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electronic configuration

Total questions: 102

Worksheet time: 2hrs 38mins

Name
Class
Date
1.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
2.

What is incorrect about this orbital diagram?

a)

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

b)

There is nothing incorrect with this diagram

c)

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

d)

All the arrows should be pointing the same direction.

3.

Which rule is violated in the following orbital diagrams?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli's Exclusion Principle

4.

No two electrons in the same atom can have the same four quantum numbers.

a)

Aufbau Principle

b)

Pauli's Exclusion Principle

c)

Hund’s Rule

d)

Noble gas notation

5.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
6.
FIND THE ELECTRONIC CONFIGURATION OF Cl (At no = 17)
a)
2,8,7
b)
2,8,8
c)
2,8,6
d)
2,8
7.

What atom matches this electron configuration?

1s22s22p63s2

a)

Calcium

b)

Magnesium

c)

Aluminum

d)

Potassium

8.

Write the electronic configuration for sodium Na (Z=11)

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s1

d)

1s2 2s2 2p6 3s2 3p4

9.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
10.

The electron configuration of an atom is 1s22s22p3.

The total number of electrons in the atom is

a)

3

b)

4

c)

5

d)

7

11.

The electron configuration of an atom is 1s2 2s2 2p6 3s2.

The number of valence electrons is

a)

8

b)

2

c)

4

d)

6

12.

According to Aufbau Principle, electrons are filled into 4s orbital before 3d orbital.


When removing the electrons, the electron needs to be removed from which sub-shell first?

a)

4s

b)

3d

c)

3p

d)

1s

13.

Cr (Z=24) shows anomalous electronic configuration.

The actual electronic configuration is

1s2 2s2 2p6 3s2 3p6 4s1 3d5.

This is because ...

a)

the half-filled d-orbital (3d5) is more stable

b)

the completely filled d-orbital (3d10) is more stable

c)

the partially filled d-orbital (3d4) is more stable

14.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
15.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
16.

What is the Aufbau principle?

a)

Within an energy level, s orbitals are the lowest energy, followed by p, d and then f. F orbitals are the highest energy for that level.

b)

The lower the principal quantum number (n) the lower the energy.

c)

All three.

d)

The Aufbau Principle states that electrons enter the lowest energy orbitals first.

17.

All orbitals of equal energy (degenerate orbitals) are occupied by one electron before any single orbital is occupied by a second electron.

a)

Aufbau Principle

b)

Pauli's Exclusion Principle

c)

Hund’s Rule

d)

Core Notation

18.

No two electrons in the same atom can have the same four quantum numbers.

a)

Aufbau Principle

b)

Pauli's Exclusion Principle

c)

Hund’s Rule

d)

Noble gas notation

19.

Which rule is violated in the following orbital diagrams?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli's Exclusion Principle

20.

Which rule is violated in the following orbital diagrams?

a)

Aufbau Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

21.

What is the maximum numbers of electrons when n=2, l=0

(a)  

22.

What electron configuration matches an oxygen ion? (Z=8)

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

23.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
24.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
25.
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
26.

What electron configuration matches an oxygen ion? (Z=8)

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

27.

Write the electronic configuration for sodium Na (Z=11)

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s1

d)

1s2 2s2 2p6 3s2 3p4

28.

State the valence electronic configuration for Mg (Z=12)

a)

3s2

b)

3s2 3p1

c)

3s2 3p3

d)

3s2 3p4

29.

Determine the element that has valence electron 3s23p1

(Z of Na = 11, Al = 13, Cl = 17, Mg = 12)

a)

Na

b)

Al

c)

Cl

d)

Mg

30.

Electron must be arrange from lowest energy to highest energy.

State the rule/principle?

a)

Hund's Rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

Zuhaizi Principle

31.

Which element is pictured?

a)

neon (Z=10)

b)

fluorine (Z=9)

c)

magnesium (Z=12)

d)

argon (Z=18)

32.

All ions matches with this electronic configuration.Except?

1s22s22p63s23p6

a)

Al3+

b)

Cl-

c)

S2-

d)

Ca2+

33.

What electron configuration matches an oxygen atom?

(Z = 8)

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

34.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
35.

In 1s2, the 1 means

a)

there is 1 electron

b)

the electrons are in the 1st energy level

c)

the shape is circular

d)

there is a -1 charge

36.

In 1s2, the s means

a)

the shape of the orbital is circular

b)

the shape of the orbital is figure 8

c)

there are six electrons

d)

it is neutral

37.

In 1s2, the 2 means

a)

there are 2 electrons in this level

b)

it is the 2nd energy level

c)

there is a +2 charge

d)

there is a -2 charge

38.
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.
39.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
40.

Which orbital shows a violation of the Aufbau Principle?

a)

A

b)

B

c)

C

d)

D

41.
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
42.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

43.

The maximum number of electrons that can be accommodated in f subshell is

a)

12

b)

10

c)

14

d)

8

44.

Which subshell has the highest energy?

a)

1s

b)

3p

c)

3d

d)

4s

45.

The correct subshell electronic configurationof 29Cu is

a)

1s2 2s2 2p6 3s2 3p6 3d10 4s2

b)

1s2 2s2 2p6 3s2 3p6 3d10 4s1

c)

1s2 2s2 2p6 3s2 3p6 3d9 4s2

d)

1s2 2s2 2p6 3s2 3p6 3d5 4s1

46.

Which sushell is not possible?

a)

5p

b)

6s

c)

3f

d)

3d

47.

The correct electronic configuration of 19K is

a)

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

b)

1s2 2s2 2p6 3s2 3p6 3d1

c)

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

d)

1s2 2s2 2p6 3s2 3p5 3d2

48.

The subshell common to all shells is

a)

s

b)

p

c)

d

d)

f

49.

The subshell electronic configuration of an element is 1s2 2s2 2p6 3s2 3p6 4s2 . It's atomic number is

a)

19

b)

15

c)

20

d)

4

50.

The maximum number of electrons in M shell is

a)

14

b)

18

c)

10

d)

8

51.

As the distance from the nucleus increases, the energy

a)

Decreases

b)

Increases

c)

First increases and then decreases

d)

No change

52.

Modern periodic table is made on the basis of

a)

Atomic mass

b)

Atomic number

c)

Number of Neutrons

d)

Mass number

53.

What is the name of the 4th element in the periodic table?

a)

Hydrogen

b)

Beryillium

c)

Lithium

d)

Sodium

54.

How many electrons are in the second shell of an atom?

a)

1

b)

2

c)

8

d)

18

55.

What is the correct configuration for electrons in atoms (the first four shells)?

a)

2, 8, 8, 18

b)

1, 2, 3, 4

c)

8, 8, 2, 18

d)

2, 8, 8, 8

56.

The mass of an atom of a chemical element expressed in atomic mass units.

a)

Atomic Mass

b)

Atomic Number

c)

Element

d)

Periodic Mass

57.

What was the name of the first periodic table?

a)

Modern Periodic Table

b)

Dobereiner Triads

c)

Newlands Octaves

d)

Mendeleev’s Periodic Table

58.

Group 1 of the periodic table is also know as....

a)

The Earth Metals

b)

Noble Gases

c)

The Alkali Metals

d)

Transition Elements

59.

Lanthanides make up elements 58-71 of the periodic table

a)

True

b)

False

60.

What is the 20th element on the periodic table?

a)

Calcium

b)

Helium

c)

Oxygen

d)

Silicon

61.

What are the three states of matter? (Select 3)

a)

Liquid

b)

Odour

c)

Solid

d)

Gas

62.

Which of the following is not a property of a solid?

a)

Has a fixed shape

b)

Can be compressed

c)

Cannot flow

d)

Particles cannot move, but vibrate on the spot

63.

Which of the following is a property of a gas?

a)

It flows

b)

The particles do not move

c)

Can be compressed

d)

It has a fixed shape

64.

Which of the following are properties of liquids?

a)

Has no fixed shape

b)

Cannot be compressed

c)

Has a fixed shape

d)

Can flow

65.

The protons in an atom have a negative charge

a)

True

b)

False

66.

The electrons in an atom have a positive charge.

a)

True

b)

False

67.

How many electrons are there in the element oxygen?

a)

16

b)

8

c)

24

d)

128

68.

What is a mistake with this sketch of the atom for the element fluorine?

a)

Too many electrons in the first shell

b)

Not enough electrons in the first shell

c)

It is not labelled

d)

There are not enough electrons

69.

Na is the chemical symbol for....

a)

Sodium

b)

Carbon

c)

Copper

70.

How many atoms are there in this compound?

a)

2

b)

4

c)

7

d)

0

71.

How many elements are in this compound?

a)

1

b)

2

c)

3

d)

7

72.

Mixtures consist of two or more elements or compounds that are NOT chemically combined

a)

True

b)

False

73.

Is this equations balanced?

a)

Yes

b)

No

74.

How many colors are there in the visible light spectrum? What are they?

a)

7. Red, orange, yellow, green, blue, pink, violet

b)

10. Red, orange, yellow, green, blue, indigo, violet, pink, grey, magenta.

c)

8. Red, orange, yellow, green, blue, indigo, violet, pink

d)

7. Red, orange, yellow, green, blue, indigo, violet

75.

What is the rule for filling the energy levels?

a)

Electrons fill them from the lowest energy to the highest

b)

Electrons fill them whatever level of energy they desire

c)

Electrons fill them from the highest energy to the lowest

76.

Higher frequency-> higher energy

a)

True

b)

False

77.

An atomic emission spectrum is produced when:

a)

Electrons are excited to higher electronic energy levels

b)

Electron transitions take place from a lower to a higher electronic energy level

c)

Electrons move from electronic energy levels n=1 to n=2

d)

Electron transitions take place from a higher to a lower electronic energy level

78.

The electron transition between which two atomic energy levels emits the most energy?

a)

Sixth to fourth

b)

First to fourth

c)

Second to seventh

d)

Third to first

79.

Electron transitions in the hydrogen emission spectrum to levels n=1, n=2, and n=3 generate lines in which parts of the electromagnetic spectrum respectively?

a)

Respectively: n=1 in infra-red; n=2 in ultra-violet; n=3 in visible

b)

Respectively: n=1 in visible; n=2 in infra-red; n=3 in ultra-violet

c)

Respectively: n=1 in ultra-violet; n=2 in infra-red ; n=3 in visible

d)

Respectively: n=1 in ultra-violet; n=2 in visible; n=3 in infra-red

80.

Which electron transition in the hydrogen atom emits visible light?

a)

n = 3 to n = 2

b)

n = 1 to n = 2

c)

n = 2 to n = 3

d)

n = 2 to n = 1

81.

Shorter wavelength -> Lower frequency

a)

True

b)

False

82.

As the energy levels increase in energy they get _______________.

a)

None of the answers is right

b)

closer together

c)

All of the answers are right

d)

further apart

83.

What is the maximum number of electrons that can hold the n=3 electronic energy level in an atom?

a)

2

b)

31

c)

50

d)

18

84.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
85.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
86.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
87.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
88.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
89.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
90.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
91.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
92.
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
93.

There are 4 different types of sublevels: s,p,d,f

a)

true

b)

false

94.
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
95.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
96.

What is the noble gas (abbreviated) electron configuration for a Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

97.

What noble gas should be used to write the abbreviated configuration for Te?

a)

Ar

b)

Kr

c)

Xe

d)

Sb

98.
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
99.

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

100.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
101.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
102.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6

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