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Unit 1 Atomic Theory Review

Total questions: 102

Worksheet time: 3hrs 45mins

Name
Class
Date
1.

Proposed that electrons move around the nucleus in specific paths a fixed distance from the nucleus..

a)

Bohr

b)

Rutherford

c)

Chadwick

d)

Thomson

2.

This picture best represents ___________________ atomic model.

a)

Thomson's

b)

Dalton's

c)

Bohr's

d)

Chadwick's

3.

In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.

a)

Atoms

b)

Parts

c)

Molecules

d)

Hydrogen

4.

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

5.

Used the word "atomos" to decsribe the uncuttable (indivisible) atom.

a)

Democritus

b)

Thomson

c)

Bohr

d)

Dalton

6.

Which one of these is Dalton's Model?

a)
b)
c)
d)
7.

Which model was created after the discovery of the nucleus?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical

d)

Plum Pudding

8.

Which model was created after the discovery of the electron cloud?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical

d)

Plum Pudding

9.

Who discovered electrons?

a)

Rutherford

b)

Bohr

c)

J.J. Thompson

d)

Democritus

10.

Ernest Rutherford discovered that the atom was mostly _________________ and has a _______________ charged nucleus.

a)

empty space, positively

b)

empty space, negatively

c)

full of protons, positively

d)

full of neutrons, negatively

11.

Which subatomic particle was discovered as a result of the cathode ray experiment?

a)

proton

b)

neutron

c)

electron

d)

nucleus

12.

Who performed the Gold Foil Experiment?

a)

J. J. Thomson

b)

Ernest Rutherford

c)

Neils Bohr

d)

John Dalton

13.

Which model was proposed by Neils Bohr?

a)

Planetary Model

b)

Plum Pudding Model

c)

Quantum Mechanical Model

d)

Solid Ball Model

14.

Which subatomic particle was discovered by James Chadwick?

a)

proton

b)

neutron

c)

electron

d)

quark

15.

Who was the first contributor to the atomic theory?

a)

John Dalton

b)

Ernest Rutherford

c)

JJ Thompson

d)

Democritus

e)

Neils Bohr

16.

Who proposed that electrons move around the nucleus in circular orbits?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

17.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

18.

Subatomic particles with a positive charge

a)

neutrons

b)

atomic mass

c)

protons

d)

isotopes

19.

Value representing the number of protons in an element

a)

Atomic Mass

b)

Mass Number

c)

Valence Electrons

d)

Atomic Number

20.

Subatomic particles that are neutral in charge

a)

Neutrons

b)

Protons

c)

Nucleus 

d)

Electrons

21.

Which two subatomic particles make up the nucleus of an atom?

a)

Protons and Electrons

b)

Neutrons and Electrons

c)

Electrons and Protons

d)

Protons and Neutrons

22.

Where are the Electrons found in the structure of an atom?

a)

In the nucleus

b)

In spaces around the nucleus

23.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

24.

In order for an atom to be neutral what has to be true?

a)

The atom has more protons than neutrons

b)

The atom has more neutrons than protons

c)

The atom has the same number of protons and neutrons

d)

The atom has the same number of protons and electrons

25.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

26.

How is the number of neutrons in the nucleus of an atom calculated?

a)

Add the number of e- and p+ together

b)

Subtract the number of e- from p+

c)

Subtract the number of p+ from the mass number

d)

Add the mass number to the number of e-

27.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

28.

The atomic number of an element that has 9 protons, 9 electrons, and 10 neutrons is _____.

a)

9

b)

10

c)

19

d)

28

29.

An element with a mass number of 11 and an atomic number of 5 has how many neutrons?

a)

11

b)

5

c)

6

d)

16

30.

Where is most of the mass in an atom located?

a)

in the nucleus

b)

in the protons

c)

in the neutrons

d)

in the electrons

31.

How many protons does indium have?

a)

49

b)

66

c)

114

d)

115

32.

Helium (He) contains (a)   neutrons.

33.

How many protons does helium (He) have?

a)

4

b)

2

c)

0

d)

1

34.

The mass number of helium (He) is (a)   ?

35.

Different isotopes of an element contain different numbers of ___.

a)

protons

b)

neutrons

c)

electrons

d)

elements

36.

If a proton is added or removed from an atom, what happens?

a)

It becomes a different element.

b)

It becomes a different isotope.

c)

Nothing happens.

37.

How many neutrons are in 1 atom of Carbon-13?

a)

6

b)

13

c)

7

d)

20

38.

How many protons are in an atom of Nitrogen-16?

a)

7

b)

9

c)

16

39.

What is the difference between Neon-20 and Neon-22?

a)

They have different numbers of electrons.

b)

They have different numbers of neutrons.

c)

Only 1 is radioactive.

d)

No difference.

40.

Which atom of these isotopes has 3 protons? The symbol for lithium is Li.

a)

Lithium-6

b)

Lithium-7

c)

All of them.

d)

Lithium-9

41.

How many neutrons are in this isotope?

a)

20

b)

41

c)

61

d)

21

42.

Which is the correct symbol for Fluorine-18?

a)
b)
c)
d)
43.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

44.

Bromine-80 has how many neutrons?

a)

41

b)

42

c)

44

d)

45

45.

How do you calculate mass number?

a)

Mass x percent

b)

Protons + Electrons

c)

Protons + Neutrons

d)

Neutrons + Protons + Electrons

46.

How many protons are in the isotope pictured above?

a)

29

b)

34

c)

63

d)

92

47.

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

a)

protons

b)

neutrons

c)

electrons

d)

alpha

48.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

49.

How many protons, neutrons, and electrons?

a)

proton = 16, neutron = 8, electron = 10

b)

proton = 8, neutron = 16, electron = 8

c)

proton = 8, neutron = 8, electron = 10

d)

proton = 6, neutron = 2, electron = 6

50.

IN AN ION THE NUMBER OF PROTONS CAN BE _________ THE NUMBER OF ELECTRONS. 

a)

greater than

b)

less than

c)

equal to

d)

unequal to

51.

IN A POSITIVE ION, THE # OF ELECTRONS _____ # PROTONS

a)

Less than

b)

Greater than

c)

Equal to

52.

IN A NEGATIVE ION, THE # OF ELECTRONS _____ # PROTONS 

a)

greater than

b)

less than

c)

equal to

53.

How many ELECTRONS does copper have if it has the following charge: Cu2+ ?

a)

64

b)

35

c)

27

d)

29

54.

If an atom has 9 protons 10 electrons and 10 Neutrons. What is the Charge of the Atom?

(a)  

55.

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

56.

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.

57.
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
58.
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
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.
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
61.
What is the name of the atom pictured here?
a)
Nitrogen
b)
Nitrogen-15
c)
Nitrogen-7
d)
Nitrogen-8
62.
Which of the following could have 82 neutrons?
a)
W-182
b)
Ta-181
c)
Cs-132
d)
Ba-138
63.

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

64.

What element do you think the average atomic mass in the data table represents?

a)

Beryllium

b)

Carbon

c)

Boron

d)

Nitrogen

65.

The average atomic mass for this element is going to be closest to what number?

a)

84

b)

85

c)

86

d)

87

66.

What element has the following mass spec data?

a)

Thulium

b)

Copper

c)

Europium

d)

Zinc

67.

What element do you think is represented by the graph?

a)

Hydrogen

b)

Helium

c)

Lithium

d)

Beryllium

68.

What do you think the average mass of this element will be closest to?

a)

107

b)

106

c)

109

d)

110

69.

What element do you think is represented by the information of the graph?

a)

Palladium

b)

Silver

c)

Cadmium

70.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

71.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
72.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
73.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

74.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

75.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

76.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

77.
What gases are in the unknown mixture?
a)
Gas B & Gas D
b)
Gas C & Gas B
c)
Gas A & Gas D
d)
Gas D & Gas C
78.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
79.

What is the vertical (up and down) column on the periodic table of the element?

a)

group or family

b)

period

c)

atomic orbital

d)

energy level

80.

What is an electron in the outermost energy level of an atom's electron cloud?

a)

atomic orbital

b)

electron cloud

c)

energy level

d)

valence electron

81.

What is a horizontal (left and right) row on the periodic table of the element?

a)

period

b)

group or family

c)

oxidation state

d)

staircase line

82.

On the periodic table of the elements, the period of an element tells what about that element?

a)

group or family

b)

vertical column

c)

number of valence electrons

d)

number of energy levels

83.

On the periodic table of the elements, what does the group tell about an element?

a)

horizontal row

b)

period

c)

number of energy levels

d)

number of valence electrons

84.

What is the atomic number of an element?

a)

The number of protons in the nucleus

b)

The number of neutrons in the nucleus

c)

The total number of protons and neutrons in the nucleus

d)

The total number of protons and electrons in an atom

85.

In the periodic table, elements are arranged in order of increasing:

a)

Atomic mass

b)

Atomic number

c)

Number of neutrons

d)

Electronegativity

86.

What is the term for the number of protons plus neutrons in an atom?

a)

Atomic number

b)

Atomic mass

c)

Isotope number

d)

Valency

87.

Protons + __________ = atomic mass

a)

electrons

b)

neutrons

c)

neither

88.

What is the nuclear symbol for the atom shown in the image?

a)

4Be

b)

4He

c)

2He

d)

2Be

89.

In nuclear fusion, what happens to the energy when smaller nuclei combine to form a larger nucleus?

a)

Energy is absorbed

b)

Energy remains constant

c)

Energy is released

90.

What is the primary process that powers the sun?

a)

Nuclear fusion – combining lighter atoms to form heavier ones – powers the sun.

b)

Nuclear fission – splitting heavier atoms to form lighter ones – powers the sun.

c)

Nuclear fusion – splitting lighter atoms to form heavier ones – powers the sun.

d)

Nuclear fission – combining heavier atoms to form lighter ones – powers the sun.

91.

All elements heavier than hydrogen were formed through what process?

a)

Nuclear Fission

b)

Nuclear Fusion

c)

Nuclear Division

d)

Nuclear Decay

92.

What is the charge of an electron?

a)

Negative

b)

Neutral

c)

Variable

d)

Positive

93.

Which scientist is known for the discovery of the electron?

a)

Ernest Rutherford

b)

Niels Bohr

c)

James Chadwick

d)

JJ Thomson

94.

What is the primary component of the atomic nucleus?

a)

Electrons

b)

Neutrons and Electrons

c)

Protons and Electrons

d)

Protons and Neutrons

95.

An ion with 2 protons, 3 neutrons, and 4 electrons has a charge of _

a)

+2

b)

-2

c)

+3

d)

9

e)

-4

96.

How many protons, neutrons, and electrons?

a)

proton = 6, neutron = 4, electron = 3

b)

proton = 4, neutron = 4, electron = 5

c)

proton = 4, neutron = 6, electron = 1

d)

proton = 4, neutron = 2, electron = 3

e)

proton = 4, neutron = 2, electron = 5

97.

If X is the symbol for an element, which of the following two symbols represent isotopes of the same element?  

  I. 7735X 

II. 7733X 

III. 8137X 

IV. 8135 X

a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
98.
What is the name of the pictured isotope?
a)
Carbon-12
b)
Carbon-13
c)

Carbon-7

d)

Carbon-19

e)

Carbon-6

99.
What is the name of the pictured isotope?
a)

Chlorine-52

b)
Chlorine-17
c)
Chlorine-35
d)
Chlorine-18
100.

This isotope of Titanium has:

​ (a)   protons

22 electrons

​ (b)   neutrons

mass number of ​ (c)  

Choose from the below words
22
26
48
70
47
21
101.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
102.
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

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