Hybridization is a process where atomic orbitals mix to form new identical hybrid orbitals of equal energy. It allows atoms to form sigma and pi bonds to share electrons with other atoms. The type of hybridization determines the shape and structure of molecules. Sp hybridization forms linear molecules, sp2 forms triangular molecules, and sp3 forms tetrahedral molecules. Examples are given of BeCl2 with sp hybridization and BF3 with sp2 hybridization. Hybridization lowers the energy of orbitals and allows more stable bonding between atoms.

1. 198213
JONISHA

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
sp HYBRIDISATION : LINIER
sp2 HYBRIDISATION : TRIANGULAR
sp3HYBRIDISATION : TETRAHEDRAL
dsp2 HYBRIDISATION : SQUARE PLANAR
dsp3 HYBRIDISATION : TRIGONAL BI PYRAMIDAL
d2sp3 HYBRIDISATION : OCTAHEDRAL
d3sp3 HYBRIDISATION : PENTAGONAL BIPYRAMIDAL

5.  SP HYBRIDISATION
• IT INVOLVES THE MIXING OF ONE s AND
ONE p ORBITAL TO PRODUCE TWO
IDENTICAL ORBITALS CALLED sp HYBRID
ORBITALS

6.  STRUCTURE OF BERYLLIUM CHLORIDE (Becl2) sp HYBRIDISATION
• BERILIYUM CHLORIDE , MOLECULE HAS ONE BERILIYUM ATOM AND
TWO CHLORINE ATOMS
• BERILIYUM HAS TWO VELENCY ELECTRONS AND CHLORINE HAS ONE
VELENCY ELECTRON FOR SHARING
Be (4) : [ He] 2s22p0 Cl (17) : [He] 2s22p63s23p6
Be (Excited state) : [He] 2s1 2px
1 2py
0 2pz
0
BeCl2 : [He]
Sp HYBRIDISATION
• DURING THE FORMATION OF BeCl2, 2s AND 2px ORBITALS OF Be
UNDERGO Sp HYBRIDISATION TO FORM TWO IDENTICAL HYBRID
ORBITALS
• THEY ARE ORIENTED LINERLY IN OPPOSITE DIRECTION AT AN ANGLE
OF 180O
• HENCE BeCl2 HAS LINER STRCTURE DUE TO Sp
HYBRIDISATION

7. SP2 HYBRIDISATION
• IT INVOLVES THE MIXING OF ONE s
ORBITAL AND 2p ORBITAL TO PRODUCE 3
IDENTICAL ORBITALS CALLED Sp2 HYBRID
ORBITALS

8.  STRUCTURE OF BORON TRIFLORIDE(BF3)
Sp2 HYBRIDISATION
• A MOLECULE OF BORON TRIFLORIDE CONTAINS ONE
BORON ATOM AND THREE FLORINE ATOMS
• ELECTRONIC CONFIGURATION OF FLORINE
1s2 2s2 2Px2 2Py2 2Pz1
• BORON (ground state) : 1s2 2s2 2p1
• BORON (excited state) : 1s2 2s2 2px1 2py1 2pz0
• 2s 2px AND 2py ORBITALS OF BORON UNDERGO SP2
HYBRIDISATION TO FORM 3Sp2 HYBRID ORBITALS
• THESE ORBITALS OVERLAP WITH 2PZ ORBITALS OF
FLORINE ATOM TO FORM THREE SIGMA BONDS
• HENCE BORON TRIFLORIDE HAS A TRI TRIANGULAR
SHAPE
• THE FLORINE ATOM LIVE AT THE CORNERS OF
EQUILATERAL TRIANGLE
• THE BOND ANGE IN BF3 IS 120O

10.  SP3 HYBRIDISATION
• IT INVOLVES THE MIXING OF 1S ORBITAL AND 3p
ORBITALS TO PRODUCE FOUR IDETICAL
ORBITALS CALLED Sp3 HYBRID ORBITALS

11.  STRUCTURE OF METHANE CH4
• ONE MOLECULE OF METHANE HAS ONE
CARBON ATOM AND FOUR HYDROGEN ATOMS
• ELECTRONIC CONFIGURATION OF CARBON :
1s2 2s2 2px1 2Py1 2pz0
• C(excited state) 1s2 2s1 2px1 2Py1 2pz1
• 12s ORIBITAL AND 32p ORBITAL OF CARBON
ATOM UNDERGO SP3 HYBRIDISATION TO
FORM 4 IDENTICAL HYBRID ORBITALS
• THESE ORBITALS ARE ORIENTED TOWARDS 4
ORNERS OF A REGULAR TETRAHEDRON Cs
• THE FOUR Sp3 HYBRIDE ORBITALS OVERLAP
WITH THE 1s ATOMIC ORBITALS OF FOUR
HYDROGEN ATOMS TO FORM SIGMA BONDS
• HENCE METHANE THERE ARE FOUR C-H
SIGMA BONDS

13. BeCl2

14.  WHY DO WE NEED HYBRIDISATION?
• CARBON HAS FOUR UNPAIRED ELECTRONS
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 WHEN HYBRIDISATION
OCCURES

15. 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

16.  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