wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Physical Science Unit 3 Review (HONORS)

Total questions: 95

Worksheet time: 5hrs 28mins

Name
Class
Date
1.

Which scientist is given credit for discovering the electron?

a)

Bohr

b)

Dalton

c)

Thomson

d)

Rutherford

2.

Who discovered that electrons travel in specific orbitals or energy levels around the nucleus?

a)

Bohr

b)

Schrodinger

c)

Democritus

d)

Rutherford

3.

Whose model of the atom is known as the "plum pudding " model?

a)

Rutherford

b)

Schrodinger

c)

Dalton

d)

Thomson

4.

Whose gold foil experiment led to his conclusion that the nucleus of an atom contained protons?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

5.

Who developed the idea that electrons are found in a cloud?

a)

Bohr

b)

Dalton

c)

Schrodinger

d)

Rutherford

6.

Whose model of the atom is represented in the image?

a)

Thomson

b)

Bohr

c)

Dalton

d)

Rutherford

7.

Whose model is the most modern interpretation of an atom?

a)

Dalton

b)

Democritus

c)

Rutherford

d)

Schrodinger

8.

What is the center of an atom called?

a)

nucleus

b)

neutron

c)

proton

d)

photon center

9.

What is the neutral particle found in the nucleus called?

a)

proton

b)

neutron

c)

electron

d)

quark

10.

What is a particle with one positive charge called?

a)

proton

b)

electron

c)

neutron

d)

quark

11.

Before Thomson published his discoveries, the smallest particle of an element was thought to be a/an

a)

Nucleus

b)

electron

c)

proton

d)

atom

12.

What is a particle with one negative charge called?

a)

electron

b)

proton

c)

quark

d)

neutron

13.

Which scientist discovered that the nucleus contained neutrons?

a)

bohr

b)

Rutherford

c)

Dalton

d)

Chadwick

14.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

15.

Rutherford and his students did experiments that showed

a)

quark

b)

nucleus

c)

proton

d)

electron

16.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

17.

Which one of the following discoveries came first?

a)

electrons

b)

neutrons

c)

quarks

d)

atoms

18.

Which one of the following is the correct order of scientific contribution of the atom?

a)

Chadwick, Dalton, Bohr, Rutherford, Democritus,Thomson

b)

Thomson, Democritus,Rutherford, Bohr, Dalton ,Chadwick

c)

Dalton, Chadwick ,Bohr, Rutherford, Democritus,Thomson

d)

Democritus, Dalton, Thomson, Rutherford, Bohr, Chadwick

19.

Which one of the following parts of the atom is the smallest?

a)

proton

b)

electron cloud

c)

nucleus

20.

This picture best represents ___________________ atomic model.

a)

Thomson's

b)

Dalton's

c)

Bohr's

d)

Chadwick's

21.

Who was the first person to come up with the Atomic Theory which included four parts.

a)

John Dalton

b)

Democritus

c)

Ernest Rutherford

d)

Niels Bohr

22.
Who developed the Quantum Mechanical Model?
a)
Erwin Schrodinger
b)
Joseph Thomson
c)
James Chadwick
d)
Ernest Rutherford
23.
Who discovered that the nucleus contains positively charged particles called protons?
a)
Ernest Rutherford
b)
James Chadwick
c)
Democritus
d)
Niels Bohr
24.
The central region of an atom where neutrons and protons are located is the __________________.
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
25.
Particles in an atom that are neutral and have no charge are 
a)
negatrons 
b)
electrons 
c)
neutrons 
d)
protons 
26.

Worked with Rutherford to discover particles with no charge -- called neutrons.

a)

James Chadwick

b)

Niels Bohr

c)

Democritus

d)

Thomson

27.

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

a)

Democritus

b)

Thomson

c)

Bohr

d)

Dalton

28.

All matter is made of

a)

energy

b)

atoms

c)

electrons

d)

compounds

29.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
30.

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

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

31.

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

32.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
33.
What number indicates the nucleus?
a)
1
b)
2
c)
3
d)
4
34.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
35.
Which of the following is NOT a part of Dalton's atomic theory?
a)
All elements are composed of atoms.
b)
Atoms are alwyas in motion.
c)
Atoms of the same element are always identical.
d)
Atoms that combine do so in simple, whole-number ratios.
36.

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

37.
What did James Chadwick discover?
a)
neutrons
b)
electrons
c)
the atomic theory
d)
protons
38.

The discovery of the electron led directly to the development of which atomic model?

a)

Planetary Model

b)

Bohr Model

c)

Solid Sphere Model

d)

Plum-Pudding Model

39.

Most of the mass of the atom is found ___.

a)

In the cloud

b)

In the nucleus

40.

Who determined that the atom is mostly EMPTY SPACE?

a)

JJ Thomson

b)

Ernest Rutherford

c)

John Dalton

d)

Heisenberg and Schrodinger

41.

The nucleus is comprised of ___

a)

Protons and Electrons

b)

Protons and Neutrons

c)

Neutrons and Electrons

d)

Just Protons

42.

The Cathode Ray Tube experiment led to this model that was developed by ___.

a)

JJ Thomson

b)

John Dalton

c)

Ernest Rutherford

d)

Democritus

43.

Who developed the solid-sphere model of the atom?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Neils Bohr

d)

John Dalton

44.

Who discovered the nucleus after conducting the famous Gold Foil experiment?

a)

Ernest Rutherford

b)

Neils Bohr

c)

JJ Thomson

d)

John Dalton

45.

Who furthered the idea that all matter is made of earth, air, fire, and water?

a)

Thales

b)

Democritus

c)

Aristotle

d)

Eratothenes

46.

Which philosopher is credited with developing the idea of the atom (atomos)?

a)

Aristotle

b)

Democritus

c)

Thales

d)

Anaximander

47.

What is the atomic 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 in the energy levels

48.

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

49.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

50.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

51.
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
52.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
53.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

54.
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-
55.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
56.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
57.

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

a)

20

b)

10

c)

35

d)

25

58.

Which of the following determines the identity of an element?

a)

number of protons

b)

atomic mass

c)

number of neutrons

d)

number of shells

59.

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

a)

groups or families

b)

towers

c)

periods

d)

atomic numbers

60.

What are the horizontal rows (left and right) in the periodic table called?

a)

Families

b)

Groups

c)

Periods

d)

Orbitals

61.

All the elements that are blue and to the left of the staircase are called...

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

62.

All the elements that are yellow and to the right of the staircase are called...

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

63.

All the elements that are in red and that make up the staircase are called...

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

64.

Which of the following elements is in group or family 2?

a)

K

b)

Cs

c)

O

d)

Ca

65.

Which of the following elements is in period 2?

a)

K

b)

H

c)

O

d)

Ca

66.

The elements in the vertical column #18 are called

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Alkaline Earth Metals

67.

All of the noble gases have similar properties. Which element has similar chemical properties of the noble gas Argon (Ar)?

a)

Iodine

b)

Oxygen

c)

Fluorine

d)

Xenon

68.

Halogens are in group...

a)

16

b)

17

c)

18

d)

15

69.

Which of the following elements are Halogens? (Select all that apply)

a)

Iodine (I)

b)

Fluorine (F)

c)

Chlorine (Cl)

d)

Sodium (Na)

e)

Potassium (K)

70.

Which of the following elements are Group 1 Alkali Metals? (Select all that apply)

a)

Iodine (I)

b)

Fluorine (F)

c)

Chlorine (Cl)

d)

Sodium (Na)

e)

Potassium (K)

71.

How many valence electrons do all of the Group 2 Alkaline Earth Metals have?

a)

1

b)

2

c)

5

d)

7

e)

8

72.

The periodic table is arranged by ______

a)

Atomic Mass

b)

Number of Electrons

c)

Atomic Number

d)

Atomic Weight

73.

The electronegativity of an element is defined as…

a)

The ability of an atom to gain or attract additional electrons.

b)

The energy required to remove an electron from an atom.

c)

The ability of an element to chemically react with other elements or compounds.

d)

The size of an atom of a particular element.

74.

Which element will have the largest atomic radius?

a)

Ne

b)

Li

c)

Cs

d)

Rn

75.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
76.

The symbols W, X, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Z
77.

What is the difference between ionization energy and electronegativity?

a)

Ionization energy is the ability to attract a valence electron while, electronegativity is the energy needed to remove a valence electron.

b)

Ionization energy is the energy needed to remove a valence electron while, electronegativity is the ability to attract a valence electron.

c)

Ionization energy is the level of attraction between electrons and the nucleus while, electronegativity is the sharing of pairs of electrons.

78.

What is the difference between electronegativity and atomic radius?

a)

electronegativity is the level of attraction between electrons and the nucleus while, atomic radius is the energy needed to remove electrons.

b)

electronegativity is the energy needed to remove electrons while, atomic radius is the level of attraction between electrons and the nucleus.

c)

electronegativity is the level of attraction between electrons and the nucleus while, atomic radius is the size of the atom

79.
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
80.

Calculate the average atomic mass of the element iron (Fe) using the following data:

[Isotope / % abundance]

[Iron 54 / 6% ] [Iron 56 / 92% ] [ Iron 57 / 2% ]

a)

53.7 amu

b)

54.9 amu

c)

5592.0 amu

d)

55.9 amu

81.
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
82.
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
83.
If an atom contains exactly three protons, then it's an atom of _____
a)
lithium
b)
gold
c)
nitrogen
d)
carbon
84.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
85.
How many neutrons does an atom of the isotope Neon-22 have?
a)
12
b)
10
c)
22
d)
20
86.
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
87.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
88.
Which of the following could have 82 neutrons?
a)
W-182
b)
Ta-181
c)
Cs-132
d)
Ba-138
89.
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
90.

What does the atomic number of an element represent?

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

91.

How can you determine the number of neutrons in an atom if you know its atomic number and mass number?

a)

Subtract the atomic number from the mass number

b)

Add the atomic number to the mass number

c)

Multiply the atomic number by the mass number

d)

Divide the mass number by the atomic number

92.

Which of the following is true about isotopes?

a)

They have different atomic numbers but the same mass number

b)

They have the same atomic number but different mass numbers

c)

They have different numbers of electrons but the same number of protons

d)

They are always ions

93.

What is the relationship between atomic number and the number of protons in an atom?

a)

They are equal

b)

Atomic number is double the number of protons

c)

Atomic number is half the number of protons

d)

There is no relationship

94.

What is the term for atoms of the same element with different numbers of neutrons?

a)

Ions

b)

Isotopes

c)

Molecules

d)

Compounds

95.

Which of the following elements is most likely to undergo radioactive decay?

a)

Helium

b)

Uranium

c)

Oxygen

d)

Nitrogen

Similar Resources on Wayground

Ch. 17 - Elements and Their Properties

95 questions

Ch. 17 - Elements and Their Properties

quiz

Worksheet

•

7th - 12th Grade

End of Module 2 Test

100 questions

End of Module 2 Test

quiz

Worksheet

•

9th - 12th Grade

Week 4 quiz Night School w/mole

93 questions

Week 4 quiz Night School w/mole

quiz

Worksheet

•

9th - 12th Grade

Unit One Optional Review Practice

91 questions

Unit One Optional Review Practice

quiz

Worksheet

•

9th - 12th Grade

Chemistry Unit 1 Test Review

98 questions

Chemistry Unit 1 Test Review

quiz

Worksheet

•

9th - 12th Grade

Atomic Structure and Key Experiments

100 questions

Atomic Structure and Key Experiments

quiz

Worksheet

•

9th - 12th Grade

IMF Practice

95 questions

IMF Practice

quiz

Worksheet

•

9th - 12th Grade

ICP Chem Final

100 questions

ICP Chem Final

quiz

Worksheet

•

9th - 12th Grade