Molecular Orbital Theory (MOT)

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.

What will be the bond order of the species with electronic configuration $\mathrm{ }1{\mathrm{s}}^2\mathrm{ }2{\mathrm{s}}^2\mathrm{ }2{\mathrm{p}}^5$?(one/two/three)

The correct bond order in the following species is

Molecules having no unpaired electrons gives rise to _____ character. (Diamagnetic/Paramagnetic)

Which one of the following species does not exist under normal conditions?

Choose the paramagnetic oxide in the following:

Which of the following pairs will have same bond order?

What will be the bond order of the diatomic species with the elemental electronic configuration :$\mathrm{ }1{\mathrm{s}}^2\mathrm{ }2{\mathrm{s}}^2\mathrm{ }2{\mathrm{p}}^5$?

A hydrogen atom is paramagnetic. A hydrogen molecule is

Which of the following statements is incorrect?

Which of the following species is least stable?

What is the bond order in ${\mathrm{O}}_2^{2-}$?

O₂ molecule is paramagnetic due to presence of :