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Worksheets

Electrons

Total questions: 108

Worksheet time: 54mins

Name
Class
Date
1.

Identify the element represented by the electron configuration below.

1s2 2s2 2p6 3s2 3p3

a)

N

b)

P

c)

S

d)

As

2.

Indicate whether the elements represented by the electron configuration below have similar chemical properties (belong to the same family).

1s2 2s2 and 1s2 2s2 2p2

a)

No, they don't belong to the same family.

b)

Yes, they belong to the same family.

3.

Indicate whether the elements represented by the electron configuration below have similar chemical properties (belong to the same family).

1s2 2s1 and 1s2 2s2 2p6 3s2 3p6 4s1

a)

No, they don't belong to the same family.

b)

Yes, they belong to the same family.

4.

How many unpaired electrons are there in the atom of Cl?

a)

0

b)

1

c)

2

d)

3

5.

How many unpaired electrons are there in the atom of Ca?

a)

0

b)

1

c)

2

d)

3

6.

What is wrong with the electron configuration below?

1s2 2s3

a)

The 1s subshell should be followed by 2p subshell.

b)

The 1s subshell should be followed by 1p subshell.

c)

The 2s subshell can hold only 2 electrons.

d)

The 2s subshell can hold only 1 electron.

7.

What is wrong with the electron configuration below?

1s2 2s2 3s2

a)

The 1s subshell should be followed by 2p subshell.

b)

The 1s subshell should be followed by 1p subshell.

c)

The 2s subshell should be followed by 2p subshell.

d)

The 2s subshell should be followed by 3p subshell.

8.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
9.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
10.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
11.
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
12.
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
13.
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
14.

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

15.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
16.

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

17.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
18.

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

a)

8

b)

10

c)

2

d)

4

19.

What is this element?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

20.

What is this element?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

21.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
22.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
23.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
24.

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

25.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
26.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
27.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
28.

What atom matches this electron configuration?

[Kr] 5s2 4d9

a)

Palladium

b)

Silver

c)

Gold

d)

Thallium

29.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
30.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
31.

Which electron configuration belongs to Cobalt?

a)

1s2 2s2 2p6 3s2 3p6 4s9

b)

1s2 2s2 2p6 3s2 3p6 4s2 4d7

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d7

32.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
33.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
34.

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)

There should only be 1 arrow in the first 2p box and one in the second 2p box

d)

All the arrows should be pointing up.

35.

What is incorrect about this orbital diagram?

a)

Only the arrows in the 2p box should be pointing up

b)

There is nothing incorrect with this diagram

c)

All the arrows should be pointing down

d)

The arrows should rotate up down, up down

36.

Which of the following is a correct electron configuration for a noble gas?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p4

c)

1s2 2s2 2p5

d)

1s2 2s2 2s6

37.

Which of the following is a correct electron configuration for an element with 6 valence electrons?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p4

c)

1s2 2s2 2p5

d)

1s2 2s2 2p3

38.

Which of the following is a correct electron configuration for an element with 5 valence electrons?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p4

c)

1s2 2s2 2p5

d)

1s2 2s2 2p3

39.

Which of the following is a correct electron configuration for the only nonmetal that is liquid at room temp?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

b)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p5

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d15

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 5p5

40.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
41.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
42.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
43.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
44.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
45.
[Ne]3s1 is the noble gas configuration for which element?
a)
sodium
b)
lithium
c)
fluorine
d)
aluminum
46.
[Ne]3s23p1 is the noble gas configuration for which element?
a)
scandium
b)
boron
c)
nitrogen
d)
aluminum
47.
[Ne]3s23p5 is the noble gas configuration for which element?
a)
chlorine
b)
fluorine
c)
sulfur
d)
aluminum
48.
[He]2s22p4 is the noble gas configuration for which element?
a)
oxygen
b)
sulfur
c)
phosphorus
d)
fluorine
49.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
50.

Sodium is an element with atoms with 11 protons. For it to be stable, does it lose or gain electrons?

a)

Lose

b)

Gain

51.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
52.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
53.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
54.

Which example shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

55.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
56.
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
57.

Which shows the correct orbital diagram for Cobalt?

a)
b)
c)
d)
58.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
59.

What element has this electron configuration?

a)

hydrogen

b)

helium

c)

lithium

d)

beryllium

60.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

61.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

62.

Which of the following is the orbital notation for oxygen?

a)
b)
c)
d)
63.

What is the element?

a)

sulfur

b)

chlorine

c)

phosphorus

d)

silicon

64.
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 there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
65.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
66.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
67.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
68.

What are valence electrons?

a)

The innermost electrons

b)

The outermost electrons

69.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

70.

How many valence electrons does Carbon have

a)

1

b)

4

71.

Electron dot notation is . . . .

a)

A representation of an element in which only valence electrons of an atom are shown

b)

A representation of how compounds are formed.

72.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
73.

Which of the elements in the picture has correct electron dot notation?

a)

1

b)

2

c)

3

d)

4

74.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

75.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

76.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

77.

How many valence electrons should Oxygen have in its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

78.

How many valence electrons should Oxygen have in its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

79.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

80.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

81.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

82.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

83.

Which of these is incorrect?

a)
b)
84.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

85.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
86.

Which elements usually form cations?

a)

non-metals

b)

metals

c)

any elements

d)

noble gases

87.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
88.

When iodine forms an iodide ion, into which orbital would the electron be going?

a)

5s

b)

4s

c)

5p

d)

3d

e)

It wont gain an electron, it would lose one.

89.

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

90.
What electron configuration matches an oxygen ion?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
91.

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

92.
Atoms that gain & lose electrons are called _________
a)
ions
b)
isotopes
c)
radioactive
d)
corrosive
93.

How many electrons may occupy an orbital?

a)

2

b)

8

c)

6

d)

10

94.

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

95.

Why do atoms become ions in the first place?

a)

They prefer to be charged

b)

They all want to be positive

c)

They all want to be negative

d)

They want to have their valence shell full

96.

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

97.

What is the electron configuration of the Sn+3 ion? (element #50)

a)

1s2 2s1

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2

d)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p6 5d10

e)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10

98.

What atom matches this electron configuration?

[Xe] 6s1 4f14 5d10

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

99.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
100.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

101.

Which element ends 4p4?

a)

sulfur

b)

arsenic

c)

selenium

d)

antimony

102.

What is a positively charged ion called?

a)

anion

b)

polyatomic ion

c)

complex ion

d)

cation

103.

Noble gases are unreactive because they have ______.

a)

low ionization energies

b)

high electron affinities

c)

valence electron configurations of ns2np3

d)

filled outer energy levels

104.

Select all that apply

Elements tend to react to acquire ______.

a)

a filled outer energy level

b)

a valence electron configuration of 2s22p6

c)

eight electrons

d)

the stable electron structure of a noble gas

105.

A positive ion forms when an atom ______.

a)

loses one or more valence electrons in order to transform into a stable noble gas

b)

loses one or more valence electrons in order to attain a noble gas configuration

c)

gains one or more valence electrons in order to attain a noble gas configuration

d)

loses or gains valence electrons in order to attain a noble gas configuration

106.

To attain a stable outer electron configuration, nonmetals ______________ one or more electrons.

a)

lose

b)

gain

c)

destroy

d)

dissolve

107.

What is a negatively charged ion called?

a)

anion

b)

cation

c)

complex ion

d)

polyatomic ion

108.

To designate the anion formed when a chlorine atom gains an electron, the name ______ is used.

a)

chloride

b)

chlorite

c)

chlorate

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