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Worksheets

Review Quiz

Total questions: 166

Worksheet time: 2hrs 9mins

Name
Class
Date
1.

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

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

2.

How do you calculate mass number?

a)

Mass x percent

b)

Protons + Electrons

c)

Protons + Neutrons

d)

Neutrons + Protons + Electrons

3.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
4.
What is the atomic number for an element with three protons?
a)
2
b)
1
c)
3
d)
6
5.
For a given element, the atomic number indicates the number of _____
a)
protons in the nucleus
b)
neutron in the nucleus
c)
electrons in the atom
d)
nucleons in the atom
6.
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
7.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
8.
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
9.
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
10.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
11.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

12.

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

a)

ions

b)

isotopes

c)

quarks

d)

molecules

13.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

14.

If an atom has 10 electrons, how many protons does it have?

a)

0

b)

1

c)

10

d)

5

15.

When the valence shell of an atom is full, the atoms is chemically _____________.

a)

Full

b)

Radioactive

c)

Stable

d)

Unstable

16.

An atom with an electrical charge is called an _____________.

a)

Atom

b)

Isotope

c)

Covalent

d)

Ion

17.

The electrons found in the outermost shell are called _____________ electrons.

a)

Energy

b)

Valence

c)

Negative

d)

Covalent

18.

A positively charged atom (more protons than electrons) is called a __________.

a)

Anion

b)

Cation

c)

Isotope

19.

A negatively charged atom (more electrons than protons) is called a __________.

a)

Anion

b)

Cation

c)

Isotope

20.

Atoms with the same number of protons but different numbers of neutrons (Carbon 14 and Carbon 12) are called ___________.

a)

Anion

b)

Cation

c)

Isotope

21.

A chemical _____________ is a new substance that forms when atoms of two or more elements are bonded together.

a)

Compound

b)

Isotope

c)

Ion

d)

Formula

22.

Atoms become ___________ when their outer energy shell (valence shell) is full.

a)

Stable

b)

Unstable

23.

____________ bonds form when they share electrons.

a)

Ionic

b)

Covalent

c)

Isotope

24.

______________ bonds form between two oppositely charged ions (cation-anion)

a)

Ionic

b)

Covalent

c)

Isotope

25.

The smallest unit of an element

a)

atom

b)

element

c)

cells

d)

ion

26.

A particle inside the nucleus of an atom that has a positive charge.

a)

electron

b)

positron

c)

proton

d)

neutron

27.

Is the amount of protons in the nucleus of an atom.

a)

Atomic Structure

b)

Atomic Mass

c)

Atomic Number

d)

Atomic Weight

28.

A part of an atom that has a negative charge, found outside of the nucleus of the atom.

a)

Neutron

b)

Proton

c)

Electron

d)

Negatron

29.

A neutral particle in the nucleus of an atom, has not positive or negative charge.

a)

Proton

b)

Atom

c)

Electron

d)

Neutron

30.

An atom that has an electric charge

a)

Neutron

b)

Isotope

c)

Ion

d)

Atom

31.

Which element is this?

a)

Nickel

b)

Neon

c)

Sodium

d)

Nitrogen

32.

What is this element?

a)

Beryllium (atomic #4)

b)

Boron (atomic #5)

c)

Carbon (atomic #6)

d)

Nitrogen (atomic #7)

33.

How many valence electrons?

a)

2

b)

3

c)

4

d)

5

34.

What is a valence electron?

a)

Electrons in the first energy shell

b)

Electrons in the second energy shell

c)

Electrons in the outer shell

d)

Total number of electrons

35.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

36.
How are electrons arranged in an atom?
a)
In groups of five
b)
In energy levels
c)
By color
d)
By shape
37.

How many electrons can fit on the 1st energy level (orbital) for any Bohr Model?

a)

2

b)

6

c)

8

d)

10

38.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
Electrons and megatrons
39.

What is a Bohr Model?

a)

a simplified representation 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

40.

Which element does this Bohr model represent?

a)

Aluminum

b)

Silicon

c)

Magnesium

d)

Cobalt

41.

How many energy levels does neon (Ne) have?

a)

1

b)

18

c)

2

d)

10

42.

Do boron (B) and aluminum (Al) have the same number of energy levels?

a)

Yes

b)

No

43.

Sodium (Na) and Sulfur (S) have the same number of energy levels?

a)

Yes

b)

No

44.

An atom has a full first energy level and 7 electrons in its second level. How many electrons does this atom have?

a)

2

b)

7

c)

9

d)

Need more information

45.

The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is what?

a)
3
b)
6
c)
8
d)
10
46.
What is this element?
1s22s22p63s2
a)
Neon
b)

Aluminum

c)

Magnesium

d)
Potassium
47.
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
d)

Bohr's Law

48.
Atoms are made up of three basic parts, which are -
a)
Protons, neutrons, electrons
b)
neutrinos, protons, neutrons
c)
quarks, protons, electrons
d)
electrons, neutrons, and quarks
49.
There are 4 different types of sublevels: s,p,d,f
a)
true
b)
false
50.

Which shape represents the shape of an "s" orbital?

a)
b)
c)
d)
51.

How many orbitals does an 's' sublevel have?

a)

1

b)

3

c)

5

d)

7

52.

What is the shape of 'p' orbitals?

a)

Dumbbell shaped

b)

Peanut shaped

c)

Spherical shaped

d)

Hybrid structure

53.

The number of orbitals in 'p' sub level

a)

2

b)

3

c)

4

54.

How many electrons can a d sublevel hold?

a)

14

b)

10

c)

2

d)

6

55.

A three-dimensional region around a nucleus where an electron may be found is called ---?

a)

orbit

b)

circle

c)

orbital

d)

circuit

56.

The s sublevel resembles this type of shape

a)

dumbell

b)

clover

c)

sphere

d)

double clover

57.

The rule that says electrons enter sublevels with the lowest energy first

a)

Pauli Principal

b)

Hund's Rule

c)

Aufbau Principal

d)

Law of Conservation of Energy

58.

The rule that says each orbital much receive one electron before an orbital in that sublevel can have two

a)

Hunds Rule

b)

Aufbau Principal

c)

Pauli Principal

d)

Law of Conservation of Energy

59.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
60.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
61.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
62.
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
63.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
64.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
65.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
66.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
67.
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
68.

What element has this electron configuration?

a)

hydrogen

b)

helium

c)

lithium

d)

beryllium

69.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

70.

What element has this electron configuration?

a)

helium

b)

lithium

c)

beryllium

d)

boron

71.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

72.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

73.

Which element is represented by this electron configuration?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

74.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

75.

Which of the following is the electron configuration for silicon?

a)
b)
c)
d)
76.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
77.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
78.

Which is the electron configuration for beryllium?

a)
b)
c)
d)
79.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
80.
Maximum number of electrons that can be placed in an s orbital.  
a)
2
b)
6
c)
10
d)
14
81.
In an orbital diagram,  an arrow represents: 
a)
an electron
b)
an orbital
c)
an element
82.

How many dots would you put around carbon, a group 14 element?

a)

4

b)

6

c)

8

d)

18

83.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

84.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

85.

How many electrons should sodium, atomic number 11, have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

86.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
87.

Which of these is correct?

a)
b)
c)
88.

What bond type shares electrons?

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

89.
What type of bond is this?
a)
ionic
b)
covalent
90.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
91.
Compounds made from only nonmetals are _________________ compounds.
a)
ionic
b)
covalent
c)
metallic
d)
chemical
92.

Where are metals located on the periodic table?

a)

right side of the staircase

b)

on the staircase

c)

left side of the staircase

93.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

94.

Which of these is correct?

a)
b)
95.

What is the the outermost shell with electrons?

a)

Shells

b)

Isotope

c)

Orbit

d)

Valence

96.

How many electrons can go in the first energy level?

a)

2

b)

8

c)

18

d)

32

97.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

98.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
99.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
100.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
101.

Electron configuration of helium (He)

a)

1s11s^1  

b)

1s21s^2  

c)

2s12s^1  

d)

2s2 2p12s^2\ 2p^1  

102.

Electron configuration of boron (B)

a)

1s2 2s1 2p11s^{2^{\ }}2s^1\ 2p^1  

b)

1s2 2s2 2p11s^2\ 2s^{2\ }2p^1  

c)

1s2 2s11s^2\ 2s^1  

d)

1s1 2s1 2p11s^1\ 2s^1\ 2p^1  

103.

Electron configuration of fluorine (F)

a)

1s1 2s2 2p51s^{1^{\ }}2s^2\ 2p^5  

b)

1s2 2s2 2p71s^2\ 2s^{2\ }2p^7  

c)

1s2 2s2 2p51s^2\ 2s^2\ 2p^{5^{ }}  

d)

1s1 2s1 2p51s^1\ 2s^1\ 2p^5  

104.
Which of the following atomic symbols is written correctly?
a)
ee
b)
hE
c)
C
d)
CL
105.
Carbon is considered an element while carbon dioxide is considered a compound. This is because carbon dioxide is –
a)
a gas at room temperature.
b)
made of two different elements.
c)
given off by green plants.
106.
What is the term for combining 2 or more atoms together?
a)
atoms
b)
elements
c)
molecules
d)
compounds
107.
What is the term for combining 2 or more DIFFERENT atoms together?
a)
atoms
b)
elements
c)
molecules
d)
compounds
108.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

109.

Which of the following elements LOSES 1 electron in order to attain an octet?

a)

potassium

b)

calcium

c)

helium

d)

boron

e)

fluorine

110.

Which of the following elements GAINS 1 electron in order to attain an octet?

a)

Na

b)

Ca

c)

He

d)

Cl

111.

How many valence electrons does Be have?

a)

1

b)

2

c)

4

d)

6

112.

Does Be fulfill the Octet Rule?

a)

Yes

b)

No

113.

How many electrons will Be gain/lose to satisfy the Octet Rule?

a)

Lose 2

b)

Lose 4

c)

Gain 2

d)

Gain 6

114.

When atoms LOSE electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

115.

What does Neon need to do fulfill the Octet Rule?

a)

Gain 2

b)

Lose 2

c)

Nothing - it already fulfills the Octet Rule.

116.

When atoms GAIN electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

117.

Where is a Valence electron located?

a)

The innermost shell

b)

The nucleus

c)

The outmost shell

118.

A __________ goes up and down on the periodic table.

a)

Group

b)

Period

119.

A _________ goes side to side on the periodic table.

a)

Group

b)

Period

120.

What element is in period 4, group 1?

a)

K - Potassium

b)

V - Vandium

c)

C - Carbon

d)

Ti - Titanium

121.

What two elements are in the same Period?

a)

K - Potassium and Na - Sodium

b)

Li - Lithium and Mg - Magnesium

c)

B - Boron and C - Carbon

d)

Zn - Zinc and N - Nitrogen

122.

What element is in group 2, period 6?

a)

Sr - Strontium

b)

Ba - Barium

c)

S - Sulfur

d)

O - Oxygen

123.

The _______ tells us how many energy shells an element has.

a)

group

b)

period

c)

atomic number

d)

element symbol

124.

The _________ tells us how many valence electrons an element has.

a)

Group

b)

Period

c)

Atomic Number

d)

Element

125.
What Periodic Table family is represented by the Lewis dot diagram?
a)
Halogens
b)
Alkali Metals
c)
Transition Metals
d)
Noble Gases
126.
What group on the Periodic Table contains the elements of the alkaline earth family?
a)
1
b)
2
c)
17
d)
18
127.
Gold (Au)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Earth Metal
d)
Heavy Metal
128.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
129.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
130.

The is family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

131.

Sulfur is a...

a)

metal

b)

nonmetal

c)

metalloid

132.

Noble gases are inert because

a)

They are highly reactive

b)

They are unreactive

c)

They are noble

d)

They have 8 electrons in their outer most energy level

133.
Some elements combine chemically and no longer have the same ________________ they did before forming a compound.
a)
valence electons
b)
energy
c)
properties
d)
group number
134.
A _________________ is composed of symbols and subscripts indicating the number of atoms of an element in a compound.
a)
Chemical Equation
b)
Chemical Reaction
c)
Synthesis Reaction
d)
Chemical Notation
135.
An ionic compound is held together by the _______--the force of attraction between opposite charges of the atoms.
a)
Covalent Bond
b)
Ionic Bond
c)
Synthetic Bond
d)
Molecular Bond
136.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
137.

A bond between two nonmetal atoms is a __________ bond.

a)

ionic

b)

nuclear

c)

metallic

d)

covalent

138.

Ionic bonds form between ---

a)

nonmetals.

b)

metals and nonmetals.

139.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
140.
What is the name for an ion with a positive charge?
a)
cation
b)
anion
c)
onion
d)
union
141.

If an atom gains an electron, what charge will it have?

a)

positive

b)

negative

c)

neutral

142.

Where is most of the mass of an atom found?

a)

nucleus

b)

electron cloud

c)

atomic number

d)

mass number

143.

How many total electrons can the 2nd shell or energy level hold?

a)

1

b)

2

c)

8

d)

18

144.

What happens to the valence electrons of an atom when it is a covalent bond?

a)

transfers electrons

b)

shares electrons

c)

does nothing

145.

Dot diagrams represent ____.

a)

outer shell electrons

b)

protons

c)

neutrons

d)

all electrons

146.

What is the octet rule?

a)

it states atoms need to be happy

b)

it states atoms need 8 valence electrons to be stable

c)

it states atoms need 6 valence electrons to be stable

d)

it states atoms need to share electrons to be stable

147.

What type of chemical bonds are between metals and nonmetals?

a)

ionic bonds

b)

covalent bonds

c)

metallic bonds

148.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
149.

Which occurs during a physical change?

a)

Gas bubbles

b)

Precipitate forms

c)

New substance forms

d)

The shape changes

150.

Which is more easily reversed?

a)

Physical Change

b)

Chemical Change

c)

Neither

151.
A change where one or more new substances are created.
a)
Physical Change 
b)
Chemical Change 
152.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

153.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

154.

Beryllium and sulfur will form a ______ bond

a)

ionic

b)

covalent

c)

metalloid

155.

NaCl

a)

ionic

b)

covalent

c)

metallic

156.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
157.

Atoms are most stable when their outer electron level is complete.

a)

true

b)

false

158.

How are covalent bonds formed?

a)

by atoms sharing some of their electrons

b)

by electron transfer from one atom to another

c)

by atoms exchanging electrons

d)

by atoms hanging out together

159.

Why do elements bond?

a)

to become friends

b)

to create a new element

c)

to become stable

d)

to reduce the number of atoms

160.

Objects that have opposite charges will

a)

repel each other

b)

attract each other

c)

push away from each other

d)

avoid each other

161.

Group numbers on the periodic table help us determine

a)

the size of an atom

b)

the color of an element

c)

the atomic number of an element

d)

the number of valence electrons an atom has

162.

What color indicates the nonmetals?

a)

blue

b)

red

c)

green

d)

the colors do not indicate nonmetals

163.

What color shows where metals are located on the periodic table?

a)

blue

b)

green

c)

red

d)

the colors do not indicate metals

164.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

165.

When sodium loses an electron to chlorine, sodium becomes a .......

a)

positive ion

b)

negative ion

166.

When chlorine gains an electron from sodium, chlorine becomes a ...

a)

positive ion

b)

negative ion

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