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Periodic table mega quiz

Total questions: 157

Worksheet time: 52mins

Name
Class
Date
1.
This particle is found in the nucleus and has no charge
a)
Neutron
b)
Proton
c)
Electron
2.
This particle is found in the nucleus and has a positive charge
a)
Electron
b)
Proton
c)
Neutron
3.
This is a negatively charged particle found outside the nucleus
a)
Electron
b)
Proton
c)
Neutron
4.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
5.
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
6.
Place the following scientists in order, from earliest to latest: 
A) Ernest Rutherford
B) J.J. Thomson
C) John Dalton
a)
B,C,A
b)
C,A,B
c)
A,C,B
d)
C,B,A
7.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
8.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
9.
Which scientist proposed a model of the atom in which the electrons are orbiting at different levels?
a)
Niels Bohr
b)
James Chadwick
c)
John Dalton
d)
Ernest Rutherford
10.
Which scientist saw the atom as a positively charged sphere with negative particles (electrons) embedded within?
a)
J.J. Thomson
b)
Niels Bohr
c)
John Dalton
d)
Ernest Rutherford
11.
Bohr's model of the atom proposed that ___.
a)
electrons move around the nucleus in fixed orbits
b)
neutrons move around the nucleus
c)
neutrons do not exist, but are just paired protons and electrons
d)
the nucleus spins
12.
J.J. Thomson's model of the atom is given this name because he believed that electrons were spread randomly throughout a positive sphere.
a)
plum pudding model
b)
orbital model
c)
Thomson's model
d)
plasma model
13.
Which scientist is responsible for first discovering that all the atoms of a particular element are identical but are different from the atoms of all other elements?
a)
Dalton
b)
Thomson
c)
Bohr
d)
Rutherford
14.
Which scientist is responsible for first discovering that all the atoms of a particular element are identical but are different from the atoms of all other elements?
a)
Dalton
b)
Thomson
c)
Bohr
d)
Rutherford
15.

Order the atomic models below from the oldest to the most recent.

a)

2, 1, 3, and 4

b)

1, 2, 4, and 3

c)

3, 2, 4, and 1

d)

3, 1, 2, and 4

16.
Which scientist proposed a model of the atom in which the individual atoms were thought of as tiny solids like balls or marbles?
a)
John Dalton
b)
James Chadwick
c)
Ernest Rutherford
d)
J.J. Thomson
17.
Bohr proposed a model of the atom as a large positive sphere with negatively charged electrons revolving around the center in orbits. What was this model nicknamed?
a)
The Planetary Model
b)
The Billiard Ball Model
c)
The Nuclear Model
d)
The Plum Pudding Model
18.
One of the Dalton's conclusions concerning his atomic theory was that all the atoms of the same element are ___.
a)
the same
b)
different
c)
combined
d)
reacted
19.
Which statement is true according to current thinking?
a)
An atom is mostly empty space.
b)
An atom is a collection of particles, so tightly packed that there is little empty space.
c)
The atomic nucleus is very mobile, and moves around inside a cloud of electrons.
d)
The size of atoms changes over time, pulsating from large to small to large again.
20.
Whose model of an atom is displayed in the picture?
a)
Thomson
b)
Rutherford
c)
Dalton
d)
Bohr
21.

Protons are:

a)

Negative

b)

Positive

c)

No charge

d)

Atomic Number

22.

Neutrons have

a)

Negative

b)

Positive

c)

No charge

d)

Atomic Number

23.

Electrons are

a)

Negative

b)

Positive

c)

No charge

d)

Atomic Number

24.

In the nucleus you can find the

a)

Protons, neutrons, and electrons

b)

Protons and neutrons

c)

Protons and electrons

d)

Neutrons

25.

All of the mass is located in the:

a)

Electron cloud

b)

Radiation

c)

Church

d)

Nucleus

26.

The smallest subatomic particle

a)

Protons

b)

Neutrons

c)

Electrons

d)

Atoms

27.

An element has an atomic number of 9 and a mass of 19 amu. What is the number of protons this element has?

a)

9

b)

19

c)

10

d)

28

28.

An element has an atomic number of 9 and a mass of 19 amu. What is the number of electrons this element has?

a)

9

b)

19

c)

10

d)

28

29.

An element has an atomic number of 9 and a mass of 19 amu. What is the number of neutrons this element has?

a)

9

b)

19

c)

10

d)

28

30.

What is represented by the letter T?

a)

Nucleus

b)

Electron

c)

Proton

d)

Neutrons

31.

What is represented by the letter S?

a)

Nucleus

b)

Electron

c)

Proton

d)

Neutrons

32.

What is represented by the letter Q?

a)

Nucleus

b)

Electron

c)

Proton

d)

Neutrons

33.

What is represented by the letter R?

a)

Nucleus

b)

Electron

c)

Proton

d)

Neutrons

34.

The atomic number is the same as the number of

a)

Protons

b)

Neutrons

c)

Mass

d)

Atom

35.

What gives you the identity of an element?

a)

Mass

b)

Atomic number

c)

Protons

d)

Electrons

36.

An element has 3 electrons and a mass of 7. How many protons does this element have?

a)

3

b)

7

c)

4

d)

10

37.

How many protons does Boron, B have?

a)

5

b)

11

c)

6

38.

How many neutrons does hydrogen have?

a)

1

b)

0

39.

How many protons does an element with an atomic number of 32 and a mass of 73 have?

a)

32

b)

73

c)

41

40.

How many electrons does Lithium have if it has an atomic number of 3 and a mass of 7?

a)

3

b)

7

c)

4

41.

What is the mass number of a Potassium (K) atom that has 20 neutrons?

a)

18

b)

19

c)

20

d)

39

42.

An atom of Chlorine, Cl, has an atomic number of 17 and a mass of 35. How many subatomic particles are INSIDE the nucleus?

a)

17

b)

35

c)

18

43.

An atom of Chlorine, Cl, has an atomic number of 17 and a mass of 35. How many subatomic particles are OUTSIDE the nucleus?

a)

17

b)

35

c)

18

44.

What is the number of neutrons in an oxygen atom with a mass number of 16?

a)

8

b)

16

c)

24

d)

7

45.

Which subatomic particle is located in the electron cloud of an atom?

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

46.

If an element has an atomic number of 12, what is its number of protons?

a)

6

b)

12

c)

18

d)

24

47.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
48.
Which element has an electron configuration of 2.5?
a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
49.
Which element has an electron configuration of 2.8.8?
a)
Lead
b)
Flourine
c)
Neon
d)
Argon
50.
What is the electron configuration of Aluminium?
a)
2.8.3
b)
2.11
c)
13
d)
2.8.2
51.
What is the electron configuration of chlorine?
a)
17
b)
2.7
c)
2.8.7
d)
2.8.4
52.
Which element has the electron configuration of 2.8.2?
a)
Magnesium
b)
Sodium
c)
Sulfur
d)
Arsenic
53.
Which element has the electron configuration of 2.8.4?
a)
Neon
b)
Boron
c)
Gallium
d)
Silicon
54.
What is the electron configuration of beryllium?
a)
2.2
b)
2.4
c)
4
d)
6
55.
Which element has the electron configuration of 2.7?
a)
Krypton
b)
Iodine
c)
Flourine
d)
Barium
56.

In ascending order, the maximum number of electrons each shell can hold is

a)

2, 8, 8, 32

b)

2, 8, 18, 32

c)

2, 6, 8, 32

d)

2, 3, 4, 5

57.

Boron (B) has 5 electrons. Its electron configuration is

a)

5

b)

2, 2, 1

c)

1, 2, 2

d)

2, 3

58.

The electron configuration of Nitrogen is

a)

0, 2, 5

b)

N, 2, 5

c)

7

d)

2, 5

59.

The electron configuration of sulfur is

a)

2, 8, 6

b)

2, 8, 8

c)

3, 8, 6

d)

0, 2, 8

60.

How many protons does Magnesium have?

a)

24

b)

12

c)

2

d)

16

61.

An element has an electron configuration of 2,8. Which element is this?

(a)  

62.

The electron configuration of oxygen is 2, 6. What is its atomic number?

a)

2

b)

6

c)

8

d)

4

63.

Aluminium has 13 electrons. How many electron shells would make up the atom?

a)

1

b)

2

c)

3

d)

4

64.

What is the electron configuration of carbon?

a)

2, 2, 2

b)

2, 4

c)

2, 6

d)

1, 5

65.

How many protons does Chlorine have?

a)

16

b)

19

c)

18

d)

17

66.

Which element has the electron configuration 2, 8, 1?

a)

Aluminium

b)

Sodium

c)

Neon

d)

Magnesium

67.

What is the electron configuration of Neon?

a)

2, 8

b)

2, 7

c)

2, 8, 1

d)

2, 6

68.

Which element has the electron configuration 2, 8, 7?

a)

Sulfur

b)

Fluorine

c)

Argon

d)

Chlorine

69.

What is the electron configuration of phosphorus?

a)

2, 8, 5

b)

2, 8, 7

c)

2, 8, 6

d)

2, 7, 6

70.

Which element has the electron configuration 2, 8, 2?

a)

Silicon

b)

Aluminium

c)

Magnesium

d)

Calcium

71.

What is the electron configuration of argon?

a)

2, 8, 5

b)

2, 8, 6

c)

2, 8, 7

d)

2, 8, 8

72.

According to the periodic table what element is in group 9 period 4?

a)

Hydrogen

b)

Magnesium

c)

Cobalt

d)

Sulfur

73.

According to the periodic table what element is in group 7 period 4?

a)

Hydrogen

b)

Manganese

c)

Plutonium

d)

Nitrogen

74.

According to the periodic table what element is in group 1 period 1?

a)

Hydrogen

b)

Manganese

c)

Oxygen

d)

Nitrogen

75.

How many valence electrons does Aluminum have?

a)

1

b)

3

c)

5

d)

7

76.

How many valence electrons does Lithium have?

a)

1

b)

3

c)

5

d)

7

77.

How many valence electrons does Helium have?

a)

2

b)

4

c)

6

d)

8

78.

How many valence electrons do group 14 elements have?

a)

2

b)

4

c)

6

d)

8

79.

How many valence electrons do group 16 elements have?

a)

2

b)

4

c)

6

d)

8

80.

How many valence electrons do group 1 elements have?

a)

1

b)

2

c)

3

d)

8

81.

Where is a Valence electron located?

a)

The innermost shell

b)

The nucleus

c)

The outmost shell

82.

A __________ goes up and down on the periodic table.

a)

Group

b)

Period

83.

A _________ goes side to side on the periodic table.

a)

Group

b)

Period

84.

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

85.

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

a)

group

b)

period

c)

atomic number

d)

element symbol

86.

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

a)

Group

b)

Period

c)

Atomic Number

d)

Element

87.

There are_______ periods and _________ groups in the periodic table.

a)

8, 7

b)

18, 7

c)

15, 10

d)

7, 18

88.

How many valence electrons does this atom have?

a)

4

b)

2

c)

6

89.

Elements more reactive the further __________ on the periodic table.

a)

Right

b)

Left

90.

How many energy shells does Fe - Iron have?

a)

26

b)

2

c)

4

d)

55

91.

What period does the element I - Iodine belong to?

a)

17

b)

6

c)

3

d)

5

92.

On the periodic table, Periods are

a)

Horizontal rows

b)

Vertical columns

93.

On the periodic table, Groups (also known as Families) are

a)

Horizontal rows

b)

Vertical columns

94.

What is a valence electron?

a)

Electrons in the first energy level

b)

Electrons in the second energy level

c)

Electrons in the outer level

d)

Total number of electrons

95.

The period number tells you the number of _______ that an atom has

a)

valence electrons

b)

energy levels

c)

total number of electrons

d)

physical properties

96.

The group (or family) number tells you the number of _______ that an atom has

a)

valence electrons

b)

energy levels

c)

total number of electrons

d)

physical properties

97.

Most of the elements on the Periodic Table are

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

98.

Choose the elements that are metals

a)

Potassium

b)

Aluminum

c)

Bromine

d)

Oxygen

e)

Gold

99.

Which element is a metalloid?

a)

Calcium

b)

Mercury

c)

Boron

d)

Argon

100.

Which elements are nonmetals?

a)

Hydrogen

b)

Xenon

c)

Copper

d)

Silicon

e)

Oxygen

101.

Calcium has how many valence electrons?

a)

1

b)

2

c)

4

d)

20

102.

Chlorine has how many valence electrons?

a)

1

b)

3

c)

7

d)

17

103.

Helium has how many valence electrons?

a)

1

b)

2

c)

3

d)

4

104.

Magnesium has how many energy levels?

a)

1

b)

2

c)

3

d)

12

105.

Carbon has how many energy levels?

a)

1

b)

2

c)

4

d)

6

106.

Which element has 2 energy levels and 3 valence electrons?

a)

Boron

b)

Magnesium

c)

Aluminum

d)

Calcium

107.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
108.
There are more metals than non metals in the periodic table.
a)
True
b)
False
109.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
110.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
111.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
112.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
113.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
114.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
115.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
116.

Which of the following is an alloy?

a)

stainless steel

b)

chromium

c)

nickel

d)

lead

117.

Metallic bonding is...

a)

a type of covalent bond.

b)

a type of ionic bond.

c)

an attraction between positive ions and a sea of delocalised electrons.

118.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
119.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

120.
Why are alloys generally used to make everyday objects?
a)
Alloys are often stronger and less active than pure metals.
b)
Alloys have higher melting point than pure metals.
c)
Alloys are less expensive to produce than pure metals.
d)
Alloys have ionic bonds instead of metallic bonds.
121.

Which property allows metals to be drawn into wires?

a)

Malleability

b)

Ductility

c)

Conductivity

d)

Solubility

122.

What is the primary reason metals are good conductors of electricity?

a)

They are dense

b)

They are shiny

c)

They have a high melting point

d)

They have delocalized electrons

123.

Which of the following is a characteristic of metals?

a)

Brittle

b)

Non-malleable

c)

High melting point

d)

Poor conductor of heat

124.

The diagram shows metallic bonding.


Which labels are correct?

a)

X: atomic nucleus

Y: outer electron

b)

X: metal atom

Y: mobile electron

c)

X: metal cation

Y: mobile electron

d)

X: positive ion

Y: negative ion

125.

The Electron Sea Model explains why metals are ....

a)

excellent conductors

b)

are very reactive

c)

accept electrons easily

d)

form ionic compounds

126.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
127.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
128.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
129.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
130.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
131.
Is carbon considered a metal or a non-metal?
a)
metal
b)
nonmetal
c)
other
132.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
133.
What would you name this molecule?
a)
SNa3
b)
H3O
c)
NaCl
d)
H2O
134.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
135.
Which of the following describes covalent bonds?
a)
Bonds form because of opposite charges
b)
Bonds form to fill outer electron shells
c)
Electrons are transferred between atoms
d)
Covalent bonds are magical
136.
Most atoms have no net charge because they have....
a)
an equal number of charged and non-charged particles
b)
neutrons in their nuclei
c)
an equal number of electrons and protons
d)
an equal number of neutrons and protons
137.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
None
d)
conduct electricity
138.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
139.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
140.
How many covalent bonds does carbon need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
141.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
142.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
143.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
144.
Ions that are made of more than one atom are called...
a)
ionic compounds
b)
crystals
c)

polyatomic ions

d)
ionic bonds
145.
Which is most likely to form a negative ion...
a)

an element from Group 7

b)
a metal
c)
an element from Group 1
d)
an element with atoms that have eight valence electrons
146.
A(n) _____________ is an atom or group of atoms that has an electric charge. 
a)
ion
b)
electron
147.
When an atom loses a valence electron, it becomes a(n) _________ion.
a)
positive 
b)
negative
148.

Calcium Oxide, CaO

a)

Covalent Bond

b)

Ionic Bond

149.

Calcium Chloride, CaCl2

a)

Covalent Bond

b)

Ionic Bond

150.

Why do ionic bonds form?

a)

so the number of protons equals the number of electrons

b)

to fill the outermost energy level to make the atom stable

c)

so an atom can become unstable

151.

If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?

a)

Al+3

b)

Al+13

c)

Al+10

d)

Al-10

152.

if NONMETALS are more likely to GAIN electrons, they will form ...

a)

anions

b)

neutral atoms

c)

cations

153.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
154.

In the chemical formula for an ionic compound, which item is written first?

a)

positive ion (cation)

b)

negative ion (anion)

c)

subscript

d)

it's alphabetical

155.
What element always has an oxidation number of +1?
a)
Hydrogen
b)
Fluorine
c)
Chlorine
d)
Iodine
156.

The transfer of Valence electrons from a metal to a non metal is known as

a)

Covalent Bonding

b)

Metallic bonding

c)

Molecular bonding

d)

Ionic Bonding

157.

A(n) _________ is an ion with a positive (+) charge.

a)

anion

b)

cation

c)

ion

d)

solute

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