Bond order of carbon and oxygen in ch3oh co2 co co3.
The Correct Answer and Explanation is :
To determine the bond order between carbon and oxygen in various compounds like CH₃OH, CO₂, CO, and CO₃²⁻, we must analyze each molecule’s structure and bonding.
1. Methanol (CH₃OH)
- Methanol has a C-O single bond between the carbon and the hydroxyl (OH) group. There is no resonance in this molecule, so the bond order is simply the number of bonds: Bond Order = 1.
2. Carbon Dioxide (CO₂)
- In CO₂, the carbon atom is double-bonded to each oxygen atom in a linear structure (O=C=O). Each C=O bond is a double bond with no resonance. Thus, the Bond Order = 2 for each C-O bond.
3. Carbon Monoxide (CO)
- Carbon monoxide has a triple bond between carbon and oxygen, with a lone pair on both the carbon and oxygen. The Lewis structure shows one sigma and two pi bonds, so Bond Order = 3 for the C-O bond.
4. Carbonate Ion (CO₃²⁻)
- The carbonate ion (CO₃²⁻) has three resonance structures, each with one C=O double bond and two C-O single bonds. In these structures, the double bond is delocalized, and the bonding is averaged over the three C-O bonds. The bond order calculation for CO₃²⁻ is the total number of bonds divided by the number of bond sites:
[
\text{Bond Order} = \frac{4}{3} = 1.33
]
Thus, the C-O bond order in CO₃²⁻ is approximately 1.33.
Summary of Bond Orders
- CH₃OH (Methanol): 1
- CO₂ (Carbon Dioxide): 2
- CO (Carbon Monoxide): 3
- CO₃²⁻ (Carbonate Ion): 1.33
Explanation
Bond order provides insight into bond strength and stability. Higher bond orders (like 2 or 3) indicate stronger bonds, while a bond order of 1.33, as seen in the resonance-stabilized CO₃²⁻, reflects partial double-bond character due to resonance.