Question

Describe the hybrid orbitals used by the central atom and the types of bonds formed in cocl2 (c is central). hybrid orbitals: sp sp2 sp3 sp3d sp3d2 how many σ and π bonds are present in the molecule? σ bonds: π bonds

Answer 1

CoCl2 with C as the central atom uses sp hybridization to form two sigma (σ) bonds with chlorine atoms, along with two pi (π) bonds as part of the double bonds with each chlorine.

Step-by-step explanation:

In the molecule CoCl2 with carbon (C) as the central atom, the hybridization of the central carbon is sp hybridization. The molecule has a linear geometry, which corresponds with the carbon atom making use of its 2s orbital and one of its 2p orbitals to create two sp hybrid orbitals. These hybrid orbitals form sigma (σ) bonds with each chlorine atom.

Additionally, the carbon atom will form a double bond with each chlorine, consisting of a σ bond and a pi (π) bond. The σ bonds in CoCl2 result from the head-on overlap of sp orbitals of carbon with the orbitals of chlorine atoms, while the π bonds result from the side-by-side overlap of unhybridized p orbitals.

Overall, CoCl2 has a total of two σ bonds (one in each C-Cl bond) and two π bonds (one in each C-Cl double bond).