Answer
The localized electron model describes the bonding in hydrogen cyanide and phosgene by depicting the arrangement of the shared electron pairs between the atoms, which form the respective single, double, and triple bonds.
Work Step by Step
To describe the bonding in hydrogen cyanide (HCN) and phosgene (COCl₂) using the localized electron model, we need to consider the arrangement of the shared electron pairs between the atoms.
Hydrogen Cyanide (HCN):
In hydrogen cyanide, the carbon atom forms a triple bond with the nitrogen atom, and a single bond with the hydrogen atom.
- The carbon-nitrogen triple bond consists of one sigma (σ) bond and two pi (π) bonds, formed by the overlap of the atomic orbitals.
- The carbon-hydrogen single bond is a sigma (σ) bond, formed by the overlap of the carbon and hydrogen atomic orbitals.
- The localized electron model explains the bonding in HCN by showing the shared electron pairs between the atoms, forming the triple bond and the single bond.
Phosgene (COCl₂):
In phosgene, the carbon atom forms a double bond with the oxygen atom and single bonds with the two chlorine atoms.
- The carbon-oxygen double bond consists of one sigma (σ) bond and one pi (π) bond, formed by the overlap of the atomic orbitals.
- The carbon-chlorine single bonds are sigma (σ) bonds, formed by the overlap of the carbon and chlorine atomic orbitals.
- The localized electron model explains the bonding in phosgene by showing the shared electron pairs between the atoms, forming the double bond and the two single bonds.
