HYBRIDISATION : Derivation Of Wave Function For The Following Orbital Hybridisation Type : sp ( BeH2 ) , sp2 ( BF3 ) , sp3 ( CH4 )

HYBRIDISATION
STEPS INVOLVED IN HYBRIDISATION
TYPES OF HYBRIDISATION
sp HYBRIDISATION ( BeH2 )
sp2 HYBRIDISATION ( BF3 )
sp3 HYBRIDISATION (CH4 )
DERIVATION OF WAVE FUNCTION FOR sp sp2 AND sp3 HYBRIDISATION
REFERENCE

1. TOPIC :- HYBRIDISATION : Derivation Of Wave Function For The Following Orbital Hybridisation Type : sp ( BeH 2 ) , sp 2 ( BF 3 ) , sp 3 ( CH 4 )

2. CONTENT HYBRIDISATION STEPS INVOLVED IN HYBRIDISATION TYPES OF HYBRIDISATION sp HYBRIDISATION ( BeH 2 ) sp 2 HYBRIDISATION ( BF 3 ) sp 3 HYBRIDISATION (CH 4 ) DERIVATION OF WAVE FUNCTION FOR sp sp 2 AND sp 3 HYBRIDISATION REFERENCE

3. HYBRIDISATION “It is process of mixing and recasting of atomic orbital of same atom with slightly different energies to form equal number of new orbital of equal energy, maximum symmetry and orientation in space.” Linus Carl Pauling  (February 28, 1901 – August 19, 1994 ) Chemist Linus Pauling first developed the hybridisation theory in 1931 in order to explain the structure of simple  molecules such as  methane (CH 4 ) using  atomic orbital's. For his scientific work, Pauling was awarded the Nobel Prize in Chemistry in 1954. LINUS CARL PAULING

4. Steps Involved In Hybridisation : Formation Of An Excited State : No. Of unpaired electron in ground state of an atom is less than the observed valency of atom in its stable compd. Then one or more electron are uncoupled and promoted to the vacant orbitals of higher energy level. Mixing And Recasting Of Atomic Orbital : Mixing & redistribution of atomic orbital of the atom having same energy to form new orbital of equal energy.

5. Orientation Of Hybrid Orbitals : Hybrid orbital orients themselves in a space in such a way that they minimize the inter electronic repulsion to acquire max. Stability. Energy Of Orbitals : Hybrid Orbitals Have Equivalent Energy And Differ Only In Orientation.

6. TYPES OF HYBRIDISATION : Types Of Hybridisation Which We Have To Study Are : sp hybridisation ( BeH 2 ) sp 2 hybridisation ( BF 3 ) sp 3 hybridisation (CH 4 )

7. sp hybridisation for BeH 2 ( beryllium hydride ) molecule : It is the process of mixing and recasting of one s and one p orbital of same atom with nearly equal energy to form two sp hybridised orbital having equivalent energy, maximum symmetry and definite orientation in a space. Need for hybridisation : The observed valency of Be in BeH 2 is two and it has a bond angle of 180⁰ with a linear geometry which can be explained on the basis of hybridisation. sp hybridisation of Be atom : Ground state electronic configuration for Be is 1s 2 2s 2 1s 2 2s 2 2 Px 2 Py 2 Pz Be in excited state has electronic configuration 1s 2 2s 1 2p 1 1s 2 2s 2 2 Px 2 Py 2 Pz

8. Be in hybridised state has electronic configuration : 1s 2 sp hybridised orbital Orbital Overlap : the two half filled sp hybrid orbital of Be atom overlap axially with half filled 1s orbital of two hydrogen atom to form two Be – H ( sp – sp ) sigma bond

9. Bond angle : The H – Be—H bond angle in BeH 2 is 180⁰ Geometry : linear

10. sp 2 hybridisation for BF 3 ( boron trifluride ) molecule : It is the process of mixing and recasting of one s and two p orbital of same atom with nearly equal energy to form three sp 2 hybridised orbital having equivalent energy, maximum symmetry and definite orientation in a space. Need for hybridisation : The observed valency of boron in BF 3 is three and it has a bond angle of 120⁰ with a trigonal planar geometry which can be explained on the basis of hybridisation. sp 2 hybridisation of Boron atom : Ground state electronic configuration for Boron is 1s 2 2s 2 2p 1 1s 2 2s 2 2 Px 2 Py 2 Pz Boron in excited state has electronic configuration 1s 2 2s 1 2 Px 1 2 Py 1 1s 2 2s 2 2 Px 2 Py 2 Pz

11. Boron in hybridised state has electronic configuration : 1s 2 sp 2 hybridised orbital Orbital Overlap : each half filled sp 2 hybrid orbital of Boron atom overlap axially with half filled 2p z orbital of fluorine atom containing electron with opposite spin thus the BF 3 molecule is formed. Each B – F bond is formed by ( sp 2 – p ) axial overlap. Hence it is a strong sigma bond

12. Bond angle : The F – B—F bond angle in BF 3 is 120⁰ Geometry : Trigonal Planar

13. sp 3 hybridisation for CH 4 ( methane ) molecule : It is the process of mixing and recasting of one s and three p orbital of same atom with nearly equal energy to form four sp 3 hybridised orbital having equivalent energy, maximum symmetry and definite orientation in a space. Need for hybridisation : The observed valency of carbon in methane is four and it has a bond angle of 109⁰ 28′ with a tetrahedron geometry which can be explained on the basis of hybridisation. sp 3 hybridisation of carbon atom : Ground state electronic configuration for carbon is 1s 2 2s 2 2p 2 1s 2 2s 2 2 Px 2 Py 2 Pz carbon in excited state has electronic configuration 1s 2 2s 1 2 Px 1 2 Py 1 2 Pz 1 1s 2 2s 2 2 Px 2 Py 2 Pz

14. carbon in hybridised state has electronic configuration : 1s 2 sp 3 hybridised orbital Orbital Overlap : each half filled hybrid orbital of carbon atom overlap axially with half filled 1s orbital of hydrogen atom containing electron with opposite spin thus the CH 4 molecule is formed.

15. Bond angle : The H – C bond angle in CH 4 is 109⁰ 28′ Geometry : Tetrahedral

16. Derivation of wave function for sp hybridisation for BeH 2

17. Derivation of wave function for sp 2 hybridisation for BF 3

18. Derivation of wave function for sp 3 hybridisation for CH 4

19. REFERENCE Inorganic Chemistry By, Madan Malik And Tuli Inorganic Chemistry By, J. D. Lee Advance Inorganic Chemistry By, Cotton And Wilkinson