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The correct order of decreasing C-O bond...

The correct order of decreasing `C-O` bond length of (1) `CO,(II)CO_(3)^(2-) (III)CO_(2)` is .

A

`CO gt CO_(2) gt CO_(3)^(2-)`

B

`CO_(3)^(2-) gt CO_(2) gt CO`

C

`CO_(2) gt CO gt CO_(3)^(2-)`

D

`CO_(2) gt CO_(3)^(2-) gt CO`

Text Solution

AI Generated Solution

The correct Answer is:
To determine the correct order of decreasing C-O bond length for the compounds CO (carbon monoxide), CO3^(2-) (carbonate ion), and CO2 (carbon dioxide), we need to analyze the types of bonds present in each molecule and their corresponding bond lengths. ### Step 1: Analyze the bond in Carbon Monoxide (CO) - Carbon monoxide (CO) has a triple bond between carbon and oxygen. - Triple bonds consist of one sigma bond and two pi bonds, which are very strong and short. - Therefore, CO has the shortest bond length among the three compounds. **Hint:** Remember that the more bonds between two atoms (single, double, triple), the shorter the bond length. ### Step 2: Analyze the bond in Carbon Dioxide (CO2) - Carbon dioxide (CO2) has a double bond between carbon and each oxygen atom (C=O). - A double bond consists of one sigma bond and one pi bond, which is longer than a triple bond but shorter than a single bond. - Thus, CO2 has a bond length that is longer than CO but shorter than that of carbonate. **Hint:** Compare the bond types: double bonds are longer than triple bonds but shorter than single bonds. ### Step 3: Analyze the bond in Carbonate Ion (CO3^(2-)) - The carbonate ion (CO3^(2-)) has resonance structures, where the C-O bonds are not purely single or double. - The bonds in carbonate are considered to be equivalent to a bond order of 1.33 (due to resonance), which is longer than a double bond but shorter than a single bond. - Therefore, the bond length in carbonate is longer than that in CO2. **Hint:** Remember that resonance can affect bond lengths, making them longer than a pure double bond. ### Step 4: Order the bond lengths - Based on the analysis: 1. CO (triple bond) - shortest bond length 2. CO2 (double bond) - shorter than carbonate 3. CO3^(2-) (resonance with bond order of 1.33) - longest bond length ### Conclusion The correct order of decreasing C-O bond length is: **CO > CO2 > CO3^(2-)** ### Final Answer The correct order of decreasing C-O bond length is: **CO > CO2 > CO3^(2-)**.
To determine the correct order of decreasing C-O bond length for the compounds CO (carbon monoxide), CO3^(2-) (carbonate ion), and CO2 (carbon dioxide), we need to analyze the types of bonds present in each molecule and their corresponding bond lengths. ### Step 1: Analyze the bond in Carbon Monoxide (CO) - Carbon monoxide (CO) has a triple bond between carbon and oxygen. - Triple bonds consist of one sigma bond and two pi bonds, which are very strong and short. - Therefore, CO has the shortest bond length among the three compounds. **Hint:** Remember that the more bonds between two atoms (single, double, triple), the shorter the bond length. ...
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