The correct order of increasing `C-O` bond lengths in `CO, CO_3^(2-)` and ` CO_2` is :

Options

A. `CO_2 lt CO_3^(2-) lt CO`
B. `CO lt CO_3^(2-) lt CO_2`
C. `CO_3^(2-) lt CO_2 lt CO`
D. `CO lt CO_2 lt CO_3^(2-)`

Answer

D

Explanation

A bond length is the average distance between the centres of nuclei of two bonded atoms. A multiple bond (double or triple bonds) is always shorter than the corresponding single bond.
The C-atom in `CO_3^(2-)` is `sp^2` hybridised as shown :

The C-atom in `CO_2` is sp hybridised with bond distance carbon -oxygen is 122 pm.
`O=C=Oharr.^+O-=C-barOharrbarO-C-=overset+O`
The C-atom in CO is sp hybridised with C-O bond distance is 110 pm.
`:C-=O^(+):`
So, the correct order is
`CO lt CO_2 lt CO_3^(2-)`