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Unit 3 Test Review

Total questions: 107

Worksheet time: 2hrs 46mins

Name
Class
Date
1.

Who proposed the idea that matter could not be divided into smaller and smaller pieces forever?

a)

Democritus

b)

John Dalton

c)

J.J. Thomson

d)

Ernest Rutherford

2.

According to Dalton's Atomic Theory, what are compounds formed by?

a)

Atoms of the same element

b)

Atoms of different elements

c)

Atoms of two or more elements in fixed whole number ratios

d)

Atoms of different elements in different ratios

3.

What did J.J. Thomson's Cathode Ray Tube Experiment suggest about the atom?

a)

Atoms are indivisible and indestructible particles

b)

Atoms are made of even smaller particles called electrons

c)

Atoms have a small, dense, positively charged center called the nucleus

d)

Atoms are mostly open space

4.

What did Robert Millikan determine through his Oil Drop Experiment?

a)

The charge of an electron

b)

The mass of an electron

c)

The charge to mass ratio of an electron

d)

The existence of neutrons

5.

What did James Chadwick confirm the existence of?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Nucleus

6.

Who proposed the planetary model of the atom?

a)

Democritus

b)

John Dalton

c)

Niels Bohr

d)

Ernest Rutherford

7.

What did Democritus name the smallest piece of matter?

a)

Atomos

b)

Electron

c)

Proton

d)

Nucleus

8.

Who discovered the electron?

a)

James Chadwick

b)

J.J. Thomson

c)

Niels Bohr

d)

Ernest Rutherford

9.

What did Rutherford's Gold Foil Experiment reveal about the atom?

a)

Atoms are indivisible and indestructible particles

b)

Atoms are made of even smaller particles called electrons

c)

Atoms have a small, dense, positively charged center called the nucleus

d)

Atoms are mostly open space

10.

What did J.J. Thomson's Cathode Ray Experiment prove about atoms?

a)

Atoms are indivisible and indestructible particles

b)

Atoms are made of even smaller particles called electrons

c)

Atoms have a small, dense, positively charged center called the nucleus

d)

Atoms are mostly open space

11.
Who discovered that the nucleus contains positively charged particles called protons?
a)
Ernest Rutherford
b)
James Chadwick
c)
Democritus
d)
Niels Bohr
12.

This model was the first to show a nucleus, consisting of protons and neutron.  Electrons surround the nucleus but are not shown in distinct energy levels. 

a)

Rutherford's "Nuclear Model" of the atom

b)
The "Plum Pudding Model" of the atom
c)
The "Quantum Mechanical Modell" of the atom
d)
Democritus's model of the atom
13.
This was the first model of the atom ever proposed. It was simple and described atoms as tiny spheres that could not be broken down into smaller pieces.
a)

Democritus's model of the atom

b)
The "Plum Pudding Model" of the atom
c)

The "Rutherford Nuclear Model" of the atom

d)
The "Quantum Mechanical Model" of the atom
14.
This model added on to previous models by showing electrons existed at certain "energy levels". However it does not accurately show what those levels look like.
a)
The "Bohr Model" of the atom
b)

The "Rutherford Nuclear Model" of the atom

c)
The "Plumb Pudding Model" of the atom
d)
The "Quantum Mechanical Model" of the atom
15.
This model was developed after J.J. Thompson discovered electrons, a particle smaller than an atom. Is shows electrons floating freely in a positive space.
a)
The "Plum Pudding Model" of the atom
b)

The "Rutherford Nuclear Model" of the atom

c)
Democritus's model of the atom
d)
The "Quantum Mechanical Model" of the atom
16.
Ernest Rutherford discovered that atoms were mostly _________________. 
a)
negatively charged
b)
positively charged
c)
electrons
d)
empty space. 
17.
What scientist is best known for his gold foil experiment?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
18.

Who named the positive center of the atom the "nucleus?"

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

19.

Which scientists believed an atom was indivisible? (Choose all correct responses.)

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

20.

Which scientist discovered that the atom has parts - which means it can be divided?

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

21.

In the atomic model nicknamed the "plum pudding" model, what do the plums represent?

a)

the nucleus

b)

the atom

c)

the electrons

d)

the positive material

22.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

23.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

24.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
25.

Atoms of the same element with a different number of neutrons

a)

Ion

b)

alloy

c)

Isotope

d)

Quarks

26.
A charged atom
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
27.
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
28.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
29.

Calculation used to find the number of neutrons in an atom

a)

Mass Number- Atomic Number

b)

Atomic Number - Mass Number

c)

Mass Number - Electrons

d)

protons = electrons = neutrons

30.
How many protons does an aluminium atom have? (Use the image to help you)
a)
27
b)
14
c)
40
d)
13
31.
How many neutrons does a sodium atom have? (Use the image to help you)
a)
23
b)
11
c)
12
d)
34
32.
Atoms of the same element must always have the same number of _________
a)
electrons
b)
neutrons
c)
isotopes
d)
protons
33.
The _________ of an element equals the number of protons in an atom of that element
a)
mass number
b)
atomic weight
c)
atomic number
d)
isotopes
34.

The __________ of an atom is the sum of the protons and neutrons in the nucleus of that atom.

a)

mass number

b)

atomic number

c)

ionic charge

d)

isotope weight

35.

Cations have what charge?

a)

+

b)

-

36.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

37.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

38.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

39.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
40.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

41.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

42.

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

43.

How many protons, neutrons, and electrons?

a)

proton = 6, neutron = 4, electron = 1

b)

proton = 4, neutron = 4, electron = 5

c)

proton = 1, neutron = 6, electron = 10

d)

proton = 4, neutron = 2, electron = 3

44.

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

45.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
46.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

47.
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
48.

Changing the number of protons in an atom will change the atom's _____

a)

color

b)

atomic weight/mass

c)

net charge

d)

identity (name of element)

49.
Calculate the atomic number of an atom with :
2 protons
3 neutrons
4 electrons
a)
2
b)
3
c)
4
d)
5
50.

When nuclei decay, massive amounts of __________ is released.

a)

energy

b)

electrons

c)

protons

d)

neutrons

51.

What type of decay is shown here

23892U ---> 23490Th + 42He.

a)

alpha

b)

beta

c)

gamma

52.
After 4 half-lives, 1g of a sample of Krypton-85 remains unchanged.  What was the original mass of the sample?
a)
16g
b)
32g
c)
0.0625g
d)
4g
53.

Identify the type of nuclear decay shown here

21483Bi → 0-1e + 21484Po

a)

alpha

b)

beta

c)

gamma

54.
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.
55.
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
56.
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
57.

Finish this equation

20983Bi--> _______ + 20581Tl

a)

42He

b)

0-1e

c)

y

58.
The most dangerous type of radiation is the ____. 
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
59.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
60.

Identify the missing substance in each of the following nuclear reaction.

_____→13756 Ba + 0−1 e

a)

13755Ba

b)

13757La

c)

13856Ba

d)

13755Cs

61.
In the symbol 20682Pb what does 206 stand for?
a)
Mass number
b)
Atomic number
c)
Atomic mass
d)
Number of protons
62.
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 
63.
Two or more nuclei combine to form one larger nucleus in the process of nuclear _____.
a)
Fusion
b)
Fission
c)
Tracing
d)
Decay
64.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Decay
65.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
decay
d)
gamma radiation
66.
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
67.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
68.
Has a mass of 4 and a charge of +2
a)
Alpha
b)
Beta
c)
Gamma
69.
Has the symbol
a)
Alpha
b)
Beta 
c)
Gamma
70.
What is the term used for describing when an element changes into a new element through radioactive decay?
a)
mutation
b)
transmutation
c)
alchemy
71.

What type of radioactive decay is this example?

a)

Alpha

b)

Negative Beta

c)

Positive Beta

d)

Gamma

72.

What type of radioactive decay is this example?

a)

alpha

b)

negative beta

c)

positive beta

d)

gamma

73.

What type of radioactive decay is this example?

a)

alpha

b)

beta minus

c)

beta plus

d)

gamma

74.
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
75.

In a correctly written symbol what would be located in the "Z" position?

a)

number of neutrons

b)

atomic number

c)

number of electrons

d)

mass number

76.

Which of the following correctly display nuclear fission?

a)
b)
c)
d)
e)
77.

Finish this song title: Don't stop...

a)

the Car

b)

Believing

c)

Me Now

d)

the Music

78.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
79.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)

Zinc (Zn)

b)

Copper (Cu)

c)

Nickel (Ni)

d)

Germanium (Ge)

80.

Write the configuration for Phosphorus (P)

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

d)

1s2 2s2 2p5 3s2 3p3

81.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
82.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
83.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

84.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

85.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

86.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
87.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
88.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

89.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
90.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
91.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

92.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
93.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
94.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
95.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
96.

What is the electron configuration of Ca+2?

a)

1s2 2s2 2p6 3s2 3p6 4s2

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p6 4s4

d)

1s2 2s2 2p6 3s2 3p6 4s2 4p2

97.

The Ca+2 ion is isoelectronic with what -1 ion?

a)

F-1

b)

Cl-1

c)

Br-1

d)

K-1

e)

Ar-1

98.

Which of the following are isoelectronic with O-2 ion?

a)

Flourine

b)

Mg+1

c)

Flouride

d)

Nitride

e)

Neon

99.

1s2 2s2 2p6 is the electron configuration of which ION?

a)

Aluminum

b)

Chloride

c)

Beryllium

d)

Boron

e)

Neon

100.

What is the electron configuration of the Sc+2 ion? (Element #21).

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2 3p6 3d2

c)

1s2 2s2 2p6 3s2 3p6 4s2

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d2

101.

Which levels do electrons get removed from first, when they are lost?

a)

1st level

b)

outer levels

c)

valence shells

d)

s and p levels

e)

d levels

102.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Pauli's Exclusion Principle

c)

Hund's Rule

d)

Heisenberg uncertainty principle

103.

What is incorrect about this orbital diagram?

a)

Both arrows in the filled 2p box should be pointing the same direction

b)

In the there should only be 1 arrow in the first 2p box and one in the 2nd 2p box

c)

There is nothing incorrect with this diagram

d)

All the arrows should be pointing the same direction.

104.

Which rule is violated in the following orbital diagrams?

a)

Hund's Rule

b)

Pauli's Exclusion Principle

c)

Aufbau Principle

105.

What is meant by isolectronic?

a)

Group of atoms or ions have the same electronic configuration

b)

Group of atoms or ions have the same protonic configuration

c)

Group of atoms or ions have the same electrical properties

d)

Group of atoms or ions have the same electron charge

106.

What is the example of species that are isolectronic?

a)

Li+ and H+

b)

S2- and O2-

c)

Li+ and He

d)

F- and Cl-

107.
Write the electronic structure for Cu+1 ion
a)
[Ar]4s13d10
b)
[Ar]4s13d9
c)
[Ar]4s03d10
d)
[Ar]3d10

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