It is PPT on HYBRIDISATION of orbitals. It is relative to class 11 CBSE. I prepared this for school project. It is very useful as it provides you a lot in nutshell.

1. HYBRIDISATION
Class:- XI-A
Computer Science
~Vishal Singh
Roll- No. 56

2. • WHAT IS HYBRIDISATION?
HYBRIDISATION IS A PROCESS IN WHICH TWO OR
MORE ATOMIC ORBITALS OF VALENCE SHELL OF AN
ATOM MIX UP TO FORM THE SAME NUMBER OF
IDENTICAL ORBITALS OF EQUAL ENERGY.

3. PURPOSE OF HYBRIDISATION
• THE PURPOSE OF HYBRIDISATION IS TO SEE THE
TYPES OF BONDS THAT THE ATOMS SHARE WITH
EACH OTHER, IT MAY BE SIGMA OR PI BONDS
• THE DIFFERENT TYPES OF BONDS ALLOW
DIFFERENT PROPERTIES LIKE HOW PI BONDS DO
NOT ALLOW ROTATION WHEREAS SIGMA BONDS ARE
ROTATIONAL.

4. FEATURES OF HYBRIDISATION :-
• THE HYBRID ORBITALS ARE EQUIVALENT IN ENERGY AND
SHAPE .
• THE ORBITALS TAKING PART IN HYBRIDISATION MUST HAVE
ONLY SMALL DIFFERNCE IN ENERGY.
• THE NUMBER OF HYBRID ORBITALS IS THE SAME AS THE
NUMBER OF ATOMIC ORBITALS THAT UNDERGO
HYBRIDISATION.
• BOTH HALF FILLED AND COMPLETELY FILLED TAKE PART IN
HYBRIDISATION.
• HYBRID ORBITALS FORM MORE STABLE BONDS
• THE TYPE OF HYBRIDISATION GIVES THE SHAPE OF
MOLECULES.

6. 1. Sp hybridisation
This involves the mixing up of one s orbital
and one p orbital of valence shell of an
atom to form two new equivalent orbitals.
These sp orbitals are oriented at an angle
of 180°.
• The two sp orbitals are linear.
• It is also known as diagonal
hybridization
• For Example: BeF2

7. BeF2
•Be shows divalency in its compounds.
•One 2s and one 2p orbital of Be hybridise to form two sp
hybrid orbitals and they are
oriented in linear manner
•Each of the sp orbitals overlaps axially with half filled 2p
orbital of fluorine to form 2 Be-F
bonds.
•BeF2 is linear and bond angle of 180°.

8. 2. sp2 hybridisatoin
The intermixing of one s and two p orbitals of the
valency shell of an atom to form 3 identical orbitals
called sp2 hybridisation.
Also called Trigonal hybridisation
The three sp2 hybrid orbitals are oriented in trigonal
planar symmetry at angles of 120° with each other.
Sp2 orbitals have 33% s character and 67% p character.
Eg- BF3

9. BF3 Molecule
• One of the 2s electron is promoted to the vacant 2p orbital, then the
excited state of B has three unhybridised orbitals
The 3 sp2 hybrid orbitals of boron overlap with half filled 2p orbitals to
form three B-F bonds.
• It is planar

10. 3. sp3 hybridisation
• The intermixing of one s and three p orbitals of the valence shell of an
atom to give rise to 4 identical orbitals called sp3 hybridisation.
• Four sp3 hybrid orbitals are directed towards the four corners of a
tetrahedron.
• Each sp3 has 25% s character and 75% p character.
• Bond angle is 109°28’
• Also known as tetrahedral hybridisation
• Eg- methane

11. Methane (CH4)
• Methane carbon is sp3 hybridised.
• Each sp3 hybrid orbital of carbon overlaps
axially with half filled orbital of H atom forming
four C-H sigma bonds
• Methane have a tetrahedral shape.
• C-H bond length is 1.09 A°.

12. WHY DO WE NEED HYBRIDISATION?
• CARBON HAS FOUR UNPAIRED ELECTRONS
SO,IT CAN HAVE FOUR EQUAL ENERGY BONDS.
• THE HYBRIDISATION OF ORBITALS IS ALSO
GREATLY FAVOURED BECASUSE HYBRIDISED
ORBITALS ARE LOWER IN ENERGY COMPARE
• TO THEIR SEPARATED, UNHYBRIDISED
COUNTERPARTS
• THIS RESULTS IN MORE STABLE
COMPOUNDS WHENHYBRIDISATION OCCURES

13. ADVANTAGE OF HYBRIDISATION?
• THE MOST IMPORTANT ADVANTAGE IS
THE DETERMINATION OF SHAPE AND
GEOMETRY OF THE MOLECULE
• IT DETERMINES THE POSITION AND
STRUCTURE OF THE COMPOUND
• IT EXPLAINS THE VARIOUS
PROBABILITIES OF PHYSICAL AND
CHEMICAL BEHAVIOR

14. CONCLUSION
• IN CHEMISTRY, ORBITAL
HYBRIDISATTION IS CONCEPT OF
MIXING ATOMIC ORBITALS INTO NEW
HYBRID ORBITALS.
• IT IS SUITABLE FOR PAIRING OF
ELECTRONS TO FORM CHEMICAL
BONDS IN VALANCE BOND THEORY.

15. Thank
You