hey guys tell me about hybridisation
Answers
hii!!
here is ur answer
hybridization is intermixing of pure atomic orbitals and redistributing into new hybrid orbitals which have almost same energy
no of hybrid orbitals= surrounding atoms+half of (group number-valency +/- charge)
no.of orbitals. hybridization
2 sp hybridization
3. sp2
4. sp3
5. Sp3d
6. sp3d2
examples:
CH4
no of hybrid orbitals = 4+1/2(4-4)
= 4+0
=4
that means sp3 hybridization
here no of surrounding atoms=4
group no of carbon=4
and valency =4
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Answer:
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hybridization is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory. Hybrid orbitals are very useful in the explanation of molecular geometry and atomic bonding properties and are symmetrically disposed in space.
Hybridisation describes the bonding of atoms from an atom's point of view. For a tetrahedrally coordinated carbon (e.g., methane CH4), the carbon should have 4 orbitals with the correct symmetry to bond to the 4 hydrogen atoms.
Carbon's ground state configuration is 1s2 2s2 2p2 or more easily read:
C ↑↓ ↑↓ ↑ ↑
1s 2s 2p 2p 2p
The carbon atom can use its two singly occupied p-type orbitals, to form two covalent bonds with two hydrogen atoms, yielding the singlet methylene CH2, the simplest carbene. The carbon atom can also bond to four hydrogen atoms by an excitation (or promotion) of an electron from the doubly occupied 2s orbital to the empty 2p orbital, producing four singly occupied orbitals.
C* ↑↓ ↑ ↑ ↑ ↑
1s 2s 2p 2p 2p
The energy released by the formation of two additional bonds more than compensates for the excitation energy required, energetically favouring the formation of four C-H bonds.
In CH4, four sp3 hybrid orbitals are overlapped by hydrogen 1s orbitals, yielding four σ (sigma) bonds (that is, four single covalent bonds) of equal length and strength.
A schematic presentation of hybrid orbitals overlapping hydrogen orbitals translates into Methane's tetrahedral shape
sp2 Edit
Three sp2 orbitals.
Ethene structure
See also: trigonal planar molecular geometry
Other carbon compounds and other molecules may be explained in a similar way. For example, ethene (C2H4) has a double bond between the carbons.