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Unit 3 Review

Total questions: 106

Worksheet time: 3hrs 38mins

Name
Class
Date
1.

Which reaction produces harmful radioactive waste?

a)

Fission

b)

Photosynthesis

c)

chain reaction

d)

Fusion

2.

_____is the joining of atomic nuclei

a)

Fusion

b)

chain reaction

c)

Photosynthesis

d)

Fission

3.

_______is the splitting of atomic nuclei

a)

Fission

b)

nuclear reaction

c)

Fusion

d)

bayler reaction

4.

Which process occurs naturally in the centre of stars like the Sun

a)

Bi-multiple reaction

b)

Fission

c)

chemical

d)

fusion

5.
What is a chain reaction?
a)
When electrons are emitted causing electricity
b)
When a nuclear fission reaction occurs, the protons emitted can strike other nuclei in the sample, and cause them to split
c)
When a nuclear fission reaction occurs, the neutrons emitted can strike other nuclei in the sample, and cause them to split
d)
When a nuclear fission reaction occurs, the electrons emitted can strike other nuclei in the sample, and cause them to split
6.

How is the alpha particle written in a nuclear equation?

a)

42He

b)

24He

c)

0-1e

d)

00γ

7.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
8.

Gamma rays have

a)

no mass

b)

a huge mass

c)

a small mass

d)

an average mass

9.

During beta-particle emission, a neutron splits into a____________________.

a)

proton and electron

b)

neutron and electron

c)

neutron and proton

10.
Has the symbol
a)
Alpha
b)
Beta 
c)
Gamma
11.
Has the highest penetrating power.  Can penetrate our body.  Even several cm thick of lead or several meters thick of concrete cannot stop all of it.
a)
Alpha
b)
Beta
c)
Gamma
12.

Has the lowest penetrating power.  Can only penetrate 0.05 mm into the body and can be stopped by the skin.

a)
Alpha
b)
Beta
c)
Gamma
d)

Electron capture

13.
Uranium-238  decays into  Thorium-234  by emitting .........
a)
an alpha particle
b)
a beta particle
c)
gamma rays
d)
visible light
14.
Radioactive materials have unstable...
a)
electrons
b)
protons
c)
nuclei
d)
neutrons
15.
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
16.
What is Half-life?
a)
The amount of time it takes for some of the nuclei in a sample of the isotope to decay
b)
The amount of time it takes for half the electrons in a sample of the isotope to decay
c)
The amount of time it takes for half the nuclei in a sample of the isotope to decay
d)
the amount of time it takes to double the nuclei in a sample of the isotope to decay
17.

elements in Group 1A of the periodic table; the ions of the elements in this group have a 1+ charge

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

isotopes

18.

elements in Group 2A of the periodic table; the ions of the elements in this group have 2+ charge

a)

alkaline earth metals

b)

alkali metals

c)

isotopes

d)

halogens

19.

the electrode at which oxidation occurs; it is the positively charged electrode within a cathode ray tube

a)

anode

b)

isotopes

c)

diatomic elements

d)

cathode

20.

the smallest particle of an element that retains the chemical identity of the element; made up of positively charged protons, negatively charged electrons, and neutrons

a)

atom

b)

cathode

c)

isotopes

d)

electron

21.

the weighted average of the masses of the existing isotopes of an element; the sum of the masses of an element’s isotopes each multiplied by its natural abundance

a)

average atomic mass

b)

atomic number

c)

excited state

d)

ground state

22.

the number of protons in the nucleus of an atom

a)

atomic number

b)

average atomic mass

c)

mass number

d)

period

23.

the electrode at which reduction occurs; it is the negatively charged electrode within a cathode ray tube

a)

cathode

b)

anode

c)

mass number

d)

electron

24.

a stream of electrons produced at the negative electrode (cathode) of a tube containing a gas at low pressure

a)

cathode ray

b)

anode

c)

diatomic elements

d)

cathode

25.

elements that exist as diatomic molecules in nature; they include oxygen, hydrogen, nitrogen, fluorine, chlorine, iodine, and bromine

a)

diatomic elements

b)

electron

c)

excited state

d)

ground state

26.

a negatively charged particle within an atom; it has a mass of 0.000549 amu

a)

electron

b)

neutron

c)

proton

d)

diatomic elements

27.

an electron that has absorbed energy and, therefore, exists at a higher energy level

a)

excited state

b)

neutron

c)

diatomic elements

d)

metalloids

28.

the normal state of an electron or atom; at this state the electron or atom has the lowest possible energy

a)

ground state

b)

excited state

c)

metalloids

d)

anode

29.

a vertical column on the periodic table with similar electron configurations, chemical properties, and the same number of valence electrons

a)

group

b)

period

c)

proton

d)

neutron

30.

elements in Group 7A (17); they are the most reactive nonmetals

a)

halogens

b)

alkali metals

c)

alkaline earth metals

d)

isotopes

31.

an atom that has the same number of protons as another, identical atom, but with differing numbers of neutrons

a)

isotopes

b)

proton

c)

neutron

d)

halogens

32.

the sum of the number of protons and neutrons in the nucleus of an atom

a)

mass number

b)

atomic number

c)

average atomic mass

d)

proton

33.

an element that typically has a high melting point, is ductile, malleable, and shiny, and a good conductor of heat and electricity

a)

metal

b)

metalloids

c)

halogen

d)

atom

34.

elements found on the stair-step line of the periodic table with properties of metals and nonmetals

a)

metalloids

b)

halogens

c)

neutron

d)

metal

35.

a neutral particle within the nucleus of an atom; it has a mass of 1.00867 amu

a)

neutron

b)

proton

c)

electron

d)

atom

36.

elements in Group 8A (18); they do not readily react with other elements due to a satisfied octet; they are inert

a)

noble gases

b)

halogens

c)

metal

d)

metalloids

37.

elements that typically have a low melting point,a dull surface, breaks easily, and is a poor conductor of heat and electricity

a)

nonmetal

b)

noble gases

c)

halogens

d)

metalloids

38.

a horizontal row on the periodic table; the elements within the same period have the same number of energy levels

a)

period

b)

group

c)

metal

d)

halogens

39.

natural law that states that the chemical and physical properties of elements are periodic functions of their atomic numbers

a)

periodic law

b)

anode

c)

noble gases

d)

proton

40.

an arrangement of the elements by their atomic numbers so that elements are periodic functions of their atomic numbers

a)

periodic table

b)

periodic law

c)

metalloids

d)

metal

41.

a positively charged particle within the nucleus of an atom; it has a mass of 1.00720 amu

a)

proton

b)

neutron

c)

electron

d)

isotopes

42.

the percentage of an isotope that occurs in nature

a)

relative abundance

b)

periodic law

c)

average atomic mass

d)

excited state

43.

the attractive force among the particles in the nucleus of an atom; in a stable atom, it overcomes the forces of repulsion among protons

a)

strong nuclear force

b)

relative abundance

c)

transition elements

d)

valence electrons

44.

elements found in the middle column of the periodic table; they have multiple oxidation states

a)

transition elements

b)

valence electrons

c)

relative abundance

d)

strong nuclear force

45.

electrons in the outermost energy level of an atom

a)

valence electrons

b)

proton

c)

neutron

d)

electrons

46.

Who is your favorite chemistry teacher?

a)

Ms. Jones

b)

Ms. Jones

47.
a)
Periods
b)
Groups
48.
a)
Periods
b)
Groups
49.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
50.
The blue atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
51.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
52.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
53.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
54.

What charge do protons have?

a)

Positive

b)

Negative

c)

Neutral

55.

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

56.

The number of electrons in an atom is equal to the...

a)

Atomic number

b)

Protons

c)

Atomic Mass

d)

Neutrons

57.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

58.

Elements in the same group have : (2 correct answers)

a)

Similar chemical properties

b)

Similar names

c)

Same number of outer (valence) electrons)

d)

The same number of protons

59.

Which of the three particles has the smallest mass?

a)

proton

b)

neutron

c)

electron

60.

The plum pudding model is discovered by

a)

J.J. Thompson

b)

Ernest Rutherford

c)

James Chadwick

d)

Albert Eisntein

61.

Who discovered the electron?

a)

Thompson

b)

Rutherford

c)

Chadwick

d)

Newton

62.

Who proved that the neutron existed?

a)

Thompson

b)

Rutherford

c)

Chadwick

d)

Newton

63.

Who did gold foil experiment for the first time?

a)

Thompson

b)

Rutherford

c)

Chadwick

d)

Newton

64.

Which one is the result of Rutherford's gold foil experiment?

a)

atom is mostly empty space, with their particles packed into a dense nucleus at the centre

b)

the electrons are scattered

throughout the atom

c)

the electrons and the protons are grouped closely together in the center

d)

the protons and neutrons are scattered

throughout the atom

65.

What are the 3 subatomic particles of an atom?

a)

shell, proton, electron

b)

cloud, neutrons, protons

c)

nucleus, protons, electrons

d)

protons, neutrons, electrons

66.

A region around the nucleus of an atom where electrons are likely to be found.

a)

Electron Cloud or shell

b)

Nucleus

c)

Protons

d)

Electrons

67.

JJ Thomson was credited for the discovery of the:

a)

Center of the universe

b)

Proton

c)

Electron

d)

Neutron

68.

The first universally accepted theory on atoms was proposed in 1803 by:

a)

Winston Churchill

b)

John Dalton

c)

James Bond

d)

J J Thomson

69.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
70.
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 

c)

He discovered that atoms had nuclei 

d)

He discovered that atoms could be divided into smaller parts

71.

Niels Bohr suggested that electrons:

a)

Are found in specific orbits

b)

Are scattered throughout the atom

c)

Move according to their energy level

d)

Are positive

72.

Rutherford discovered this part of the atom:

a)

Nucleus

b)

Neutron

c)

Proton

d)

Electron

73.

Which conclusion could be made from Ernest Rutherford’s gold foil experiment?

a)

Atoms are made up of mostly empty space.

b)

Atoms are mainly solid and block alpha particles.

c)

The volume of the nucleus is large compared to the rest of the atom.

d)

The mass of the nucleus is small compared to the rest of the atom.

74.

What did Ernest Rutherford’s gold foil experiment demonstrate about atoms?

a)

Their positive charge is located in a small region that is called the nucleus.

b)

Their negative charge is located in small particles that are called electrons.

c)

Their nucleus makes up the majority of the volume of the atom.

d)

Their electrons are floating in a sea of positive charges.

75.

What is the correct order of scientists in order of their work related to the atomic theory from earliest to most recent?

a)

Ernest Rutherford, JJ Thomson, John Dalton, & Democritus

b)

JJ Thomson, John Dalton, Ernest Rutherford, & Democritus

c)

Democritus, John Dalton, JJ Thomson, Ernest Rutherford.

d)

John Dalton, JJ Thomson, Democritus, & Ernest Rutherford

76.

Which one of these is Dalton's Model?

a)
b)
c)
d)
77.

Why did Ernest Rutherford and his colleagues perform the Gold-Foil Experiment?

a)

They wanted to test and confirm the Plum-Pudding model

b)

They wanted to test John Dalton's Model

c)

They were looking for electrons

d)

They wanted to come up with their own Atomic Model

78.

Which of the following was an observation made by Rutherford to support that atoms have a dense positive nucleus?

a)

He observed that all alpha particles did go through a gold-foil in straight lines

b)

He observed that most alpha particles did not go through a gold-foil and stopped on one side of the gold foil.

c)

He observed that a small number of alpha particles bounced off the gold-foil at very large angles

d)

He observed that all alpha particles slightly deflected from the straight line when going through a gold-foil

79.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
80.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
81.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

82.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
83.

This is the distance between two peaks. What is this called?

a)

amplitude

b)

wavelength

c)

longitude

d)

trough

84.

The lower the frequency the ______ the energy.

a)

higher

b)

lower

c)

neither, stays the same

85.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
86.
Which wave has a greater frequency?
a)
A
b)
B
87.
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
88.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
89.
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)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
90.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
91.
Oxygen has 8 protons. What is oxygen's atomic number?
a)
16
b)
8
c)
15.999
d)
0
92.
A neutral atom of Carbon-13 has ________ electrons and _________ neutrons
a)
13, 13
b)
6, 7
c)
7, 7
d)
6, 6
93.
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
94.
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
95.
Do the following atoms belong to the same element? Explain
       Aluminum-27
       An atom with 14 protons and 13 neutrons
a)
Yes because they have the same number of protons
b)
Yes because they have the same mass
c)
No because they have different number of protons
d)
No because they have different number of neutrons
96.
What is the atomic number of Neon, Ne?
a)
10
b)
20.1798
c)
10.1798
d)
7
97.
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
98.
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
99.
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
100.
Fluorine has an atomic number of 9. What can you conclude about an atom of fluorine from this fact?
a)
it has 9 protons
b)
it weighs 9 grams
c)
it has 9 electron shells
d)
it has a boiling point of 9 degree celsius
101.
In what part of an atom can protons be found?
a)
inside the electron
b)
inside the neutron
c)
inside the atomic nucleus
d)
inside the electron shells
102.
If a sulfur atom has 16 protons, 16 electrons, and 16 neutrons, its atomic mass is:
a)
16
b)
32
c)
48
d)
64
103.
If a hydrogen atom has 1 proton, 1 electron, and 1 neutron, its atomic number is:
a)
1
b)
2
c)
3
d)
4
104.
On the periodic table, how is atomic mass represented?
a)
As an average of the mass of different isotopes
b)
as the exact mass of every atom
c)
as the mass of the most common isotopes
d)
As the masses of all protons added together
105.
What do carbon-12 and carbon-14 have in common?
a)
they have same number of protons
b)
they have the same number of neutrons
c)
they have the same atomic mass
d)
they have the same atomic weight
106.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom

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