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FINAL EXAM REVIEW

Total questions: 100

Worksheet time: 1hrs 17mins

Name
Class
Date
1.

What is Energy?

a)

The ability to do anything

b)

The ability to cause change/ do work

c)

The investigation of nature

d)

A fact of life

2.

What is an example of kinetic energy?

a)

A bird sitting in a tree

b)

A bouncy ball on the table

c)

A car driving on the highway

d)

A book on shelf

3.

What is an example of potential energy?

a)

A bowling ball rolling down a lane

b)

A car parked in a lot

c)

An apple falling from a tree

d)

Sunlight heating up the atmosphere

4.

Energy cannot be created or destroyed.

a)

True

b)

False

5.

What is nuclear energy?

a)

Energy in the nucleus of an atom

b)

Energy in the particles of an object

c)

Energy that is carried by electromagnetic waves

d)

Energy in a system of objects

6.

What is the definition of friction?

a)

A force that resists the sliding of two objects that are touching

b)

A force that increases sliding between two objects

c)

The change from potential to kinetic energy

d)

A transformation from radiant to mechanical energy

7.

What transformation occurs in a toaster?

a)

Electrical to radiant

b)

Electrical to thermal

c)

Thermal to mechanical

d)

Solar to electrical

8.

What type of energy transformation occurs when a piece of wood burns?

a)

Electrical energy is released as radiant energy

b)

Stored chemical energy is released as thermal energy

c)

Mechanical energy is stored as chemical energy

d)

No transformation occurs

9.

What is the equation for kinetic energy?

a)

KE = 1/2 m x v2

b)

KE = Speed (m/s) + height (m)

c)

KE = Distance (m) / time (s)

d)

KE = Mass (g) * gravity * height (m)

10.

What is potential energy?

a)

The energy an object has due to its atomic structure.

b)

The energy an object has due to its chemical composition.

c)

The energy an object has due to its motion.

d)

The energy an object has due to its position or condition.

11.

What is kinetic energy?

a)

The energy an object has due to its position or condition

b)

The energy an object has due to its motion

c)

The energy an object has due to its chemical composition

d)

The energy an object has due to its atomic structure

12.

Which object has the most potential energy?

a)

A ball resting on the ground.

b)

A ball being thrown at 100 miles per hour.

c)

A ball on top of a refrigerator.

d)

A ball resting on the edge of a cliff.

13.

Four cars are positioned at the top of a hill. Which car has the most potential energy?

a)

A

b)

B

c)

C

d)

D

14.
The heat from a lamp allows a lizard to remain warm. This is an example of which type of heat transfer?
a)
radiation
b)
conduction
c)
convection
d)
insulation
15.
Which will most likely occur when raw egg is placed on black pavement on a hot, summer day?
a)
The pavement will conduct the heat and cook the egg.
b)
The egg will reflect the heat and make the pavement hotter underneath.
c)
The egg will absorb the heat  and leave the pavement hotter underneath.
d)
The pavement will absorb the heat from the egg, and the egg will stay raw.
16.
Which best describes the process of convection?
a)
Convection is the primary way  heat travels  through rays.
b)
Convection is the primary way heat travels  through metals.
c)
Convection is the primary way heat travels  through appliances.
d)
Convection is the primary way heat travels  through liquids and gasses.
17.
Which is NOT an insulator.
a)
Wool
b)
Plastic
c)
Copper
d)
Glass
18.
What is the difference between a conductor and an insulator?
a)
An insulator allows electricity to flow through it easily and a conductor does not
b)
A conductor allows electricity to flow through it easily and an insulator does not.
c)
An insulator is magnetic and a conductor is not
d)
A conductor is magnetic and an insulator is not
19.
A great conductor of energy is:
a)
wood
b)
plastic
c)
metal
d)
cloth
20.
What kind of properties can only be observed when a substance changes into a different substance?
a)
physical properties
b)
chemical properties
21.
Which type of property is the ability to conduct electricity?
a)
physical property
b)
chemical property
22.
Properties that can be observed without changing the identity of the substance.
a)
Physical
b)
Chemical
23.
Example for physical property
a)
odor
b)
burns in air
c)
reacts with water to create hydrogen gas
d)
rust
24.
Example for chemical property
a)
color
b)
hardness
c)
toxicity
d)
solubility
25.

Which of the following is the appropriate measurement for volume ?

a)

56 mL

b)

10 grams

c)

47 centimeters

d)

4 quarts

26.
In the metric system what is a liter used to measure?  
a)
solids
b)
liquids
27.

What is a unit used to measure the volume of a solid object?

a)

milliters

b)

pounds

c)

cubic centimeters

d)

grams

28.

When reading the volume of water in a graduated cylinder, you should always ______________

a)

look at the water level above the curve (meniscus)

b)

hold the graduated cylinder in the air to read the meniscus (curve)

c)

estimate the water level

d)

look at the bottom of the meniscus (curve)

29.

Calculate the volume of the rock

a)

10.0 cm3

b)

10.0 mL

c)

30.0 cm3

d)

40.0 cm3

30.

We start with 50 mL in a graduated cylinder and drop in an object. The water rises to 64 mL. What is the volume of this object?

a)

64 mL

b)

64 cm3

c)

14 mL

d)

14 cm3

31.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
32.

The definition of volume

a)

The amount of matter an object has

b)

The amount of matter within a certain amount of space

c)

The amount of space inside something

d)

The amount of space something takes up

33.

What causes an object to sink in water?

a)

if the object's density is less than the water's density.

b)

if the object's density is the same as water's density.

c)

if the object's density is greater than water's density.

d)

if the object's density is zero

34.
What is the density of a substance that has a mass of 30g and a volume of 6 liters?
a)
24 g/l
b)
5 g/l
c)
36 g/l
d)
180 g/l
35.

The attraction between particles gives solids a definite

a)

shape and volume

b)

shape and color

c)

shape and position

d)

flow and radius

36.

The temperature at which a solid begins to liquefy is its ______ point.

a)

freezing

b)

boiling

c)

melting

d)

mass

37.

The amount of energy required for a liquid at its boiling point to become a gas is _____________.

a)

heat of fusion

b)

heat of vaporization

c)

transpiration

d)

freezing point

38.

Which of the following is a state of matter?

a)

particle

b)

thermal

c)

plasma

d)

diffuse

39.

When the temperature of a substance is lowered, its particles

a)

vibrate more quickly

b)

stop vibrating completely

c)

escape the attractive forces of the other particles

d)

vibrate more slowly

40.

An example of a substance that can undergo sublimation is

a)

glass

b)

liquid crystals

c)

water

d)

dry ice (frozen carbon dioxide)

41.

When a gas becomes a liquid it is called

a)

condensation

b)

evaporation

c)

sublimation

d)

freezing

42.
Between what two points is the most energy being added to the system
a)
A -B
b)
B-C
c)
C-D
d)
D-E
43.
Which line segment demonstrates vaporization occurring?
a)
B-C
b)
C-D
c)
D-E
d)
E-F
44.
As substance goes from D to E what happens to the distance between the particles?
a)
particles get closer together
b)
particles disappear
c)
particles get far apart
45.
At what temperature is this substance melting?
a)
50C
b)
100C
c)
0C
46.

Identify the mode of heat transfer in the given picture.

a)

Conduction

b)

Convection

c)

Radiation

47.

Identify the mode of heat transfer in the given picture.

a)

Conduction

b)

Convection

c)

Radiation

48.

Heat flows from a warmer place to a cooler one.

a)

True

b)

False

49.
Which scientist developed the atomic theory?
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
James Chadwick
50.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
51.
What did Thomson discover?
a)
electron
b)
proton
c)
neutron
d)
electron cloud
52.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

53.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
54.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
55.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
56.

He claimed that matter was made of small, hard particles that he called “atomos.”

a)

Democritis

b)

Dalton

c)

Moseley

d)

Einstein

57.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
58.
Which liquid is the least dense?
a)
oil
b)
water
c)
syrup 
d)
plastic bottle
59.

What is the density of water?

a)

0 g/mL

b)

1 g/mL

c)

10 g/mL

d)

100 g/mL

60.

All matter consists of particles called

a)

Units

b)

Atoms

c)

Cubes

d)

Pints

61.

The nucleus of an atom contains protons and_______________

a)

Electrons

b)

Haptons

c)

Neutrons

d)

Wontons

62.

Electrons move around_________________the nucleus

a)

Inside

b)

Outside

c)

On top of

d)

Without

63.

An element is determined by the number of ___________________ (also known as its atomic number).

a)

Neutrons

b)

Electrons

c)

Protons

d)

Wontons

64.

A ___________________ is a combination of two or more atoms that are held together by covalent bonds.

a)

Moles

b)

Ions

c)

Molecules

d)

Megatrons

65.

The number of _______ in one atom of an element determines the atom's identity.

a)

Protons

b)

Electrons

c)

Neutrons

d)

Isotope

66.

The arrangement of electrons in energy levels around an atomic nucleus.

a)

Electron shell

b)

Electron affinity

c)

Electron configuration

d)

Electrical charge

67.

A negatively charged particle, located in the outermost shell of an atom.

a)

Valence electron

b)

Muon

c)

Neutrino

d)

Lepton

68.

How many neutrons are in an atom of carbon-14?

a)

6

b)

8

c)

10

d)

14

69.

An atom with the same number of protons and electrons (no charge) and the expected atomic mass or number of neutrons from the periodic table.

a)

Neutral/Normal Atom

b)

Ion

c)

Isotope

70.

An atom that has gained or lost electrons in an attempt to become stable/bond with another atom.

a)

Normal/Neutral Atom

b)

Ion

c)

Isotope

71.

A negatively charged ion that has gained electrons to satisfy the octet rule (metals do this)

a)

Anion

b)

Cation

c)

Neutral Atom

d)

Isotope

72.

A positively charged ion that has lost electrons to satisfy the octet rule (non-metals do this)

a)

Anion

b)

Cation

c)

Neutral Atom

d)

Isotope

73.

Atoms of the same element that have different mass than expected because they have a different number of neutrons.

a)

Neutral Atom

b)

Ion

c)

Isotope

d)

Cation

74.

A weak bond between two ions of opposite charge (a metal that loses electrons and a non-metal that gains electrons)

a)

Ionic Bond

b)

Covalent Bond

c)

Alloy

d)

Mixture

75.

A strong bond between two non-metals that share electrons to satisfy the octet rule.

a)

Ionic Bond

b)

Covalent Bond

c)

Alloy

d)

Mixture

76.

If an atom has 9 protons and 10 electrons it has a charge of ____.

a)

0

b)

-1

c)

+1

d)

-2

77.

If an atom has 4 protons and 2 electrons it has a charge of ____.

a)

0

b)

-2

c)

+2

d)

+1

78.

Who invented the Periodic Table?

a)

Mendeleev

b)

Bohr

c)

Lewis

d)

Democritus

79.

The first energy shell can hold ______ electrons.

a)

2

b)

8

c)

18

80.

Elements in the same group or column have the same ...

a)

# of valence electrons

b)

# of shells

c)

# of protons

d)

Mass Number

81.

Rows on the periodic table are called ___________.

a)

Periods

b)

Sentences

c)

Fences

82.

The columns in the periodic table are called ___________.

a)

Towers

b)

Herds

c)

Groups

83.

Elements in the same group have __________

a)

Similar Properties

b)

Same number of shells

c)

Similar Mass

84.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

85.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

86.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

87.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

88.

Which of the following is an ionic compound?

a)

HCl

b)

H2O

c)

MgO

d)

CO2

89.

When one atom transfers one or more valence electrons to another atom, a(n) __________ is formed.

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

hair bond

90.

What is the ionic charge of a Calcium ion?

a)

2+

b)

2-

c)

3+

d)

3-

91.

Which element will be paired to Sulfur for it to become a covalent compound?

a)

Potassium

b)

Magnesium

c)

Aluminum

d)

Carbon

92.

What is the ionic charge of an Oxygen ion?

a)

2+

b)

2-

c)

4+

d)

4-

93.

What type of bond is formed between Li and F?

a)

Covalent

b)

Ionic

c)

Metallic

d)

Carbon

94.

Which of the following is an Covalent compound?

a)

NaCl

b)

CaCl2

c)

KI

d)

CO

95.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
96.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
97.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
98.
How many Aluminum are in Al2O3?
a)
3
b)
2
c)
5
99.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
100.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4

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