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Final Exam Practice Questions

Total questions: 123

Worksheet time: 2hrs 12mins

Name
Class
Date
1.
The phase of matter that has definite shape and definite volume is:
a)
solid.
b)
liquid.
c)
gas.
d)
plasma.
2.
In nature, heat always flows from a:
a)
cold object to a warm object.
b)
small object to a big object.
c)
warm object to a cold object.
d)
large object to a small object.
3.
As the kinetic energy of the molecules in a substance increases, the temperature of the substance __________.
a)
increases
b)
decreases
4.

Anything that has mass and takes up space.

a)

Matter

b)

Molecule

c)

Mass

d)

Volume

5.

Convert

 450 K450\ K  to Celsius

a)

 723oC723^oC  

b)

 277oC277^oC  

c)

 177 oC177\ ^oC  

d)

 623oC623^oC  

6.
Frank has an eraser. It has a mass of 4g, and a volume of 2cm3. What is its density?
a)
8 g/cm3
b)
2 g/cm3
c)
1/2 g/cm3
d)
24 g/cm3
7.
A student knows the mass of an object. What other variable does the student need to know to calculate the object's density?
a)
Color
b)
Weight
c)
Volume
d)
Length
8.

A green powder is heated & a gas is given off while it turns to a black solid. This describes

a)

Physical Change

b)

Chemical Change

c)

Change in State

d)

Change in Temperature

9.
Ice melting
a)
Chemical Change
b)
Physical Change
10.

An _______________ is made up of one or more of the same kind of atom chemically combined.

a)

atom

b)

element

c)

molecule

d)

compound

11.

___________ are the smallest unit of an element that maintains the properties of that element.

a)

Atoms

b)

Elements

c)

Compounds

d)

Mixtures

12.

A __________________ is a substance that has definite physical and chemical properties such as appearance, melting point, and reactivity.

a)

mixture

b)

pure substance

c)

compound

d)

element

13.

A ______________ mixture is one that does not have a uniform composition.

a)

heterogeneous

b)

homogenous

c)

pure substance

14.

Which of these is a compound?

a)

Aluminium (Al)

b)

Carbon Dioxide (CO2)

c)

Nitrogen (N)

d)

Sand

15.

Which is the best synonym for potential energy?

a)

Stored energy

b)

Energy of motion

c)

Energy due to gravity

d)

Mechanical energy

16.

Which of the following examples is an endothermic reaction?

a)

Potassium Chloride dissolves in water the temperature drops.

b)

Acid mixed with Sodium Carbonate the temperature drops.

17.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

18.

Which scientist described a positively charged core (“nucleus”) in the middle of a lot of empty space?

a)

Chadwick

b)

Thomson

c)

Rutherford

d)

Bohr

19.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
20.

Of the three subatomic particles, _____________ are comparatively small and negatively charged.

a)

Protons

b)

Neutrons

c)

Electrons

d)

Funtron

21.

The number of protons in an atomic nucleus determines what an element is and is called its ____________________.

a)

Family Name

b)

Mass Number

c)

Atomic Number

d)

Group Name

22.

The sum of the number of protons plus the number of neutrons in an atom is called the atom's ___________________.

a)

Atomic Number

b)

Handle

c)

Mass Number

d)

Charge

23.

Atoms that have different atomic masses but the same number of protons are called _____________,

a)

friends

b)

ions

c)

enemies

d)

isotopes

24.

Atoms that have the same number of protons but different numbers of electrons are called _____________,

a)

friends

b)

ions

c)

enemies

d)

isotopes

25.

What subatomic particles are in the nucleus of an atom?

a)

Only protons

b)

Protons and neutrons

c)

Only neutrons

d)

Only electrons

e)

Protons and electrons

26.

If the atom has 25 electrons, how many protons does it need to have to be neutral?

a)

5 protons

b)

25 protons

c)

it doesn't need protons

d)

15 protons

27.
How many protons are in Beryllium?
a)
4
b)
9
c)
5
d)
2
28.
How many neutrons does a Hydrogen atom have?
a)
1
b)
2
c)
3
d)
0
29.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
30.

Horizontal (SIDE TO SIDE) rows on the periodic table are

a)

groups

b)

periods

31.

The period number tells you the number of

a)

protons

b)

energy levels

c)

valence electrons

32.

How many energy levels does Au have? Just give me the number.

(a)  

33.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

34.

If an atom does not have a full valence shell, it is considered

a)

stable

b)

unstable

c)

unreactive

35.
Lowest energy state of an atom
a)
Ground
b)
Excited
36.

What is the ground state electron configuration of Br?

a)

2-8-18-7

b)

2-8-18-8

c)

2-3

d)

2-8-17-8

37.

What happens to energy as an atom goes from ground state to excited state?

a)

It increases

b)

It decreases

c)

It remains the same

38.

Which is a possible excited state electron configuration for Si?

a)

2-8-4

b)

1-9-4

c)

2-8-8

d)

2-8-3-1

39.
What family is silver a part of?
a)
Transition Metals
b)
Noble Gases
c)
Alkali Metals
d)
Alkaline Earth Metals
40.
___________ is the only metal that is a liquid at room temperature.
a)
Platinum
b)
Water
c)
Tin
d)
Mercury
41.

what is the biggest group on the table

a)

metals

b)

nonmetals

c)

metaloids

d)

halogens

42.

what is the name of group number 1

a)

halogens

b)

noble gases

c)

alkali

d)

alkaline earth

43.

An element is ductile if . . .

a)

it can be broken with a hammer.

b)

it can be pulled into a long thin wire-like structure

c)

if it can be crushed into a powder

d)

it can be shaped into a shape

44.

Aluminum is a _______ conductor of electricity and heat.

a)

good conductor

b)

semi-conductor

c)

poor conductor

d)

non-conductor

45.

When new chemical bonds form, energy ____________.

a)

is taken into the system.

b)

is released from the system.

c)

stays the same in the system.

46.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
47.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
48.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
49.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

50.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
51.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

52.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
53.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
54.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
55.
How many electrons are represented by a single straight line in a Lewis structure?
a)
1
b)
2
c)
4
d)
6
56.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
57.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
58.

What type of bond would form between O and H?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

59.

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.

60.

What is the percent by mass of Oxygen in water? H2O.

a)

33 %

b)

88.9%

c)

11.1%

d)

50%

61.
What is the molar mass of Carbon Dioxide (CO2)?
a)
12 amu
b)
12 g
c)
44 g
d)
44 amu
62.
What is the molar mass of Hydrogen Peroxide (H2O2)?
a)
48 g/mole
b)
34.02 g/mole
c)
36.5 g/mole
d)
35.5 g/mole
63.
What is the formula for Sodium Bromide? 
a)
NaBr
b)
NaBr2
c)
Na2Br
d)
Na3Br
64.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

65.

How many grams are in 1.2 moles of neon?

a)

0.059 grams

b)

7.2 x 1023 grams

c)

2.0 x 10-24 grams

d)

24 grams

66.

Sodium and chlorine react to form sodium chloride. Sodium and chlorine are examples of

a)

Reactants

b)

Products

c)

Exothermic reactions

d)

Precipitates

67.
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.
68.
Is the following equation balanced?...
Al + O2 --> 2Al2O3
a)
Yes!
b)
No!
69.
In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?
a)
10:6 
b)
3:4
c)
4:3
d)
2:3
70.

solute + solvent =

a)

solution

b)

equation

71.
The substance being dissolved in a solution.
a)
sands
b)
solute
c)
solvent
d)
alloy
72.

A solution that is considered unsaturated would _____.

a)

be dark in color.

b)

have a strong scent.

c)

have a large amount of solute.

d)

have a small amount of solute.

73.

What are the units of molarity?

a)

M

b)

m

c)

Ml

d)

Mr

74.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
75.

According to Table F, which barium salt is insoluble in water?

a)

BaCO3

b)

BaCl2

c)

Ba(ClO4)2

d)

Ba(NO3)2

76.

According to Table G, which substance forms an unsaturated solution when 80. grams of the substance are stirred into 100. grams of H2O at 10.°C?

a)

KNO3

b)

KI

c)

NH3

d)

NaCl

77.

Which compound becomes less soluble in water as the temperature of the solution is increased?

a)

HCl

b)

KCl

c)

NaCl

d)

NH4Cl

78.

When 5 grams of KCl are dissolved in 50. grams of water at 25°C, the resulting mixture can be described as

a)

heterogeneous and unsaturated

b)

heterogeneous and supersaturated

c)

homogeneous and unsaturated 

d)

homogeneous and supersaturated

79.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

80.
From 30 degrees to 55 degrees, what state of matter is the substance?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
81.

If you add heat, energy ____________, so atoms move faster.

a)

decreases

b)

increases

c)

stays the same

82.
In which segment is the kinetic energy remaining constant?
a)
A-B
b)
B-C
c)
C-D
d)
E-F
83.
True or false: melting and freezing occur at the same temperature!
a)
True
b)
False
c)
I don't know
84.
A substance's heating curve is shown in the graph.  What is its boiling point?
a)
100 C
b)
60 C
c)
80 C
d)
20 C
85.

From point A to point E, the sample is going through an

a)

exothermic process by releasing heat to the surroundings

b)

exothermic process by absorbing heat from the surroundings

c)

endothermic process by releasing heat to the surroundings

d)

endothermic process by absorbing heat from the surroundings

86.

The melting point of the sample is

a)

-60 ºC

b)

-100 ºC

c)

60 ºC

d)

100 ºC

87.
Sublimation is
a)
when solid turns into gas
b)
when gas turns into plasma
c)
when liquid turns into gas
d)
when gas turns into solid
88.

What is collision theory?

a)

Molecules must collide in the correct orientation with enough energy to bond.

b)

Molecules need enough energy to collide and react.

c)

Atoms constantly collide and react.

d)

The minimum energy needed for atoms to react

89.

Which PE Diagram represents an endothermic reaction?

a)

A

b)

B

90.

What is the rate of reaction?

a)

How much energy is needed for a reaction to occur.

b)

The energy required to break a bond.

c)

The time it takes for a reaction to occur.

d)

Collision Theory

91.

What is the purpose of a catalyst?

a)

Helps to slow down a reaction

b)

Raises the activation energy

c)

Lowers the activation energy

d)

Is consumed by the reaction

92.

What factors effect rate of reaction?

a)

Temperature, Concentration, Pressure and Energy

b)

Surface Area, Concentration, Energy and Pressure

c)

Temperature, Pressure, Concentration and Surface area

d)

Pressure, Surface area, Density and Energy

93.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
94.
Which letter represents the PE of the reactants?
a)
B
b)
A
c)
C
d)
D
95.
Which letter represents the change of the heat of the reaction?
a)
B
b)
E
c)
C
d)
D
96.

What are the two factors that help determine that equilibrium is reached?

a)

Forward reaction rate is faster than the reverse and the concentrations are equal

b)

Forward and reverse reaction rates are equal and concentrations are equal

c)

Forward and reverse reaction rates are equal and concentrations are constant

97.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
98.

The entropy will usually increase when

a)

a molecule is broken into two or more smaller molecules

b)

a reaction occurs that results in an increase in the number of moles of gas

c)

a solid changes to a liquid

d)

all of these

99.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

100.

An Arrhenius acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

101.

One alternate acid-base theory states that an acid is an

a)

H+ donor

b)

H+ acceptor

c)

OH- donor

d)

OH- acceptor

102.
the reaction of an acid and a base to form a neutral solution of water and a salt
a)
neutralization reaction
b)
hydronium ion concentration
c)
ph
d)
a salt
103.
something measured by pH
a)
neutralization reaction
b)
hydronium ion concentration
c)
pH
d)
a salt
104.
A neutral solution has a pH of 
a)
7
b)
11
c)
3
d)
1
105.
Sodium chloride, sodium nitrate, and calcium sulfate are all 
a)
sugars
b)
hydroniums
c)
indicators
d)
salts
106.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
107.

Which of the following is a strong electrolyte when dissolved in water?

a)

NaNO3

b)

C2H5OH

c)

C12H22O11

d)

CH4

108.
Complete the sentence.
A substance that is more basic has a _____ pH than a substance that is acidic.
a)
lower
b)
higher
c)
the same
d)
none of the above
109.

Which of the following is the strongest acid?

a)

1

b)

5

c)

3

d)

8

110.

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

a)

4.0

b)

1.0 E-4

c)

10

d)

Cannot be determined from the information

111.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
112.

This term refers to the amount of time it takes for half of a certain substance to undergo radioactive decay.

a)

alpha life

b)

beta life

c)

radioactivity time

d)

half-life

113.

What happens to an atom's atomic number when it undergoes alpha decay?

a)

decreases by 1

b)

decreases by 2

c)

increases by 1

d)

increases by 2

114.

________________________ is used in many smoke detectors.

a)

americium-241

b)

neptunium-237

c)

uranium-235

115.

______________ is used in the diagnosis of thyroid disease.

a)

iodine-131

b)

phosphorus-32

c)

carbon-14

d)

americium-241

116.

What percentage of the original isotope is left after 2 half-lives?

a)

100%

b)

75%

c)

50%

d)

25%

117.

In the equation, 146C --> 147N + 0-1B, the _______ decay of radioactive carbon-14 results in the creation of a new nitrogen-14 atom.

a)

Gamma

b)

Beta

c)

Alpha

118.

In a(n) ___________, particles released from one nuclear reaction collide with other particles and cause more nuclear reactions.

a)

nuclear fission reaction

b)

nuclear fusion reaction

119.

In ___ _____reactions, small nuclei combine, producing a large nucleus and releasing large amounts of energy.

a)

nuclear fission

b)

nuclear fusion

120.

an isotope with an unstable nucleus

a)

nuclear radiation

b)

radioactivity

c)

radioisotope

d)

background radiation

121.
True or False:  During nuclear decay atoms of one element can change into atoms of a different element altogether. 
a)
True
b)
False
122.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
123.
What element is the ?
a)
Ag-115
b)
Cd-115
c)
Pd-115
d)
Not Listed

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