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Unit 3 Test Review

Total questions: 114

Worksheet time: 4hrs 58mins

Name
Class
Date
1.

elements in Group 1A of the periodic table; the ions of the elements in this group have a 1+ charge

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

isotopes

2.

elements in Group 2A of the periodic table; the ions of the elements in this group have 2+ charge

a)

alkaline earth metals

b)

alkali metals

c)

isotopes

d)

halogens

3.

the electrode at which oxidation occurs; it is the positively charged electrode within a cathode ray tube

a)

anode

b)

isotopes

c)

diatomic elements

d)

cathode

4.

the smallest particle of an element that retains the chemical identity of the element; made up of positively charged protons, negatively charged electrons, and neutrons

a)

atom

b)

cathode

c)

isotopes

d)

electron

5.

the weighted average of the masses of the existing isotopes of an element; the sum of the masses of an element’s isotopes each multiplied by its natural abundance

a)

average atomic mass

b)

atomic number

c)

excited state

d)

ground state

6.

the number of protons in the nucleus of an atom

a)

atomic number

b)

average atomic mass

c)

mass number

d)

period

7.

the electrode at which reduction occurs; it is the negatively charged electrode within a cathode ray tube

a)

cathode

b)

anode

c)

mass number

d)

electron

8.

a stream of electrons produced at the negative electrode (cathode) of a tube containing a gas at low pressure

a)

cathode ray

b)

anode

c)

diatomic elements

d)

cathode

9.

elements that exist as diatomic molecules in nature; they include oxygen, hydrogen, nitrogen, fluorine, chlorine, iodine, and bromine

a)

diatomic elements

b)

electron

c)

excited state

d)

ground state

10.

a negatively charged particle within an atom; it has a mass of 0.000549 amu

a)

electron

b)

neutron

c)

proton

d)

diatomic elements

11.

an electron that has absorbed energy and, therefore, exists at a higher energy level

a)

excited state

b)

neutron

c)

diatomic elements

d)

metalloids

12.

the normal state of an electron or atom; at this state the electron or atom has the lowest possible energy

a)

ground state

b)

excited state

c)

metalloids

d)

anode

13.

a vertical column on the periodic table with similar electron configurations, chemical properties, and the same number of valence electrons

a)

group

b)

period

c)

proton

d)

neutron

14.

elements in Group 7A (17); they are the most reactive nonmetals

a)

halogens

b)

alkali metals

c)

alkaline earth metals

d)

isotopes

15.

an atom that has the same number of protons as another, identical atom, but with differing numbers of neutrons

a)

isotopes

b)

proton

c)

neutron

d)

halogens

16.

the sum of the number of protons and neutrons in the nucleus of an atom

a)

mass number

b)

atomic number

c)

average atomic mass

d)

proton

17.

an element that typically has a high melting point, is ductile, malleable, and shiny, and a good conductor of heat and electricity

a)

metal

b)

metalloids

c)

halogen

d)

atom

18.

elements found on the stair-step line of the periodic table with properties of metals and nonmetals

a)

metalloids

b)

halogens

c)

neutron

d)

metal

19.

a neutral particle within the nucleus of an atom; it has a mass of 1.00867 amu

a)

neutron

b)

proton

c)

electron

d)

atom

20.

elements in Group 8A (18); they do not readily react with other elements due to a satisfied octet; they are inert

a)

noble gases

b)

halogens

c)

metal

d)

metalloids

21.

elements that typically have a low melting point,a dull surface, breaks easily, and is a poor conductor of heat and electricity

a)

nonmetal

b)

noble gases

c)

halogens

d)

metalloids

22.

a horizontal row on the periodic table; the elements within the same period have the same number of energy levels

a)

period

b)

group

c)

metal

d)

halogens

23.

natural law that states that the chemical and physical properties of elements are periodic functions of their atomic numbers

a)

periodic law

b)

anode

c)

noble gases

d)

proton

24.

an arrangement of the elements by their atomic numbers so that elements are periodic functions of their atomic numbers

a)

periodic table

b)

periodic law

c)

metalloids

d)

metal

25.

a positively charged particle within the nucleus of an atom; it has a mass of 1.00720 amu

a)

proton

b)

neutron

c)

electron

d)

isotopes

26.

the percentage of an isotope that occurs in nature

a)

relative abundance

b)

periodic law

c)

average atomic mass

d)

excited state

27.

the attractive force among the particles in the nucleus of an atom; in a stable atom, it overcomes the forces of repulsion among protons

a)

strong nuclear force

b)

relative abundance

c)

transition elements

d)

valence electrons

28.

elements found in the middle column of the periodic table; they have multiple oxidation states

a)

transition elements

b)

valence electrons

c)

relative abundance

d)

strong nuclear force

29.

electrons in the outermost energy level of an atom

a)

valence electrons

b)

proton

c)

neutron

d)

electrons

30.

Which reaction produces harmful radioactive waste?

a)

Fission

b)

Photosynthesis

c)

chain reaction

d)

Fusion

31.

_____is the joining of atomic nuclei

a)

Fusion

b)

chain reaction

c)

Photosynthesis

d)

Fission

32.
What is a chain reaction?
a)
When electrons are emitted causing electricity
b)
When a nuclear fission reaction occurs, the protons emitted can strike other nuclei in the sample, and cause them to split
c)
When a nuclear fission reaction occurs, the neutrons emitted can strike other nuclei in the sample, and cause them to split
d)
When a nuclear fission reaction occurs, the electrons emitted can strike other nuclei in the sample, and cause them to split
33.

How is the alpha particle written in a nuclear equation?

a)

42He

b)

24He

c)

0-1e

d)

00γ

34.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
35.

Gamma rays have

a)

no mass

b)

a huge mass

c)

a small mass

d)

an average mass

36.

During beta-particle emission, a neutron splits into a____________________.

a)

proton and electron

b)

neutron and electron

c)

neutron and proton

37.

The plum pudding model is discovered by

a)

J.J. Thompson

b)

Ernest Rutherford

c)

James Chadwick

d)

Albert Eisntein

38.

Who proved that the neutron existed?

a)

Thompson

b)

Rutherford

c)

Chadwick

d)

Newton

39.

Who did gold foil experiment for the first time?

a)

Thompson

b)

Rutherford

c)

Chadwick

d)

Newton

40.

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

41.

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

42.

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

43.
True or False: An isotope is when the protons and neutrons are the same, but the electrons are different.
a)
True
b)
False
44.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
45.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
46.

What is the most reactive nonmetal?

a)

Fluorine

b)

Iodine

c)

Chlorine

d)

Bromine

47.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
48.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
49.
The general trend of metal ion size is that they decrease in size as you move from ______ to ______ on the PT.
a)
Right to left
b)
Left to right
c)
Diagonally
d)
Top to bottom
50.
Noble gases are characterized by...
a)
High reactivity
b)
Being solid at room temperature
c)
Low ionization energy
d)
Full valence shell of electrons
51.

Calculate the average atomic mass of silver.

a)

106.38649amu

b)

111.91896amu

c)

107.8677amu

d)

121

52.

Calculate the average atomic mass of silver.

a)

106.38649amu

b)

111.91896amu

c)

107.8677amu

d)

121

53.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
54.
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.
55.
An isotope has three forms.  30% have a mass of 4 amu, 20% have a mass of 5 amu and 50% have a mass of 3 amu.  Average atomic mass will be closest to
a)
2 amu
b)
3 amu
c)
4 amu
d)
5 amu
56.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
57.
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
58.

Magnesium exists as the three isotopes shown. What is the average atomic mass of magnesium?

a)

20.74 amu

b)

22.56 amu

c)

18.39 amu

d)

24.31

59.

Naturally occurring chlorine that is put in pools is 75.53 percent 35Cl (mass = 34.969 amu) and 24.47 percent 37Cl (mass = 36.966 amu). Calculate the average atomic mass.

a)

35.46 amu

b)

35.00 amu

c)

37.00 amu

d)

17.00 amu

60.
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
61.
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
62.

Isotopes of an element contain an equal number of protons but a different number of ____________________.

a)

neutrons

b)

electrons

c)

atomic numbers

63.

How many protons are in the isotope pictured above?

a)

29

b)

34

c)

63

d)

92

64.

How many neutrons are in the isotope pictured above?

a)

29

b)

34

c)

63

d)

92

65.

The mass number of an isotope is made up of which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, neutrons and electrons

66.

What is the number of protons in phosphorus-31?

a)

15

b)

16

c)

31

d)

46

67.

The atomic number of an element is the total number of which subatomic particle found in the nucleus?

a)

Electron

b)

Neutron

c)

Proton

d)

Neutrons + Protons

68.

An unknown element has two naturally occurring isotopes. One has a mass of 10.01 amu and % abundance of 19.8%. The other has a mass of 10.99 amu and % abundance of 80.2%. Calculate the atomic mass.

a)

1079.6

b)

107.95 amu

c)

21 amu

d)

10.8 amu

69.

Element X has 13 neutrons with a mass number of 28. Element Y has 13 protons. These elements are:

a)

Different elements

b)

Isotopes

70.

Element Q has 56 protons and 18 neutrons.

Element R has 56 protons and 17 neutrons. These elements are:

a)

different elements

b)

isotopes

71.

What is the mass number of an element with 11 protons and 12 neutrons?

a)

1

b)

11

c)

12

d)

23

72.

Which of the following have the same MASS NUMBERS? (You must choose more than one answer)

a)

scandium - 46

b)

sodium - 21

c)

titanium -46

d)

boron - 11

73.

How many electrons are in a neutral atom of magnesium?

a)

10

b)

12

c)

24

d)

24.3

74.

What is the number of protons in neon - 22?

a)

10

b)

12

c)

22

d)

32

75.

Which subatomic particles are found in the nucleus of an atom? Choose all that apply.

a)

protons

b)

neutrons

c)

electrons

d)

alpha

76.

In which of the following is the number of neutrons correctly represented?

a)

chromium - 50 has 24 neutrons

b)

silver - 108 has 60 neutrons

c)

zinc - 67 has 37 neutrons

d)

carbon -14 has 6 neutrons

77.

What atomic particle determines the element?

a)

protons

b)

neutrons

c)

electrons

d)

nucleus

78.

What particle(s) are located in the nucleus?

a)

protons only

b)

neutrons only

c)

electrons only

d)

protons and neutrons

e)

protons and electrons

79.

What particle in the atom has no charge and a mass of 1?

a)

proton

b)

neutrons

c)

electrons

d)

ion

80.

What particle(s) have a charge?

a)

protons only

b)

electrons only

c)

protons and electrons

d)

electrons and neutrons

81.

(challenge) An atom has 10 protons and 10 electrons. What happens to the charge if you add 1 more electron?

a)

It becomes a negative ion

b)

It becomes a positive ion

c)

nothing changes

d)

It becomes a different element

82.

An atom of HELIUM has 2 protons. If you add 1 more proton, what happens?

a)

It becomes an ion

b)

It becomes a different kind of element

c)

Nothing

83.

Challenge: what is the mass of an atom with 2 protons, 2 neutrons, and 2 electrons?

a)

mass = 2

b)

mass = 4

c)

mass = 6

d)

mass = 8

84.

Challenge: What is the charge of an atom with 3 protons and 2 electrons?

a)

0 (neutral)

b)

+1

c)

-1

85.

The atomic number is the same as......

a)

the number of protons

b)

the number of electrons

c)

the number of neutrons

d)

the number of protons plus neutrons

86.

How many neutrons does lithium have?

a)

3

b)

4

c)

6

d)

7

87.

What is the atomic number of silicon?

a)

14

b)

28

c)

42

d)

7

88.

What is the best mass number for silver?

a)

47

b)

107

c)

108

d)

154

89.

How many neutrons does beryllium have?

a)

4

b)

5

c)

9

d)

13

90.

How many electrons does helium have?

a)

2

b)

4

c)

6

d)

8

91.

How do you find the number of neutrons in an atom?

a)

It's the same as the atomic #

b)

It's the same as the mass number

c)

Subtract the atomic # from the mass number

d)

Add the mass number and the atomic #

92.

According to the wave-mechanical model of the atom, electrons in an atom

a)

travel in defined circles

b)

are most likely found in an excited state

c)

have a positive charge

d)

are located in orbitals outside the nucleus

93.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
94.
In the Thomson Model, he discovered the existence of what particle?
a)
Electrons
b)
Protons
c)
Neutrons
d)
Quarks
95.
Which model is this?
a)
Thomson Model
b)
Cloud Model
c)
Bohr Model
d)
Rutherford Model
96.
Which model involved gold foil?
a)
Thomson Model
b)
Rutherford Model
c)
Cloud Model
d)
Bohr Model
97.
While making his model of an atom, what structure did Rutherford discover (containing protons and neutrons)?
a)
the Nucleus
b)
the Electron Cloud
c)
the quarks
d)
the atomic mass
98.
According to the Bohr Model, electrons are only found in specific orbits around the nucleus called __________________________
a)
Energy Levels
b)
Electron Lanes
c)
Electron Places
d)
Atomic Mass
99.
Which model is this?
a)
Thomson Model
b)
Rutherford Model
c)
Cloud Model
d)
Bohr Model
100.
Which model of the atom proposed that atoms were positive spheres with negative electrons in them?
a)
Heliocentric Model
b)
Solid Sphere Model
c)
Plum Pudding Model
d)
Planetary Model
101.

Who was the Greek philosopher who called the smallest particle of matter as "atom"?

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

102.
Which scientist developed the plum pudding/chocolate chip cookie model
a)
Dalton
b)
Thompson 
c)
Rutherford
d)
Democritus
103.
Which scientist saw the atom as a solid sphere?
a)
Dalton
b)
Thomson
c)
Rutherford
d)
Bohr
104.

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

a)

Atom is mostly empty space

b)

The nucleus is positively charged

c)

The atom has a small dense nucleus

d)

All answers are correct

105.

The smallest particle of an element that still represents that element.

a)

Nucleus

b)

electron

c)

proton

d)

atom

106.

What is the center of an atom called?

a)

nucleus

b)

electron cloud

c)

proton center

d)

photon center

107.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

108.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

109.

Who was the Greek philosopher who called the smallest particle of matter an "atom"?

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

110.
Who is the scientist who proposed the "solar system" model of an atom where the electrons orbit around the nucleus?
a)
Democritus
b)
Niels Bohr
c)
Ernest Rutherford
d)
Chadwick
111.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
112.

The majority of an atom's mass exists where?

a)

In the nucleus

b)

In the electron cloud

c)

In the space between the nucleus and the electrons

d)

In the neutrons

113.
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
114.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

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