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Electron Configurations

Total questions: 49

Worksheet time: 26mins

Name
Class
Date
1.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

2.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

3.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
4.

Below are the quantum number classifications, except... .

a)

Primal quantum number (n)

b)

Azimuthal quantum number (a)

c)

Magnetic quantum number (m)

d)

Spin projection quantum number (s)

5.

A quantum number determining orbital orientation around the atom’s core is called... .

a)

n

b)

l

c)

m

d)

s

6.

A subshell containing 7 orbitals is called ... subshell.

a)

s

b)

p

c)

d

d)

f

7.

Below are the examples on how to fill the atomic quantum number, except... .

a)

n = 2, l =1, m = 0, s = -1/2

b)

n = 1, l =3, m = 0, s = +1/2

c)

n = 3, l =1, m = 0, s = -1/2

d)

n = 3, l = 2, m = +2, l = +1/2

8.

The total amount of electrons that can be filled within p subshell are ... electrons.

a)

6

b)

10

c)

14

d)

18

9.

Primal quantum number (n) states that... .

a)

The direction of its spinning axis, when it rotates the core

b)

Sum of shells in an atom

c)

Orbital orientation of an electron

d)

The location of the outmost subshell in an atom

10.

The magnetic quantum number (m), has value within... .

a)

0 up to (n-1)

b)

0, 1, 2, 3, ...

c)

-l up to. +l

d)

-1/2 and +1/2

11.

A theory stating that electrons have the trend of taking the orbitals from the lowest energy level to the highest is the theory of... .

a)

Pauli exclusion’s principle

b)

Aufbau principle

c)

Hund’s rule

d)

Heissenberg’s probability

12.

Below are the examples of the electron configuration which can be abbreviated with noble gas notation, except... .

a)

1s1

b)

1s2 2s2

c)

1s2 2s2 2p3

d)

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

13.

Below are the correct answer of the writing of electron configuration, except... .

a)

6f2

b)

2p5

c)

3d7

d)

4s3

14.

Symbol d in the configuration of 3d10 states... .

a)

The total amount of the atom shells

b)

Its subshell of the located electron

c)

The amounnt of electrons filling the subshell

d)

The atomic valence in modern periodic table of the elements

15.

A subshell that contains 5 orbitals is ... subshell.

a)

d

b)

s

c)

f

d)

p

16.

A theory stating that it is forbidden for 2 electrons having the same value of atomic quantum numbers is explained by... .

a)

Hund

b)

Aufbau

c)

Pauli

d)

Schrodinger

17.

Orbital energy of an atom is characterized by ... quantum number.

a)

Spin projection and magnetic

b)

Magnetic and azimuthal

c)

Primal and spin projection

d)

Primal and azimuthal

18.

Orbital shape of an atom is characterized by ... quantum number.

a)

Spin projection

b)

Primal

c)

Magnetic

d)

Azimuthal

19.
This "rule" of Quantum Chemistry states that it is impossible to know both the position and velocity of an electron at the same time.
a)
Hund's Rule
b)
Heisenberg Uncertainty Principle
c)
Aufbau Principle
d)
Pauli Exclusion Principle
20.
According to the Aufbau Principle, which sublevel should starting filling with electrons after 5s?
a)
6s
b)
5p
c)
4d
d)
3f
21.
The second energy level (n=2) contains a total of 5 electrons...how many more electrons can fit in the 2nd energy level?
a)
0
b)
3
c)
5
d)
7
22.
This "rule" of Quantum Chemistry states that no 2 electrons in an atom can be in the exact same state...each electron in an atom can be described by a unique set of quantum numbers.
a)
Hund's Rule
b)
Heisenberg Uncertainty Principle
c)
Aufbau Principle
d)
Pauli Exclusion Principle
23.
According to the Aufbau Principle, which sublevel should starting filling with electrons before the 3p sublevel?
a)
3s
b)
2p
c)
4s
d)
4p
24.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
25.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

26.
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
27.

Correctly pair the orbital with its "block" location

a)

s orbital, "gold" block

b)

p orbital, red block

c)

d orbital, darker green/brown block

d)

f orbital, blue block

28.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

Columns 1-2

b)

Columns 13-18

c)

Actinides/Lanthanides

d)

Columns 3-12

29.

The outermost energy level is called the

a)

Appearance shell

b)

Ultimate shell

c)

Electron shell

d)

Valence shell

30.

As a general rule, the valence level of an atom never has more than _____ electrons.

a)

2

b)

4

c)

8

d)

32

31.

Konfigurasi elektron unsur X dengan nomor atom 24 adalah…..

a)

[Ar] 3d2 4s2

b)

[Ar] 3d5 4s1

c)

[Ar] 4s2 3d10

d)

[Ar] 4s1 3d4 4p3

e)

[Ar] 3d8 4s2 4p2

32.

Fe3+Fe^{3+^{ }}  Diketahui nomor atom Fe = 26, konfigurasi elektron ion adalah . (ion Fe 3 plus )

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d6 

b)

1s2 2s2 2p6 3s2 3p6 3d5 

c)

1s 2 2s2 2p6 3s2 3p6 4s2 3d3

d)

1s2 2s2 2p6 3s2 3p6 4s1 3d4

e)

1s2 2s2 2p6 3s2 3p6 3d6 

33.

 

Nomor atom unsur X sama dengan 27. Jumlah elektron tidak berpasangan dalam ion X2+X^{2+}  adalah…

a)

1

b)

2

c)

3

d)

5

e)

7

34.

Atom suatu unsur mempunyai 3 kulit atom dan 7 elektron valensi. Dalam intinya terdapat 20 neutron. Nomor atom itu adalah . . . .

a)

3

b)

7

c)

9

d)

17

e)

37

35.

Konfigurasi elektron yang tidak mengikuti aturan Hund adalah…

a)
b)
c)
d)
e)
36.

Pengisian Elektron yang benar menurut aturan Aufbau dan Hund pada tabel pengisian elektron-elektron ke dalam subkulit berikut yaitu….

a)

I dan V

b)

I dan II

c)

II danV

d)

III dan V

e)

IV dan V

37.
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.
38.

Two electrons in the 1s orbital must have different spin quantum numbers to satisfy

a)

Aufbau Principle

b)

Hund's rule

c)

the Pauli exclusion principle.

d)

quantum rule

39.

In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?

a)

4s2, 3d1

b)

3d3

c)

4s3

d)

4s2 4p1

40.

According to Pauli Exclusion Principle, how many electrons may occupy a single orbital?

a)

1

b)

2

c)

4

d)

8

41.

What is the electron configuration of Argon?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p6 3s2

d)

1s2 2s2 2p6 3s2 3p6

42.

Which pair of ions have the same electronic configuration? ( Hint: more than one answer)

a)

Mg2+ and Al3+

b)

Al3+ and F-

c)

Sc3+ and F-

43.
 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.
44.
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
45.

Which sub-level holds a maximum of 14 electrons?

a)

s

b)

p

c)

d

d)

f

46.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
47.
In an orbital diagram,  an arrow represents: 
a)
an electron
b)
an orbital
c)
an element
48.
What does Hund's rule states ?
a)
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
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
49.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
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

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