Chapter 10, Problem 10.5DQ

(a)

Interpretation Introduction

Interpretation:

The formation of hydrogen bonds in terms of electrostatic interactions has to be given.

Concept Introduction:

Dipole moment is defined as the product of the charge and the separation between the two atoms. Polar molecules possess permanent dipole moment.

A hydrogen bonding is partially an electrostatic attraction between $\text{H}$ atom which is bonded to more electronegative atom such as $\text{N, O, or}\text{F}$ and another adjacent atom bearing a lone pair of electron. The hydrogen bonding takes place within a molecule is called as intramolecular hydrogen bonding.

(b)

Interpretation Introduction

Interpretation:

The formation of hydrogen bonds in terms of molecular orbitals has to be given.

Concept introduction:

Dipole moment is defined as the product of the charge and the separation between the two atoms. Polar molecules possess permanent dipole moment.

A hydrogen bonding is partially an electrostatic attraction between $\text{H}$ atom which is bonded to more electronegative atom such as $\text{N, O, or}\text{F}$ and another adjacent atom bearing a lone pair of electron. The hydrogen bonding takes place within a molecule is called as intramolecular hydrogen bonding.

Molecular orbital (MO) theory:  is a method for determining molecular structure in which electrons are not assigned to individual bonds between atoms, but are treated as moving under the influence of the nuclei in the whole molecule.

According to this theory there are two types of orbitals,

• Bonding orbitals
• Antibonding orbitals

Electrons in molecules are filled in accordance with the energy; the anti-bonding orbital has more energy than the bonding orbitals.