Hybridization of Carbon in (CH3)2CO

Hybridization is a concept of mixing atomic orbitals to form new hybrid orbitals for bonding. The hybridization of each carbon in the compound (CH3)2CO can be determined by following the steps given below:

Step 1: Determine the total number of valence electrons in the compound

- Carbon has four valence electrons
- Hydrogen has one valence electron
- Oxygen has six valence electrons

Therefore, the total number of valence electrons in the compound (CH3)2CO is:

2(C) + 6(H) + 1(O) = 2×4 + 6×1 + 1×6 = 20 valence electrons

Step 2: Determine the molecular geometry of the compound

- The central atom is carbon
- The surrounding atoms are two hydrogen atoms and one oxygen atom

Therefore, the molecular geometry of the compound (CH3)2CO is trigonal planar.

Step 3: Determine the hybridization of each carbon

- In the trigonal planar geometry, the carbon atom is surrounded by three regions of electron density (one double bond and two single bonds)
- The hybridization of carbon is determined by the number of regions of electron density around it

Therefore, the hybridization of each carbon in the compound (CH3)2CO is:

- The carbon atom in the double bond is sp2 hybridized
- The carbon atoms in the single bonds are sp3 hybridized

Hence, the correct answer is option C, i.e., sp3, sp2.