Molecular Orbitals for First- and Second-Row Diatomic Molecules
This Demonstration considers the molecular orbitals for the diatomic molecules through. The conceptual relationship to the constituent atomic orbitals is shown in a schematic energy diagram. Antibonding MOs are shown in red. The bond order of a molecule is defined as the number of electrons occupying bonding MOs minus the number occupying antibonding MOs, all divided by 2, to coincide with the conventional chemical definition of single, double, and triple bonds. The molecules and have bond orders equal to 0, and exist only as weakly-associated van der Waals dimers. also has bond order 0, but forms a weak chemical bond attributed to some 2s-2p hybridization. The "molecular data" checkbox brings up the ground state electron configuration and spectroscopic designation for each diatomic. The dissociation energy is also given, showing an expected increase with bond order.
Snapshot 1: the simplest diatomic molecule , with bond order 1; the hydrogen molecule ion is also stable with a formal bond order of 1/2 and =2.79 eV
Snapshot 2: the nitrogen molecule has an excess of six occupied bonding over antibonding orbitals, thus a bond order of 3, a triple bond
Snapshot 3: diatomic oxygen is predicted to be paramagnetic in a triplet electronic state, a major triumph of molecular-orbital theory
Reference: S. M. Blinder, Chap. 11, Introduction to Quantum Mechanics, Amsterdam: Academic Press, 2004.