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REVIEW FOR Physical Science EXAM

Total questions: 127

Worksheet time: 6hrs 21mins

Name
Class
Date
1.
Place the following scientists in order, from earliest to latest: 
Rutherford, Dalton, Bohr, Thomson
a)
Dalton, Rutherford, Bohr, Thomson
b)
Thomson, Dalton, Rutherford, Bohr
c)
Dalton, Thomson, Rutherford, Bohr
d)
Bohr, Dalton, Rutherford, Thomson
2.
How did each model of the atom help to develop the atomic theory? 
a)
Each model provided opinions that were added.
b)
Each model showed different properties of the same structure. 
c)
Each model showed new particles that had been discovered.
d)
Each model built upon the other to show new particles or properties of previously discovered particles. 
3.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
4.

An atom with atomic number 6 would have how many protons

a)

3

b)

12

c)

6

d)

cannot be determined

5.

What two particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

6.

If the mass number of this chlorine atom is 36, how many neutrons does it have?

a)

17

b)

18

c)

19

d)

can't be determined

7.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
8.
What is the mass of an atom if it has 11 protons, 12 neutrons, and 11 electrons?
a)
22
b)
11
c)
34
d)
23
9.
What particle uniquely identifies an element?
a)
Number of Valence Electrons
b)
Number of Protons
c)
Number of Electrons
d)
Atomic Mass
10.

Why is the overall charge of an atom neutral (0)?

a)

They have the same number of protons and neutrons.

b)

They have the same number of protons and electrons.

c)

They have the same number of electrons and neutrons.

11.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

12.

The horizontal (side to side) rows in the Periodic Table are called

a)

groups

b)

families

c)

periods

d)

atomic numbers

13.

What is the name of Group 2?

a)

transition metals

b)

halogens

c)

alkali metals

d)

alkaline earth metals

14.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
15.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
16.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
17.
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
18.
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
19.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
20.
What is an isotope? 
a)
A charged atom
b)
An atom with different amounts of neutrons
c)
An atom with different amounts of protons
d)
A neutral atom
21.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

22.
subatomic particles found on the outermost shell & responsible for the atom's reactivity
a)
neutrons
b)
valence electrons
c)
isotopes
d)
ions
23.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
24.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
25.
The smallest particle of an element that shows all the properties of that element.
a)
Subatomic Particles
b)
Atom
c)
Quarks
d)
Gluons
26.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
27.
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
28.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
29.
Which subatomic particles are found in the nucleus of an atom?
a)
Protons and Electrons
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons, Neutrons and Electrons
30.
Complete the missing label on the diagram.
a)
Neutron
b)
Centre
c)
Nucleus
d)
Sub atomic particle
31.
Which particle is negatively charged?
a)
proton
b)
atom
c)
neutron
d)
electron
32.

Which one of these is true?

a)

Opposite charges repulse each other

b)

Opposite charges attract each other

c)

Same charges attract each other

d)

Same charges neither repulse nor attract each other

33.
In an atom, electrons move in definite orbits around the nucleus.
a)
Thomson
b)
Rutherford
c)
Bohr
d)
Democritus
34.
Place the following scientists in order, from earliest to latest: 
Rutherford, Dalton, Bohr, Thomson
a)
Dalton, Rutherford, Bohr, Thomson
b)
Thomson, Dalton, Rutherford, Bohr
c)
Dalton, Thomson, Rutherford, Bohr
d)
Bohr, Dalton, Rutherford, Thomson
35.
Who discovered the nucleus using the gold foil experiment?
a)
Democritus
b)
Robert Millikan
c)
James Chadwick
d)
Ernest Rutherford
36.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
37.
How did each model of the atom help to develop the atomic theory? 
a)
Each model provided opinions that were added.
b)
Each model showed different properties of the same structure. 
c)
Each model showed new particles that had been discovered.
d)
Each model built upon the other to show new particles or properties of previously discovered particles. 
38.

Which is NOT part of an atom?

a)

protons

b)

neutrons

c)

neurons

d)

electrons

39.

Most of an atom is made up of...

a)

energy

b)

protons

c)

empty space

d)

neutrons

40.

Electrons are located______.

a)

outside the nucleus

b)

inside the nucleus

41.
Place the following scientists in order, from earliest to latest: 
Rutherford, Dalton, Bohr, Thomson
a)
Dalton, Rutherford, Bohr, Thomson
b)
Thomson, Dalton, Rutherford, Bohr
c)
Dalton, Thomson, Rutherford, Bohr
d)
Bohr, Dalton, Rutherford, Thomson
42.
How did each model of the atom help to develop the atomic theory? 
a)
Each model provided opinions that were added.
b)
Each model showed different properties of the same structure. 
c)
Each model showed new particles that had been discovered.
d)
Each model built upon the other to show new particles or properties of previously discovered particles. 
43.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
44.

An atom with atomic number 6 would have how many protons

a)

3

b)

12

c)

6

d)

cannot be determined

45.

What two particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

46.

If the mass number of this chlorine atom is 36, how many neutrons does it have?

a)

17

b)

18

c)

19

d)

can't be determined

47.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
48.
What is the mass of an atom if it has 11 protons, 12 neutrons, and 11 electrons?
a)
22
b)
11
c)
34
d)
23
49.
What particle uniquely identifies an element?
a)
Number of Valence Electrons
b)
Number of Protons
c)
Number of Electrons
d)
Atomic Mass
50.

Why is the overall charge of an atom neutral (0)?

a)

They have the same number of protons and neutrons.

b)

They have the same number of protons and electrons.

c)

They have the same number of electrons and neutrons.

51.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

52.

The horizontal (side to side) rows in the Periodic Table are called

a)

groups

b)

families

c)

periods

d)

atomic numbers

53.

What is the name of Group 2?

a)

transition metals

b)

halogens

c)

alkali metals

d)

alkaline earth metals

54.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
55.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
56.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
57.
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
58.
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
59.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
60.
What is an isotope? 
a)
A charged atom
b)
An atom with different amounts of neutrons
c)
An atom with different amounts of protons
d)
A neutral atom
61.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

62.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
63.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
64.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
65.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
66.
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
67.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
68.

What is one way Neutrons are different from electrons?

a)

they both are negative

b)

neutrons have no charge, while electrons have a negative charge

c)

Both are in the nucleus( center of atom)

d)

Electrons are inside nucleus and neutrons are outside the nucleus.

69.

What is the atomic number?

a)

35

b)

18

c)

17

d)

52

70.

How many protons and electrons does this element have?

a)

35

b)

18

c)

17

d)

52

71.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
72.
Which of the following is a pure substance?
a)
O2
b)
Al2CO5
c)
C6H12O6
d)
SiO2
73.
Which of the following chemical formulas represents a compound? 
a)
C3
b)
O2
c)
CH3CHO
d)
H2
74.
What is water?
a)
element
b)
compound
c)
mixture
75.
What is krypton?
a)
element
b)
compound
c)
mixture
76.
When two or more elements chemically combine
a)
element
b)
compound
c)
mixture
d)
solution
77.
a)
Element
b)
Compound
78.

Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), and Cesium (Cs) are all in the same column (group) on the periodic table. Why are they all grouped together?

a)

They all end with the letters (ium)

b)

They share the same characteristics.

c)

They are in alphabetical order

d)

That is where they just happen to be on the periodic table and are not grouped for any particular reason.

79.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

80.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
81.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
82.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
83.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
84.
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
85.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
86.

What is one way Neutrons are different from electrons?

a)

they both are negative

b)

neutrons have no charge, while electrons have a negative charge

c)

Both are in the nucleus( center of atom)

d)

Electrons are inside nucleus and neutrons are outside the nucleus.

87.

What is the atomic number?

a)

35

b)

18

c)

17

d)

52

88.

How many protons and electrons does this element have?

a)

35

b)

18

c)

17

d)

52

89.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
90.
Which of the following is a pure substance?
a)
O2
b)
Al2CO5
c)
C6H12O6
d)
SiO2
91.
Which of the following chemical formulas represents a compound? 
a)
C3
b)
O2
c)
CH3CHO
d)
H2
92.
What is water?
a)
element
b)
compound
c)
mixture
93.
What is krypton?
a)
element
b)
compound
c)
mixture
94.
When two or more elements chemically combine
a)
element
b)
compound
c)
mixture
d)
solution
95.
a)
Element
b)
Compound
96.

Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), and Cesium (Cs) are all in the same column (group) on the periodic table. Why are they all grouped together?

a)

They all end with the letters (ium)

b)

They share the same characteristics.

c)

They are in alphabetical order

d)

That is where they just happen to be on the periodic table and are not grouped for any particular reason.

97.
What is the atomic number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
98.
What is the mass number defined as?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
99.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
100.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

101.

What is the atomic number of Barium, Ba? (enlarge the periodic table)

a)

20

b)

38

c)

56

d)

88

102.

What is the atomic number of Nickel? (enlarge the periodic table)

a)

110

b)

28

c)

46

d)

78

103.

How many protons are in a sodium atom, Na? (tap to enlarge the periodic table)

a)

Sodium has 1 proton.

b)

Sodium has 3 protons.

c)

Sodium has 11 protons

104.

An element has the mass number 12 and atomic number 6. The number of neutrons in it is:

a)

6

b)

10

c)

4

d)

8

105.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

106.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

107.

How many neutrons does C-14 [atomic #6] contain? (tap to enlarge the image)

a)

6

b)

7

c)

14

d)

8

108.

How many neutrons does an atom of the isotope Neon-22 have? (tap to enlarge the image)

a)

12

b)

10

c)

22

d)

20

109.

How many neutrons does an atom of Nitrogen-13 have? (tap to enlarge the image)

a)

6

b)

7

c)

13

d)

5

110.

If an atom has 10 electrons, how many protons does it have?

a)

0

b)

1

c)

10

d)

5

111.

How many electrons are in an atom with an atomic number of 50?

a)

5

b)

8

c)

50

d)

2

112.
Oxygen has 8 protons. What is oxygen's atomic number?
a)
16
b)
8
c)
15.999
d)
0
113.
A neutral atom of Carbon-13 has ________ electrons and _________ neutrons
a)
13, 13
b)
6, 7
c)
7, 7
d)
6, 6
114.
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
115.
The  mass of an atom is located  in the ___________ and the volume of an atom is made of the ____________
a)
electron cloud, nucleus
b)
electron cloud, energy levels
c)
nucleus, electron cloud
d)
nucleus, neutrons
116.
A neutral atom of the isotope 2612Mg would consist of
a)
12 protons, 26 neutrons, 26 electrons
b)
26 protons, 12 neutrons, 26 electrons
c)
26 protons, 14 neutrons, 14 electrons
d)
12 protons, 14 neutrons, 12 electrons
117.

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

a)

6

b)

8

c)

10

d)

14

118.

How many protons does this isotope of titanium have?

a)

22

b)

26

c)

48

d)

70

119.
Two atoms of different elements will definitely have different numbers_____
a)
Nuclei
b)
Protons
c)
Neutrons
d)
Electrons
120.
An ion forms when an atom gains or loses
a)
Protons
b)
Neutrons
c)
Electrons
121.
A neutral atom would become an ion that has a charge of 2+ by 
a)
Losing two protons
b)
Losing two neutrons
c)
Losing two electrons
122.
Isotopes are atoms that have different
a)
Mass numbers
b)
Element names
c)
Atomic Numbers
123.
A positively charged ion is formed when
a)
A neutron is lost
b)
An electron is lost
c)
A neutron is gained
d)
An electron is gained
124.
If neutral copper atom (atomic number 29) becomes an ion that has a charge of 2+, how many electrons does the resulting ion have?
a)
27
b)
28
c)
29
d)
31
125.
Two neutral atoms that have the same atomic number and different mass numbers are
a)
Ions
b)
Isotopes
c)
Alpha particles
d)
Different elements
126.
An ion that has a negative charge is formed when an atom 
a)
Loses neutrons
b)
Loses electrons
c)
Gains neutrons
d)
Gains electrons
127.
What information would allow you to determine whether two atoms are of the same or different elements
a)
The charge on each atom
b)
The number of neutrons each has
c)
The number of protons in their nuclei
d)
The location of the electrons in their electron clouds

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