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)

Calculate the bond order and predict the magnetic property of ${\mathrm{B}}_2$ molecule.

The correct bond order in the following species is

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

Choose the paramagnetic oxide in the following:

Assertion. Bond order can assume any value including zero.

Reason. Higher the bond order, shorter is the bond length and greater is the bond energy.

From the following select the molecule that cannot exist.

Consider the following molecules: $\mathrm{O}_{2}, \mathrm{Cl}_{2}, \mathrm{Li}_{2}, \mathrm{H}_{2}, \mathrm{B}_{2}, \mathrm{C}_{2}$ and $\mathrm{N}_{2}$
Let $a=$ number of molecules having (bond order $=1$ ) $\mathrm{b}=\text { number of molecules } \text { having (bond order }=2)$
$\mathrm{c}=$ number of molecules having (bond order $=3$ ) $\mathrm{d}=$ number of paramagnetic molecules. Find the value of $(a \times b \times c \times d \times 4.2)$

Which of the following molecule is paramagnetic in nature?

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 :$\mathrm{ }1{\mathrm{s}}^2\mathrm{ }2{\mathrm{s}}^2\mathrm{ }2{\mathrm{p}}^5$?