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Among the given species the one which co...

Among the given species the one which contains weakest carbon - oxygen bond : `CO_2,CH_3COO^(-),CO,CO_3^(2-)`

A

`CO_2`

B

`CH_3COO^-`

C

`CO`

D

`CO_3^(2-)`

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given species contains the weakest carbon-oxygen bond among `CO2`, `CH3COO^(-)`, `CO`, and `CO3^(2-)`, we will analyze the bond orders of the carbon-oxygen bonds in each species. ### Step 1: Analyze the structure of CO2 - **CO2** has a linear structure with two double bonds between carbon and oxygen. - **Bond Order Calculation**: Each C=O bond has a bond order of 2. - Therefore, the bond order for CO2 is 2. ### Step 2: Analyze the structure of CH3COO^(-) - **CH3COO^(-)** (acetate ion) has a structure where one carbon is bonded to three hydrogens (methyl group) and is also bonded to a carbonyl (C=O) and an oxygen with a negative charge (O^-). - The resonance structures show that the C=O bond can be represented as a double bond and the C-O bond can be represented as a single bond. - **Bond Order Calculation**: The C=O bond has a bond order of 2, and the C-O bond has a bond order of 1. However, due to resonance, the average bond order for the C=O bond in acetate is 1.5 (since there are two resonance forms contributing to the bond character). ### Step 3: Analyze the structure of CO - **CO** (carbon monoxide) has a triple bond between carbon and oxygen. - **Bond Order Calculation**: The bond order for CO is 3. ### Step 4: Analyze the structure of CO3^(2-) - **CO3^(2-)** (carbonate ion) has a resonance structure where one carbon is bonded to three oxygen atoms. The carbon-oxygen bonds can be represented as one double bond and two single bonds in various resonance forms. - **Bond Order Calculation**: The average bond order for the C-O bonds in CO3^(2-) can be calculated as follows: - There are 4 bonds (1 double bond and 2 single bonds) shared among 3 C-O bonds. - Thus, the bond order = Total bonds / Number of bonds = 4/3 ≈ 1.33. ### Step 5: Compare the bond orders - CO2: Bond order = 2 - CH3COO^(-): Average bond order ≈ 1.5 - CO: Bond order = 3 - CO3^(2-): Average bond order ≈ 1.33 ### Conclusion The species with the weakest carbon-oxygen bond is **CO3^(2-)** since it has the lowest bond order of approximately 1.33. ### Final Answer The species with the weakest carbon-oxygen bond is **CO3^(2-)**.
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