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Review for Unit 2 Matter and Atomic Structure

Total questions: 139

Worksheet time: 2hrs 4mins

Name
Class
Date
1.

The smallest part of an element that has all the properties of that element.

a)

PROTON

b)

NEUTRON

c)

ELECTRON

d)

ATOM

2.

Positively charged particle in the nucleus of an atom.

a)

PROTON

b)

NEUTRON

c)

ELECTRON

d)

ATOM

3.

A subatomic particle that has no charge and that is found in the nucleus of an atom.

a)

PROTON

b)

NEUTRON

c)

ELECTRON

d)

ATOM

4.

A subatomic particle that has a negative charge in the orbitals.

a)

PROTON

b)

NEUTRON

c)

ELECTRON

d)

ATOM

5.

The simplest form of matter

a)

Molecule

b)

Compound

c)

Element

d)

Water

6.

This is equal to the number of protons in the nucleus of an atom.

a)

Atomic Mass

b)

Atomic Number

c)

Isotopic Number

d)

Atomic Radius

7.

Electrons located on the outermost energy level of an atom.

a)

Protons

b)

Valet Electrons

c)

Valence Electrons

d)

Orbital

8.

The center of an atom that contains the protons and the neutrons.

a)

NUCLEUS

b)

ORBITAL

c)

ENERGY LEVEL

d)

CELL

9.

The charge of the proton is

a)

POSITIVE

b)

NEGATIVE

c)

NEUTRAL

10.

The charge of the electron is

a)

POSITIVE

b)

NEGATIVE

c)

NEUTRAL

11.

The charge of the neutron is

a)

POSITIVE

b)

NEGATIVE

c)

NEUTRAL

12.

How many protons does the element gold have?

a)

79

b)

196.967

c)

196

d)

118

13.

Adam analyses a sample of a substance. He concludes that it consists of more than one type of atom chemically combined. What does the substance represent

a)

an element

b)

a compound

c)

a heterogeneous mixture

d)

a homogeneous mixture

14.

What composes an element?

a)

atoms of the same structure

b)

compounds of the same structure

c)

mixtures of different substances

d)

molecules of different structures

15.

A student leaves a bowl of ice cream on a table, where it turns to a liquid. The student places the liquid ice cream back into the freezer overnight. How do the motion of the particles in the ice cream change when it is placed in the freezer?

a)

the particles slow down and move closer together

b)

the particles speed up and move closer together

c)

The particles slow down and move farther apart

d)

the particles speed up and move farther apart

16.

Which statement best describes a gas?

a)

a gas has particles that are close together but can slide past one another

b)

a gas has particles that have large distances between them and move freely

c)

a gas has particles that are close together but move freely

d)

a gas has particles that have not space between them and do not move

17.

A student sketches the particles of a particular substance in the three states of matter. Which state of matter is shown by each sketch.

a)

A is solid, B is liquid, and C is gas

b)

A is gas, B is solid, and C is liquid

c)

A is liquid, B is gas, and C is solid

d)

A is liquid, B is solid, and C is gas

18.

A substance changed from one state to another. The image shows its particle motion in the first state and the second state. How is the transition between State 1 and State 2 best described?

a)

solid state to liquid state

b)

liquid state to solid state

c)

liquid state to gaseous state

d)

gaseous state to solid state

19.

Which particle diagram can be classified as a compound?

a)
b)
c)
d)
20.

What are the building blocks of matter?

a)

Atoms

b)

Molecules

c)

Compounds

d)

Cells

e)

Legos

21.

__ have a +1 charge.

a)

Quarks

b)

Protons

c)

Gluons

d)

Electrons

e)

Neutrons

22.

Which subatomic particle has the smallest mass?

a)

protons

b)

neutrons

c)

electrons

23.

Most of an atom is made up of...

a)

energy

b)

protons

c)

empty space

d)

neutrons

24.

Electrons are located______.

a)

outside the nucleus

b)

inside the nucleus

25.

Which two particles have about the same amount of mass (1amu)?

a)

neutrons and protons

b)

protons and electrons

c)

electrons and neutrons

26.

Neutrons are located______.

a)

outside the nucleus

b)

inside the nucleus

27.

Elements are identified by the number of ___ it has.

a)

neutrons

b)

gluons

c)

quarks

d)

electrons

e)

protons

28.

The subatomic particles are:

a)

neutrons, quarks, & electrons

b)

gluons, electrons, & protons

c)

quarks & gluons

d)

electrons, neutrons, & protons

e)

protons & neutrons

29.

__ have a -1 charge.

a)

Quarks

b)

Protons

c)

Gluons

d)

Electrons

e)

Neutrons

30.

__ have a 0 charge (neutral).

a)

Quarks

b)

Protons

c)

Gluons

d)

Electrons

e)

Neutrons

31.

Three __ make up each particle inside the nucleus.

a)

Quarks

b)

Protons

c)

Gluons

d)

Electrons

e)

Neutrons

32.

The number of protons in an atom is called its ___. This is also unique for each element.

a)

isotope

b)

element symbol

c)

Gluons

d)

mass number

e)

atomic number

33.

Different ___ of an element have different mass numbers because they have different numbers of neutrons.

a)

isotopes

b)

ions

c)

Gluons

d)

mass numbers

e)

atomic numbers

34.

Atoms can gain or lose electrons and become ___, which are atoms that have a positive or negative charge because they have unequal numbers of protons and electrons.

a)

isotopes

b)

ions

c)

Gluons

d)

molecules

e)

atomic numbers

35.

Around 400 B.C.E., the philosopher ____ introduced the idea of the atom as the basic building block matter.

a)

Democritus

b)

John Dalton

c)

JJ Thomson

d)

Earnest Rutherford

e)

Niels Bohr

36.

Around 1800, the English chemist __ reintroduced the idea of the atom.

a)

Democritus

b)

John Dalton

c)

JJ Thomson

d)

Ernest Rutherford

e)

Niels Bohr

37.

In 1897, ____ discovered the first subatomic particle, the electron, while researching cathode rays.

a)

Democritus

b)

John Dalton

c)

JJ Thomson

d)

Ernest Rutherford

e)

Niels Bohr

38.

___ discovered the nucleus of the atom in 1911.

a)

Erwin Schrödinger

b)

John Dalton

c)

JJ Thomson

d)

Ernest Rutherford

e)

Niels Bohr

39.

Thomson's model of the atom could be described as follows:

a)

nucleus in the center with regions around the nucleus, called orbitals, where electrons are most likely to be (Electron cloud model)

b)

electrons move around the nucleus only at fixed distances from the nucleus based on the amount of energy they have.

c)

negative electrons are scattered throughout a sphere of positive charge. (Plum pudding model)

d)

the electrons move through empty space around the tiny positive nucleus like planets orbiting the sun. (Planetary model)

e)

solid, hard spheres

40.

____ proposed a model where electrons move around the nucleus only at fixed distances, called energy levels, from the nucleus based on the amount of energy they have.

a)

Erwin Schrödinger

b)

John Dalton

c)

JJ Thomson

d)

Ernest Rutherford

e)

Niels Bohr

41.

Bohr's model of the atom could be described as follows:

a)

nucleus in the center with regions around the nucleus, called orbitals, where electrons are most likely to be (Electron Cloud Model)

b)

electrons move around the nucleus only at fixed distances from the nucleus based on the amount of energy they have.

c)

negative electrons are scattered throughout a sphere of positive charge. (Plum pudding model)

d)

the electrons move through empty space around the tiny positive nucleus like planets orbiting the sun. (Planetary model)

e)

solid, hard spheres

42.

Which of the following is the description of the model is still accepted by scientists today and it is based on orbitals

a)

nucleus in the center with regions around the nucleus, called orbitals, where electrons are most likely to be (Electron Cloud model)

b)

electrons move around the nucleus only at fixed distances from the nucleus based on the amount of energy they have.

c)

negative electrons are scattered throughout a sphere of positive charge. (Plum pudding model)

d)

the electrons move through empty space around the tiny positive nucleus like planets orbiting the sun. (Planetary model)

e)

solid, hard spheres

43.

In the 1920s, ___ proposed that electrons travel in waves, which means their exact positions cannot be determined. He developed an equation to calculate the chances of an electron being in any given place. Using his equation, he identified regions around the nucleus, called orbitals, where electrons are most likely to be.

a)

Erwin Schrödinger

b)

John Dalton

c)

JJ Thomson

d)

Ernest Rutherford

e)

Niels Bohr

44.
The mass listed on the periodic table for each element is known as the 
a)
average atomic mass
b)
atomic mass
c)
atomic weight
d)
weighted mass
45.

To calculate average atomic mass, you need

a)

the atomic mass of each isotope

b)

the percent abundance of each isotope

c)

the atomic mass and percent abundance of each isotope

d)

to find the average of the atomic masses of each isotope

46.

What is the relative mass of an electron?

a)

1 amu

b)

0 amu

47.

An element has two isotopes, one with a mass of 39 and one with a mass of 41. If the average mass is 40.6, which isotope is more abundant?

a)

mass of 39

b)

mass of 41

c)

they are both equally abundant

48.

A state of matter that has a definite volume and shape.

a)

solid

b)

liquid

c)

gas

d)

matter

49.

Fourth state of matter plasma exists at

a)

high temperature

b)

low temperature

c)

room temperature

50.

Stainless steel is an example of

a)

Element

b)

Compound

c)

Heterogeneous mixture

d)

Homogeneous mixture

51.

Boiling point is an example of extensive physical properties.

a)

True

b)

False

52.
Who believed that electrons were scattered amongst positively charged material.
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Niels Bohr
53.
Believed that atoms are small, hard particles that were "indivisible"
a)
Democritus
b)
Aristotle
c)
Schrodinger
d)
Greek Philosophers
54.
Did experiments to show that atoms form compound in set ratios.
a)
John Dalton
b)
Schrodinger
c)
Niels Bohr
d)
JJ Thomson
55.
Discovered that the atom has a small, dense, positively charged nucleus.
a)
Ernest Rutherford
b)
Heisenberg
c)
Democritus
d)
JJ Thomson
56.
Believed that electrons traveled around the nucleus in definite paths.
a)
Niels Bohr
b)
John Dalton
c)
Modern Atomic Theory
d)
Ernest Rutherford
57.
Determined that electron paths cannot be predicted and exist inside the Electron Cloud.
a)
Schrodinger & Heisenberg
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
58.
Believed that all atoms of the same element would be the same.
a)
John Dalton
b)
JJ Thomson
c)
Niels Bohr
d)
Modern Atomic Theory
59.
How many protons does an atom with an atomic number of 28 and a mass number of 40 have?
a)
28
b)
68
c)
12
d)
40
60.
The following element has _____________ electrons.
a)
114
b)
289
c)
175
d)
403
61.
How many neutrons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?
a)
20
b)
25
c)
2
d)
18
62.
How many protons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
74
c)
40
d)
36
63.
What scientist is best known for his gold foil experiment?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
64.
What scientist first developed 4 rules for atomic theory, and helped kick start modern chemistry?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
65.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
66.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
67.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
68.

What is an isotope?

a)

A charged atom

b)

Two atoms of the same element with different amounts of neutrons

c)

Two atoms of the same element with different amounts of protons

d)

A neutral atom

69.

how many electrons does an uncharged atom of Neon have?

a)

8

b)

9

c)

10

d)

11

70.

Which two components of an atom contribute to the mass?

a)

Protons and neutrons

b)

Protons and electrons

c)

neutrons and electrons

71.

What has atoms arranged in an ordered pattern?

a)

Protons

b)

Crystals

c)

Solids

d)

Matter

72.

Anything that takes up space is called WHAT?

a)

Atoms

b)

Crystals

c)

Solids

d)

Matter

73.
Which of the following tells you that a chemical change may have occurred?
a)
Change Shape
b)
Melting
c)
Vaporizing
d)
Change in color
74.
What happens in ALL chemical changes?
a)
Change in state of matter
b)
A new substance is formed
c)
Bubbles are produced
d)
An explosion
75.
Is wood burning a physical or chemical change?
a)
Physical 
b)
Chemical
76.
Is Gatorade powder dissolving in water physical or chemical change?
a)
Physical 
b)
Chemical
77.
Is mold growing on cheese a physical or chemical change?
a)
Physical 
b)
Chemical
78.
Is sharpening a pencil a physical or chemical change?
a)
Physical 
b)
Chemical
79.
Is copper tarnishing a physical or chemical change?
a)
Physical 
b)
Chemical
80.
The Law of Conservation of Mass tells us matter can't  ______________.
a)
change color
b)
change state of matter
c)
be created or destroyed
d)
change temperature
81.

Which of the following is not a clue that a chemical reaction has taken place?

a)

Changing size

b)

Changing color

c)

A gas being formed

d)

Formation of a precipitate

82.

An ice cream cone melts in a kid's hand while walking outside on a hot summer day. What is this an example of?

a)

Physical property

b)

Chemical property

c)

Physical change

d)

Chemical change

83.

Water boils at 100˚C. What is this an example of?

a)

Physical property

b)

Chemical property

c)

Physical change

d)

Chemical change

84.

Benzene is a compound that is highly flammable. What is this an example of?

a)

Physical property

b)

Chemical property

c)

Physical change

d)

Chemical change

85.

Copper is a good conductor of heat and electricity. What is this an example of?

a)

Physical property

b)

Chemical property

c)

Physical change

d)

Chemical change

86.
Physical properties are
a)
properties that can be observed without changing the identity of the substance
b)
properties that describe how a substance changes into a completely different substance
87.
which one is the definition of chemical property?
a)
a property or characteristic of a substance that is observed during a reaction where the chemical composition of a substance is changed
b)
any change that results in the formation of new chemical substances
c)
combustibility
88.

Melting point is...

a)

The temperature at which a solid can change to a liquid

b)

The temperature at which a solid can change to a gas

c)

The temperature at which a gas can change to a liquid

d)

The temperature at which a liquid can change to a solid

89.

The melting point of water is...

a)

100 degrees Celsius

b)

14 degrees Celsius

c)

32 degrees Celsius

d)

0 degrees Celsius

90.

The boiling point of water is...

a)

32 degrees Celsius

b)

109 degrees Celsius

c)

100 degrees Celsius

d)

-29 degrees Celsius

91.

What word describes the relationship between the mass of a material and its volume?

a)

Volume

b)

Weight

c)

Height

d)

Density

92.

The ability to be hammered into different shapes is __________.

a)

ductility

b)

malleability

c)

density

d)

volume

93.

If a substance is ductile, it can be _______________.

a)

very heavy for its size

b)

easily breakable

c)

used to insulate wires

d)

rolled into thin wires

94.

Which set of properties, intensive or extensive, are based on the size of a sample?

a)

intensive

b)

extensive

95.

What kind of physical property is this? Color

a)

intensive

b)

extensive

96.

What kind of physical property is this? Energy

a)

intensive

b)

extensive

97.

What kind of physical property is this? Number of Atoms

a)

intensive

b)

extensive

98.

What kind of physical property is this? Density

a)

intensive

b)

extensive

99.

Melting point

a)

Intensive Property

b)

Extensive Property

100.

Which instrument is used to measure an intensive property?

a)
b)
c)
d)
101.

Which of the following properties is related to mass and volume, but not an extensive property?

a)

Number of Atoms

b)

Moles

c)

Density

d)

Potential Energy

102.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
103.

Which Russian chemist is commonly considered to be the developer of the modern Periodic Table of the Elements?

a)

Nikolay Basov

b)

Pavel Cherenkov

c)

Antoine Lavoisier

d)

Dmitri Mendeleev

104.

Which French nobleman is widely considered the "father of modern chemistry"?

a)

Blaise Pascal

b)

Dmitri Mendeleev

c)

Antoine Lavoisier

d)

Louis Pasteur

105.

Who developed the Law of Conservation of Mass?

a)

Amedeo Avogadro

b)

Henri Becquerel

c)

John Dalton

d)

Demokritos

e)

Antoine Lavoisier

106.

Who discovered electrons?

a)

Joseph Priestly

b)

Henri Becquerel

c)

John Dalton

d)

Robert Millikan

e)

J. J. Thomson

107.

Who discovered protons?

a)

Joseph Priestly

b)

Ernest Rutherford

c)

John Dalton

d)

Robert Millikan

e)

J. J. Thomson

108.

Who developed the Atomic Theory?

a)

Joseph Priestly

b)

Ernest Rutherford

c)

John Dalton

d)

Robert Millikan

e)

J. J. Thomson

109.

Who developed the Law of Multiple Proportions?

a)

Antoine Lavoisier

b)

Robert Boyle

c)

John Dalton

d)

Robert Millikan

e)

J. J. Thomson

110.

Who developed the Law of Definite Proportions?

a)

Antoine Lavoisier

b)

Robert Boyle

c)

John Dalton

d)

Joseph Proust

e)

J. J. Thomson

111.

Who named atoms?

a)

Antoine Lavoisier

b)

Robert Boyle

c)

John Dalton

d)

Democritos

e)

J. J. Thomson

112.

Who discovered the charge/mass of an electron?

a)

Joseph Priestly

b)

Henri Becquerel

c)

John Dalton

d)

Robert Millikan

e)

Antoine Lavoisier

113.
After the nucleus of a radioactive element undergoes changes, the element can transform into ...
a)
  (a)  a different isotope of the same element.
b)
(b) an entirely different element.
c)
Both (a) and (b)
d)
Neither (a) nor (b)
114.
Alpha particles.....
a)
a) are positively charged.
b)
b) consist of two protons and four neutrons.
c)
c) can penetrate any thickness of matter
d)
d) All of the above 
115.
The process of nuclear change in an atom of radioactive material is called... 
a)
nuclear decay
b)
nuclear mass
c)
isotopes
d)
radon
116.
During beta decay, a nucleus .... 
a)
gives up two protons and two neutrons.
b)
  maintains the same number of protons and neutrons.
c)
  loses a proton and gains a neutron.
d)
gains a proton and loses a neutron. 
117.
When a nucleus undergoes nuclear decay by gamma rays, the atomic number of the element....
a)
remains the same
b)
  decreases by one.
c)
increases by one.
d)
increases by two.
118.
The process of the production of lighter nuclei from heavier nuclei is called
a)
mass energy
b)
magneticism
c)
fusion
d)
fission
119.
The type of radioactive particle that can be stopped by a sheet of paper is the ____.
a)
alpha particle
b)
beta particle
c)
gamma ray
d)
uranium
120.
The most penetrating type of radiation is the ____.  
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
121.
A helium nucleus with two protons and two neutrons is called a(n) ____.  
a)
alpha particle
b)
electroscope
c)
beta particle
d)
gamma ray
122.
Negatively charged particles emitted from a nucleus at a high speed are ____.  
a)
alpha particle
b)
gamma rays
c)
beta particles
d)
X rays
123.
The three types of nuclear radiation in increasing order of penetrating power are ____.  
a)
  alpha, beta, gamma 
b)
X ray, beta, gamma
c)
alpha, gamma, beta 
d)
X ray, gamma, beta 
124.
Radioactive tracers are useful in ____.
a)
calculating the ages of fossils 
b)
fueling nuclear reactions 
c)
determining medical problems 
d)
treating brain tumors 
125.
The process by which nuclei having low masses are united to form nuclei with larger masses is ____.  
a)
a chain reaction 
b)
fission
c)
a chemical reaction 
d)
fusion 
126.

What type of decay is shown here

23892U ---> 23490Th + 42He.

a)

alpha

b)

beta

c)

gamma

127.

What type of nuclear decay is shown here

13756Ba →→ 13756Ba + γ rays

a)

alpha

b)

beta

c)

gamma

128.

Finish this equation

20983Bi--> _______ + 20581Tl

a)

42He

b)

0-1e

c)

y

129.

Identify the type of nuclear decay shown here

21483Bi → 0-1e + 21484Po

a)

alpha

b)

beta

c)

gamma

130.

finish the equation


22688Ra --> ____ + 22688Ra

a)

42He

b)

0-1e

c)

y

131.

Carbon-14 and carbon-12 have the same number of protons but a different number of neutrons. These different forms of the same element are called

a)

radioactive

b)

isotopes

c)

nuclei

d)

tracers

132.

The mass number of a nucleus is equal to ______.

a)

the number of protons plus the number of neutrons

b)

the number of electrons

c)

the number of protons

d)

the number of neutrons

133.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
134.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
135.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

136.

An atom of tin has an atomic number of 50 and a mass number of 119. How many protons, electrons, and neutrons are found in one neutral atom of tin?

a)

50 protons, 69 electrons, 50 neutrons

b)

50 protons, 50 electrons, 69 neutrons

c)

69 protons, 50 electrons, 69 neutrons

d)

69 protons, 69 electrons, 50 neutrons

137.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
138.
An element with 4.35% have a mass of 49.9461 amu, 83.79% have amass of 51.9405 amu, 9.50% have a mass of 52.9407 amu, and 2.36% have a mass of 53.9389amu.
a)
51.99 amu
b)
52.19 amu
c)
53.45 amu
d)
17.33 amu
139.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.

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