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LUCKNOW UNIVERSITY
Internal assessment
M.Sc. semester – III
TOPIC- Molecular orbital theory
Submitted to-
Department of chemistry
Isabella Thoburn college
Lucknow.
Submitted by-
Name – Sneha Manjul
Class – M.Sc. Semester III
Roll no – Z/22/19
Session – 2022- 2023
CHEMISTRY PRESENTATION
MOLECULAR
ORBITAL THEORY
INTRODUCTION
 MOT - initially developed by Robert S. Mullikan.
- the bonding between atoms is described.
- provides answers to more complex
questions.
- allows one to predict the distribution of
electrons
 And this in turn can help predict molecular
properties such as shape, magnetism, and Bond
Order.
PRINCIPLES OF MOT
 In molecules, atomic orbitals combine to form
molecular orbitals which surround the
molecule.
Molecular Orbitals
Bonding Antibonding
 Molecular bonds have lower potential energy
than in separate atomic orbitals.
 Thus, electrons prefer to stay in a molecular
bond.
Equal no. of orbitals Order of Energy
Atomic orbitals of
like energies.
Following both
the Pauli exclusion
principle and Hund's
rule
Principles
Antibonding
Molecular
Orbital
Bonding
Molecular
Orbital
SIGMA BONDS (σ)
 They are symmetrical about the axis

Antibonding
Sigma Orbital
(abbreviated σ*)
Bonding Sigma
Orbital
(abbreviated σ)
PI BONDS (π)
 The pi bonding bonds as a side to side
overlap, which then causes there to be no
electron density along the axis, but there is
density above and belong the axis.
DETERMINING BOND ORDER
 Bond Order indicates the strength of the bond.
The higher the Bond Order, the stronger the
bond.
Bond Order= 1/2(a-b)
where, a = number of e- in bonding Molecular Orbitals
b = number of e- in antibondng Molecular Orbitals.
STABILITY OF THE MOLECULE
 If the Bond Order is Zero, then no bonds are
produced and the molecule is not stable (for
example He2).
 If the Bond Order is 1, then it is a single
covalent bond.
 The higher the Bond Order, the more stable
the molecule is.
sneha manjul msc 3 sem chemistrypresentation-mot-paper 5.pdf

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sneha manjul msc 3 sem chemistrypresentation-mot-paper 5.pdf

  • 1. LUCKNOW UNIVERSITY Internal assessment M.Sc. semester – III TOPIC- Molecular orbital theory Submitted to- Department of chemistry Isabella Thoburn college Lucknow. Submitted by- Name – Sneha Manjul Class – M.Sc. Semester III Roll no – Z/22/19 Session – 2022- 2023
  • 3. INTRODUCTION  MOT - initially developed by Robert S. Mullikan. - the bonding between atoms is described. - provides answers to more complex questions. - allows one to predict the distribution of electrons  And this in turn can help predict molecular properties such as shape, magnetism, and Bond Order.
  • 4. PRINCIPLES OF MOT  In molecules, atomic orbitals combine to form molecular orbitals which surround the molecule. Molecular Orbitals Bonding Antibonding
  • 5.  Molecular bonds have lower potential energy than in separate atomic orbitals.  Thus, electrons prefer to stay in a molecular bond.
  • 6. Equal no. of orbitals Order of Energy Atomic orbitals of like energies. Following both the Pauli exclusion principle and Hund's rule Principles
  • 8.
  • 9. SIGMA BONDS (σ)  They are symmetrical about the axis  Antibonding Sigma Orbital (abbreviated σ*) Bonding Sigma Orbital (abbreviated σ)
  • 10.
  • 11.
  • 12. PI BONDS (π)  The pi bonding bonds as a side to side overlap, which then causes there to be no electron density along the axis, but there is density above and belong the axis.
  • 13.
  • 14. DETERMINING BOND ORDER  Bond Order indicates the strength of the bond. The higher the Bond Order, the stronger the bond. Bond Order= 1/2(a-b) where, a = number of e- in bonding Molecular Orbitals b = number of e- in antibondng Molecular Orbitals.
  • 15. STABILITY OF THE MOLECULE  If the Bond Order is Zero, then no bonds are produced and the molecule is not stable (for example He2).  If the Bond Order is 1, then it is a single covalent bond.  The higher the Bond Order, the more stable the molecule is.