Problem: Use the molecular orbital diagram shown to determine the bond order for NO +. Is NO+ paramagnetic or diamagnetic? In molecular orbital names, s = sigma and p = pi.a. 3, paramagneticb. 2, paramagneticc. 2.5, paramagneticd. 2, diamagnetice. 3, diamagnetic

Construct the molecular orbital diagram of NO⁺ and calculate for the bond order and determine if its paramagnetic or diamagnetic

Step 1: Calculate the total number of valence electrons present.

Step 2: Draw the molecular orbital diagram.

Step 3: Determine if there's an unpaired MO (paramagnetic or diamagnetic)

Step 4: Calculate the bond order of the molecule/ion. Recall that the formula for bond order is:

$\boxed{\mathbf{Bond}\mathbf{ }\mathbf{order}\mathbf{ }\mathbf{=}\mathbf{ }\frac{\mathbf{1}}{\mathbf{2}}\left[\mathbf{\#}\mathbf{ }{\mathbf{e}}^{\mathbf{-}}\mathbf{ }\mathbf{in}\mathbf{ }\mathbf{bonding}\mathbf{ }\mathbf{MO}\mathbf{ }\mathbf{-}\mathbf{ }\mathbf{\#}\mathbf{ }{\mathbf{e}}^{\mathbf{-}}\mathbf{ }\mathbf{in}\mathbf{ }\mathbf{anti}\mathbf{-}\mathbf{bonding}\mathbf{ }\mathbf{MO}\mathbf{ }\right]}$