Hybridization:
It is defined as the concept of mixing 2 atomic orbitals make a new atomic orbitals here mixing of two orbitals have same energy . In this process atomic orbitals with equal energy level are mixed than can be mixing of ‘s’ , ‘p’ , ‘d’ orbitals.
Formula :-
1/2 [V+ M -C + A ]
Here,
V = No. of valence electrons
M = mono valent atom
C = Positive charge
A = Negative charge
TRICK 1 :-
[ Number of σ (sigma) Bond + No. of Lone pairs = Hybridization ]
IF Sum is 2 then Hybridization is → (SP)
Similarly for 3 → (SP²) For 4 → (SP³) For 5 → (SP³d)
For 6 → ( sp²d ²) For 7 → (SP³d³)
Note : π (pi) bond not consider in Hybridization.
➥Let’s learn with some Examples
NH3 =
No. of σ Bonds in NH3 {3} + No. of lone Pairs in N {1}
So Hybridization is 3 + 1 = 4 (SP3)
PCl5 =
No. of σ Bonds in PCl5 {5} + No. of lone Pairs in P {0}
So Hybridization is 5 + 0 = 5 (SP3d)
CO2 =
No. of σ Bonds in CO2 {2} + No. of lone Pairs in C {0}
So Hybridization is 2 + 0 = 2 (SP)
TRICK 2 :-
Hybridization ➼
No. of valence e + No. of atom Univalent ± charge
2
Note:- (1) Oxygen is not a univalent atom. So if it come then ignore it.
(2 )Here that sign (±) Show that if charge on compound is(+ve) then we take (-ve)in formula and if charge is (-ve) then take (+ve)
➥Let’s learn with some Examples
NH3 → (5 +3 +0 ) ÷ 2 = 8 /2 = 4
We got 4 so Hybridization is (SP³)
NOTE:- Here ,’5′ is valance electrons in Nitrogen and it is bonded with’3′ . univalent atoms (i.e. 3 Hydrogen )
And 0 Net Charge on it is zero ‘0’ .
NH4+ → (5+ 4 -1 ) ÷ 2 = 8/2 = 4
So, Hybridization is (SP3)
NOTE:- Here this compound has (+ve) charge so we took (-ve) charge , in Formula.
PCl5 → (5+5+0 ) ÷ 2 = 5 So Hybridization = SP3d
CO2 → (4 + 0 + 0) ÷ 2 = 2 So Hybridization is = SP
NOTE:- Here we not consider oxygen in formula because Oxygen is not an univalent atom.
IF7 → (7+7 + 0) ÷ 2 = 7 So Hybridization is = SP3d3
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TRICK FOR Increasing or decreasing order…read now………