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History of the Atom

Total questions: 46

Worksheet time: 1hrs 1mins

Name
Class
Date
1.
Who discovered that the nucleus contains positively charged particles called protons?
a)
Ernest Rutherford
b)
James Chadwick
c)
Democritus
d)
Niels Bohr
2.
Who discovered the electron?
a)
Niels Bohr
b)
Democritus
c)
Joseph Thomson
d)
John Dalton
3.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
4.
The central region of an atom where neutrons and protons are located is the __________________.
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
5.
Particles in an atom that are neutral and have no charge are 
a)
negatrons 
b)
electrons 
c)
neutrons 
d)
protons 
6.

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

a)

Democritus

b)

Thomson

c)

Bohr

d)

Dalton

7.

Proposed that electrons move around the nucleus in specific layers, or shells.

a)

Bohr

b)

Rutherford

c)

Chadwick

d)

Thomson

8.

What is a particle with one negative charge called?

a)

electron

b)

proton

c)

quark

d)

neutron

9.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

10.

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

11.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
12.
What number indicates the nucleus?
a)
1
b)
2
c)
3
d)
4
13.
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.
14.
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
15.

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

16.
Who performed the Gold Foil Experiment?
a)
J. J. Thomson
b)
Ernest Rutherford
c)
Neils Bohr
d)
John Dalton
17.
Which model is this?
a)
Thomson Model
b)
Cloud Model
c)
Bohr Model
d)
Rutherford Model
18.

Who created the plum pudding model?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

John Dalton

19.

What particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

d)

Protons, neutrons, and electrons

20.

What is the mass number of bromine?

a)

35

b)

45

c)

80

d)

79.904

21.

The atomic number is equal to _.

a)

the number of protons

b)

the number of neutrons only

c)

the total number of protons and neutrons

d)

the number of protons, neutrons, and electrons

22.

How many neutrons does this bromine atom have?

a)

35

b)

45

c)

80

d)

115

23.

What is the mass number of this Neon atom?

a)

10

b)

11

c)

21

d)

20

24.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

25.

What changes when an atom becomes an ion?

a)

The number of electrons

b)

The number of protons

c)

The number of neutrons

d)

Both the number of neutrons and electrons

26.

How many neutrons does this Neon atom have?

a)

21

b)

11

c)

10

d)

12

27.

What happened to this Magnesium atom to make it an ion?

a)

It LOST electrons

b)

It GAINED electrons

c)

It GAINED protons

d)

It LOST protons

28.

What is the atomic number of this element?

a)

12

b)

24

c)

23

d)

35

29.

Adding or subtracting neutrons makes the element change into

a)

an ion

b)

a mixture

c)

an isotope

d)

a neutral atom

30.

What is the charge on a lithium atom that loses 1 electron?

a)

+1

b)

0

c)

-1

d)

-2

31.

What is the representation of an isotope?

a)

N-3

b)

Al+3

c)

Si

d)

P-33

32.
Isotopes are atoms that have different
a)
Mass numbers
b)
Element names
c)
Atomic Numbers
33.
Two atoms that have different numbers of protons are 
a)
Different ions
b)
Different isotopes
c)
Different elements
34.
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
35.
Two neutral atoms that have the same atomic number and different mass numbers are
a)
Ions
b)
Isotopes
c)
Alpha particles
d)
Different elements
36.

A negatively charged ion that has gained electrons to satisfy the octet rule (metals do this)

a)

Anion

b)

Cation

c)

Neutral Atom

d)

Isotope

37.

A positively charged ion that has lost electrons to satisfy the octet rule (non-metals do this)

a)

Anion

b)

Cation

c)

Neutral Atom

d)

Isotope

38.

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

a)

0

b)

-1

c)

+1

d)

-2

39.
Can an atom of Helium have 3 neutrons?
a)
Yes, because it can be an ion
b)
No, because protons identify the atom
c)
Yes, because it can be an isotope
d)
No, because only neutral atoms exist
40.
Can an atom of Helium have 3 electrons?
a)
Yes, because it can be an ion
b)
No, because protons identify the atom
c)
Yes, because it can be an isotope
d)
No, because only neutral atoms exist
41.
Can an atom of Hydrogen have 2 protons?
a)
Yes, because it can be an ion
b)
No, because protons identify the atom
c)
Yes, because it can be an isotope
d)
No, because only neutral atoms exist
42.
What is the charge on a lithium atom that looses 1 electron?
a)
+1
b)
0
c)
-1
d)
-2
43.
How many protons does this isotope of titanium have? Hint titanium has an atomic number of 22.
a)
48
b)
22
c)
26
d)
70
44.
Which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
45.

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

46.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number

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