Molecular Orbital Theory

Explain Molecular Orbital Theory.

Bonding molecular orbitals are formed if two atomic orbitals are overlapping destructively.

Explain the type of overlapping of atomic orbitals involved in the formation of bonding molecular orbital.

The number of antibonding electrons in a molecule of carbon monoxide are:

The shape of an atomic orbital is determined by the type of the atomic orbital (s, p, d or f), while the shape of a molecular orbital is determined by the shapes of atomic orbitals that make the molecule.

Write the moleuclar orbital diagram of Lithium diatomic molecule.

How many molecular orbitals are formed by the overlapping of $2\mathrm{p}$ atomic orbitals?

Draw the molecular orbital energy level diagram of boron diatomic molecule.

Label the molecular orbitals formed by the combination of atomic orbitals $2\mathrm{s}+2\mathrm{s}$.

Explain how p-p orbital overlapping along the internuclear axis.

Explain how s-s orbital overlapping along the internuclear axis.

Shape of p_x-orbital and s-orbital is _____ respectively.

Explain how pi$\left(\mathrm{\pi }\right)$ bond form.

Write the salient features of molecular orbitals.

Write any three differences between molecular orbitals and atomic orbitals.

Define molecular orbitals.

If an extra electron is added to the hypothetical molecule ${\mathrm{C}}_2,$ this extra electron will occupy the molecular orbital:-

Which of the following order of energies of molecular orbitals is correct for ${\mathrm{N}}_2$?

The correct statement with regard to ${{\mathrm{H}}_2}^{+} \mathrm{and} {{\mathrm{H}}_2}^{-}$ is:

Consider the following molecular geometries:

$\mathrm{NO}, \mathrm{CO}, {\mathrm{O}}_2$
Select correct statement(s) about these: