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Atomic structure, Isotopes, Average Atomic mass, Nuclear

Total questions: 128

Worksheet time: 5hrs 32mins

Name
Class
Date
1.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
2.
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
3.
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.
4.

Who came up with this model of an atom?

a)

J.J. Thompson

b)

Ernest Rutherford

c)

Neils Bohr

d)

James Chadwick

5.
Which of the following is proposed by Erwin Schrodinger?
a)
Planetary model of the atom
b)
Plum pudding model of the atom
c)
Saturnian model of the atom
d)
Electron cloud model of the atom
6.
Discoverer of the neutron?
a)
Jimmy
b)
Chadwick
c)
Charleston
d)
Rutherford
7.
Earth, Air, Fire, and Water were the fundamental elements propose by ___.
a)
Aristotle
b)
Democritus
c)
Plato
d)
Galileo
8.
The atom is mostly empty space is a confirmed idea made by who?
a)
Rutherford
b)
Nagaoka
c)
Bohr
d)
Chadwick
9.
Ernst Rutherford discovered which part of the atom through the use of gold foil?
a)
Proton
b)
Neutron
c)
Electron
d)
Orbitals
10.

Which is the correct sequence of the scientists who made major changes in the model of the atom?

1-JJ Thomson

2-Erwin Schrodinger

3-John Dalton

4-Niels Bohr

5-Ernest Rutherford

a)

2, 1, 4, 3, 5

b)

3, 1, 5, 4, 2

c)

5, 3, 2, 1, 4

d)

4, 3, 2, 1, 5

11.

Which scientist saw the atom as a positively charged sphere with negative particles (electrons) embedded within?

a)

J.J. Thomson

b)

Niels Bohr

c)

John Dalton

d)

Ernest Rutherford

12.

Which scientist proposed a model of the atom in which the electrons are orbiting at different levels?

a)

Niels Bohr

b)

James Chadwick

c)

John Dalton

d)

Ernest Rutherford

13.

Which scientist discovered that most of an atom's mass is contained in its nucleus and the rest is nearly empty space?

a)

Rutherford

b)

Dalton

c)

Bohr

d)

Thomson

14.

Order the atomic models below from the oldest to the mot recent.

a)

2, 1, 3, and 4

b)

1, 2, 4, and 3

c)

3, 2, 4, and 1

d)

3, 1, 2, and 4

15.

Which scientist proposed a model of the atom in which the individual atoms were thought of as tiny solids like balls or marbles?

a)

John Dalton

b)

James Chadwick

c)

Ernest Rutherford

d)

J.J. Thomson

16.

Whose model of an atom is displayed in the picture?

a)

Thomson

b)

Rutherford

c)

Dalton

d)

Bohr

17.

Whose model of an atom is displayed in the picture?

a)

Rutherford

b)

Dalton

c)

Thomson

d)

Bohr

18.

Current model

a)

Bohr Model

b)

Quantum Mechanical Model

c)

Plum Pudding Model

d)

Planetary

19.

Discovered electron

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Chadwick

20.
He unknowingly discovered the electron as a result of cathode ray tube experiments.    
a)
Thomson
b)
Chadwick
c)
Democritus
d)
Aristotle
21.
He believed that all matter was continuous and that four basic elements existed (earth, wind, fire, water).
a)
Democritus
b)
Aristotle
c)
Chadwick
d)
Thomson
22.

Discovered mass of proton = mass of neutron

a)

Bohr

b)

Chadwick

c)

Rutherford

d)

Schrodinger

23.

This model this model was the first to show a nucleus, consisting of protons and neutron. Electrons surround the nucleus but are not shown in distinct energy levels.

a)

The "Rutherford Model" of the atom

b)

The "Plum Pudding Model" of the atom

c)

The "Quantum Mechanical Model" of the atom

24.

This model was developed after J.J. Thompson discovered electrons, a particle smaller than an atom. It shows electrons floating freely in a positive region.

a)

The "Plum Pudding Model" of the atom

b)

The "Rutherford Model" of the atom

c)

Democritus's model of the atom

d)

The "Quantum Mechanical Model" of the atom

25.
Ernest Rutherford discovered that atoms were mostly _________________. 
a)
negatively charged
b)
positively charged
c)
electrons
d)
empty space. 
26.
In the gold foil experiment, most of the positively charged alpha particles passed through the gold foil, but some were deflected or bounced back.  What did we conclude because of this?  
a)
Atoms are small indivisible spheres
b)
Atoms are mostly empty space with a small, dense, positive center
c)
Atoms have negatively charged particles which orbit the nucleus
d)
Light is a wave, not a particle
27.

What was the purpose of Rutherford's Gold Foil Experiment?

a)

To study the behavior of electrons in a magnetic field.

b)

To investigate the structure of the atom and determine the distribution of positive charge within it.

c)

To investigate the properties of different types of metals.

d)

To measure the speed of light in a vacuum.

28.

What did Rutherford expect to happen to the alpha particles as they passed through the gold foil?

a)

All alpha particles would pass straight through the gold foil.

b)

The alpha particles would be absorbed by the gold foil.

c)

The alpha particles would change color as they passed through the gold foil.

d)

Some alpha particles would be deflected or bounce back

29.

What did Rutherford observe during the Gold Foil Experiment?

a)

Deflection of alpha particles at large angles

b)

Scattering of alpha particles in all directions.

c)

No deflection of alpha particles.

d)

Absorption of alpha particles by the gold foil.

30.

What conclusion did Rutherford draw from his observations?

a)

The atom has a small, dense, positively charged nucleus at its center, with electrons orbiting around it.

b)

The atom has a small, dense, positively charged nucleus at its center, with protons orbiting around it.

c)

The atom has a large, dense, positively charged nucleus at its center, with electrons orbiting around it.

d)

The atom has a small, dense, negatively charged nucleus at its center, with electrons orbiting around it.

31.
A neutral atom of Carbon-13 has ________ electrons and _________ neutrons
a)
13, 13
b)
6, 7
c)
7, 7
d)
6, 6
32.
What is true about a neutral atom?
a)
The number of protons equal the number of neutrons
b)
The number of protons equal the number of electrons
c)
The number of neutrons equal the number of electrons
d)
The number of protons, neutrons, and electrons are all different
33.
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
34.
Oxygen has 8 protons. What is oxygen's atomic number?
a)
16
b)
8
c)
15.999
d)
0
35.
Isotopes are atoms of the same element that have the same number of __________ but different number of __________ . Therefore, isotopes of the same element have different masses. 
a)
protons, neutrons
b)
protons, electrons
c)
neutrons, protons
d)
electrons, protons
36.
Nitrogen has three occurring isotopes: Nitrogen-13, Nitrogen-14, Nitrogen-15. Which isotope is the most abundant?
a)
Nitrogen-13
b)
Nitrogen-14
c)
Nitrogen-15
d)
Based on the information given, it cannot be determined
37.
The number in the upper corner of an element tile (7 for nitrogen) is called _____
a)
the proton number
b)
the atomic number
c)
the electron number
d)
the mass number
38.
For a given element, the atomic number indicates the number of _____
a)
protons in the nucleus
b)
neutron in the nucleus
c)
electrons in the atom
d)
nucleons in the atom
39.
If an atom contains exactly three protons, then it's an atom of _____
a)
lithium
b)
gold
c)
nitrogen
d)
carbon
40.
The sum of the number of protons and the number of neutrons is called the _____
a)
atomic number
b)
mass number
c)
isotope number
d)
average weight
41.
The nucleus contains _____
a)
only protons
b)
protons and neutrons
c)
protons and electrons
d)
electrons and neutrons
42.
Which subatomic particle has a positive charge?
a)
Proton
b)
Neutron
c)
Electron
43.
Which subatomic particle has a negative charge?
a)
Proton
b)
Neutron
c)
Electron
44.

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

45.
The mass number of an element that has 18 protons, 18 electrons, and 19 neutrons is _____.
a)
12.5
b)
13
c)
25
d)
37
46.
Which statement is true about oxygen-17 and oxygen-18?
a)
They do not have the same number of protons.
b)
Their atoms have an identical mass.
c)
They are isotopes of oxygen.
d)
The have the same mass number.
47.
What is the charge of an atom that has lost one electron?
a)
1-
b)
2-
c)
1+
d)
2+
48.
What is the charge of an atom that has gained one electron?
a)
1-
b)
2-
c)
1+
d)
2+
49.

What were J. J. Thomson's three contributions to the atomic theory?

a)

Discovered the electron

b)

Discovered the nucleus -did the gold foil experiment

c)

Used the cathode ray tube in his discovery

d)

Created a model of the atom with electrons moving around the nucleus in fixed orbits

e)

Created the "plum pudding" model of the atom

50.

What are two facts about Democritus's?

a)

Greek philosopher

b)

Created the atomic theory

c)

Used the cathode ray tube in his discovery

d)

Believed that the universe was made of tiny "uncuttable" particles

e)

Discovered that the atom is mostly empty space

51.

What is Neils Bohr's contribution to the atomic theory?

a)

Created the atomic theory

b)

Created a model of the atom with electrons moving around the nucleus in a fixed orbits

c)

Discovered that the proton had a positive charge

d)

Believed that atoms of a given element are identical

e)

Discovered the electron

52.

What were Ernest Rutherford's three contributions to atomic theory?

a)

Discovered that the atom is mostly empty space

b)

Discovered the nucleus- did the gold foil experiment

c)

Used the cathode ray tube in his discovery

d)

Discovered the electron

e)

Discovered that the proton had a positive charge

53.
An atom has an atomic number of 15 and a mass number of 31. How many protons are there in the atom?
a)
15
b)
31
c)
16
d)
47
54.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
55.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

56.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
57.

An atom has 12 protons and 13 neutrons in its nucleus. Which is the correct symbol?

a)
b)
c)
d)
58.

Cobalt has an atomic mass of 59 and an atomic number of 27. What does this information reveal about most cobalt atoms?

a)

They contain more neutrons than protons

b)

They naturally have a net negative charge

c)

They attract protons more strongly than electrons

d)

They form ions with a chrage of +27 in compounds

59.
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
60.
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.
How many protons does this element have?
a)
32
b)
33
c)
34
d)
no way to know
61.
An element has three different isotopes. One has a mass of 35.00 amu; another has a mass of 36.00  amu; and another has a mass of 38.00  amu. What is the average atomic mass of this element?
a)
36.33 amu
b)
37.00 amu
c)
12.11 amu
d)
impossible to tell
62.
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
63.
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
64.
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.
65.
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
66.
What is Half-life?
a)
The amount of time it takes for some of the nuclei in a sample of the isotope to decay
b)
The amount of time it takes for half the electrons in a sample of the isotope to decay
c)
The amount of time it takes for half the nuclei in a sample of the isotope to decay
d)
the amount of time it takes to double the nuclei in a sample of the isotope to decay
67.
The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after 7.2 minutes has elapsed?
a)
100.0g
b)
50.0g
c)
12.5g
d)
8.5g
68.
After the third half-life, how much of the sample is left?
a)
1/2
b)
1/3
c)
1/16
d)
1/8
69.

Describe the structure of an alpha particle.

a)

a fast-moving electron

b)

2 protons and 2 neutrons

c)

a slow-moving neutron

d)

a hydrogen nucleus

70.

The mass number of Neptunium (Np) is (a)   .

71.

The atomic number of Neptunium (Np) is (a)   .

72.

The atomic number of Actinium (Ac) is (a)   .

73.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
74.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
75.

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

a)

proton and electron

b)

neutron and electron

c)

neutron and proton

76.
Barium-122 has a half-life of 2 minutes. A fresh sample weighing 80 g was obtained. If it takes 10 minutes to set up an experiment using barium-122, how much barium-122 will be left when the experiment begins?
a)
0.25g
b)
2.5g
c)
25g
d)
80g
77.
What percent of carbon-14 would be left after 5730 years?
a)
100%
b)
75%
c)
50%
d)
25%
78.
What is the half-life of iodine-131?
a)
32 days
b)
8 days
c)
16 days
d)
24 days
79.

What type of decay is shown here

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

a)

alpha

b)

beta

c)

gamma

80.

Finish this equation

20983Bi--> _______ + 20581Tl

a)

42He

b)

0-1e

c)

y

81.

Identify the type of nuclear decay shown here

21483Bi → 0-1e + 21484Po

a)

alpha

b)

beta

c)

gamma

82.
The process of nuclear change in an atom of radioactive material is called... 
a)
nuclear decay
b)
nuclear mass
c)
isotopes
d)
radon
83.
Has the symbol
a)
Alpha
b)
Beta
c)
Gamma
84.
Has the symbol
a)
Alpha
b)
Beta
c)
Gamma
85.
Has the symbol
a)
Alpha
b)
Beta 
c)
Gamma
86.

How is the alpha particle written in a nuclear equation?

a)

42He

b)

24He

c)

0-1e

d)

00γ

87.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
88.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
89.
Has the lowest penetrating power.  Can only penetrate 0.05 mm into the body and can be stopped by a piece of paper or clothing.
a)
Alpha
b)
Beta
c)
Gamma
90.
Has the highest penetrating power.  Can penetrate our body.  Even several cm thick of lead or several meters thick of concrete cannot stop all of it.
a)
Alpha
b)
Beta
c)
Gamma
91.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
92.

In a correctly written symbol what would be located in the "Z" position?

a)

number of neutrons

b)

atomic number

c)

number of electrons

d)

mass number

93.

22087Fr —› ____ + 42He

a)

22089Ac

b)

22490Th

c)

21685At

d)

21688Ra

94.
How many protons are in this atom?
a)
3
b)
4
c)
6
d)
10
95.

The diagram shows 32 atoms.

16 of the Red are parent isotopes

16 of the Green are daughter isotopes

How many half-lives have occurred?

a)

0

b)

1

c)

2

d)

3

96.

The % of the parent isotope remaining after 1 Half Life.

a)

50%

b)

25%

c)

12.5%

d)

6.25%

97.

A radioactive nuclide has a ____ stable nucleus than a non-radioactive nucleus of the same element.

a)

more

b)

less

c)

identical

d)

small

98.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
99.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
half-life
d)
gamma radiation
100.
How is nuclear fusion different from nuclear fission?
a)
In fusion, the product is a larger atomic nucleus.
b)
Fission produces energy but fusion does not.
c)
Fusion produces energy but fission does not.
d)
In fission, the product is a larger atomic nucleus.
101.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
102.
This is an example of ---
a)
Radioactive Decay
b)
Nuclear Fission
c)
Nuclear Fusion
d)
Fossil fuel reaction
103.
Which type of nuclear radiation is being emitted here?
a)
alpha
b)
beta
c)
gamma
d)
none
104.

A radioactive nucleus has a ____ stable nucleus than a non-radioactive nucleus of the same element.

a)

more

b)

less

c)

identical

d)

small

105.
Takes two small nuclei and combines them into a larger nucleus
a)
fission
b)
fusion
106.
How is nuclear fusion different from nuclear fission?
a)
In fusion, the product is a larger atomic nucleus.
b)
Fission produces energy but fusion does not.
c)
Fusion produces energy but fission does not.
d)
In fission, the product is a larger atomic nucleus.
107.

Which of these diagrams represents the type of nuclear reaction that produces energy in the Sun?

a)

A

b)

B

c)

C

d)

D

108.
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.
109.

The three types of nuclear radiation are _______ radiation, _________radiation, and _____________ radiation.

a)

alpha, beta, and gamma

b)

theta, beta, and kappa

c)

alpha, beta, positron

110.

After one ____________ of a radioactive element, half of the original radioactive material remains.

a)

half-life

b)

cycle

c)

decay

111.

The conversion of an atom of one element to an atom of another element is called (a)   .

112.

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

113.

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

a)

nuclear fission

b)

nuclear fusion

114.

emitted helium nucleus

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

115.

energetic electron from decomposed neutron

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

116.

high-energy photons emitted by a radioisotope

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

117.

particle of charge +1 and mass equal to that of an electron

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

118.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
119.
What is the name of the atom pictured here?
a)
Nitrogen
b)
Nitrogen-15
c)
Nitrogen-7
d)
Nitrogen-8
120.
Atom 1 has Mass=12  Protons=6
Atom 2 has Mass= 14 Electrons=6
Are these atoms isotopes of each other or different elements?
a)
Different Elements - Mg & Si
b)
Different Elements - Ar & Ca
c)
Isotopes of Carbon
d)
Isotopes of Magnesium
121.

Which of the following is necessary to calculate the atomic mass of an element?

a)

the atomic mass of carbon-12

b)

the atomic number of the element

c)

the relative masses of the element's protons and neutrons

d)

the masses of each isotope of the element

122.

The atomic mass of an element depends upon the ___.

a)

relative abundance of protons in that element

b)

mass and relative abundance of each isotope of that element

c)

mass of each isotope of that element

d)

mass of each electron in that element

123.

Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37, The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant?

a)

Cl-35

b)

Cl-37

c)

Cannot be determined from the information provided.

124.

In the adjoining figure, the circles with the + sign represent protons and the empty circles represent neutrons. Determine which atoms in the figure are isotopes of each other.

a)

1 and 2

b)

1 and 3

c)

2 and 3

d)

1, 2, and 3

125.

Vitellium (Vi) has the following composition:

Vi–188: 187.9122 amu; 10.861%

Vi–191: 190.9047 amu; 12.428%

Vi–193: 192.8938 amu; 76.711%

Based on this data, what can you predict about the average atomic mass of vitellium?

a)

It will be equal to the arithmetic mean of the masses of the three isotopes.

b)

It will be closer to the mass of Vi–188.

c)

It will be closer to the mass of Vi–193.

d)

It will be equal to the mass of Vi–193.

126.

The average atomic mass of oxygen is 15.9994 amu. The atomic masses of its three isotopes are as follows:

O-16: 15.995 amu; O-17: 16.999 amu; O-18: 17.999 amu

Which isotope is most likely to have the greatest abundance in nature?

a)

O–16

b)

O–17

c)

O-18

d)

all three isotopes may be equally abundant

127.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
128.
If the half-life of uranium-232 is 70 years, how many half-lives will it take for 10 g of it to be reduced to 1.25 g?
a)
1 half-life
b)
2 half-lives
c)
3 half-lives
d)
4 half-lives

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