Question

Hybridization of carbon in H3C-CH3 ?

Answer 1

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Hybrid orbital are formed by the overlapping of orbitals having almost same energy.

Single bond= one sigma bond = sp3 hybridization

Double bond = one sigma bond + one pie bond = sp2 hybridization

Triple bond = one sigma bond + two pie bond = sp hybridization

(a)



 According to structure, C1 & C2 are making 4 sigma bonds(single bond) each with the help of one s hybrid orbital & 3 p hybrid orbital, hence C1& C2 are sp3 hybridised

Answer 2

Answer:

Hybridization is the concept of combining two atomic orbitals to create a new type of hybridized orbitals. Typically, this mixing produces hybrid orbitals with completely distinct energies, shapes, etc. In hybridization, the same-energy level atomic orbitals are primarily involved.

Explanation:

Each carbon of ethane (H₃C-CH₃) possesses four sigma bonds, zero lone pair of electrons, and zero pi-bond.

The lone pair of electrons and pi-bonds are not included in the hybridization. So, only the Sigma bonds are included in the hybridization of a molecule.

With each carbon, three C-H bonds are formed and one C-C bond is formed. So, the total number of sigma bonds is 4.

Thus, each carbon possesses 4 sigma bonds, and its hybridization is sp³.

Hence, the hybridization of carbon in H₃C-CH₃ is sp³.

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