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P2 T2 G9-10 LONG REVIEWER

Total questions: 150

Worksheet time: 2hrs 54mins

Name
Class
Date
1.

TRUE or FALSE: In order to change the state of matter, you need increase or decrease the energy (heat).

a)

TRUE

b)

FALSE

2.

TRUE or FALSE: The particles in solids move around a lot and spread out.

a)

TRUE

b)

FALSE

3.

TRUE or FALSE: Liquids have a fixed volume but not a fixed shape.

a)

TRUE

b)

FALSE

4.

TRUE or FALSE: Gases have the least kinetic energy out all 3 states of matter.

a)

TRUE

b)

FALSE

5.

Phase change from liquid to gas is called:

a)

Freezing

b)

Condensation

c)

Vaporization

d)

Sublimation

6.

Phase change from solid to gas is called:

a)

Freezing

b)

Condensation

c)

Vaporization

d)

Sublimation

7.

Phase change from liquid to solid is called:

a)

Melting

b)

Freezing

c)

Deposition

d)

Condensation

8.

Phase change from gas to liquid is called:

a)

Melting

b)

Freezing

c)

Deposition

d)

Condensation

9.

Phase change from gas to solid is called:

a)

Sublimation

b)

Freezing

c)

Deposition

d)

Vaporization

10.

When changing a substance from liquid to solid, the energy has to...

a)

INCREASE

b)

DECREASE

11.

When changing a substance from gas to liquid, the energy has to...

a)

INCREASE

b)

DECREASE

12.

When changing a substance from liquid to gas, the energy has to...

a)

INCREASE

b)

DECREASE

13.

Which of the following statements is NOT true about gases?

a)

Gases do not have fixed shape or volume

b)

Gas particles do not move much, but vibrate

c)

Gas particles have a lot of free space

d)

Unlike solids, gases can be compressed

14.

Which of the following statements is true about liquids?

a)

Particles do not move around much, but vibrate

b)

Particles have a lot of free space and spread out

c)

Liquids have fixed shape & volume

d)

Particles are less closely packed than solids

15.

Which of the following statements is true about phase changes?

a)

Solid turning into liquid is called freezing

b)

When ice melts, the kinetic energy is decreased

c)

Liquid turning into gas is called condensing

d)

When water boils, the kinetic energy is increased

16.

Which of the following statements is true about solids?

a)

Particles do not move around much, but vibrate

b)

Particles have a lot of free space and spread out

c)

Solids have fixed shape but not volume.

d)

Particles are less closely packed than gas.

17.

Look at the picture. Which state of matter is in beaker C?

a)

Solid

b)

Liquid

c)

Gas

d)

Blue thingys

18.

Look at the picture. Which state of matter is in beaker A?

a)

Solid

b)

Liquid

c)

Gas

d)

Blue thingys

19.

What is melting? (Definition)

a)

When liquid turns in solid.

b)

When solid turns into gas.

c)

When gas turns into liquid.

d)

When solid turns into liquid.

20.

What is sublimation? (Definition)

a)

When liquid turns in solid.

b)

When solid turns into gas.

c)

When gas turns into solid.

d)

When solid turns into liquid.

21.
At higher temperatures
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
22.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
23.

Freezing

a)

Solid to gas

b)

Liquid to solid

c)

Gas to solid

24.

Boiling

a)

liquid to gas

b)

gas to solid

c)

gas to liquid

25.
Which state of matter has a definite shape?
a)
solid
b)
liquid
c)
gas
26.

What is happening when my ice cream changes from a solid to a liquid?

a)

freezing

b)

melting

c)

burning

27.

The state of matter that has no definite size or shape is

a)

Solid

b)

Liquid

c)

Gas

28.

Particles in a ______________________ move quickly and are far apart.

a)

gas

b)

solid

c)

liquid

29.

Particles of a liquid

a)

are tightly packed together and stay in a fixed position.

b)

are free to move around one another but still touch.

30.

Solid to Gas

a)

Deposition

b)

Sublimation

c)

Evaporation

31.

What is condensation?

a)

gas to solid

b)

gas to liquid

c)

liquid to solid

32.

The slower the particles in a substance move,

a)

the colder it is.

b)

the warmer it is.

c)

the more energy it has.

33.

Is this a picture of something hot or cold?

a)

Hot

b)

Cold

34.

Is this a picture of something hot or cold?

a)

Hot

b)

Cold

35.
The temperature of a substance increases as___.
a)
the substance expands
b)
the average kinetic energy of its particles increases
c)
the substance's volume increases
d)
the substance's mass increases
36.

Definite shape and definite volume

a)

Solid

b)

Liquid

c)

Gas

37.

Has a definite volume but not a definite shape

a)

Solid

b)

Liquid

c)

Gas

38.

Liquid to Gas

a)

Condensation

b)

Evaporation

c)

Sublimation

39.
All matter is made up of .....
a)
Compounds
b)
Atoms
c)
Molecules
d)
Sunshine
40.
Are made from a combination of 2 or more elements...
a)
Molecules
b)
Pure Substances
c)
Compounds
d)
Elements
41.
H2 would be a .....
a)
Molecule
b)
Compound
c)
Solid
d)
Problem
42.
CO2 would be a .....
a)
Compound
b)
Molecule
c)
Compound AND Molecule
d)
Sandwich
43.
A combination that can be separated by physical processes is a .....
a)
Pure Substance
b)
Glucose
c)
Element
d)
Mixture
44.
A mixture that is NOT evenly distributed is called ....
a)
Compounded
b)
Homogenous
c)
Heterogenous
d)
Salty
45.
If you change a substance into a new substance...
a)
Partial Change
b)
Physical Change
c)
Chemical Change
d)
Freezing
46.
Which is NOT a chemical change?
a)
Leaves changing colors in the fall
b)
Iron rusting
c)
Digesting Lunch
d)
Ice Melting
47.
Mixture, such as mixed nuts or dry soup mix, in which different materials are unevenly distributed and are easily identified.
a)
suspension
b)
homogeneous mixture
c)
heterogeneous mixture
d)
colloid
48.
Substance with atoms that are all alike.
a)
element
b)
compound
c)
homogeneous mixture
d)
heterogeneous mixture
49.
Which of the following is not a homogeneous mixture?
a)
orange juice
b)
vinegar
c)
soft drinks
d)
pool water
50.
What type of mixture is this?
a)
homogenous mixture
b)
chemical
c)
heterogeneous mixture 
d)
solid mix
51.
Which of the following is not an element?
a)
water
b)
hydrogen
c)
carbon
d)
oxygen
52.
Which of the following IS a mixture?
a)
air
b)
hydrogen
c)
water
d)
sugar
53.
Oxygen gas is an example of a.....
a)
pure element
b)
pure compound
c)
heterogeneous mixture
d)
homogeneous mixture
54.
Water vapor is an example of a.....
a)
pure element
b)
pure compound
c)
heterogeneous mixture
d)
homogeneous mixture
55.
Table salt is an example of a.....
a)
pure element
b)
pure compound
c)
heterogeneous mixture
d)
homogeneous mixture
56.
A gold bar is an example of a.....
a)
pure element
b)
pure compound
c)
heterogeneous mixture
d)
homogeneous mixture
57.
Which of the following would you use to separate sand from iron?
a)
a bar magnet
b)
paper
c)
hot plate
58.
What type of substance is gelatin?
a)
colloid
b)
comound
c)
substance
d)
suspension
59.

Is the following a pure substance or mixture? Baking Soda ( NaHCO3NaHCO_3 ) 

a)

pure substance

b)

mixture

60.

Is the following a pure substance or mixture? Trimix (oxygen, nitrogen, and helium) found in a scuba tank

a)

pure substance

b)

mixture

61.

Is the following an element or compound? A silicon (Si) chip.

a)

element

b)

compound

62.

Is the following an element or compound? hydrogen peroxide (H2O2)

a)

element

b)

compound

63.

Is the following a homogeneous or heterogeneous mixture? coffee mixed with cream and sugar

a)

homogeneous mixture

b)

heterogeneous mixture

64.

Is the following homogeneous or heterogeneous? Fruit salad

a)

homogeneous mixture

b)

heterogeneous mixture

65.

Classify the particle diagram.

a)

element

b)

compound

c)

mixture of elements

d)

mixture of compounds

e)

mixture of elements and compounds

66.

Classify the particle diagram.

a)

element

b)

compound

c)

mixture of elements

d)

mixture of compounds

e)

mixture of elements and compounds

67.

Classify the particle diagram.

a)

element

b)

compound

c)

mixture of elements

d)

mixture of compounds

e)

mixture of elements and compounds

68.

Classify the particle diagram.

a)

element

b)

compound

c)

mixture of elements

d)

mixture of compounds

e)

mixture of elements and compounds

69.

Classify the particle diagram.

a)

element

b)

compound

c)

mixture of elements

d)

mixture of compounds

e)

mixture of elements and compounds

70.

How would you classify this image?

a)

homogeneous mixture

b)

heterogeneous mixture

71.

How would you classify this image?

a)

homogeneous mixture

b)

heterogeneous mixture

72.

Is the following a pure substance or mixture? Brass (Cu and Zn)

a)

pure substance

b)

mixture

73.

How would you classify this image?

a)

homogeneous mixture

b)

heterogeneous mixture

74.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
75.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
76.

JJ Thomson was credited for the discovery of the:

a)

Center of the universe

b)

Proton

c)

Electron

d)

Neutron

77.

The first universally accepted theory on atoms was proposed in 1803 by:

a)

Winston Churchill

b)

John Dalton

c)

James Bond

d)

J J Thomson

78.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
79.
What contribution did John Dalton make to atomic theory? 
a)

He discovered that every atom was positively charged.

b)

He discovered that every element consisted of one type of atom 

c)

He discovered that atoms had nuclei 

d)

He discovered that atoms could be divided into smaller parts

80.

Niels Bohr suggested that electrons:

a)

Are found in specific orbits

b)

Are scattered throughout the atom

c)

Move according to their energy level

d)

Are positive

81.

Rutherford discovered this part of the atom:

a)

Nucleus

b)

Neutron

c)

Proton

d)

Electron

82.

Which conclusion could be made from Ernest Rutherford’s gold foil experiment?

a)

Atoms are made up of mostly empty space.

b)

Atoms are mainly solid and block alpha particles.

c)

The volume of the nucleus is large compared to the rest of the atom.

d)

The mass of the nucleus is small compared to the rest of the atom.

83.

What did Ernest Rutherford’s gold foil experiment demonstrate about atoms?

a)

Their positive charge is located in a small region that is called the nucleus.

b)

Their negative charge is located in small particles that are called electrons.

c)

Their nucleus makes up the majority of the volume of the atom.

d)

Their electrons are floating in a sea of positive charges.

84.

What is the correct order of scientists in order of their work related to the atomic theory from earliest to most recent?

a)

Ernest Rutherford, JJ Thomson, John Dalton, & Democritus

b)

JJ Thomson, John Dalton, Ernest Rutherford, & Democritus

c)

Democritus, John Dalton, JJ Thomson, Ernest Rutherford.

d)

John Dalton, JJ Thomson, Democritus, & Ernest Rutherford

85.

Which one of these is Dalton's Model?

a)
b)
c)
d)
86.

Why did Ernest Rutherford and his colleagues perform the Gold-Foil Experiment?

a)

They wanted to test and confirm the Plum-Pudding model

b)

They wanted to test John Dalton's Model

c)

They were looking for electrons

d)

They wanted to come up with their own Atomic Model

87.

Which of the following was an observation made by Rutherford to support that atoms have a dense positive nucleus?

a)

He observed that all alpha particles did go through a gold-foil in straight lines

b)

He observed that most alpha particles did not go through a gold-foil and stopped on one side of the gold foil.

c)

He observed that a small number of alpha particles bounced off the gold-foil at very large angles

d)

He observed that all alpha particles slightly deflected from the straight line when going through a gold-foil

88.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
89.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
90.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

91.

Which of the following are not the postulates of Dalton's atomic theory

a)

Atoms are indivisible and indestructible

b)

Atoms of the same element are alike and that of the other elements are different

c)

Atoms of all elements are alike

d)

Atoms of elements combine in a fixed whole number ratio

92.

In 1897 JJ Thomson studied the characteristics & the constituents of the cathode rays. Which of the following is not a conclusion of his experimental study?

a)

cathode rays consist of negatively charged particles called protons.

b)

atoms of all elements contain electrons and irrespective of how they are emitted they are identical.

c)

Since atoms are electrically neutral they must contain some positively charged particles.

d)

cathode rays consist of negatively charged particles called electrons.

93.
Relatively soft
a)
Ionic
b)
Covalent
94.
High Melting & Boiling Points
a)
Ionic
b)
Covalent
95.
Soluble in Water
a)
Ionic
b)
Covalent
96.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
97.
Predict the bond that will form between Se and Cl
a)
Ionic
b)
Covalent
98.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
99.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
100.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
101.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
102.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
103.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
104.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

105.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

106.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

107.

TRUE OR FALSE: Ionic compounds have high boiling points because they consist of a strong ionic bond.

a)

TRUE

b)

FALSE

108.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
109.
The ability of a material to be shaped in all directions without cracking or breaking.
a)
hardness
b)
ductility
c)
malleability
d)
conductivity
110.

Examine the image: How many bonds are formed looking at the model of the compound? And also indetify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

111.

How do covalent bonds form?

a)

Donating & receiving valence electrons between atoms

b)

Oppositely charged ions attract each other & form bonds

c)

Scientists are still not sure how they form

d)

Sharing valence electrons between atoms

112.

The formation of a covalent bond relies on the interaction or bonding of...

a)

2 Nonmetals

b)

1 Nonmetal & 1 Metal

c)

2 Metals

d)

2 Noble Gases

113.

This is the displayed formula for what covalent compound?

a)

Water

b)

Hydrogen peroxide

c)

Hydrogen oxide

d)

Ethanol

114.

This is the displayed formula for what covalent molecule?

a)

Water

b)

Chlorine

c)

Chloride

d)

Ethanol

115.

Chlorine is a diatomic element which means in nature, it is found in two's. (Cl2) Chlorine shares one pair of electrons to make sure each atom complete the octet rule. This creates a...

a)

single bond

b)

double bond

c)

triple bond

116.

Oxygen is a diatomic element which means in nature, it is found in two's. (O2) Oxygen shares two pairs of electrons to make sure each atom completes the octet rule. This creates a...

a)

single bond

b)

double bond

c)

triple bond

117.

Nitrogen is a diatomic element which means in nature, it is found in two's. (N2) Nitrogen shares three pairs of electrons to make sure each atom completes the octet rule. This creates a...

a)

single bond

b)

double bond

c)

triple bond

118.

What does this picture illustrate? (Select all that apply)

a)

Sharing valence electrons

b)

Covalent bonding

c)

transferring valence electrons

d)

ionic bonding

e)

two nonmetals

119.

How many covalent bonds are created in a single water molecule?

a)

0

b)

1

c)

2

d)

3

e)

4

120.

How many covalent bonds are created in a single ammonia molecule?

a)

0

b)

1

c)

2

d)

3

e)

4

121.

How many pairs of valence electrons are being shared in a single water molecule?

a)

0 pair - 0 valence electrons

b)

1 pair - 2 valence electrons

c)

2 pair - 4 valence electrons

d)

3 pair - 6 valence electrons

122.

How many pairs of valence electrons are being shared in a single ammonia molecule?

a)

0 pair - 0 valence electrons

b)

1 pair - 2 valence electrons

c)

2 pair - 4 valence electrons

d)

3 pair - 6 valence electrons

123.

What type of elements share electrons and form covalent bonds?

a)

Nonmetals

b)

Metals

c)

Metalloids

d)

A Metal & A Nonmetal

124.

What type of bond will this compound likely form H-Cl?

a)

Ionic compound

b)

Covalent compound

c)

Metallic compound

125.

What type of bond will this ammonia compound likely form (NH3)?

a)

Ionic compound

b)

Covalent compound

c)

Metallic compound

126.

What type of bond will this compound likely form [Na]+ & [Cl]- ?

a)

Ionic compound

b)

Covalent compound

c)

Metallic compound

127.

What type of bond will this ammonium chloride compound likely form?

a)

Ionic compound

b)

Covalent compound

c)

Metallic compound

128.

When assigning the number of individual atoms in a chemical formula it is written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

129.

How many total atoms are in the ionic compound Ca(NO3)2 (Calcium nitrate)?

a)

3

b)

5

c)

6

d)

9

e)

10

130.

How many total atoms are in the covalent compound C4H10 (Butane)?

a)

6

b)

8

c)

10

d)

12

e)

14

131.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

132.

Which of the following is NOT a step in forming an ionic bond?

a)

One atom shares its electrons with another one

b)

Opposite charged ions form due to the transfer of electrons

c)

One atom gives electrons to another one

d)

Oppositely charged ions attract

133.

An ionic bond is the attraction between: (Select ALL that apply)

a)

oppositely charged ions

b)

similarly charged ions

c)

metals and nonmetals

d)

neutral atoms

e)

cations and anions

134.

Which of the following is the correct formula for these two ions: Al+3 & S-2

a)

AlS3

b)

Al2S3

c)

Al3S2

d)

Al3S

135.

If I had a cation with a charge of 2+ how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 4 electrons

d)

lost 4 electrons

136.

If I had an anion with a charge of 3- how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 3 electrons

d)

lost 3 electrons

137.

Looking at the periodic table, when the alkali metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

138.

Looking at the periodic table, when the alkaline earth metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

139.

Looking at the periodic table, when the halogens form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

140.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

141.

In the compound aluminum oxide, which is the cation?

a)

[ Al ] +3

b)

Al

c)

[ O ] -2

d)

O

142.

When ionic compounds form what is the overall charge?

a)

neutral

b)

positive

c)

negative

143.

What is responsible for bringing cations and anions together?

a)

the size of the ions

b)

the opposite charges are attracted to one another

c)

the similar charges are attracted to one another

d)

depends on what period they're in

144.

What is another name of an ionic compound

a)

salt

b)

cation

c)

anion

d)

polyatomic ion

145.

Which is the correct name for CaBr2?

a)

Calcium Bromine

b)

Bromine Calcium

c)

Calcium Bromide

d)

Bromine Chloride

e)

Calcium Bromate

146.

What is the name for CsBr?

a)

Cesium Bromide

b)

Calcium Bromine

c)

Calcium Bromide

d)

Cesium Bromine

e)

Bromine Ceside

147.

Which of the following is the correct formula for Sodium Nitride ( [ Na ] + & [ N ] 3- )

a)

NaN3

b)

Na3N

c)

Na2N3

d)

Na3N2

148.

Which of the following is the correct formula for Potassium Sulfide

a)

K2S

b)

KS2

c)

K3S

d)

K2S3

149.

When assigning ionic charge it is always written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

150.

When assigning the number of individual atoms in a chemical formula it is written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

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