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Chemistry Final Review (21-22)

Total questions: 172

Worksheet time: 2hrs 35mins

Name
Class
Date
1.

The nucleus of the atom contains

a)

protons and neutrons

b)

protons and electrons

c)

alpha particles

d)

only protons

2.

He was the first to suggest that atoms were

indivisible, indestructible, fundamental units of matter.

a)

Rutherford

b)

Thomson

c)

Bohr

d)

Democritus

3.

J. J. Thomson's experiments using cathode ray tubes led to the discovery of the

a)

electron

b)

neutron

c)

positron

d)

proton

4.

J. J. Thomson’s model of the atom was a ball of positive charge with negatively charged ______________ embedded inside.

a)

electrons

b)

protons

c)

neutrons

5.

Rutherford concluded that atoms consist of a very small, dense region of positive (+) charge, called the

a)

Electron Shells

b)

Orbitals

c)

Electron Cloud

d)

Nucleus

6.

In the Gold Foil Experiment, Rutherford directed a stream of positively charged particles, called ________________ at a very thin sheet of gold foil.

a)

alpha particles

b)

electrons

c)

gluons

d)

quarks

7.

In the Gold Foil Experiment, Rutherford observed that

a)

ALL the alpha particles passed straight through

b)

MOST alpha particles passed straight through, but SOME were deflected or bounced back

c)

ALL alpha particles were deflected and bounced back

8.

When most of the alpha particles passed directly through the gold atoms, Rutherford concluded that the atom is mostly

a)

empty space

b)

positively charged

c)

dark matter

d)

rigid

9.

Rutherford observed that a few of the alpha particles were deflected. What does this evidence suggest about the structure of the atom?

a)

The atom contains a positively charged nucleus.

b)

The atom is a ball of positive charge with electrons embedded inside.

c)

The atom is small.

d)

The atom negatively charged.

10.

The modern model of the atom is based on the work of

a)

one scientist over a short period of time

b)

one scientist over a long period of time

c)

many scientists over a short period of time

d)

many scientists over a long period of time

11.

Which statement describes the charge of an electron and the charge of a proton?

a)

An electron and a proton both have a charge of +1.

b)

An electron and a proton both have a charge of -1.

c)

An electron has a charge of +1, and a proton has a charge of -1.

d)

An electron has a charge of -1, and a proton has a charge of +1.

12.

In which pair do the particles have approximately the same mass?

a)

proton and electron

b)

proton and neutron

c)

neutron and electron

d)

neutron and beta particle

13.

The atomic number of an atom is always equal to the

total number of

a)

neutrons in the nucleus

b)

protons in the nucleus

c)

neutrons plus protons in the atom

d)

protons plus electrons in the atom

14.

Which particles are found in the nucleus of an atom?

a)

protons and electrons

b)

positrons and neutrons

c)

protons and neutrons

d)

positrons and electrons

15.

All atoms of a given element must have the same

a)

atomic mass

b)

atomic weight

c)

mass number

d)

atomic number

16.

The mass of an electron is

a)

equal to the mass of a proton

b)

equal to the mass of a neutron

c)

greater than the mass of a proton

d)

less than the mass of a neutron

17.

What is the mass number of an atom that has five protons, five electrons, and six neutrons?

a)

5

b)

6

c)

10

d)

11

18.

What is the total number of neutrons in the nucleus of a neutral atom that has 13 protons and a mass number of 27?

a)

13

b)

14

c)

27

d)

40

19.

What is the number of electrons in an atom that has 25 protons and 21 neutrons?

a)

25

b)

21

c)

4

d)

46

20.

Which statement describes how an atom in the ground state becomes excited?

a)

The atom absorbs energy, and one or more electrons move to a higher electron shell.

b)

The atom absorbs energy, and one or more electrons move to a lower electron shell.

c)

The atom releases energy, and one or more electrons move to a higher electron shell.

d)

The atom releases energy, and one or more electrons move to a lower electron shell.

21.

Which quantity identifies an element?

a)

atomic number

b)

mass number

c)

number of neutrons

d)

atomic mass

22.

Which element is not present in the mixture?

a)

A

b)

D

c)

X

d)

Z

23.

The bright-line spectrum of sodium is produced when energy is

a)

absorbed as electrons move from higher to lower electron shells

b)

absorbed as electrons move from lower to higher electron shells

c)

released as electrons move from higher to lower electron shells

d)

released as electrons move from lower to higher electron shells

24.

Which electron configuration represents an atom in an excited state?

a)

2–7

b)

2–6–2

c)

2–8–1

d)

2–8–8–2

25.

What is the electron configuration of a sulfur atom in the ground state?

a)

2–4

b)

2–6

c)

2–8–4

d)

2–8–6

26.

What is Senor Adamit's son's name?

a)

Noam

b)

Snarlybartfast

c)

Senor Adamit Junior

d)

Oso perezoso

27.

What are Crabs?

a)

Not important

b)

Cephalapods

c)

Bivalves

d)

Gross

28.

According to the wave-mechanical model, an orbital is defined as the

a)

circular path for electrons

b)

circular path for neutrons

c)

most probable location of electrons

d)

most probable location of neutrons

29.

In the diagrams provided, the circles of different colors represent the atoms of different elements. Which diagram represents a mixture?

a)

I

b)

II

c)

III

d)

IV

30.

Which beaker contains only one type of element?

a)

A

b)

B

c)

C

d)

D

31.

Which beaker contains a compound?

a)

A

b)

B

c)

C

d)

D

32.

Which beaker(s) contain a pure substance? (check all that apply)

a)

A

b)

B

c)

C

d)

D

33.

Which is the best description of one particle of table salt (NaCl)?

a)

mixture

b)

compound

c)

element

34.

Classify the sample

a)

Pure substance

b)

Mixture

35.

Classify the sample

a)

Element

b)

Compound

36.

Classify the sample

a)

Pure Substance

b)

Mixture of Elements

c)

Mixture of Compounds

37.

What is a pure substance made of two or more elements that are chemically combined called?

a)

A. element

b)

B. compound

c)

C. mixture

38.

Classify the Sample.

a)

Pure Substance

b)

Mixture of Elements

c)

Mixture of Compounds

d)

Mixture of Elements and Compounds

39.

Which chemical formula could be represented by this sample?

a)

NaCl

b)

H2

c)

C6H12O6

d)

Cu

40.

Classify the sample. Look carefully.

a)

Pure Substance

b)

Mixture of Elements

c)

Mixture of Compounds

d)

Mixture of Element and Compound

41.

Which of the following formulas represents a compound?

a)

He

b)

Cl2

c)

MgO

d)

Ag

42.

In the diagrams provided, the circles of different colors represent the atoms of different elements. Which diagram represents a mixture?

a)

I

b)

II

c)

III

d)

IV

43.

Which beaker contains only one type of element?

a)

A

b)

B

c)

C

d)

D

44.

Which beaker contains a compound?

a)

A

b)

B

c)

C

d)

D

45.

Which beaker(s) contain a pure substance? (check all that apply)

a)

A

b)

B

c)

C

d)

D

46.

Which is the best description of one particle of table salt (NaCl)?

a)

mixture

b)

compound

c)

element

47.

Classify the sample

a)

Pure substance

b)

Mixture

48.

Classify the sample

a)

Element

b)

Compound

49.

Classify the sample

a)

Pure Substance

b)

Mixture of Elements

c)

Mixture of Compounds

50.

What is a pure substance made of two or more elements that are chemically combined called?

a)

A. element

b)

B. compound

c)

C. mixture

51.

Classify the Sample.

a)

Pure Substance

b)

Mixture of Elements

c)

Mixture of Compounds

d)

Mixture of Elements and Compounds

52.

Which chemical formula could be represented by this sample?

a)

NaCl

b)

H2

c)

C6H12O6

d)

Cu

53.

Classify the sample. Look carefully.

a)

Pure Substance

b)

Mixture of Elements

c)

Mixture of Compounds

d)

Mixture of Element and Compound

54.

Which of the following formulas represents a compound?

a)

He

b)

Cl2

c)

MgO

d)

Ag

55.

Phase change going from Liquid to Solid...

a)

Melting

b)

Freezing

c)

Condensation

d)

Sublimation

56.

Phase change going from a Gas to a Liquid...

a)

Sublimation

b)

Deposition

c)

Ionization

d)

Condensation

57.

Phase change going from a Liquid to a Gas...

a)

Vaporization

b)

Deposition

c)

Condensation

d)

Melting

58.

Phase change going from a Solid to a Gas...

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Recombination

59.

Phase change going from a Solid to a Liquid...

a)

Freezing

b)

Condensation

c)

Melting

d)

Sublimation

60.

Phase change going from a Gas to a Solid...

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Vaporization

61.

Is the substance gaining or losing energy?

a)

Gaining

b)

Losing

62.

Are the particles moving faster or slower as time goes on?

a)

Faster

b)

Slower

63.

What state/phase is the object likely from points A to B?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

64.

What is happening to the particles in the substance between points A and B?

a)

Melting

b)

Freezing

c)

Speeding Up

d)

Slowing Down

65.

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

a)

Melting

b)

Freezing

c)

Vaporizing

d)

Sublimating

66.

Is the process shown endothermic or exothermic?

a)

Endothermic

b)

Exothermic

67.

Where on the graph are phase changes taking place?

a)

1

b)

2

c)

3

d)

4

e)

5

68.

Which phase changes are occuring during segment B-C?

a)

Melting

b)

Evaporation

c)

Freezing

d)

Condensation

69.

What state/phase is the object likely from points C to D?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

70.

What state/phase is the object likely from points E to F?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

71.

As temperature of a gas increases, the volume

a)

Increases

b)

Decreases

c)

Remains constant

72.

As volume of a gas increases, the pressure

a)

Increases

b)

Decreases

c)

Remains constant

73.

As temperature of a gas increases, the pressure

a)

Increases

b)

Decreases

c)

Remains constant

74.

If a block of wood is cut up into smaller pieces, the density of the wood

a)

Increases

b)

Decreases

c)

Remains the same

75.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
76.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
77.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
78.

Covalent bonds are between...

a)

Metal and Nonmetal

b)

Nonmetal and Nonmetal

79.

Ionic bonds are between...

a)

Metal and Nonmetal

b)

Nonmetal and Nonmetal

80.

How are covalent bonds formed?

a)

electrons are shared

b)

electrons are transferred

81.

How are ionic bonds formed?

a)

electrons are transferred

b)

electrons are shared

82.

O2

a)

Ionic compound

b)

Covalent compound

83.

CaCl2

a)

Ionic Compound

b)

Covalent Compound

84.

H2O

a)

Ionic Compound

b)

Covalent Compound

85.

CO2

a)

Ionic Compound

b)

Covalent Compound

86.

The overall charge of an ionic compound is always _______.

a)

positive (+)

b)

neutral (0)

c)

negative (-)

87.

When Calcium (Ca) loses 2 electrons, what charge does it have?

a)

+2

b)

+1

c)

0

d)

-1

88.

When Oxygen (O) gains 2 electrons, what charge does it have?

a)

+2

b)

+1

c)

-1

d)

-2

89.

1 covalent bond = ________________

a)

1 shared electron

b)

2 shared electrons

c)

3 shared electrons

d)

4 shared electrons

90.

How many electrons are being shared in H2O?

(Hint: Each bond has 2 electrons.)

a)

2

b)

4

c)

6

d)

8

91.

How many bonds are there in the compound CH3Cl?

a)

3

b)

4

c)

6

d)

7

92.

How many LONE PAIRS of electrons are there in the molecule HCl?

a)

1

b)

3

c)

4

d)

6

93.

How many unpaired electrons does oxygen have?

a)

2

b)

4

c)

6

d)

8

94.

How many bonds can Carbon (C) form?

a)

1

b)

2

c)

3

d)

4

95.

What is an ion?

a)

An atom with a positive or negative charge

b)

An atom with a neutral charge

c)

An atom with no electrons

d)

An atom with no protons

96.

Ionic bonds are between...

a)

Metal and Nonmetal

b)

Nonmetal and Nonmetal

97.

Ionic compounds are formed between what type of ions?

a)

positive (+) and negative (-) ions

b)

two positive (+) ions

c)

two negative (-) ions

98.

How are ionic bonds formed?

a)

electrons are transferred

b)

electrons are shared

99.

When Calcium (Ca) loses 2 electrons, what charge does it have?

a)

+2

b)

+1

c)

0

d)

-1

100.

When Oxygen (O) gains 2 electrons, what charge does it have?

a)

+2

b)

+1

c)

-1

d)

-2

101.
Metals tend to 
a)
gain electrons
b)
lose electrons
102.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
103.
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
104.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
105.

Metals become

a)

positive (+) ions

b)

negative (-) ions

106.

Nonmetals become

a)

positive (+) ions

b)

negative (-) ions

107.

Which of the following is an Ionic Compound?

a)

MgCl2

b)

H2O

c)

O2

d)

NH3

108.

Which of the following is an Ionic Compound?

a)

Al2O3

b)

Cl2

c)

CO2

d)

CH4

109.

How many valence electrons does a metal ion have?

a)

0

b)

1

c)

2

d)

8

110.

How many valence electrons does a nonmetal ion have?

a)

0

b)

1

c)

2

d)

8

111.

Which of the following is a correct Lewis Structure for sodium (Na) ion?

a)
b)
c)
d)
112.

Which of the following is a correct Lewis Structure for chlorine (Cl) ion?

a)
b)
c)
d)
113.

Which is the correct way to draw the Lewis dot structure for Potassium Fluoride (KF)?

a)
b)
c)
d)
114.

Which is the correct way to draw the Lewis dot structure for Calcium Chloride (CaCl2)?

a)
b)
c)
d)
115.

A Cation is an ion with a __________ charge.

a)

positive

b)

negative

c)

neutral

116.

An Anion is an ion with a ________ charge.

a)

positve

b)

negative

c)

neutral

117.

When an atom loses an electron, it becomes a:

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

118.

When an atom gains an electron, it becomes a:

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

119.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
120.

Ionic bonds form between a

a)

two metals

b)

nonmetal and nonmetal

c)

metal and nonmetal

d)

two metalloids

121.

Covalent bonds form between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

two metals

d)

two metalloids

122.

According the "Octet rule", how many valence electrons does an atom need to have a stable electron configuration?

a)

1

b)

5

c)

8

d)

10

123.

Which group in the periodic table has elements with a stable electron structure? (Full outer shell)

a)

Group 1

b)

Group 2

c)

Group 14

d)

Group 18 (Noble Gases)

124.

H and He are exceptions to the Octet Rule. How many electrons can they have in their outer shell?

a)

1

b)

2

c)

8

d)

10

125.

How does Lithium become an ion?

a)

Lose 1 electron

b)

Gain 7 electrons

c)

Lose 3 electrons

d)

Gain 1 electron

126.

How does Fluorine become an ion?

a)

Gain 1 electron

b)

Lose 1 electron

c)

Lose 7 electrons

d)

Lose 2 electrons

127.

When a bond is formed, energy is _____________.

a)

absorbed

b)

released

128.

When a bond is broken, energy is _____________.

a)

absorbed

b)

released

129.

All chemical bonds involve

a)

valence electrons

b)

protons

c)

neutrons

130.

In an Ionic bond, electrons _______________ between atoms.

a)

are shared

b)

are transferred

c)

flow freely

131.

In Covalent bond, electrons _______________ between atoms.

a)

are shared

b)

are transferred

c)

flow freely

132.

In Metallic bond, electrons _______________ between atoms.

a)

are shared

b)

are transferred

c)

flow freely

133.

The nucleus of the atom contains

a)

protons and electrons

b)

protons and neutrons

c)

neutrons and electrons

d)

electrons and protons

134.

The element Sulfur (S) is classified as a

(Use the Periodic Table)

a)

metal

b)

nonmetal

c)

metalloid

135.

The element Hydrogen (H) is classified as a

(Use the Periodic Table)

a)

metal

b)

nonmetal

c)

metalloid

136.

Which Family does the element Helium (He) belong to?

(Use the Periodic Table)

a)

Alkali Metals

b)

Transition Metals

c)

Halogens

d)

Noble Gases

137.

Aluminum (Al) is found in which Period?

(Use the Periodic Table)

a)

Period 2

b)

Period 3

c)

Period 12

d)

Period 13

138.

Iron (Fe) is found in which Group?

(Use the Periodic Table)

a)

Group 1

b)

Group 4

c)

Group 8

d)

Group 26

139.

How many electron shells (energy levels) does Magnesium have?

a)

1

b)

2

c)

3

d)

4

140.
How many Protons does Bromine have?
a)
45
b)
79.904
c)
80
d)
35
141.
How many Neutrons does Bromine have?
a)
35
b)
80
c)
45
d)
79.905
142.

Which element has 14 protons?

(Use the Periodic Table)

a)

C

b)

Fe

c)

Si

d)

N

143.

I am usually a good conductor and shiny / lustrous

a)

Metal

b)

Metalloid

c)

Non-metal

144.

Lewis Dot Structure shows us the...

a)

Energy Levels of electrons

b)

Valence electrons

c)

number of protons

d)

total number of electrons

145.

The atomic number is equal to the

a)

atomic mass

b)

group number

c)

number of protons

d)

period number

146.

What is the atomic mass of

iron (Fe)?

a)

26

b)

13

c)

55.845

d)

23.423

147.

Elements in Group 15 have how many valence electrons?

a)

1

b)

5

c)

6

d)

15

148.

How many valence electrons does Calcium have?

a)

20

b)

40

c)

2

d)

8

149.

How many valence electrons does this atom have?

a)

2

b)

4

c)

6

d)

12

150.

This is the Lewis Dot Structure of an element "X". Which Group does this element belong to?

a)

Group 13

b)

Group 14

c)

Group 15

d)

Group 16

151.

Which of the these is the correct Bohr model for Aluminum?

a)
b)
c)
d)
152.

Which of the following is the correct Lewis Dot Structure for Oxygen?

a)
b)
c)
d)
153.

Covalent bonds are between...

a)

Metal and Nonmetal

b)

Nonmetal and Nonmetal

154.

How are covalent bonds formed?

a)

electrons are shared

b)

electrons are transferred

155.

1 covalent bond = ________________

a)

1 shared electron

b)

2 shared electrons

c)

3 shared electrons

d)

4 shared electrons

156.

How many bonds are there in the compound CH3Cl?

a)

3

b)

4

c)

6

d)

7

157.

How many LONE PAIRS of electrons are there in the molecule HCl?

a)

1

b)

3

c)

4

d)

6

158.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
159.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
160.

Which of the following elements is an exception to the "Octet" rule?

a)

Carbon (C)

b)

Hydrogen (H)

c)

Oxygen (O)

d)

Sodium (Na)

161.

How many bonds does Carbon (C) form?

a)

1

b)

2

c)

3

d)

4

162.

How many bonds does Oxygen (O) form?

a)

1

b)

2

c)

3

d)

4

163.

How many bonds does Hydrogen (H) form?

a)

1

b)

2

c)

3

d)

4

164.

How many bonds does Nitrogen (N) form?

a)

1

b)

2

c)

3

d)

4

165.

How many bonds do the elements in Group 17 ("Halogens") form?

(F, Cl, Br, I)

a)

1

b)

2

c)

3

d)

4

166.

Which of the following is a correct drawing of the molecule H2?

a)
b)
c)
d)
167.

Which of the following is the correct drawing for the molecule Cl2?

a)
b)
c)
d)
168.

Which of the following is the correct drawing of the molecule H2O?

a)
b)
c)
d)
169.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
170.

Which of the following is a covalent molecule?

(Use the Periodic Table)

a)

NaCl

b)

MgO

c)

O2

d)

K2S

171.

Which of the following is a covalent molecule?

(Use the Periodic Table)

a)

CCl4

b)

MgCl2

c)

KF

d)

K2S

172.

Which of the following is an example of a "diatomic" molecule?

a)

N2

b)

NH3

c)

H2O

d)

NaCl

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