The Valence Shell Electron Pair Repulsion Theory (VSEPR)
Do you know !!
Theories of Covalent Bonds:
There are three theories of covalent bonds.
(i) VSEPRT, Resonance Theory,
(ii) VBT
(iii) MOT.
Valence Shell Electron Pair Repulsion (VSEPR) Theory is used to predict:
VSEPR stands for Valence Shell Electron Pair Repulsion.
VSEPR theory is good enough to explain
- molecule geometries
- bond angles.
A summary of molecular shapes is given in the following table:

VSEPR Theory Main Postulates
According to vsepr, two types of electron pairs around the central atom of a molecule and it has the following postulates:
- Two types of electron pairs are present around the central atom of a molecule. Electron pair which is shared between two atoms and is responsible for the covalent bond is called a “bond pair” while electron pair which is not shared between two atoms is called a “lone pair”.

(vsepr )
Lone pair-lone pair > Lone pair-bond pair > Bond pair-bond pair
- To reduce repulsion these electron pairs move to maximum angles apart from each other and are directed in different directions in space. So they are responsible for molecular geometries.
linear Geometry
For two electron pairs, geometry is linear and the bond angle is 180o.
Triangular Planar Geometry
For three electron pairs, the geometry is triangular planar and the bond angle is 120o.
Tetrahedral Geometry
For four electron pairs, the geometry is tetrahedral and the bond angle is 109.5o.
- If more than one electron pairs are there in the same region they behave like a single pair. e.g.
Sulphur in SO2 shows three electron pairs behaviour.
..
O : : S : O
- Deviation from the ideal bond angle occurs if lone pair of electrons is there.
- The effect of a bonding electron pair decreases with the increasing electronegativity of an atom forming a molecule.
Shape of molecules with two electron pairs:
e.g (i) BeCl2
Cl : Be : Cl
or
Cl ─ Be ─ Cl Linear Geometry
( 180o )
The central atom Be has two electron pairs so the molecule is linear with a bond angle of 180o.
e.g (ii) CO2
O : : C : : O
or O = C = O Linear Geometry
Four pairs around the central Carbon atom behave like two pairs so the CO2 molecule is linear with a bond angle of 180o.
e.g (iii) HCN
H : C : : : N
or H ─ C ≡ N Linear Geometry
Four pairs around the central Carbon atom behave like two pairs so the HCN molecule is linear with a bond angle of 180o.
The shape of molecules with three electron pairs:
e.g (i) BF3
The central atom B has three electron pairs so the molecule is a triangular planner with a bond angle 120o.
e.g (ii) SO2
Two electron pairs that Sulphur has shared with one of the oxygen act as single pair so SO2 shows the behaviour of three electron pairs. Hence electron geometry in SO2 is a triangular planner while molecule geometry is an angular or bent structure. In SO2 deviation from the ideal bond, angle occurs due to the presence of a lone pair.
e.g (iii) SnCl2
In stannous chloride, Sn has 5s2 5p2 valence electrons. The two unpaired electrons of the 5p orbital take part in the bond formation of a covalent bond with chlorine, while the pair of electrons of 5s remains a lone pair and does not participate in bond formation. Hence electron geometry in SnCl2 is a triangular planner while molecule geometry is an angular or bent structure. In SnCl2 deviation from the ideal bond, angle occurs due to the presence of a lone pair.
Shape of molecules with four electron pairs:
e.g (i) CH4

The central atom C has four electron pairs so the molecule is tetrahedral with a bond angle of 109.5o.
e.g (ii) NH3

The central atom N has four electron pairs so electron geometry in NH3 is tetrahedral while molecule geometry is pyramidal. In NH3 deviation from the ideal bond angle occurs due to the presence of a lone pair of electrons and the angle reduces to 107.5 o.
e.g (iii) H2O

The central atom O has four electron pairs so electron geometry in H2O is tetrahedral while molecule geometry is angular or bent structure. In H2O deviation from the ideal bond angle occurs due to the presence of two lone pairs of electrons and the angle reduces to 104.5 o.

Limitations of VSEPR Theory
Although this theory is good enough to explain molecular shapes and bond angles:
- it fails to explain the mechanism of the formation of covalent bonds.
- it fails to explain why two electrons of the same pair do not repel each other.
- it fails to explain the paramagnetic nature of oxygen.
Continue Reading
MO Diagram for Li 2 ,Li+2 , Li -2
Frequently Asked Questions-FAQs
What is the basis of VSEPR theory?
The VSEPR model, also known as the “Valence Shell Electron Pair Repulsion Theory,” is based on the idea that all atoms have a repulsion between their pairs of valence electrons, and that these atoms will always seek to arrange themselves in a way that minimises this repulsion.
Why is VSEPR theory important?
It is obvious that understanding a molecule’s form is crucial if one is to comprehend its responses. A straightforward mechanism for predicting the geometries of compounds is also desirable. The VSEPR approach is the most practical prediction technique available for main group chemicals.
What is difference between VBT and VSEPR theory?
VSEPR theory and valence bond theory are different in that VSEPR theory describes how molecules are formed, whereas valence bond theory explains how molecules are joined together chemically.
What does VSEPR stand for?
Valence shell electron pair repulsion is referred to as VSEPR. It is a theory that is used to determine how molecules will be arranged.
What does VSEPR predict?
Molecules’ shapes, including bond angles, are predicted by VSEPR.
Check out free notes !!
-> Class 10 Chemistry Full book pdf
-> Class 11 Chemistry Full book pdf
-> Class 12 Chemistry Full book pdf
For Chemistry Notes or Tutorials
We are a group of volunteers and starting a new scheme in our community. Your web site offered us with valuable information to work on. You’ve done an impressive job and our whole community will be grateful to you.
Nicely put, With thanks!canadian pharmacies that ship to us cheap prescription drugs online
Oh my goodness! Incredible article dude! Thank you, However I am having difficulties with your RSS. I don’t understand the reason why I am unable to join it. Is there anybody else having similar RSS problems? Anyone who knows the answer can you kindly respond? Thanx!
It’s the best time to make some plans for the future and it is time to be happy. I have read this post and if I could I want to suggest you some interesting things or advice. Perhaps you can write next articles referring to this article. I wish to read more things about it!
I couldn’t resist commenting. Perfectly written!
Great work! This is the type of info that should be shared around the net. Shame on the search engines for not positioning this post higher! Come on over and visit my website . Thanks =)
Hi there! I could have sworn I’ve visited this website before but after browsing through a few of the articles I realized it’s new to me. Nonetheless, I’m certainly happy I found it and I’ll be bookmarking it and checking back frequently!|
Pingback: Why the bond angle in ammonia is 107 and that in water is 104 while both of them are sp3 hybridised?
Pingback: Why CO2 is linear while H2O is bent Shape?- Chemical Bonding