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Periodic Table Review

Total questions: 94

Worksheet time: 4hrs 33mins

Name
Class
Date
1.

What are the vertical columns on the periodic table called?

a)

groups

b)

periods

c)

protons

d)

valence electrons

2.

Which of the following is a trait of group 18?

a)

They are all reactive metals

b)

they are all stable metals

c)

They chemically stable gasses

d)

They are a mix of reactive gasses and solids

3.

Which of the following would be elements that are found in the same period?

a)

Sn and Rb

b)

F and Cl

c)

K and Ba

d)

Se and Te

4.

Which element has the same properties as Phosphorus but has a larger mass?

a)

Nitrogen

b)

Lead

c)

Silicon

d)

Arsenic

5.

Which element is in Group 18 and period 4?

a)

Krypton

b)

Argon

c)

Xenon

d)

Bromine

6.

Most elements on the periodic table are classified as __________.

a)

Metals

b)

Non-Metals

c)

Metalloids

d)

Gases

7.
Which accurately describes nonmetals?
a)
Both malleable and ductile
b)
Often used in computer parts
c)
Poor conductors of electricity
d)
Always solid at room temperature
8.
Which group on the periodic table is the most reactive Metals?
a)
Alkaline-earth metals - Group 2
b)
Alkali metals - Group 1
c)
Transition metals - Group 3-7
d)
Halogens - Group 17
9.
Each horizontal row on the periodic table is called what?
a)
Periods
b)
Groups
10.
Which 2 Groups are most likely to react with each other?
a)
Groups 1 & 18
b)
Groups 1 & 17
c)
Groups 2 & 18
d)
Groups 14 & 15
11.
How Many Valence Electrons are in the element above?
a)
1
b)
3
c)
5
d)
7
12.
Which of the following statement is true?
a)
Group 18 - 18 Valence Electrons
b)
Group 15 - 1 Valence Electrons
c)
Group 13 - 3 Valence Electrons
d)
Group 11 - 8 Valence Electrons
13.
Non-Malleable, Less Dense, Insulators and Brittle describe what physical property group?
a)
Metals
b)
Non-Metals
c)
Transition Metals
d)
Metalloids
14.
Families or Groups are the vertical columns on the periodic table. How many Families/Groups are there?
a)
18
b)
7
c)
12
d)
20
15.
Elements in the same family have similar _______________.
a)
Protons
b)
Physical and Chemical Properties
c)
Shape
d)
Size
16.
Metals are ___________.
a)
Good Conductors of heat and electricity
b)
Noble Gasses 
c)
Bad Conductors of heat and electricity
d)
sometimes a gas
17.
Non-Metals are found ____________________.
a)
To the left of the stairs
b)
To the right of the stairs
c)
Includes only the elements touching the stairs
18.
Metalloids have ___________________
a)
Only properties of a metal
b)
Only properties of a non-metal
c)
Can have properties of both metals and non-metals
19.
Periods are the rows of the periodic table. How many are there?
a)
7 
b)
18
c)
12
d)
20
20.
Which element is not a metal?
a)

He

b)
Re
c)
Al
d)
B
21.
most of the elements on the periodic table are 
a)
non metals 
b)
metals 
c)
metalloids 
d)
none 
22.

Dmitri Mendeleev organized his periodic table in order of increasing.....

a)

density

b)

atomic number

c)

atomic mass

d)

none of these

23.
Which of the following has a full outer level?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
24.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
25.
How many electrons can the 2nd and 3rd energy level hold and be stable?
a)
2
b)
8
c)
as many as needed
d)
10
26.
Which of the following is an Alkali Metal? 
a)
Magnesium
b)
Chromium
c)
Sodium
d)
Fluorine 
27.
Which of the following is an Alkaline Earth Metal? 
a)
Calcium
b)
Lithium
c)
Phosphorus
d)
Copper 
28.
Which of the following is a transition metal? 
a)
Iron
b)
Oxygen
c)
Neon
d)
Barium
29.
Which of the following is a Halogen? 
a)
Bromine
b)
Rubidium
c)
Argon
d)
Beryllium
30.
Which of the following is a Noble Gas? 
a)
Krypton
b)
Chlorine
c)
Radium
d)
Gallium
31.
Which of the following is the most reactive group of metals? 
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Transition Metals
32.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
33.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
34.
An atom that has the electron configuration of 1s22s22p63s23p64s23d5 is classified as
a)
A transition element
b)
a noble gas
c)
an alkali metal
d)
an alkaline earth metal
35.

The is family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

36.

This type of element is dull, brittle solids and gases, insulators, poor conductors of heat and electricity, as well as having low melting points.

a)

metals

b)

metalloids

c)

nonmetals

37.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
38.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
39.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
40.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
41.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
42.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
43.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
44.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
45.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
46.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
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
48.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
49.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
50.

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

51.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

52.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
53.
How many electrons should Beryllium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
54.
How many electrons should Flourine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
55.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

56.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
57.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
58.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
59.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
60.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

61.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
62.

Which of these is correct?

a)
b)
c)
63.

Who do we give credit to for developing the modern periodic table?

a)

Lavoisier

b)

Einstein

c)

Mendeleev

d)

Pauli

64.

According to ________________________, atoms tend to lose, gain, or share electrons in order to become stable.

a)

octet rule

b)

Hund's rule

c)

periodic law

d)

Aufbau principle

65.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
66.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
67.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
68.

Which elements usually form cations?

a)

non-metals

b)

metals

c)

any elements

d)

noble gases

69.

Which electron configuration belongs to a Chloride (Cl-) ion?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3p7

70.

An aluminium ion would have which electron configuration?

a)

1s2 2s2 2p6 3s2

b)

1s2 2s2 2p6 3s2 3p1

c)

1s2 2s2 2p6 3s2 3p6

d)

1s2 2s2 2p6

71.
In which of the following groups are the three species isoelectronic?
a)
S2¯, K+, Ca2+
b)
Sc, Ti, V2+
c)
O2¯, S2¯, Cl¯
d)
Mg2+, Ca2+, Sr2+
72.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
73.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

74.
The electron configuration of an atom is 1s22s22p6.  The number of valence electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
75.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
76.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
77.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
78.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
79.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
80.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

81.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

82.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

83.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

84.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

85.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

86.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

87.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

88.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

89.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
90.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
91.

Which of the following is MOST reactive?

a)

Lithium

b)

Lead

c)

Tin

d)

Copper

92.

Which metal is more reactive than calcium?

a)

magnesium

b)

potassium

c)

silver

d)

aluminum

93.
Which two groups on the Periodic Table are the MOST reactive?
a)
Group 1 and Group 17
b)
Group 2 and Group 16
c)
Group 13 and Group 15
d)
Group 17 and Group 18
94.
How do you determine the number of valence electrons an element has?
a)
Look at its period
b)
Look at its group
c)
Look at its atomic number
d)
Look at its atomic mass

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