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Worksheets

Grade 8 2nd tri

Total questions: 218

Worksheet time: 6hrs 34mins

Name
Class
Date
1.

Because electron pairs repel each other molecules tend to

a)

dismantle

b)

divide

c)

take a specific form or shape

d)

dance

2.

VSEPR stands for Valence Shell Electron Pair Repulsion

a)

True

b)

False

3.

Electron pairs repel each other as far away as possible

a)

True

b)

False

4.

Besides covalent bond, lone pairs of electrons can also be counted as electron domains.

a)

True

b)

False

5.

How many Covalent bonds does ammonia have?

a)

1

b)

2

c)

3

d)

4

e)

5

6.

How many lone pairs of elctrons does ammonia have?

a)

1

b)

2

c)

3

d)

4

e)

5

7.

adding the covalent bonds to the number of lone pairs, How many electron domains does ammonia have?

a)

1

b)

2

c)

3

d)

4

e)

5

8.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
9.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
10.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
11.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
12.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
13.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
14.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
15.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
16.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
17.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
18.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
19.

What shape would PH3 have?

a)

Trigonal Planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

20.
What is the bond angle for this molecule?
a)
109.5
b)
120
c)
107
d)
90
21.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
22.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
23.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
24.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
25.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
26.
What is the molecular shape of a silicon dioxide molecule?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
27.
Determine the molecular shape of carbon tetrafluoride.
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
28.

What does VSEPR stand for?

a)

Valence Shell Electron Pair Repulsion

b)

Virtual Shell Electron Pair Repulsion

c)

Volatile Shell Electron Pair Repulsion

d)

Valence Shell Electron Pair Regulation

29.

What is the main idea behind VSEPR theory?

a)

Electron pairs repel each other and arrange themselves to maximize repulsion.

b)

Electron pairs attract each other and arrange themselves to maximize attraction.

c)

Electron pairs repel each other and arrange themselves to minimize repulsion.

d)

Electron pairs do not interact with each other and arrange themselves randomly.

30.

What does the VSEPR theory predict?

a)

The VSEPR theory predicts the shape and geometry of molecules.

b)

The VSEPR theory predicts the electrical conductivity of molecules.

c)

The VSEPR theory predicts the boiling point of molecules.

d)

The VSEPR theory predicts the color of molecules.

31.

What is the shape of a molecule with linear molecular geometry?

a)

Straight line

b)

Circle

c)

Square

d)

Triangle

32.

How many electron pairs are present in a molecule with trigonal planar molecular geometry?

a)

4

b)

2

c)

3

d)

1

33.

What is the bond angle in a molecule with trigonal planar molecular geometry?

a)

120 degrees

b)

180 degrees

c)

90 degrees

d)

60 degrees

34.

What is the shape of a molecule with tetrahedral molecular geometry?

a)

Square

b)

Linear

c)

Planar

d)

Pyramid

35.

How many electron pairs are present in a molecule with tetrahedral molecular geometry?

a)

3

b)

2

c)

1

d)

4

36.

What is the bond angle in a molecule with tetrahedral molecular geometry?

a)

90 degrees

b)

120 degrees

c)

180 degrees

d)

109.5 degrees

37.

What is the molecular geometry of a molecule with 2 bonding pairs and 2 lone pairs of electrons?

a)

trigonal planar

b)

tetrahedral

c)

linear

d)

bent

38.

What is the molecular geometry of a molecule with 3 bonding pairs and 1 lone pair of electrons?

4 lines
39.

What is the molecular geometry of a molecule with 4 bonding pairs and 0 lone pairs of electrons?

a)

trigonal planar

b)

linear

c)

octahedral

d)

tetrahedral

40.

What is the molecular geometry of a molecule with 5 bonding pairs and 0 lone pairs of electrons? (use the simulation)

a)

octahedral

b)

tetrahedral

c)

trigonal bipyramidal

d)

linear

41.

What is the molecular geometry of a molecule with 6 bonding pairs and 0 lone pairs of electrons? (use the simulation)

a)

octahedral

b)

trigonal bipyramidal

c)

tetrahedral

d)

linear

42.

What is the molecular geometry of a molecule with 2 bonding pairs and 3 lone pairs of electrons? (use the simulation)

a)

trigonal bipyramidal

b)

linear

c)

tetrahedral

d)

octahedral

43.

What does VSEPR stand for?

a)

Valence Shell Electron Pair Repulsion

b)

Virtual Shell Electron Pair Repulsion

c)

Volatile Shell Electron Pair Repulsion

d)

Valence Shell Electron Pair Regulation

44.

What is the main idea behind VSEPR theory?

a)

Electron pairs repel each other and arrange themselves to maximize repulsion.

b)

Electron pairs attract each other and arrange themselves to maximize attraction.

c)

Electron pairs repel each other and arrange themselves to minimize repulsion.

d)

Electron pairs do not interact with each other and arrange themselves randomly.

45.

What does the VSEPR theory predict?

a)

The VSEPR theory predicts the shape and geometry of molecules.

b)

The VSEPR theory predicts the electrical conductivity of molecules.

c)

The VSEPR theory predicts the boiling point of molecules.

d)

The VSEPR theory predicts the color of molecules.

46.

What is the shape of a molecule with linear molecular geometry?

a)

Straight line

b)

Circle

c)

Square

d)

Triangle

47.

How many electron pairs are present in a molecule with trigonal planar molecular geometry?

a)

4

b)

2

c)

3

d)

1

48.

What is the bond angle in a molecule with trigonal planar molecular geometry?

a)

120 degrees

b)

180 degrees

c)

90 degrees

d)

60 degrees

49.

What is the shape of a molecule with tetrahedral molecular geometry?

a)

Square

b)

Linear

c)

Planar

d)

Pyramid

50.

How many electron pairs are present in a molecule with tetrahedral molecular geometry?

a)

3

b)

2

c)

1

d)

4

51.

What is the bond angle in a molecule with tetrahedral molecular geometry?

a)

90 degrees

b)

120 degrees

c)

180 degrees

d)

109.5 degrees

52.

What is the molecular geometry of a molecule with 2 bonding pairs and 2 lone pairs of electrons?

a)

trigonal planar

b)

tetrahedral

c)

linear

d)

bent

53.

What is the molecular geometry of a molecule with 3 bonding pairs and 1 lone pair of electrons?

4 lines
54.

What is the molecular geometry of a molecule with 4 bonding pairs and 0 lone pairs of electrons?

a)

trigonal planar

b)

linear

c)

octahedral

d)

tetrahedral

55.

What is the molecular geometry of a molecule with 5 bonding pairs and 0 lone pairs of electrons? (use the simulation)

a)

octahedral

b)

tetrahedral

c)

trigonal bipyramidal

d)

linear

56.

What is the molecular geometry of a molecule with 6 bonding pairs and 0 lone pairs of electrons? (use the simulation)

a)

octahedral

b)

trigonal bipyramidal

c)

tetrahedral

d)

linear

57.

What is the molecular geometry of a molecule with 2 bonding pairs and 3 lone pairs of electrons? (use the simulation)

a)

trigonal bipyramidal

b)

linear

c)

tetrahedral

d)

octahedral

58.

What is a metallic bond?

a)

A bond where electrons are shared equally

b)

A bond where electrons are transferred

c)

A bond where electrons move freely around positively charged metal ions

d)

A bond where atoms stick together with glue

59.

Which of these materials is known for having metallic bonds?

a)

Glass

b)

Wood

c)

Iron

d)

Plastic

60.

What property of metals is due to metallic bonding?

a)

Brittleness

b)

Flexibility

c)

Transparency

d)

Electrical conductivity

61.

Why are metals typically good conductors of electricity?

a)

Because they have no electrons

b)

Because their electrons are fixed in place

c)

Because their electrons move freely

d)

Because they have a lot of non-metallic elements

62.

What happens to the electrons in a metallic bond?

a)

They are shared equally between atoms

b)

They are transferred from one atom to another

c)

They move freely around the metal

d)

They form covalent bonds

63.

Which metal is often used to make jewelry and is known for its shiny appearance due to metallic bonding?

a)

Gold

b)

Aluminum

c)

Iron

64.

What makes metals malleable (able to be hammered into shapes)?

a)

Their rigid electron bonds

b)

Their flexible electron sea

c)

Their high melting points

d)

Their non-conductive nature

65.

Which of these is NOT a characteristic of metals due to metallic bonding?

a)

High melting points

b)

Good electrical conductivity

c)

Brittle texture

d)

Shiny surface

66.

Which of these metals is used in making airplanes and is known for being both strong and lightweight?

a)

Lead

b)

Gold

c)

Aluminum

d)

Silver

67.

What happens when you heat a metal?

a)

It becomes a gas

b)

Its metallic bonds become stronger

c)

Its electrons move faster, making it more conductive

d)

It turns into a non-metal

68.

Metallic bonding is...

a)

a type of covalent bond.

b)

a type of ionic bond.

c)

an attraction between positive ions and a sea of electrons.

69.

A metallic bond is a bond between ________.

a)

nonmetals

b)

metals

c)

transition metals

d)

metalloids

70.

Which of the following is NOT a property of metals?

a)

Hard

b)

Can conduct electricity

c)

Very brittle (breaks easily)

d)

Malleable (can bend without breaking)

71.

What do electrons do in a metallic bond?

a)

They stay on the metal atom.

b)

They are transferred from atom to atom.

c)

They form a covalent bond with another atom.

d)

They float around freely.

72.

What is meant by the term "sea of electrons"?

a)

It's what we call all the free floating electrons in a metal.

b)

It's what we call electrons that are floating in a liquid.

c)

It's the total number of electrons in a metal atom.

d)

It's the total number of electrons in the ocean.

73.

Why are metals good conductors of electricity?

a)

The electric current can easily travel along the surface of the metal because it is smooth.

b)

A negative charge can easily push the sea of electrons in one direction, making a current.

c)

Metals attract electricity.

d)

Metals are malleable.

74.

Why are metals malleable? (They can bend without breaking.)

a)

Metals are very smooth.

b)

Metals have a sea of electrons.

c)

The sea of electrons form a strong metallic bond.

d)

Even though the metal ions repel each other, the electron sea holds all the atoms in place.

75.

What do we call electrons that move freely in a metallic bond?

a)

sea of electrons

b)

lone electrons

c)

unpaired electrons

d)

covalent electrons

76.

What property of metals is the image describing?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

77.

What property of metals is being shown in figure 1(b) in the image?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

78.

What is the one thing responsible for a metal being malleable, ductile, and conductive?

a)

metal atoms

b)

its covalent bonds

c)

its valence electrons

d)

its sea of free-floating electrons

79.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
80.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

81.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
82.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
83.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Hydrogen Bonds

c)

Covalent Bond

d)

Ionic Bond

84.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

85.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

86.

Which type of intermolecular force occurs between two molecules that have polar covalent bonds?

a)

dipole-dipole interactions

b)

london dispersion forces

c)

there are no intermolecular forces in this situation

87.

Hydrogen bonds are a specific type of...

a)

dipole-dipole interaction

b)

london disperion

88.

What type of intermolecular force would act on molecules held together by nonpolar covalent bonds?

a)

dipole-dipole interactions

b)

london dispersion forces

c)

hydrogen bonding

89.

Which type of intermolecular force relies on an "induced dipole"?

a)

dipole-dipole interactions

b)

london dispersion forces

c)

hydrogen bonding

90.

Is the bond in HCl polar or nonpolar? (Hint, in molecules with EN differences larger than .04, the bond is nonpolar)

a)

polar

b)

nonpolar

91.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
92.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
93.

In a polar covalent bond, electrons are shared:

a)

equally

b)

unequally

c)

between two metals

d)

between a metal and a non-metal

94.

Which of these has london dispersion forces? (Hint, london dispersion happens between molecules that contain nonpolar covalent bonds)

a)

I2

b)

NH3

c)

OCl2

d)

SH2

95.

Consider the molecule NH3. Think about its EN difference, and if the covalent bond in it is polar or nonpolar. What type of intermolecular force would happen between these molecules?

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

96.

Consider CO2. Calculate the EN difference between the two elements. What intermolecular forces would happen between CO2 molecules?

a)

London Dispersion Forces

b)

Dipole dipole interactions

c)

Hydrogen bonding

97.

Would H2O molecules hydrogen bond with each other?

a)

yes

b)

no

98.

Consider the EN difference between H and S. Would H2S molecules hydrogen bond with each other?

a)

yes

b)

no

99.

Consider the EN difference between H and F. Does HF have hydrogen bonding?

a)

yes

b)

no

100.

Consider the EN difference between H and Cl. What type of intermolecular forces would act between HCl Molecules?

a)

Dipole-dipole interactions

b)

London dispersion forces

c)

Hydrogen Bonding

101.

Consider the EN difference between C and H. What type of intermolecular forces work between CH4 molecules?

a)

london dispersion forces

b)

dipole-dipole interactions

c)

hydrogen bonding

102.

Consider the EN difference between N and H. What type of intermolecular forces would act between NH3 molecules?

a)

London Dispersion Forces

b)

Dipole-Dipole Interactions

c)

Hydrogen Bonds

103.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
104.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
105.

Why can ammonia gas be easily liquefied and helium can not?

a)

Ammonia has strong intermolecular forces of attraction

b)

The critical temperature of ammonia is very high

c)

Helium has weak intermolecular forces of attraction

d)

All of the above

106.

Which is a property of water that is a result of its hydrogen bonding??

a)

Water has an unusually high boiling point.

b)

Ice floats in liquid water.

c)

Water has high surface tension.

d)

all of the above

107.

Hydrogen bonds increase the melting and (a)   points of polar covalent compounds.

108.

In water, hydrogen bonds hold together

a)

hydrogen and oxygen atoms in different molecules.

b)

hydrogen atoms in the same molecule.

c)

hydrogen and oxygen atoms in the same molecule.

d)

hydrogen atoms in different molecules.

109.

Hydrogen fluoride is a liquid unlike other hydrogen halides since:

a)

hydrogen fluoride molecules associate due to hydrogen bonding

b)

fluorine is highly reactive

c)

hydrogen fluoride is the weakest acid of all hydrogen halides

d)

none of the above

110.

What is surface tension caused by?

a)

gravity

b)

covalent bonds

c)

intermolecular forces

d)

adhesion

e)

intramolecular force

111.

In a polar bond, the atom that is more electronegative attracts the shared electrons more strongly. This results in it having a partial (a)   charge.

112.

(a)   covalent compounds have a partial negative charge on one side and a partial positive charge on the other side.

113.

In a water molecule, the hydrogen side of the molecule has a slightly (a)   charge.

114.

Liquid ethylene (C2H2) molecules are nonpolar and do not experience hydrogen bonding, liquid water (H2O) molecules are polar and experience hydrogen bonding. Which liquid will have a higher boiling point?

a)

water

b)

ethylene

c)

water and ethylene have the same boiling point

115.

Which of the following has the highest boiling point?

a)

HBr

b)

HI

c)

HF

d)

HCl

116.

Hydrogen bonds _______as compared to the covalent bonds.

a)

are weaker

b)

have fluctuating strengths

c)

are of equal strength

d)

are stronger

117.

The correct ranking of bonds or forces in order from strongest to weakest is:

a)

covalent bond, van der Waals force, hydrogen bond

b)

van der Waals force, hydrogen bond, covalent bond

c)

hydrogen bond, covalent bond, van der Waals force

d)

covalent bond, hydrogen bond, van der Waals force

118.

Hydrogen bonds are very strong bonds.

a)

true

b)

false

119.

The unusually higher boiling point of hydrogen fluoride compared to hydrogen chloride is due to

a)

hydrogen bonds between the molecules

b)

polar character of the molecule

c)

the linear structure of the molecules

d)

ionic bonds between the molecules

120.

Polar molecules tend to have lower boiling points than nonpolar molecules.

a)

true

b)

false

121.

Intermolecular hydrogen bonding is present in salicylic acid.

a)

true

b)

false

122.

Water is a polar compound.

a)

true

b)

false

123.

Water’s extremely strong hydrogen bonding causes the high boiling point of water.

a)

true

b)

false

124.

Methylamine is a derivative of ammonia. In methylamine, the hydrogen bond is present between hydrogen and nitrogen.

a)

true

b)

false

125.

What is your favorite part of chemistry?

4 lines
126.

A substance that is formed as the result of a chemical reaction is a __________________

a)

Product

b)

Reactant

c)

Starters

d)

Enders

127.
In a chemical equation, is it true that -
a)
the reactant side and product side can have different numbers of atoms for each element
b)
there can be different elements on the reactant side and the product side
c)
an element or compound must be accompanied by a phase change
d)
the coefficients indicate the number of molecules of each reactant used and the number of molecules of each product made
128.
Which of the following models best demonstrates a balanced chemical equation?
a)
F
b)
G
c)
H
d)
J
129.
The reactants are on the left side of the chemical equation.
a)
True
b)
False
130.

How many atoms in all are in a molecule of serotonin?

C10H12N2O

a)
22
b)
24
c)
25
d)
4
131.
Coal contains carbon and other elements. Carbon dioxide forms when coal burns in the presence of oxygen. Which of these is the best evidence that a chemical reaction occurs when coal burns?
a)
The shape of the coal changes
b)
Oxygen is present
c)
A new substance is produced
d)
Coal is made up of more than one element
132.
Is burning wood a chemical or physical change?
a)
chemical
b)
physical
133.
Is glass breaking a chemical or phyiscal change?
a)
chemical
b)
physical
134.
Is hammering wood together to build a house a chemical or physical change?
a)
chemical
b)
physical
135.
Is a a rusting bicycle a chemical or physical change?
a)
chemcial
b)
physical
136.
Is melting butter for popcorn a chemical or physical change?
a)
chemical
b)
physical
137.
Is melting ice a chemical or physical change?
a)
chemical
b)
physical
138.
Is spoiling food a physical or chemical change?
a)
phyiscal
b)
chemical
139.
Is mixing lemonade powder with water a physical or chemical change?
a)
physical
b)
chemical
140.
Is mowing the lawn a phyiscal or chemical change?
a)
physical
b)
chemical
141.
Which of the following equations demonstrates an actual chemical reaction that forms a new substance? (HINT: it must follow the Law of Conservation of Mass)
a)
A
b)
B
c)
C
d)
D
142.
What is the left part of a chemical equation called?
H2 + O → H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
143.
Is this balanced?
2HgO → 2Hg + O2
a)
Yes
b)
No
144.
Is this balanced?
Al + O2 → 2Al2O3
a)
Yes
b)
No
145.
When materials combine to form new compounds it is a chemical change. Which example is a chemical change?
a)
baking powder fizzing
b)
water boiling
c)
ice melting
d)
sugar cube dissolving
146.
Which is an example of a chemical reaction?
a)
paper cut into small pieces
b)
chocolate melting in a pan
c)
flour and sugar mixed in a bowl
d)
cookies baking in an oven
147.

In a _______ change, a substance changes into a different substance

a)

physical

b)

chemical

148.

Which of these is NOT a sign a chemical change has occurred?

a)

color change

b)

temperature change

c)

bubble formation

d)

cutting material

149.

In a chemical reaction, bonds are broken and new bonds are formed that create new substances. The bonds that are broken are called what?

a)

reactants

b)

products

150.

The Law of Conservation of Mass states

a)

that matter exists in all states and reacts the same

b)

that matter can only be changed into new substances by introducing a catalyst

c)

that matter exists in the same state throughout any chemical change

d)

that matter cannot be created or destroyed

151.

SELECT 2: Which of the following 2 are chemical reactions?

a)

sugar dissolving in water

b)

water turning into steam

c)

burning wood

d)

mixing baking soda and vinegar

e)

tearing paper

152.

SELECT ALL THAT APPLY: Why is it important that chemical equations are always balanced?

a)

Matter cannot be created

b)

Matter cannot be destroyed

c)

Matter can only be rearranged

d)

Matter doe

153.

In a chemical equation, the products are found on the ______ side of the arrow

a)

right

b)

left

154.

In a chemical equation, the reactants are found on the _____ of the arrow

a)

right

b)

left

155.

An ending substance that is made during a chemical reaction

a)

reactant

b)

product

156.

A starting substance that is part of a chemical reaction

a)

Reactant

b)

Product

157.

A process in which atoms rearrange to form new substances

a)

chemical reaction

b)

chemical formula

c)

science

158.

Select the pair of words that correctly displays the general FORMAT for writing chemical equations

a)

products --> reactants

b)

products --> products

c)

reactants--> products

d)

reactants --> reactants

159.

The total mass of the reactants is 18.4g. What would the total mass of the products be? (NOTE: Refer to the Law of Conservation of Mass)

a)

18.4g

b)

9.2g

c)

4.6g

d)

36.8g

160.

Reactant 1 is 4 grams, reactant 2 is 2 grams. How many total grams is the product?

a)

4 grams

b)

2 grams

c)

6 grams

d)

10 grams

161.

What type of reaction involves the breaking down of a substance into simpler substances?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

d)

Decomposition Reaction

162.

What type of reaction involves 2 substances combining to form 1 new compound?

a)

Decomposition Reaction

b)

Single Displacement Reaction

c)

Double Displacement Reaction

d)

Synthesis Reaction

163.

What type of reaction involves one element replacing another element in a compound?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

d)

Decomposition Reaction

164.

What type of reaction involves ions from 2 compounds exchanging places to form 2 completely new compounds?

a)

Single Displacement Reaction

b)

Double Displacement Reaction

c)

Synthesis Reaction

d)

Decomposition Reaction

165.

What are the reactants in the chemical equation pictured?

a)

CH4 and CO2

b)

CH4 and O2

c)

CO2 and H2O

d)

O2 and H2O

166.

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

167.

What type of chemical reaction is this one?

Al(OH)3 --> Al2O3 + H2O

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

168.

What type of chemical reaction is this one?

CUO + CO2 --> CuCO3

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

169.

What type of chemical reaction is this one?

Ca + MgCl2 --> CaCl2 + Mg

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

170.

What type of reaction is illustrated below?

2HI --> H2 + I2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

171.

What type of reaction is illustrated below?

Zn + H2S --> ZnS + H2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

172.

3KOH + H3PO4 --> K3PO4 + 3H2O

a)

Combination

b)

Decomposition

c)

Single replacement

d)

Double replacement

173.
A compound that contains only carbon and hydrogen and that produces carbon dioxide and water when burned is called a(n)
a)
binary compound
b)
carbonate
c)
ionic compound
d)
hydrocarbon
174.
Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a)
double replacement 
b)
decomposition 
c)
combustion 
d)
single replacement
175.

Which of the following reactions is classified as a combustion reaction?

a)
The reaction between iron and sulfur to form iron(II) sulfide
b)
The reaction between hydrochloric acid and sodium hydroxide to produce water and salt
c)
The reaction between a hydrocarbon fuel (such as methane) and oxygen to produce carbon dioxide and water
d)
The reaction between silver nitrate and sodium chloride to form silver chloride and sodium nitrate
176.

Which of the following is an example of a combination reaction?

a)
Reaction between iron and sulfur to form iron(II) sulfide
b)
Reaction between magnesium and hydrochloric acid to form magnesium chloride
c)
Reaction between copper and oxygen to form copper oxide
d)
Reaction between sodium and water to form sodium hydroxide
177.

In which type of reaction does a single element replace another element in a compound?

a)

Displacement reaction

b)
Combustion reaction
c)
Decomposition reaction
d)

Double Displacement reaction

178.

Which of the following is an example of a double displacement reaction?

a)

The reaction between hydrochloric acid and sulfuric acid

b)

The reaction between iron (III) oxide and carbon monoxide

c)

The reaction between potassium hydroxide and nitric acid

d)

The reaction between silver nitrate and sodium chloride

179.

Which reaction type often involves a metal reacting with an acid to produce hydrogen gas?

a)
Decomposition reaction
b)
Single displacement reaction
c)
Combustion reaction
d)
Double displacement reaction
180.

Which of the following is NOT a characteristic of a combustion reaction?

a)
Formation of a solid product
b)

  • Oxygen is a reactant

c)

  • A single product is formed

d)

  • Energy is released in the form of heat and light

181.

What type of reaction occurs when iron reacts with oxygen to form iron(III) oxide?

a)
Combustion reaction
b)

Combination reaction

c)
Decomposition reaction
d)
Acid-base reaction
182.

Which characteristic is unique to combustion reactions?

a)
Production of water and carbon dioxide
b)
Absence of oxygen requirement
c)
Production of heat and light
d)
Formation of solid products only
183.

In a combination reaction, what typically happens to the reactants?

a)
They separate into multiple products
b)
They remain unchanged
c)
They disappear completely
d)
They combine to form a single product.
184.

Which characteristic is common to both displacement and double displacement reactions?

a)
Release of energy
b)
Exchange of ions
c)
Change in color
d)
Formation of a gas
185.

What is the mass of 1 mole of nitrogen gas?

a)

56.0 g

b)

28.0 g

c)

14.0 g

d)

12.0 g

186.

The relative molecular mass of calcium hydroxide is

a)

40.1

b)

57.1

c)

74.1

d)

91.1

187.

An oxide of sulfur contains equal percentages by mass of sulfur and oxygen. The formula of the oxide is

a)

SO

b)

SO2

c)

SO3

d)

SO4

188.

Element X forms an acid with the formula H3XO4. The relative molecular mass of acid is 98.0. What is the relative atomic mass of X?

a)

81.0

b)

34.0

c)

33.0

d)

31.0

189.

What is the mass of aluminium contained in 204 g of aluminium oxide?

a)

27 g

b)

54 g

c)

108 g

d)

150 g

190.

One mole of hydrogen and one mole of ammonia have the same

a)

mass in grams

b)

number of molecules

c)

number of atoms

d)

relative molecular mass

191.

The number of molecules in 1 mole of a gas is z. What is the number of oxygen molecules in 8 g of oxygen gas?

a)

8z

b)

z

c)

0.5z

d)

0.25z

192.

How many molecules are there in 6 dm3 of carbon dioxide (measured at r.t.p.)?

a)

1.51 x 1023

b)

6.02 x 1023

c)

12.04 x 1023

d)

2.41 x 1024

193.

How many atoms are contained in 32 g of methane, CH4?

a)

6.02 x 1023

b)

1.20 x 1024

c)

2.40 x 1024

d)

6.02 x 1024

194.

Which amount contains the largest mass?

a)

1 mole of water molecules

b)

0.25 mole of magnesium oxide

c)

10 moles of hydrogen atoms

d)

6 dm3 of sulfur dioxide gas at r.r.p.

195.
In the reaction represented by the equation N2 + 3H2 --> 2NH3, what is the mole ratio of nitrogen to ammonia?
a)
1:1
b)
1:2
c)
1:3
d)
2:3
196.
The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) --> 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?
a)
1.0 mol
b)
2.0 mol
c)
3.0 mol
d)
6.0 mol
197.
For the reaction represented by the equation
2Na + 2H2O --> 2NaOH + H2, how many grams of hydrogen are produced if 120. g of sodium and 80. g of water are available?
a)
4.5 g
b)
45 g
c)
80. g
d)
200. g
198.
In most chemical reactions the amount of product obtained is
a)
equal to the theoretical yield.
b)
less than the theoretical yield.
c)
more than the theoretical yield
d)
more than the percentage yield
199.
For the reaction represented by the equation Cl2 + 2KBr --> 2KCl + Br2, calculate the percentage yield if 200. g of chlorine react with excess potassium bromide to produce 410. g of bromine.
a)
73.4%
b)
82.1%
c)
91.0%
d)
98.9%
200.
Which branch of chemistry deals with the mass relationships of elements in compounds and the mass relationships among reactants and products in chemical reactions?
a)
qualitative analysis
b)
stoichiometry
c)
entropy
d)
chemical kinetics
201.
In a chemical reaction
a)
the mass of the reactants equals the mass of the products.
b)
the mass of the products is greater than the mass of reactants.
c)
the number of atoms in the reactants and products must change.
d)
energy as heat must be added to the reactants.
202.
Which observation does not indicate that a chemical reaction has occurred?
a)
formation of a precipitate
b)
production of a gas
c)
evolution of heat and light
d)
change in total mass of substances
203.
How would oxygen be represented in the formula equation for the reaction of methane and oxygen to yield carbon dioxide and water?
a)
oxygen
b)
O
c)
O2
d)
O3
204.
When the equation Fe3O4 + Al --> Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?
a)
3
b)
4
c)
6
d)
9
205.

The number of moles of 50g CaCO3 (M=100)

a)

0.1

b)

5

c)

0.5

d)

0.05

206.

Volume of 2 moles of oxygen gas

a)

24 dm3

b)

12 dm3

c)

48 dm3

d)

48 cm3

207.

Concentration of 5dm3 dilute hydrochloric acid (number of moles of HCl is 0.5 mol)

a)

0.01 mol/cm3

b)

0.1 mol/cm3

c)

2.5 mol/cm3

d)

25 mol/cm3

208.

The right formulae used to calculate the number of moles?

a)

n = m/M

b)

n = V/24

c)

n = VxCM

d)

n = 24xV

209.

Valency of Al is 3, valency of O is 2. What is the formula of compound formed from Al and O

a)

Al2O3

b)

Al3O2

c)

AlO

d)

3Al2O

210.

The charge of NO3 in compound Ca(NO3)2

a)

1-

b)

2-

c)

1+

d)

2+

211.

What is the meaning of "100g of 10% HCl solution"?

a)

the solution contain 10g HCl and 90g H2O

b)

the solution contain 90g HCl and 10g H2O

c)

the solution contain 100g HCl

d)

the solution does not contain water

212.

2 mol of Mg reacts with 2 mol of HCl solution following the equation:

Mg + 2HCl --> MgCl2 + H2

What is the limiting reagent in this reaction?

a)

Mg

b)

HCl

c)

MgCl2

d)

H2

213.

1 mol of CaCO3 reacts to form 0.6 mol of CaO following the equation:

CaCO3 --> CaO + CO2

What is the percentage yield of this reaction?

a)

60%

b)

160%

c)

100%

d)

80%

214.

Determine the value of x and y in the equation:

Na2CO3 + xHCl --> yNaCl + CO2 + H2O

a)

x=1, y=2

b)

x=2, y=2

c)

x=2, y=1

d)

x=1, y=1

215.

Iron reacts with hydrochloric acid. What are products of this reaction?

a)

FeCl2, H2

b)

FeCl3, H2

c)

FeCl2, H2O

d)

FeCl, H2O

216.

What is the chemical symbol for the metals sodium, potassium, lead, and zinc, respectively?

a)

Na, K, Fe, Zn

b)

S, P, Fe, Zn

c)

Na, K, Pb, Zn

d)

Na, P, Pb, Zn

217.

Something that can make you smile immediately

a)
b)
c)
d)
218.

Relative molecular mass of CO2 (C=12, O=16)

a)

44

b)

32

c)

24

d)

56

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