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Review: Atomic Particles and Theories

Total questions: 118

Worksheet time: 5hrs 14mins

Name
Class
Date
1.
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
2.
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
3.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
4.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
5.
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
6.

Match the following

a)

Protons

1.

Atomic number

b)

Protons + Neutrons

2.

Atomic Mass

c)

Electrons

3.

= the # of protons in a neutral atom.

d)

Isotope

4.

Same protons but different neutrons.

e)

Ions

5.

Atoms that lost/gained electrons

7.

An atom that has a +3 charge has

a)

the same number of protons and electrons

b)

Lost 3 electrons

c)

Gained 3 electrons

d)

Gained 3 protons

8.

What is the mass of an atom of calcium with 20 protons, 22, neutrons and 20 electrons?

4 lines
9.
Where are electrons of an atom found?
a)
Nucleus
b)
Electron Cloud
c)
Some are in the nucleus and some in the electron cloud.
d)
They are moving everywhere.
10.

An atom has an atomic number of 15 and a mass number of 31. How many protons are there in the atom?

a)

15

b)

31

c)

16

d)

47

11.
What is in the nucleus of an atom?
a)
Neutrons and protons 
b)
Protons
c)
Protons and Electrons
d)
Electrons and Nuetrons
12.
An atom has an atomic number of 19 and a mass number of 29. How many neutrons are in the atom?
a)
30
b)
19
c)
10
d)
38
13.

The numbers of protons, neutrons, and electrons in each of four different ions are shown in the table below. Which ion has the greatest mass?

a)

G

b)

E

c)

A

d)

Z

14.
Compared to the charge and mass of a proton, an electron has...
a)
the same charge and a smaller mass
b)
the same charge and same mass
c)
an opposite charge and a smaller mass
d)
an opposite charge and the same mass
15.

When an atom contains more electrons than protons, it is

a)

a neutral atom with no charge

b)

an ion and negatively charged

c)

an ion and positively charged

d)

an isotope and has more mass

16.

When an atom contains more neutrons than another atom, it is

a)

a neutral atom with no charge

b)

an ion and negatively charged

c)

an ion and positively charged

d)

an isotope and has more mass

17.

What is 'E' pointing to?

a)

electron cloud

b)

electron

c)

nucleus

d)

proton

e)

neutron

18.

Who was the first person to "think" of an atom?

a)

Democritus

b)

J.J. Thompson

c)

Rutherford

d)

Bohr

19.

What experiment was used to discover the nucleus?

a)

Cathode Ray Tube

b)

Gold Foil

c)

Chromatography

d)

Gel Electrophorese

20.

Which one of these is Dalton's Model?

a)
b)
c)
d)
21.

Who discovered the nucleus?

a)

Rutherford

b)

Bohr

c)

J.J. Thompson

d)

Democritus

22.

What experiment was used to discover electrons?

a)

Cathode Ray Tube

b)

Gold Foil

c)

Chromatography

d)

Gel Electrophorese

23.

What model is the current model of the atom?

a)

Rutherford's

b)

Bohr's

c)

The Quantum Mechanical Model

d)

Dalton's

24.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
25.
The central region of an atom where neutrons and protons are located is the __________________.
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
26.
Matter always has mass.
a)
true
b)
false
27.

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

a)

James Chadwick

b)

Niels Bohr

c)

Democritus

d)

Thomson

28.

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

a)

Bohr

b)

Rutherford

c)

Chadwick

d)

Thomson

29.

This picture best represents ___________________ atomic model.

a)

Thomson's

b)

Dalton's

c)

Bohr's

d)

Chadwick's

30.

Democritus was known for

a)

discovering the electron

b)

discovering the proton

c)

creating the term atom, meaning indivisible

d)

discovering the nucleus

31.
What contribution did John Dalton make to atomic theory? 
a)
He discovered that every atom was positively charged. 
b)
He discovered that every element consisted of one type of atom that couldn't be divided. 
c)
He discovered that atoms had nuclei. 
d)
He discovered that atoms could be divided into smaller parts. 
32.
All matter is made of what?
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
33.
The word atom comes from a Greek word "atomos" that means
a)
Invisible
b)
Indivisible
c)
Undivided
d)
Indestructable 
34.

The percentage of copper and oxygen in samples of “CuO” obtained by different methods were found to be the same. This illustrates the law of:

a)

Constant proportions

b)

Conservation of mass

c)

Multiple proportions

d)

Reciprocal proportions

35.

If two or more compounds are composed of the same two elements, then the ratio of the masses of the second element that is combined with a certain mass of the first element is always a ratio of small whole numbers. This statement is called the law of

a)

definite proportions.

b)

conservation of mass.

c)

atomic theory.

d)

multiple proportions.

36.

The fact that every sample of a particular chemical compound contains the same elements in exactly the same proportions by mass is known as the law of

a)

conservation of energy.

b)

conservation of mass.

c)

atomic theory.

d)

definite proportions.

37.

2. Atoms of a given element are identical in size, _____, and other properties.

a)

shape

b)

mass

c)

source

d)

charge

38.

3. Atoms cannot be subdivided, _________ or __________.

a)

divided or conquered

b)

created or destroyed

c)

bought or sold

d)

to be or not to be

39.

4. Atoms of different elements combine in whole number ______ to form chemical compounds.

a)

atoms

b)

compounds

c)

chemicals

d)

ratios

40.

In chemical reactions, atoms are __________, ____________, or ___________.

a)

combined, separated, rearranged

b)

combined, shifted, reorganized

c)

added, subtracted, combined

d)

subdivided, created or destroyed

41.

Compared to other subatomic particles, the proton is _____

a)

heavy and neutral

b)

heavy and negatively charged

c)

heavy and positively charged

d)

light and negatively charged

42.

Compared to other subatomic particles, the electron is _____

a)

heavy and positively charged

b)

light and positively charged

c)

light and neutral

d)

light and negatively charged

43.

Which subatomic particles determine the identity of an element?

a)

electrons

b)

protons

c)

neutrons

d)

photons

44.
Nuclei are held together by the strongest of the four fundamental forces of physics, _____
a)

the electrostatic force

b)

the gravitational force

c)

the strong nuclear force

d)

the weak nuclear force

45.
Neutrons serve as a kind of _____
a)
charge carrier
b)
shock absorber for collisions
c)
shield for radiation
d)
buffer between the protons
46.

A neutron changes into a proton and an electron during ________________.

a)

alpha decay

b)

beta decay

c)

gamma decay

d)

all of the above

e)

alpha & beta decay

47.

This particle has 2 protons and 2 neutrons like a helium nucleus.

a)

alpha particle

b)

beta particle

c)

gamma photon

d)

alpha and gamma particles

e)

none of the above

48.

This type of decay creates a new element

a)

alpha

b)

gamma

c)

alpha and beta

d)

none of the above

e)

beta

49.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
50.

What is Atomic Mass Number ?

a)

Number of Protons

b)

Number of Neutrons

c)

Number of Protons and Neutrons

d)

Number of Protons and Electrons

51.

The formula used to calculate the number of neutrons is:

a)

Mass Number - Atomic Number

b)

Protons + Electrons

c)

Atomic Number - Mass Number

d)

Protons x2

52.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

53.

Which pair of properties describes the elements in Group (Family) 1?

a)

They are chemically stable

b)

They have 8 valence electrons

c)

They are the most reactive metals

d)

They are the most reactive non metals

54.

This element does not match the properties of any other group so it stands alone. It is placed above Group 1 but it is not part of that group. It is very reactive, colorless, odorless, and a gas at room temperature.

a)

Hydrogen

b)

Helium

c)

Nitrogen

d)

Oxygen

55.
How many neutrons does the isotope of lithium have?
a)

8

b)

3

c)

5

56.
If a hydrogen atom has 1 proton, 1 electron, and 1 neutron, its atomic number is:
a)
1
b)
2
c)
3
57.
If a sulfur atom has 16 protons, 16 electrons, and 16 neutrons, its atomic mass is:
a)
16
b)
32
c)
48
58.
How is carbon-12 different from carbon-14?
a)

They have a different number of protons

b)

they have a different number of electrons

c)

they have a different number of neutrons

59.

Electrons orbit a certain distance from the nucleus. Either radiate or absorb energy when jumping orbitals.

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

60.

The atom is mostly large empty space with a small, dense nucleus at the center

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

61.

Atom is a positively charged cloud with embedded negative electrons

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

62.

Atoms are indivisible (cannot be broken down)

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

63.

What scientist proposed this atomic model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

64.

What scientist proposed this atomic model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

65.

What scientist proposed this atomic model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

66.

What scientist proposed this atomic model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

67.

In a famous experiment conducted by Ernest Rutherford, positively charged alpha particles were scattered by a thin gold foil. Which of the following is a conclusion that resulted from this experiment?

a)

The nucleus is negatively charged

b)

The atom is a dense solid and is indivisible

c)

The mass is conserved when atoms react chemically

d)

The nucleus is very small and the atom is mostly empty space

68.

What subatomic particle was discovered in the cathode ray tube experiment?

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

69.

What evidence led Niels Bohr to believe that electrons occupy specific energy levels in atoms?

a)

Excited electrons emit colored light at every possible wavelength.

b)

Excited electrons emit colored light at only certain wavelengths.

c)

Electrons emit colored light only when in an excited state.

d)

Electrons emit colored light only when in ground state.

70.
Has a mass of 4 and a charge of +2
a)
Alpha
b)
Beta
c)
Gamma
71.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
72.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
73.

A radioactive nucleus has a ____ stable nucleus than a non-radioactive nucleus of the same element.

a)

more

b)

less

c)

identical

d)

small

74.
Takes two small nuclei and combines them into a larger nucleus
a)
fission
b)
fusion
75.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
half-life
d)
gamma radiation
76.
How is nuclear fusion different from nuclear fission?
a)
In fusion, the product is a larger atomic nucleus.
b)
Fission produces energy but fusion does not.
c)
Fusion produces energy but fission does not.
d)
In fission, the product is a larger atomic nucleus.
77.
Which type of nuclear radiation is being emitted here?
a)
alpha
b)
beta
c)
gamma
d)
none
78.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
79.

Which of these diagrams represents the type of nuclear reaction that produces energy in the Sun?

a)

A

b)

B

c)

C

d)

D

80.

During nuclear fission, a nucleus _________.

a)

grows

b)

divides

c)

shrinks

d)

combines with another

81.
When a nucleus undergoes nuclear decay by gamma rays, the atomic number of the element....
a)
remains the same
b)
  decreases by one.
c)
increases by one.
d)
increases by two.
82.
The type of radioactive particle that can be stopped by a sheet of paper is the ____.
a)
alpha particle
b)
beta particle
c)
gamma ray
d)
uranium
83.
The most penetrating type of radiation is the ____.  
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
84.
A helium nucleus with two protons and two neutrons is called a(n) ____.  
a)
alpha particle
b)
electroscope
c)
beta particle
d)
gamma ray
85.

Which equation correctly represents the alpha decay of polonium-214?

a)

A

b)

B

c)

C

d)

D

86.
a)

A

b)

B

c)

C

d)

D

87.

... has that symbol

a)
Alpha
b)
Beta 
c)
Gamma
d)

positron

88.
Solve this equation for alpha decay.
20985At = ___ + 42He
a)
20583Bi
b)
20986Rn
c)
20781Tl
d)
20885At
89.
Solve this equation for alpha decay.
22688Ra = ___ + 42He
a)
22286Rn
b)
22689Ac
c)
22484Po
d)
22588Ra
90.
Solve this equation for beta decay.
6027Co = ___ + 0-1e
a)
5625Mn
b)
6028Ni
c)
5823V
d)
5927Co
91.
Solve this equation for beta decay.
146C = ___ + 0-1e
a)
104Be
b)
147N
c)
102He
d)
136C
92.
The following is an example of what type of reaction?
24395Am  →  23993Np + 42He 
a)
alpha decay
b)
beta decay
c)
gamma decay
93.
What is the missing isotope that will balance the following nuclear equation?
94Be  +  11H →  _____  +  42He
a)
105B
b)
105Ne
c)
63Li
d)
63C
94.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
95.
Solve this equation for alpha decay.
22688Ra = ___ + 42He
a)
22286Rn
b)
22689Ac
c)
22484Po
d)
22588Ra
96.
What is the missing isotope that will balance the following nuclear equation?
94Be  +  11H →  _____  +  42He
a)
105B
b)
105Ne
c)
63Li
d)
63C
97.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
Beta
c)
Gamma 
d)
none
98.
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
99.
An element has three different isotopes. One has a mass of 35.00 amu; another has a mass of 36.00  amu; and another has a mass of 38.00  amu. What is the average atomic mass of this element?
a)
36.33 amu
b)
37.00 amu
c)
12.11 amu
d)
impossible to tell
100.
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
101.
Atom 1 has Mass=12  Protons=6
Atom 2 has Mass= 14 Electrons=6
Are these atoms isotopes of each other or different elements?
a)
Different Elements - Mg & Si
b)
Different Elements - Ar & Ca
c)
Isotopes of Carbon
d)
Isotopes of Magnesium
102.
What is the name of the atom pictured here?
a)
Nitrogen
b)
Nitrogen-15
c)
Nitrogen-7
d)
Nitrogen-8
103.

Element X has two isotopes. If 54% of the element has an atomic mass of 49.6 amu, and 56% of the element has an atomic mass of 42.4 amu, the average atomic mass of element X is equal to which of the following?

a)

(0.54 x 49.6) + (0.56 x 42.4)

b)

(0.54 - 49.6) x (0.56 + 42.4)

c)

(0.54 + 49.6) x (0.56 + 42.4)

104.

What are the subatomic particles found in the nucleus of an atom?

a)

Protons and electrons

b)

Protons and neutrons

c)

Neutrons and electrons

d)

Protons, neutrons, and electrons

105.

What is the electrical charge of protons?

a)

Positive

b)

Negative

c)

Neutral

d)

No charge

106.

How many electrons are found in the first energy level?

a)

1

b)

2

c)

6

d)

8

107.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
108.
What is the charge of a neutron?
a)
Positive
b)
Negative
c)
Neutral/no charge
109.
What is the center of the atom called?
a)
Orbital
b)
Nucleus
c)
Proton
d)
Electron shell
110.
Identify the element in the picture
a)
Boron
b)
Carbon
c)
Nitrogen
d)
Lithium
111.

How many electrons does Aluminum have?

a)

11

b)

12

c)

13

112.

Using the periodic table of elements, how many electrons in a neutral atom of carbon?

a)

12

b)

5

c)

6

d)

13

113.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
114.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
115.

An element will always have the same number of 

a)
neutrons
b)
protons
c)
isotopes
d)
atoms
116.
How are electrons arranged in an atom?
a)
In groups of five
b)
In energy levels
c)
By color
d)
By shape
117.

What is a Bohr Model?

a)

A model of an atom

b)

Vertical column in periodic table

c)

Horizontal row in periodic table

d)

Only shows the element symbol and it's outer most electron shell

118.

What does the Bohr Model represent?

a)

The structure of molecules

b)

The structure of the Solar System

c)

The structure of an atom

d)

The structure of Carle Place

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