Question:
The correct order of $C-O $ bond length among $CO,CO_3^{2-}$, $CO_2$ is
The correct order of $C-O $ bond length among $CO,CO_3^{2-}$, $CO_2$ is
Updated On: Jul 9, 2024
- $CO_2 < CO_3^{2-} < CO$
- $CO < CO_3^{2-} < CO_2$
- $CO_3^{2-} < CO_2 < CO$
- $CO < CO_2 < CO_3^{2-}$
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The Correct Option is D
Solution and 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 = O \leftrightarrow ^+ O \equiv C - _O^- \leftrightarrow $
$ \hspace37mm$ $_O^- - C \equiv _O^+$
The C-atom in CO is sp hybridised with C-O bond distance is 110 pm.
$ \, \, \, \, \, \, \, :C \equiv O^+ :$
So, the correct order is
$ \, \, \, \, \, \, CO < CO_2 < CO_3^{2-}$
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 = O \leftrightarrow ^+ O \equiv C - _O^- \leftrightarrow $
$ \hspace37mm$ $_O^- - C \equiv _O^+$
The C-atom in CO is sp hybridised with C-O bond distance is 110 pm.
$ \, \, \, \, \, \, \, :C \equiv O^+ :$
So, the correct order is
$ \, \, \, \, \, \, CO < CO_2 < CO_3^{2-}$
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Concepts Used:
Molecular Orbital Theory
The Molecular Orbital Theory is a more sophisticated model of chemical bonding where new molecular orbitals are generated using a mathematical process called Linear Combination of Atomic Orbitals (LCAO).
Molecular Orbital theory is a chemical bonding theory that states that individual atoms combine together to form molecular orbitals. Due to this arrangement in MOT Theory, electrons associated with different nuclei can be found in different atomic orbitals. In molecular orbital theory, the electrons present in a molecule are not assigned to individual chemical bonds between the atoms. Rather, they are treated as moving under the influence of the atomic nuclei in the entire molecule.
