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NEET CHEMISTRYMedium

The correct order of C-O bond length among CO, CO32−CO_3^{2-}, and CO2CO_2 is:

A

CO2<CO32−<COCO_2 < CO_3^{2-} < CO

B

CO<CO32−<CO2CO < CO_3^{2-} < CO_2

C

CO32−<CO2<COCO_3^{2-} < CO_2 < CO

D

CO<CO2<CO32−CO < CO_2 < CO_3^{2-}

Step-by-Step Solution

  1. Relationship: Bond length is inversely proportional to bond order. Higher bond order implies stronger attraction and shorter bond length.
  2. Analyze CO: Carbon monoxide has a triple bond between Carbon and Oxygen. Bond Order = 3.
  3. Analyze CO2CO_2: Carbon dioxide (O=C=OO=C=O) has double bonds between Carbon and Oxygen. Bond Order = 2.
  4. Analyze CO32−CO_3^{2-}: The carbonate ion exhibits resonance. The double bond is delocalized over three C-O bonds. Bond Order = Total BondsResonance Structures=43≈1.33\frac{\text{Total Bonds}}{\text{Resonance Structures}} = \frac{4}{3} \approx 1.33.
  5. Comparison:
  • Bond Order: CO(3)>CO2(2)>CO32−(1.33)CO (3) > CO_2 (2) > CO_3^{2-} (1.33)
  • Bond Length: CO<CO2<CO32−CO < CO_2 < CO_3^{2-}
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