Chapter 6, Problem 9P

Interpretation Introduction

Interpretation: Whether ${\text{H}}_{\text{2}}$ or ${\text{He}}_{\text{2}}{}^{+}$ that has the larger bond energy should be determined.

Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.

Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.

Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.

In sigma $\left(\sigma \right)$ bonding orbital, electron density is shared directly between bonding atoms, along bonding axis. In sigma $\left({\sigma }^{*}\right)$ antibonding orbital, the orbital is empty. In these orbital’s electrons are along nuclear axis.

In pi $\left(\pi \right)$ bonding orbital, bonding electron lies above and below bonding axis and has no electron on bonding axis.

In pi $\left({\pi }^{*}\right)$ antibonding orbital, the orbital is empty. In these orbital, electrons are perpendicular to nuclear axis.