What is the $O-O$ bond length in an ozone $(O_3)$ molecule (in $pm$)?

Taking into account hybridization and resonance effects,rank the following $C-O$ bonds in order of decreasing bond length. The structure provided is the carbonate ion $(CO_3^{2-})$.

In the anion $HCOO^-$,the two carbon-oxygen bonds are found to be of equal length. What is the reason for it?

What is the correct increasing order of $C-O$ bond length in $CO$,$CO_3^{2-}$,and $CO_2$?

The resonance hybrid of the nitrate ion $(NO_3^-)$ is represented as:

Identify the relationship between the following two structures: $\begin{matrix} \overset{\Theta}{\overset{\centerdot \,\centerdot}{C}}H_2-C(=O)-CH_3 \end{matrix}$ and $\begin{matrix} CH_2=C(O^{\Theta})CH_3 \end{matrix}$