Hybridization of carbon atoms attached with halogens in haloalkanes & haloarenes are

$sp^3$ & $sp^2$ hybridized respectively

The correct answer is Option (2) → $sp^3$ & $sp^2$ hybridized respectively

1. Haloalkanes

• Structure: In a haloalkane (R−X), the halogen (X) is attached to an alkyl group (R). The carbon atom (C) bonded to the halogen is saturated, meaning it forms four single sigma bonds.
• Example: Chloromethane ($CH_3​Cl$) or Bromoethane ($CH_3​CH_2​Br$).
• Hybridization: A carbon atom with four single bonds (four sigma bonds and no lone pairs) utilizes four equivalent orbitals for bonding, corresponding to one s-orbital and three p-orbitals.
• Conclusion: The carbon atom attached to the halogen in a haloalkane is $sp^3$ hybridized.

2. Haloarenes

• Structure: In a haloarene (Ar−X), the halogen (X) is attached directly to a carbon atom of an aromatic ring (like a benzene ring). The carbon atom bonded to the halogen is also part of a double bond within the aromatic system.
• Example: Chlorobenzene ($C_6​H_5​Cl$).
• Hybridization: The carbon atom attached to the halogen in the ring forms:
• Two sigma bonds with adjacent ring carbons.
• One sigma bond with the halogen.
• One π bond (as part of the delocalized aromatic system).
• This arrangement involves one s-orbital and two p-orbitals for the sigma framework.
• Conclusion: The carbon atom attached to the halogen in a haloarene is $sp^2$ hybridized.

Summary:

• Haloalkane → $sp^3$ hybridized carbon.
• Haloarene → $sp^2$ hybridized carbon.

The correct option is: $sp^3$ & $sp^2$ hybridized respectively