Question

Question: Order the following species with respect to the carbon-oxygen bond length (longest to shortest): $\mathbf{CO}\mathbf{,}{\mathbf{CO}}_{\mathbf{2}}\mathbf{,}{\mathbf{CO}}_{\mathbf{3}}^{\mathbf{2}\mathbf{-}}\mathbf{,}{\mathbf{CH}}_{\mathbf{3}}\mathbf{OH}$

Short answer

Answer

The order is $\mathbf{CO}⟩{\mathbf{CH}}_{\mathbf{3}}\mathbf{OH}⟩{\mathbf{CO}}_{\mathbf{3}}^{\mathbf{2}\mathbf{-}}⟩{\mathbf{CO}}_{\mathbf{2}}$

Step-by-step solution

Definition of bond length:

The distance at which the energy is found to be minimum is the equilibrium internuclear distance, more commonly referred to as the bond length.

Bond length and electrons relation:

The number of bound electrons helps in determining the length of the bond(the bond order). The stronger is the attraction between the two atoms and the shorter is the bond length, the higher will be the bond order

Respective bond lengths of given compounds:

The carbon-oxygen bond length of $\mathbf{CO}\mathbf{,}{\mathbf{CO}}_{\mathbf{2}}\mathbf{,}{\mathbf{CO}}_{\mathbf{3}}^{\mathbf{2}\mathbf{-}}\mathbf{,}{\mathbf{CH}}_{\mathbf{3}}\mathbf{OH}$ are 143pm, 116pm, 129pm, and 142.5pm respectively. Therefore, the order is role="math" $\mathbf{CO}⟩{\mathbf{CH}}_{\mathbf{3}}\mathbf{OH}⟩{\mathbf{CO}}_{\mathbf{3}}^{\mathbf{2}\mathbf{-}}⟩{\mathbf{CO}}_{\mathbf{2}}$