wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Atoms (Mega-Review)

Total questions: 118

Worksheet time: 2hrs 58mins

Name
Class
Date
1.

What charge does a proton have?

a)

positive

b)

negative

c)

neutral

2.

What charge does a neutron have?

a)

positive

b)

negative

c)

neutral

3.

What charge does an electron have?

a)

positive

b)

negative

c)

neutral

4.

There are equal numbers of ___ and ___ in an atom (if it's neutral)

a)

protons and neutrons

b)

protons and electrons

c)

neutrons and electrons

5.

What two particles are in the nucleus of an atom?

a)

protons and electrons

b)

electrons and neutrons

c)

protons and neutrons

6.
What subatomic particle(s) would be found orbiting the nucleus?
a)
Neutrons only
b)
Electrons only
c)
Protons and Neutrons
d)
Protons and Electrons
7.
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
8.
The first energy level can hold up to how many electrons?
a)
8
b)
4
c)
2
d)
5
9.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
10.
What are the 3 subatomic particles that make-up the atom?
a)
protons, neutrons, and isotopes
b)
neutrons, isotopes, and electrons
c)
positives, negatives, and electrons
d)
protons, neutrons, and electrons
11.
all matter is made of what 
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
12.
How many protons does this atom have?
a)
2.5
b)
6
c)
5
d)
10.811
13.
An atom is made up mostly of
a)
protons
b)
gravity
c)
empty space
d)
electricity
14.

How many protons does an atom of Sodium (Na) have?

a)

12

b)

11

c)

23

15.

The atomic number is the number of ____ in the nucleus. It's the element's "identification"!

a)

electrons

b)

neutrons

c)

protons

16.

Why is the Proton important within the atom?

a)

I'ts important because it tells you the identity of the atom

b)

It's important becaue the atom repells other atoms.

c)

Important becuase is exerts a strong force to balance the atom.

d)

Important because it determines chemical reactivity

17.

Never trust an atom because they make up

a)

Nothing

b)

Protons

c)

everything

d)

somethings

18.

The atomic number on the periodic table can tell us. Use period table https://ptable.com/#Properties

a)

# of electrons

b)

# of protons and the identitiy of the atom.

c)

# of neutrons

d)

# or protons and neutrons.

19.

Use the periodic table: If an atom have 12 protons what element is it. https://ptable.com/#Properties

a)

Magnesium

b)

Manganese

c)

Carbon

d)

Hydrogen

20.

An atom that has a neutral charge has 13 protons how many electrons does it have?

a)

11

b)

0

c)

13

d)

26

21.

An atom has 34 protons, what element is it? Use periodic table https://ptable.com/#Properties

a)

Selenium

b)

Chlorine

c)

Technetium

d)

Sodium

22.

How many neutrons are in Krypton (Kr)?

a)

36

b)

84

c)

50

d)

48

23.
Fluorine is atomic number 9, and has a mass of 19. How many electrons would it have?
a)
9
b)
6
c)
19
d)
10
24.
Fluorine is atomic number 9, and has a mass of 19. How many protons would it have?
a)
9
b)
6
c)
19
d)
10
25.
Fluorine is atomic number 9, and has a mass of 19. How many neutrons would it have?
a)
9
b)
6
c)
19
d)
10
26.
Who proposed the first atomic view of matter?
a)
Lavoisier
b)
Empedocles
c)
Democritus
d)
Priestley
27.

The theory of Democritus held that everything is composed of _________.

a)

atoms

b)

numbers

c)

shapes

28.

Early ideas of matter being composed of earth, wind, water, and fire were proposed by

a)

Democritus

b)

Zeus

c)

Einstein

d)

Aristotle

29.

JJ Thomson was credited for the discovery of the

a)

center of the universe

b)

proton

c)

electron

d)

neutron

30.

Which device did JJ Thomson use to discover the electron?

a)

X-ray machine

b)

scanning tunneling electron microscope

c)

spectrometer

d)

cathode ray tube

31.

The atomic model associated with Thomson is the

a)

plum pudding model

b)

nuclear mode.

c)

planetary model

d)

the electron cloud model

32.

The CRT when powered up produces a beam that is

a)

red in color and positively charged.

b)

magnetic and negatively charged.

c)

deflected only when exposed to certain frequencies of light.

d)

red, blue, or green.

33.

The CRT was also known as the ____________ in the early 1950's through the 1990's.

a)

radio

b)

refrigerator

c)

MRI used in hospitals

d)

TV

34.

In what location did Rutherford suggest the electrons were located?

a)

in the nucleus.

b)

outside the nucleus.

c)

only where the alpha particles were deflected.

d)

outside the atom after they collided with the alpha particle.

35.

Which is a finding attributed to Rutherford's Gold Foil Experiment?

a)

atoms are indivisible and have a dense positive nucleus.

b)

atoms are divisible and have multiple layers of electrons scattered uniformly about the atom.

c)

atoms are like plum pudding with positive and negative charges uniformly scattered throughout the atom.

d)

atoms are mostly empty space with a dense positive nucleus.

36.

Rutherford used what type of radiation to bombard the gold foil?

a)

alpha particles.

b)

beta particles.

c)

gamma radiation.

d)

neutrinos.

37.

What did Rutherford expect to happen to the alpha particles bombarding the gold foil?

a)

they would be absorbed by the gold.

b)

they would be deflected by the gold.

c)

they would go completely through the gold foil.

d)

the would be changed into beta radiation by the gold foil.

38.

What evidence did Rutherford use to support the idea that the atom was mostly empty space?

a)

the vast majority of the alpha particles went through the foil unaffected.

b)

the vast majority of the alpha particles were deflected at 90 degrees.

c)

one alpha particle was deflected by the gold foil.

d)

beams of alpha particles were deflected by magnets.

39.
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.
40.
Niels Bohr suggested that electrons.......
a)
are found in specific orbits
b)
electrons are scattered throughout the atom
c)
electrons move according to their energy level
d)
electrons are positive
41.
His atomic model was depicted similar to a planetary/solar system
a)
Bohr
b)
Thomson
c)
Rutherford
d)
Dalton
42.
Which scientist saw the atom as a solid sphere?
a)
Dalton
b)
Thomson
c)
Rutherford
d)
Bohr
43.
Proposed the Modern Electron Cloud Model of the atom
a)
Schrodinger & Heisenberg
b)
Dalton
c)
Chadwick
d)
Rutherford
44.
What does this image represent?
a)
Billiard Ball Model
b)
Plum Pudding
c)
Gold Foil
d)
Solar System Model
45.
What does this image represent
a)
Billiard Ball
b)
Solar System
c)
Plum Pudding
d)
Electron Cloud
46.
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
47.
Believed that atoms are small, hard particles that were "indivisible"
a)
Democritus
b)
Aristotle
c)
Schrodinger
d)
Greek Philosophers
48.

Whose created this atom model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

e)

Heisenberg and Schrodinger

49.

The Quantum Mechanical Model is the most recent/modern atomic model.

a)

True

b)

False

50.
What charge does an atom have if it LOSES an electron? 
a)
Positive (+)
b)
Negative (-)
51.
What charge does an atom have if it GAINS an electrons?
a)
Positive (+)
b)
Negative (-)
52.

Which particles change the charge in atoms when ions are formed?

a)

Protons

b)

Electrons

c)

Neutrons

53.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
54.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
55.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

56.
Atoms are most stable when their outer shell is filled with electrons.
a)
true
b)
false
57.

An atom with the same number of protons and electrons (no charge) and the expected atomic mass or number of neutrons from the periodic table.

a)

Neutral/Normal Atom

b)

Ion

c)

Isotope

58.

An atom that has gained or lost electrons in an attempt to become stable/bond with another atom.

a)

Normal/Neutral Atom

b)

Ion

c)

Isotope

59.

If an atom has 9 protons and 10 electrons it has a charge of ____.

a)

0

b)

-1

c)

+1

d)

-2

60.

If an atom has 4 protons and 2 electrons it has a charge of ____.

a)

0

b)

-2

c)

+2

d)

+1

61.

If an atom has a charge of +3 and an atomic number of 5 it should have _______ electrons.

a)

1

b)

2

c)

3

d)

4

62.

If an atom has a charge of -2 and an atomic number of 16 it should have _______ electrons.

a)

14

b)

16

c)

18

d)

20

63.

If an atom has a charge of 0 (neutral) and an atomic number of 8 it should have ____ electrons.

a)

0

b)

8

c)

7

d)

9

64.

Atoms of the same element that have different mass than expected because they have a different number of neutrons.

a)

Neutral Atom

b)

Ion

c)

Isotope

d)

Cation

65.

You need to look at the ______________ on the periodic table to figure out if an atom is an isotope or not.

a)

atomic number

b)

symbol

c)

element name

d)

atomic mass

66.

If an atom has an expected atomic mass of 14, and it has 7 protons and 8 neutrons it is a ____________.

a)

Anion

b)

Normal Atom

c)

Isotope

d)

Cation

67.
How many neutrons would Fe-56 have?
a)
56
b)
26
c)
30
d)
33
68.
How many protons does P-30 have?
a)
30
b)
16
c)
12
d)
15
69.
If an atom of nickel has a charge of +3, how many electrons does the atom have?
a)
28
b)
25
c)
26
d)
31
70.
How many neutrons would V-49 have?
a)
26
b)
49
c)
23
d)
50.94
71.
How many protons does Pb-209 have?
a)
127
b)
209
c)
82
d)
291
72.
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
73.

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

a)

9

b)

7

c)

16

d)

20

74.

Q.Isotopes must have the same number of protons but different numbers of ________

a)

electron rings

b)

charges

c)

neutrons

d)

electrons

75.
An atom is electrically neutral when
a)
protons and neutrons are the same
b)
protons and electrons are the same
c)
neutrons and electrons are the same
d)
neutrons balance the protons and electrons
76.
How many neutrons does a Flourine-14 isotope have?
a)
4
b)
5
c)
9
d)
14
77.
How many neutrons does a Sulfur-32 isotope have?
a)
15
b)
16
c)
32
d)
12
78.

In the following pair, are they isotopes or different elements.

Element x has 56 protons and 81 neutrons.

Element y has 56 protons and 82 neutrons.

a)

isotopes of same element

b)

different elements

79.

In the following pair, are they isotopes or different elements.

Element x has an atomic number of 20 and a mass number of 40.

Element y has an atomic number of 20 and a mass number of 41.

a)

isotopes of same element

b)

different elements

80.

In the following pair, are they isotopes or different elements.

Element x has 17 protons and 18 neutrons.

Element y has 18 protons and 17 neutrons.

a)

isotopes of same element

b)

different elements

81.

To figure out the mass of an atom based on its subatomic particles you would add ______ & ________.

a)

Protons & Electrons

b)

Protons & Neutrons

c)

Neutron & Electrons

82.
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
83.
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
84.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
85.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

86.

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

a)

20

b)

38

c)

56

d)

88

87.

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

88.

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

a)

ions

b)

isotopes

c)

quarks

d)

molecules

89.

The average atomic mass on the periodic table is found from...

a)

calculating the weighted average mass of all the isotopes of that element

b)

Calculating different types of elements together

c)

calculations the average of all elements in that period together.

d)

making a guess about how much all the isotopes might wiegh together.

90.

The mass of an element is 15 and the number of protons is 7 how many neutrons does it have?

a)

15

b)

7

c)

8

d)

22

91.

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)

15.99, Oxygen

b)

10.81, Boron

c)

10.81, Oxygen

d)

15.99, Boron

92.

Which of the following represents isotopes of the same element?

a)

818O and 718O

b)

919F and 1019Ne

c)

919F and 919Ne

d)

816O and 818O

93.

What is the average atomic mass for thallium, Tl, if there are two isotopes with the following masses and abundances? Tl-203 has a mass of 203 amu with an abundance of 29.5 % Tl-205 has a mass of 205 amu with an abundance of 70.5 %

a)

203.12 amu

b)

204.31 amu

c)

204.41 amu

d)

204.0 amu

94.

A sample of cesium is 75% Cs-133, 20% Cs-132, and 5% Cs-134. What is the average atomic mass?

a)

132.97 amu

b)

133.00 amu

c)

133.16 amu

d)

132.85 amu

95.

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

96.
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
97.
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
98.

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

99.

"A random and spontaneous process where an unstable nucleus emits radioactive radiation until the nucleus becomes more stable.."

The statement above refer to...

a)

Half -life

b)

Nuclei decay

c)

Radioactivity

d)

Radioactive decay

100.
The process of nuclear change in an atom of radioactive material is called... 
a)
nuclear decay
b)
nuclear mass
c)
isotopes
d)
radon
101.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
102.
The rate at which a radioactive element decays is its ____.
a)
quarter life
b)
whole life
c)
wonderful life 
d)
half life
103.
If the half life of a radioactive element is 100yrs, how long would it take for the radioactivity to reduce by one half?
a)
200yrs
b)
100yrs
c)
50yrs
d)
300yrs
104.

A certain radioactive sample has a half life of 2 years. After 6 years, how much of the sample is left?

a)

1/2

b)

1/3

c)

1/16

d)

1/8

105.
Marie Curie was the first woman to win a...
a)
Golden Globe
b)
Nobel Prize
c)
Oscar
d)
 Emmy Award
106.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
107.
The three types of nuclear radiation in increasing order of penetrating power are ____.  
a)
  alpha, beta, gamma 
b)
X ray, beta, gamma
c)
alpha, gamma, beta 
d)
X ray, gamma, beta 
108.

A sample of Radium-228 decays from 100g to 12.5g. How many half lives did it experience?

a)

1

b)

2

c)

3

d)

4

109.

Iodine-131 has a half life of 8.07 days. What fraction of a sample of Iodine-131 is left unchanged after 16.14 days?

a)

1/2

b)

1/4

c)

1/8

d)

1/16

110.

The radioactive isotope Nickel-63 has a half life of 100 years. How much of a 10 gram sample remains after 300 years?

a)

1 gram

b)

1.25 grams

c)

0.50 grams

d)

0.075 grams

111.

The half-life of Iodine-131 is 8 days. What does this mean?

a)

The lifespan of Iodine-131 is 8 days

b)

Iodine-131 takes 8 days to become a radioactive material

c)

Iodine-131 takes 8 days to decay to half the amount of its original amount

d)

Iodine-131 takes days to become a non-radioactive material

112.

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 2.4 minutes has elapsed?

a)

100.0g

b)

50.0g

c)

12.5g

d)

8.5g

113.

If 10 mg of iodine 131 is given to a patient, how much is left after 27 days? The half-life of iodine-131 is 9 days.

a)

5.0mg

b)

2.5mg

c)

1.25mg

d)

10mg

114.

Those patients who develop tyroid cancer are treated with a certain radioactive isotope before attending surgery. The isotope is ...

a)

As-74

b)

Tc-99

c)

I-131

d)

Na-24

115.

The radioactive surgery used in archaeology to date organic remains is...

a)

C-12

b)

U-238

c)

C-14

d)

U-235

116.

Uranium has two isotopes but only one of them is radioactive. Which one?

a)

U-235

b)

U-238

117.

The most dreadful accident involving a Nuclear Power Plant happened in 1986 in...

a)

Kiev

b)

Chernobyl

118.

When and where were dropped the first two atomic bombs by US forces?

a)

In 1945 over the Japanese cities of Hiroshima and Tokyo

b)

In 1942 over the Japanese cities of Nagasaki and Tokyo

c)

In 1942 over the Japanese cities of Hiroshima and Nagasaki

d)

In 1945 over the Japanase cities of Hiroshima and Nagasaki

Similar Resources on Wayground

8R Science Final Review- 1

118 questions

8R Science Final Review- 1

quiz

Worksheet

•

8th Grade

Week 3 JC - Periodic Table, Chem Reac, Common Gases, Materials

116 questions

Week 3 JC - Periodic Table, Chem Reac, Common Gases, Materials

quiz

Worksheet

•

6th - 8th Grade

SY 24-25 Life Science 8 Final Exam Practice Questions

117 questions

SY 24-25 Life Science 8 Final Exam Practice Questions

quiz

Worksheet

•

8th Grade - University

Electron Transport Chain Photosynthesis

114 questions

Electron Transport Chain Photosynthesis

quiz

Worksheet

•

8th - 12th Grade

Year In review Math to use

117 questions

Year In review Math to use

quiz

Worksheet

•

6th - 8th Grade

pure substances vs mixtures zachry

118 questions

pure substances vs mixtures zachry

quiz

Worksheet

•

8th Grade

Sci 8 Final Review

123 questions

Sci 8 Final Review

quiz

Worksheet

•

8th Grade

DA #3 Review

122 questions

DA #3 Review

quiz

Worksheet

•

6th - 8th Grade