

ionic compound

b)

contains a multivalent ion

c)

contains a polyatomic ion

d)

covalent compound

47.

Check all that apply.


ZnCO3

zinc carbonate

a)

ionic compound

b)

contains a multivalent ion

c)

contains a polyatomic ion

d)

covalent compound

48.

Check all that apply.


Br2I4

dibromine tetraiodide

a)

ionic compound

b)

contains a multivalent ion

c)

contains a polyatomic ion

d)

covalent compound

49.

What are compounds made of?

a)

Ions

b)

Elements

c)

Molecules

d)

Atoms

50.

What are polyatomic ions?

a)

an ion that is between nonmetals

b)

Ions with no charge

c)

A positive or negatively charged group of atoms

d)

a metal and nonmetal

51.

What is a molecule?

a)

A covalently bonded group of atoms

b)

A negatively charged nonmetal ion

c)

A compound formed by sharing electrons

d)

A positively charged metal ion

52.

How many electrons are shared in a single bond?

a)

2

b)

4

c)

8

d)

6

53.

What are the properties of covalent compounds?

a)

Made up of nonmetals sharing electrons

b)

Solid, liquid, or gas

c)

High melting and boiling points

d)

Can conduct electricity when dissolved in water

54.

What is the main reason for elements to form compounds?

a)

To become more stable

b)

To form covalent bonds

c)

To gain metallic properties

d)

To increase their atomic number

55.

Organize these options into properties of ionic compounds or properties of covalent compounds

Categorize the following

Made up a (+) metallic ions and (-) nonmetallic ions after metal transferred e- to nonmetal

Arranged in regular repeating patterns and crystals

High melting and boiling points

Can conduct electricity when dissolved in water

Made up of nonmetals sharing e-

Molecules that can be solid, liquid, or gas

Low melting and boiling point

Cannot conduct electricity when dissolved in water

Properties of Ionic Compounds
Properties of Covalent Compounds
56.

Match the bonds with the amount of electrons

a)

Triple bond

1.

6 electrons (3 pairs) shared

b)

Double bond

2.

4 electrons (2 pairs) shared

c)

Single bond

3.

2 electrons (1 pairs) shared

57.

Cations are ​ (a)   ​ charged metal ion because the metals ​ (b)   electrons

Choose from the below words
positively
lose
negatively
gain
58.

Anions are ​​ (a)   charged metal ion because the metals ​ (b)   ​electrons

Choose from the below words
negatively
gain
positvely
lose
59.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
60.
What's the formula for chlorine dioxide
a)
ClO2
b)
CLO
c)
ClO3
d)
HClO2
61.

Name the following covalent compound.

NO

a)

Mononitrogen Oxide

b)

Nitrogen monoxide

c)

Nitrogen Oxide

62.

Name N2O3

a)

Nitrogen Oxide

b)

Dinitrogen Trioxide

c)

Nitrogen Trioxide

63.

Match the following

a)

CF4

1.

Carbon Tetrafluoride

b)

CH4

2.

Carbon Tetrahydride

c)

SCl2

3.

Sulfur Dichloride

d)

NBr3

4.

Nitrogen TriBromide

e)

CO2

5.

Carbon Dioxide

64.

Hydrogen needs _____ electrons in its valence shell to be stable.

a)

4

b)

8

c)

2

d)

3

65.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
66.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
67.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
68.
The chemical formula of carbon tetrachloride is
a)
CCl
b)
C₄Cl
c)
CCl₄
d)
C(IV)Cl
69.

Which is the correct Lewis Dot Structure for NH3?

a)

b)

c)

70.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
71.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)

b)

c)

d)

72.

Write the chemical formula for Phosphorus Mononitride

(a)  

73.

What is the molecular structure of water?

a)

1 Hydrogen

2 Oxygen

b)

1 Hydrogen

1 Oxygen

c)

2 Hydrogen

2 Oxygen

d)

2 Hydrogen

1 Oxygen

74.

Which side of the water molecule has a slightly positive charge?

a)

Oxygen

b)

Hydrogen

c)

It's all positive

d)

It's all negative

75.

Which side of the water molecule has a slightly negative charge?

a)

It's all negative

b)

It's all positive

c)

Hydrogen

d)

Oxygen

76.

What is the boiling point of water?

a)

0 C

b)

100 C

c)

200 C

d)

50 C

77.

What is the freezing point of water?

a)

0 C

b)

100 C

c)

200 C

d)

50 C

78.

What is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius?

a)

Surface Tension

b)

Density

c)

Polarity

d)

Specific Heat Capacity

79.

True or False: Ice is Less Dense than Water

a)

True

b)

False

80.

What is the property of the surface of a liquid that allows it to resist an external force, due to the cohesive nature of its molecules?

a)

Cohesion

b)

Surface Tension

c)

Adhesion

d)

Polarity

81.

What is the movement of water within the spaces of a porous material due to the forces of adhesion, cohesion, and surface tension

a)

Malleability

b)

Conductivity

c)

Freezing Point

d)

Capillary Action

82.

How is this lizard able to run across water?

a)

Capillary Action

b)

The lizard is really light

c)

The water is a little frozen

d)

Surface Tension

83.

A synthesis reaction has two or more reactants (formulas on the LEFT of the arrow) but only one product (on the RIGHT). Which is a synthesis reaction?

a)

2 Mg + O2 --> 2 MgO

b)

NH4NO3 --> N2O + 2 H2O

c)

2 Fe + 3 CuCl2 --> 2 FeCl3 + 3 Cu

d)

CaBr2 + K2S --> 2 KBr + CaS

84.

Which is a synthesis reaction?

a)

2 Al + Fe2O3 --> Al2O3 + 2 Fe

b)

2 Bi(NO3)3 + 3 K2S --> Bi2S3 + 6 KNO3

c)

3 Ca + N2 --> Ca3N2

d)

2 HCl --> H2 + Cl2

85.

Which is a synthesis reaction?

a)

2 BiCl3 + 3 H2S --> Bi2S3 + 6 HCl

b)

Mg + 2 HCl --> MgCl2 + H2

c)

2 H2O --> 2 H2 + O2

d)

P4 + O2 --> P4O10

86.

A decomposition reaction has one reactant breaking down into more than one product. Which is a decomposition reaction?

a)

2 Mg + O2 --> 2 MgO

b)

NH4NO3 --> N2O + 2 H2O

c)

2 Fe + 3 CuCl2 --> 2 FeCl3 + 3 Cu

d)

CaBr2 + K2S --> 2 KBr + CaS

87.

Which is a decomposition reaction?

a)

2 Al + Fe2O3 --> Al2O3 + 2 Fe

b)

2 Bi(NO3)3 + 3 K2S --> Bi2S3 + 6 KNO3

c)

3 Ca + N2 --> Ca3N2

d)

2 HCl --> H2 + Cl2

88.

Which is a decomposition reaction?

a)

2 BiCl3 + 3 H2S --> Bi2S3 + 6 HCl

b)

Mg + 2 HCl --> MgCl2 + H2

c)

2 H2O --> 2 H2 + O2

d)

P4 + O2 --> P4O10

89.

A single replacement reaction has one element and one compound on BOTH the left and right sides of the arrow. Which is single replacement?

a)

2 Mg + O2 --> 2 MgO

b)

NH4NO3 --> N2O + 2 H2O

c)

2 Fe + 3 CuCl2 --> 2 FeCl3 + 3 Cu

d)

CaBr2 + K2S --> 2 KBr + CaS

90.

Which is a Single Replacement reaction?

a)

2 Al + Fe2O3 --> Al2O3 + 2 Fe

b)

2 Bi(NO3)3 + 3 K2S --> Bi2S3 + 6 KNO3

c)

3 Ca + N2 --> Ca3N2

d)

2 HCl --> H2 + Cl2

91.

A doublereplacement reaction has 2 compounds on BOTH the left and right sides of the arrow. Which is double replacement?

a)

2 Mg + O2 --> 2 MgO

b)

NH4NO3 --> N2O + 2 H2O

c)

2 Fe + 3 CuCl2 --> 2 FeCl3 + 3 Cu

d)

CaBr2 + K2S --> 2 KBr + CaS

92.

Which is a Double Replacement reaction?

a)

2 Al + Fe2O3 --> Al2O3 + 2 Fe

b)

2 Bi(NO3)3 + 3 K2S --> Bi2S3 + 6 KNO3

c)

3 Ca + N2 --> Ca3N2

d)

2 HCl --> H2 + Cl2

93.

A combustion reaction has O2 (element) for one of the reactants (LEFT), and the products are CO2 and H2O (both compounds. Which is the combustion reaction?

a)

Cr2(SO4)3 + 6 NaOH --> Cr(OH)3 + 3 Na2SO4

b)

CH4 + 2 O2 --> CO2 + 2 H2O

94.

Which is a combustion reaction?

a)

C3H8 + 5 O2 --> 3 CO2 + 4 H2O

b)

Mg + 2 HCl --> MgCl2 + H2

95.

What kind of reaction is

2 HCl --> H2 + Cl2?

a)

synthesis

b)

decomposition

c)

single replacement

d)

combustion

96.

What kind of reaction is

2 Al + Fe2O3 --> Al2O3 + 2 Fe?

a)

synthesis

b)

double replacement

c)

single replacement

d)

combustion

97.

What kind of reaction is

C3H8 + 5 O2 --> 3 CO2 + 4 H2O?

a)

synthesis

b)

double replacement

c)

single replacement

d)

combustion

98.

What kind of reaction is

2 Mg + O2 --> 2 MgO ?

a)

synthesis

b)

double replacement

c)

single replacement

d)

combustion

99.

In this photosynthesis word equation, what is the end product that is needed by humans to use as energy?

a)

oxygen

b)

glucose

c)

light energy

d)

water

100.

What is the chemical formula for glucose?

a)

C6H12O6

b)

O2

c)

CO2

d)

H2O

101.

Is the following equation balanced?

Al + O2 ---> 2Al2O3

a)

Yes

b)

No

102.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
103.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
104.
How many oxygen atoms are present in the following? 
4Ca(OH)2
a)
4
b)
6
c)
8
d)
1
105.

The small numbers in a chemical formula:

(the BLUE numbers)

a)

Subscripts

b)

Coefficients

c)

Numbers

d)

Molecules

106.

Balance this equation:

H2 + Cl2 ---> HCl

a)

It is balanced.

b)

H2 + Cl2 ---> 2HCl

c)

3H2 + Cl2 ---> 6HCl

d)

H2 + 3Cl2 ---> 6HCl

107.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
108.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
109.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
110.

Is this endothermic or exothermic?

a)

exothermic

b)

endothermic

111.

Temperature changes are due to changes in ________

a)

Matter

b)

Energy

c)

Motion

d)

Bonds

112.

What type of reaction occurs in hand warmers?

a)

exothermic

b)

endothermic

113.

Baking bread and cooking an egg are examples of....?

a)

Endothermic Process

b)

Exothermic Process

114.

If a chemical reaction is EXOTHERMIC, the temperature would....

a)

stay the same

b)

increase

c)

decrease

115.

In an endothermic reaction, heat is ...

a)

absorbed

b)

released

116.

 In an exothermic reaction, heat is ...

a)

absorbed

b)

released

117.
What is the molar mass of Mg3N2?
a)
191.6 g/mol
b)
76.64 g/mol
c)
38.32 g/mol
d)
100.95 g/mol
118.

What is the molar mass of barium perchlorate Ba(ClO4)2

a)

189.90 g/mol

b)

240.24 g/mol

c)

272.24 g/mol

d)

336.20 g/mol

e)

304.24 g/mol

119.

A sample of copper weighing 6.93 g contains how many moles of copper atoms?

a)

9.17 mol

b)

0.0645 mol

c)

0.0645 mol

d)

1.09 mol

e)

6.56 x 1022 mol

120.

What is the molar mass of calcium hydroxide, Ca(OH)2?

a)

74.1 g/mole

b)

57.1 g

c)

58.1 mole

d)

57.1 mole/g

e)

74mole

121.

Find the mass in grams of 0.75 moles of magnesium (Mg).

a)

32 grams

b)

2.21 x 10 ^23 grams

c)

18 grams

d)

25 grams

e)

84 grams

122.

Which has a larger molar mass in one mole: Al or Cl?

a)

Al

b)

Cl

c)

they're the same

d)

You can't guess that without more information

123.

How many moles of water are there in 24.3g of water?

a)

2.16 mol

b)

1.35 mol

c)

3.35 g

d)

1.65 mol/g

e)

2.16 g/mol

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