Question

Assume that the third-period element phosphorus forms a diatomic molecule, P_2, in an analogous way as nitrogen does to form N_2. Select the correct electronic configuration for P_2. [Ne_2](sigma_3s)^2(sigma*_3s)^2(pi_3py)^2(pi_3pz)^2(sigma_3px)^1 [Ne_2](sigma_3s)^2(sigma*_3s)^2(pi_3px)^2(pi_3py)^2(pi_3pz)^1 [Ne_2](sigma_3s)^2(sigma*_3s)^2(pi_3py)^2(pi_3pz)^2(sigma_3px)^1 Calculate its bond order. What are its magnetic properties? diamagnetic paramagnetic

Answer 1

Now determine the bond order which is one-half the difference between the number of electron in bonding molecular orbitals and the number in antibonding molecular orbitals. Bond orser = 1/2 (Number of e^- in bonding MOs) - (Number of e^- in antibonding MOs) = 1/2 (8) - (2) = 3 The P2 molecule has no unpaired electrons, it is diamagnetic.