Bond order and magnetic moment of ${\mathrm{CO}}^{+}$ is

CO⁺ (13 electrons)

In the case of CO, the 2s atomic orbital on oxygen is much lower than the energy than the 2s atomic orbital of carbon ,this discrepancy of energy allows the $\mathrm{\pi }$2px & $\mathrm{\pi }$2py BMO to lower the energy than sigma*2sMO in the MO diagram of CO

$$\begin{gathered} \mathrm{\sigma }1{\mathrm{S}}^2 \mathrm{\sigma }*1{\mathrm{S}}^2 \mathrm{\sigma }2{\mathrm{S}}^2 (\mathrm{\pi }2{\mathrm{P}}_{\mathrm{x}}^2=\mathrm{\pi }2{\mathrm{P}}_{\mathrm{y}}^2)\mathrm{\sigma }2{\mathrm{P}}_{\mathrm{z}}^2 \mathrm{\sigma }*2{\mathrm{S}}^1 \\ \mathrm{Bond} \mathrm{order} =\frac{{\mathrm{N}}_{\mathrm{b}} - {\mathrm{N}}_{\mathrm{a}}}{2} \\ =\frac{10-3}{2}=\frac{7}{2}=3.5 \end{gathered}$$