Explain the structure of $CO_{2}$ molecule.

(N/A) The experimentally determined carbon to oxygen bond length in $CO_{2}$ is $115 \ pm$.
The lengths of a normal carbon to oxygen double bond $(C=O)$ and carbon to oxygen triple bond $(C \equiv O)$ are $121 \ pm$ and $110 \ pm$ respectively.
The carbon-oxygen bond lengths in $CO_{2}$ $(115 \ pm)$ lie between the values for $C=O$ and $C \equiv O$.
Obviously, a single Lewis structure cannot depict this position and it becomes necessary to write more than one Lewis structure and to consider that the structure of $CO_{2}$ is best described as a hybrid of the canonical or resonance forms $I$, $II$ and $III$:
$:O=C=O: \leftrightarrow :O^{-}-C \equiv O^{+}: \leftrightarrow :O^{+}\equiv C-O^{-}:$