Chapter 7.8, Problem 7.8.1SR

Interpretation Introduction

Interpretation:

It should be determined the number of delocalized π-bonds for the given ion.

Concept introduction:

According to valence bond theory,

• The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.
• The each overlapping atomic orbital must be contained with a single unpaired.
• Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.

  Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis.

  Pi (π) bonds: the bonds in which shared un-hybridized orbital’s (p, d, etc.) electron density are concentrated in above and below of the plane of the molecule.

  Double bonds: One sigma bond and one pi bond are together known as a double bond.

According to Molecular orbital (MO) theory,

• The atomic orbitals of the atoms constituted in a molecule are combined to produce new orbitals are called Molecular Orbitals.
• Like atomic orbitals, a molecular orbital can accommodate maximum two electrons and the two electrons must have opposite spins (Pauli Exclusion Principle).
• Relative energy levels of molecules are according to the energy levels of atomic orbitals.