Name: Electronic Configuration
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Created bySameen Mumtaz

Last updated 9/2021

English

What you'll learn

Do you know structure of an atom?
Do you the fundamentals particles of an atom?
Where electrons, protons and neutrons reside in an atom?
Can you locate the position of an electron in an atom?
What are Shells and Sub-Shells?
How electrons accommodate in shell? and sub-shell?
Do you know maximum capacity of shells and sub-shells?
What is Auf-Bau principle?
How many sub-shells are there?
Are all the shells can accommodate equal number of electrons?
Practice to write electronic configuration.

Course content

5 sections • 5 lectures • 1h 5m total length

Atomic Structure.(Atoms are the basic units of matter)8:02
1.1 Position of electrons protons and neutron in an atom.
Atoms are made of extremely tiny particles called protons, neutrons, and electrons. Protons and neutrons are in the center of the atom, making up the nucleus. Electrons surround the nucleus. Protons have a positive charge. Electrons have a negative charge. The charge on the proton and electron are exactly the same size but opposite. Neutrons have no charge.

1.2 Nuclear and extra nuclear part of an atom.
As we know that the nucleus (center) of the atom contains the protons (positively charged) and the neutrons (no charge). The outermost regions of the atom are called electron shells and contain the electrons (negatively charged). Since opposite charges attract, protons and electrons attract each other. Atoms have different properties based on the arrangement and number of their basic particles.
1.3 Shells and Sub-Shells.
To understand electronic configuration, we must know about Shells and Sub-Shells.
What are Shells?
Shell is the outside part of an atom around the nucleus.
The electrons revolve around the nucleus in different energy levels or shells according to their respective energies.
Energy levels are represented by 'n' values 1, 2, 3 and so on. They are designated by the alphabets K, L, M and so on. A shell closer to the nucleus is of minimum energy.
What are Sub-Shells?
A Shell or energy level is sub divided into sub-shells or sub-energy levels.
‘n’ values of a shell is placed before the symbol for a sub-shell.
The n number determines how many of the sub shells make up the shell. For example:
The 1st shell (K) is made up of 1 sub shell, s.
The 2nd shell (L) is made up of 2 sub shells, s and p.
The 3rd shell (M) is made up of 3 sub shells, s p and d.
The 4th shell (N) is made up of 4 sub shells, p, d and f.
1.4 Presence of sub-shells in a shell.
Electrons orbit the nucleus of an atom at different ranges, called shells. Each shell has a different energy level, increasing the further it is from the nucleus. Each energy level is given a number called the principal quantum number, n. ... The n number determines how many of the sub shells make up the shell.
1.5 Maximum accommodation of electrons within a shell.
Each shell can contain only a fixed number of electrons: The first shell can hold up to two electrons, the second shell can hold up to eight (2 + 6) electrons, the third shell can hold up to 18 (2 + 6 + 10) and so on. The general formula is that the nth shell can in principle hold up to 2(n2) electrons but actually
k = 2 electrons ; L = 8 electrons; M = 8 electrons; N = 18 electrons;
O = 18 electrons; P = 32 electrons; & Q = 32 electrons.
1.6 Types of sub-shells their names with capacity.
There are 4 sub shells, s, p, d, and f. Each sub shell can hold a different number of electrons. The n number determines how many of the sub shells make up the shell.
s=2 electrons; p=6 electrons; d=10 electrons & f=14 electrons.

2- Shape of periodic Table6:54
Module - 2
2- Shape of periodic table.
2.1- Periodic Table.
2.2 Groups and periods in periodic table.
2.3 Blocks in periodic table and their position in periodic table.
Shape of periodic table.
2.1 : Periodic Table:
The periodic table, also known as the periodic table of elements, is a tabular display of elements, which are arranged by atomic number, electron configuration, and their chemical properties. Therefore we can say that “A table showing systematic arrangement of elements according to their increasing atomic number in which their properties are repeated in periodic manners called periodic table”.
2.2 : Groups and periods in periodic table.
The vertical columns on the periodic table are called groups or families. Groups probably come in most handy when predicting the properties of an element. The groups are numbered from 1-18 from left to right, and some of the groups have special names. A period is a horizontal row of the periodic table. There are seven periods in the periodic table, with each one beginning at the far left. A new period begins when a new principal energy level or shell begins filling with electrons. Period 1 has only two elements (hydrogen and helium), while periods 2 and 3 have 8 elements. Periods 4 and 5 have 18 elements. Periods 6 and 7 have 32 elements because the two bottom rows that are separated from the rest of the table belong to those periods. First three periods are called short periods and the remaining periods are called long periods.

2.3 : Blocks in periodic table and their position in periodic table.
s-block elements( group I-A and group II-A), s- block elements are all metals.)
p – block elements (group III-A, IV-A, V-A, VI-A, VII-A & VIII-A), p- block elements are mainly non-metals but they include some metalloid and metals also.
d-block(outer Transition elements), group 1B to VIIIB
f-block(inner Transition elements), Lanthanides (4f) series and Actinides(5f) series.

Auf Bau Principle.7:28
Module - 3
3 - Auf - Bau Principle.
3.1 How electrons are distributed in its atomic orbitals.(s,p,d & f)
3.2 What are energy levels?
3.3 Write electronic configuration of different elements.
Auf-Bau Principle:
The arrangement of electrons in sub-shells is called as the electronic configuration. We can fill the electrons present in various elements by using (Auf-Bau)Principle.
According to this principle, electrons fill the lowest energy subshell that is available first.
3.1 What are energy levels & sub-energy levels?
Shell or Energy Level:
Shell is the outside part of an atom around the nucleus. The electrons revolve around the nucleus in different energy levels or shells according to their respective energies.
Energy levels are represented by 'n' values 1, 2, 3 and so on. They are designated by the alphabets K, L, M and so on. A shell closer to the nucleus is of minimum energy.
Sub-Shell or Sub-Energy Level:
A Shell or energy level is sub divided into sub-shells or sub-energy levels. ‘n’ values of a shell is placed before the symbol for a sub-shell.The n number determines how many of the subshells make up the shell. For example:
1. The 1st shell (K) is made up of 1 subshell, (s).
2. The 2nd shell (L) is made up of 2 subshells, (s and p).
3. The 3rd shell (M) is made up of 3 subshells, (s p and d).
4. The 4th shell (N) is made up of 4 subshells, (s,p, d and f).
3.2 : How electrons are distributed in its atomic orbitals.
(s,p,d & f)
s=2 , p=6, d=10, f=14
The increasing order of energy the
sub-shells belonging to different
shells.
3.3 Write electronic configuration of different elements.
1 Hydrogen 1s1
2 Helium 1s2
3 Lithium 1s2, 2s1 [He]2s1
4 Beryllium 1s2 ,2s2 [He]2s2
5 Boron 1s2, 2s2, 2p1 [He]2s2, 2p1
6 Carbon 1s2 , 2s2, 2p2 [He]2s2, 2p2
7 Nitrogen 1s2, 2s2, 2p3 [He]2s2, 2p3
8 Oxygen 1s2, 2s2, 2p4 [He]2s2, 2p4
9 Fluorine 1s2, 2s2, 2p5 [He]2s2, 2p5 10 Neon 1s2, 2s2, 2p6 [He]2s2, 2p6
11 Sodium 1s2, 2s2,2p6,3s1 [Ne]3s1
12 Magnesium 1s2, 2s2,2p6,3s2 [Ne]3s2
13 Aluminum 1s2, 2s2,2p6,3s2,sp1 [Ne]3s2, 3p1
14 Silicon 1s2,2s2,2p6,3s2,3p2 [Ne]3s2, 3p2
15 Phosphorus 1s2,2s2,2p6,3s2,3p3 [Ne]3s2, 3p3
16 Sulfur 1s2,2s2,2p6,3s2,3p4 [Ne]3s2, 3p4
17 Chlorine 1s2 ,2s2, 2p6,3s2,3p5 [Ne]3s2, 3p5
18 Argon 1s2,2s2, 2p6,3s2,3p6 [Ne]3s2, 3p6
19 Potassium 1s2, 2s2,2p6,3s2,3p6,4s1 [Ar]4s1
20 Calcium 1s2,2s2,2p6,3s2,3p6,4s2 [Ar]4s2

Importance of electronic configuration.18:43
At.# Name Electronic Configuration
1 Hydrogen 1s1
2 Helium 1s2
3 Lithium 1s2, 2s1 [He]2s1
4 Beryllium 1s2 ,2s2 [He]2s2
5 Boron 1s2, 2s2, 2p1 [He]2s2, 2p1
6 Carbon 1s2 , 2s2, 2p2 [He]2s2, 2p2
7 Nitrogen 1s2, 2s2, 2p3 [He]2s2, 2p3
8 Oxygen 1s2, 2s2, 2p4 [He]2s2, 2p4
9 Fluorine 1s2, 2s2, 2p5 [He]2s2, 2p5
10 Neon 1s2, 2s2, 2p6 [He]2s2, 2p6
11 Sodium 1s2, 2s2,2p6,3s1 [Ne]3s1
12 Magnesium 1s2, 2s2,2p6,3s2 [Ne]3s2
13 Aluminum 1s2, 2s2,2p6,3s2,sp1 [Ne]3s2, 3p1
14 Silicon 1s2,2s2,2p6,3s2,3p2 [Ne]3s2, 3p2
15 Phosphorus 1s2,2s2,2p6,3s2,3p3 [Ne]3s2, 3p3
16 Sulfur 1s2,2s2,2p6,3s2,3p4 [Ne]3s2, 3p4
17 Chlorine 1s2 ,2s2, 2p6,3s2,3p5 [Ne]3s2, 3p5
18 Argon 1s2,2s2, 2p6,3s2,3p6 [Ne]3s2, 3p6
19 Potassium 1s2, 2s2,2p6,3s2,3p6,4s1 [Ar]4s1
20 Calcium 1s2,2s2,2p6,3s2,3p6,4s2 [Ar]4s2

Module -4
4- Importance of electronic configuration
4.1 Valance shell electronic configuration.
4.2 Identify atomic properties.(Groups, periods, block and chemical properties etc.
4.3 Importance of noble gas configuration.
Importance of electronic configuration : This is important because valence electrons contribute to the unique chemistry of each atom. The important aspect is that we realize that knowing electron configurations helps us determine the valence electrons on an atom as well as we can identify the atom, its position in the periodic table, group, period, total number of electrons and valence shell electrons. We can also predict the chemical properties and behavior of elements.
4.1 : Valance shell electronic configuration. 1 Hydrogen 1s1 2 Helium 1s2 3 Lithium [He]2s1 4 Beryllium [He]2s2 5 Boron [He]2s2, 2p1 6 Carbon [He]2s2, 2p2 7 Nitrogen [He]2s2, 2p3 8 Oxygen [He]2s2, 2p4 9 Fluorine [He]2s2, 2p5 10 Neon [He]2s2, 2p6 11 Sodium [Ne]3s1 12 Magnesium [Ne]3s2 13 Aluminum [Ne]3s2, 3p1 14 Silicon [Ne]3s2, 3p2 15 Phosphorus [Ne]3s2, 3p3 16 Sulfur [Ne]3s2, 3p4 17 Chlorine [Ne]3s2, 3p5 18 Argon [Ne]3s2, 3p6 19 Potassium [Ar]4s1 20 Calcium [Ar]4s2
1.Which atom is represented here?
2.What is the atomic number and atomic mass of this element?
3.How many electrons are represented in the last shell here?
4.Write the electronic configuration for this atom? Can you answer these questions ?
Can you answer these questions?
1.Which atom is represented here? Nitrogen
2.What is the atomic number and atomic mass of this element? (Atomic number) Z= 7 ,(Mass number) A=14
3.How many electrons are represented in the last shell here? 5
4.Write the electronic configuration for this atom? 1s2, 2s2, 2p3
Write a brief answer for these questions.
1.How many electrons does Silicon contain?
2.How many valence electrons does Silicon contain?
3.How many electrons can the first energy level hold?
4.Write the electronic configuration for this atom?
5.Write the valence shell electronic configuration for this atom?
Write a brief answer for these questions
1.How many electrons does Silicon contain? 14
2.How many valence electrons does Silicon contain? 4
3.How many electrons can the first energy level hold? 2
4.Write the electronic configuration for this atom? 1s2, 2s2, 2p6, 3s2, 3p2
5. Write the valence shell electronic configuration for this atom? 3s2, 3p2 1s2, 2s2, 2p6, 3s2, 3p2 K L M
4.2 : Identify atomic properties.(Groups, periods, block and chemical properties etc.
Example: Magnesium (Mg) Atomic Number : 12
Electronic Configuration : 1s2 , 2s2, 2p6, 3s2
Valence Shell Electronic Configuration of Mg : 3s2
Period Number = Number of shells = 3 so 3rd Period
Group Number = Electrons in last shell = 2 so Group II A
Block = s-block
4.3 Importance of noble gas configuration.
Atomic stability: The stability of atoms depends on whether or not their outer-most shell is filled with electrons. If the outer shell is filled, the atom is stable. Atoms with unfilled outer shells are unstable, and will usually form chemical bonds with other atoms to achieve stability. Example of an unstable atom with a single electron in its outer-most shell is Sodium. Example of an unstable atom with 7 electrons in its outer-most shell is Chlorine. Examples of stable atoms are Helium , Neon and Argon.

How we can write Electronic Configuration (PRACTICE…)24:34
Module -5
5- How we can write Electronic Configuration (PRACTICE…)
5.1 Electronic configuration of s-block elements.
5.2 Electronic configuration of p-block elements.
5.3 Electronic configuration of d-block elements.
5.4 Electronic configuration of f-block elements.
5.1 electronic configuration of s-block elements.
Elements of group IA and IIA and Helium contain their valence electrons in
s sub-shell. Therefore these elements are called s-block elements all are metals.
I A & II A
5.2 electronic configuration of p-block elements.
Elements of group IIIA and VIIIA contain their valence electrons in p subshell.
Therefore these elements are called p-block elements, mainly they are non-metals but they include some metalloid and metals also.
5.3 electronic configuration of d-block elements.
Elements of group IB and VIIIB contain their valence electrons in d sub-shell.
Therefore these elements are called d-block elements. They all are metals and also known as Outer Transition Elements.
Scandium [Ar]3d14s2
Iron Ar]3d64s2
Zinc [Ar]3d104s2
5.4 electronic configuration of f-block elements.
Elements of 4-f series (Lanthanides) an d 5-f series (Actinides) contain their valence electrons in f sub-shell. Therefore these elements are called f-block lements. They are all metals and also known as Inner Transition Elements.
4f Lanthanides Series
5f Actinides Series

Requirements

Science school or college students of Chemistry.

Description

This course is design for chemistry students of intermediate level or A-level who need help to write electronic configuration and find out the valence shell electronic configuration of elements from the periodic table.

This course is consist of four module each module further sub divided into three steps i.e. basic information review and a short quiz and finally a detailed quiz to complete this course.

Module - 1

1-Atomic Structure.

1.1 Position of electrons protons and neutron in an atom.

1.2 Nuclear and extra nuclear part of an atom.

1.3 Shells and Sub-Shells.

1.4 Presence of sub-shells in a shell.

1.5 Maximum accommodation of electrons within a shell.

1.6 Types of sub-shells their names with capacity.

Module - 2

2- Shape of periodic table.

2.1- Periodic Table.

2.2 Groups and periods blocks in periodic table.

2.3 Blocks in periodic table and their position in periodic table.

Module - 3

3 - On construction principle.

3.1 How electrons are distributed in its atomic orbitals.(s,p,d & f)

3.2 What are energy levels?

3.3 Write electronic configuration of different elements.

Module -4

4- Importance of electronic configuration

4.1 Valance shell electronic configuration.

4.2 Identify atomic properties.(Groups, periods, block and chemical properties etc.

Module -5

5- How we can write Electronic Configuration (PRACTICE…)

5.1 Electronic configuration of s-block elements.

5.2 Electronic configuration of p-block elements.

5.3 Electronic configuration of d-block elements.

5.4 Electronic configuration of f-block elements.

Who this course is for:

For students of chemistry who want to know how electronic configuration write and why its important.

What you'll learn

Explore related topics

Course content

Module -11 lecture • 8min

Module - 21 lecture • 7min

Module - 31 lecture • 7min

Module - 41 lecture • 19min

Module - 51 lecture • 25min

Requirements

Description

Who this course is for: