Chemistry - CHEMICAL BONDING Question with Solution | TestHub

Diamagnetic molecules have all electrons paired in their molecular orbitals. Paramagnetic molecules have unpaired electrons.

Li₂ (6 e⁻): $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^2({\sigma }_{2s}{)}^2$ - Diamagnetic

F₂ (18 e⁻): $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^2({\sigma }_{2s}{)}^2({\sigma }_{2s}^{\ast }{)}^2({\sigma }_{2p_z}{)}^2({\pi }_{2p_x}{)}^2({\pi }_{2p_y}{)}^2({\pi }_{2p_x}^{\ast }{)}^2({\pi }_{2p_y}^{\ast }{)}^2$ - Diamagnetic

H₂⁺ (1 e⁻): $({\sigma }_{1s}{)}^1$ - Paramagnetic

B₂ (10 e⁻): $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^2({\sigma }_{2s}{)}^2({\sigma }_{2s}^{\ast }{)}^2({\pi }_{2p_x}{)}^1({\pi }_{2p_y}{)}^1$ - Paramagnetic

C₂ (12 e⁻): $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^2({\sigma }_{2s}{)}^2({\sigma }_{2s}^{\ast }{)}^2({\pi }_{2p_x}{)}^2({\pi }_{2p_y}{)}^2$ - Diamagnetic

H₂⁻ (3 e⁻): $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^1$ - Paramagnetic

NO⁺ (14 e⁻): $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^2({\sigma }_{2s}{)}^2({\sigma }_{2s}^{\ast }{)}^2({\sigma }_{2p_z}{)}^2({\pi }_{2p_x}{)}^2({\pi }_{2p_y}{)}^2$ - Diamagnetic

The diamagnetic molecules are Li₂, F₂, C₂, and NO⁺. There are 4 such molecules.