With the help of molecular orbital approach show the `Ne_2` cannot exist as a stable species.

The species that cannot exist is

With the help of molecular orbital theory predict which of the following species are diamagnetic ? H_(2)^(+),O_(2),O_(2)^(2+)

With the help of molecular orbital theory, predict which of the following species is diamagnetic Li_(2)^(+) ,O_2 ,O_(2)^(+) , O_(2)^(2-)

On the basis of molecular orbital theory, explain why He_2 does not exist whereas Hezexists?

Use molecular orbital theory to explain why the Be_2 molecule does not exist.

Explain on the basis of molecular orbital diagram why O_2 should be paramagnetic.

Draw the molecular orbital diagram of N_2 molecule and write its molecular orbital configuration. Calculate the bond order and discuss the extra stability and diamagnetic nature of the molecule.

Depict molecular orbital diagrams of H_2 and F_(2)^(+) ion. Predict which one of the two species will be more stable.

Use the molecular orbital energy level diagram to show that N_(2) would be expected to have a triple bond. F_(2) , a single bond and Ne_(2) , no bond.

According to MOT, two atomic orbitals overlap resulting in the formation of molecular orbital formed. Number of atomic orbitals overlapping together is equal to the molecule orbital formed. The two atomic orbital thus formed by LCAO (linear combination of atomic orbital) in the phase or in the different phase are known as bonding and antibonding molecular orbitals respectively. The energy of bonding molecular orbital is lower than that of the pure atomic orbitals by an amount Delta . This known as the stabilization energy. The enerby of antibonding molecular orbital in increased by Delta' (destabilisation energy). Q . The bond order of N_(2)^(-) is equal to that of