What is the type of hybridisation of eachcarbon in the following compounds?(a) CH3 Cl, (b) (CH3) 2CO, (c) CH 3CN,(d) HCONH 2 , (e) CH3 CH=CHCN

To determine the type of hybridization of each carbon in the given compounds, we need to consider the number of sigma bonds and lone pairs around each carbon atom.

(a) CH3Cl: In CH3Cl, there is one carbon atom bonded to three hydrogen atoms and one chlorine atom. The carbon atom forms three sigma bonds and has no lone pairs. Therefore, the hybridization of the carbon atom in CH3Cl is sp3.

(b) (CH3)2CO: In (CH3)2CO, there is one carbon atom bonded to two methyl groups (CH3) and one carbonyl group (C=O). The carbon atom forms three sigma bonds and has no lone pairs. Therefore, the hybridization of the carbon atom in (CH3)2CO is sp2.

(c) CH3CN: In CH3CN, there is one carbon atom bonded to three hydrogen atoms and one nitrogen atom. The carbon atom forms three sigma bonds and has no lone pairs. Therefore, the hybridization of the carbon atom in CH3CN is sp3.

(d) HCONH2: In HCONH2, there is one carbon atom bonded to one hydrogen atom, one oxygen atom, and one nitrogen atom. The carbon atom forms three sigma bonds and has no lone pairs. Therefore, the hybridization of the carbon atom in HCONH2 is sp2.

(e) CH3CH=CHCN: In CH3CH=CHCN, there are three carbon atoms. The first carbon atom is bonded to three hydrogen atoms and one other carbon atom. The second carbon atom is bonded to two hydrogen atoms and two carbon atoms. The third carbon atom is bonded to one hydrogen atom, one carbon atom, and one nitrogen atom. The first and third carbon atoms form three sigma bonds and have no lone pairs, so their hybridization is sp3. The second carbon atom forms two sigma bonds and one pi bond, and it has no lone pairs. Therefore, the hybridization of the second carbon atom in CH3CH=CHCN is sp2.

In summary: (a) CH3Cl: sp3 hybridization (b) (CH3)2CO: sp2 hybridization (c) CH3CN: sp3 hybridization (d) HCONH2: sp2 hybridization (e) CH3CH=CHCN: sp3 and sp2 hybridization