The correct order of increasing bond length of C - H ,C - O, C - C and C = C is

Options

A. `C-H lt C- O lt C - C lt C = C`
B. `C-H lt C= C lt C - O lt C - C`
C. `C-C lt C= C lt C - O lt C - H`
D. `C-OltC-HltC-CltC=C`

Explanation

To determine the correct order of increasing bond length for the bonds C-H, C-O, C-C, and C=C, we need to analyze the nature of each bond and the atomic sizes involved. Here’s a step-by-step solution:

### Step 1: Understand Bond Length
Bond length is the distance between the nuclei of two bonded atoms. Generally, bond length is influenced by the size of the atoms involved and the type of bond (single, double, or triple).

### Step 2: Analyze Each Bond
1. **C-H Bond**: This is a single bond between carbon and hydrogen. Carbon has a larger atomic radius compared to hydrogen, but since it is a single bond, the bond length will be relatively short.
2. **C-O Bond**: This is also a single bond. Oxygen is smaller than carbon, which means the bond length will be shorter than the C-C bond but longer than the C=C bond.
3. **C-C Bond**: This is a single bond between two carbon atoms. The bond length is longer than C-H and C-O because both atoms are carbon, which have larger atomic radii compared to hydrogen and oxygen.
4. **C=C Bond**: This is a double bond between two carbon atoms. Double bonds are shorter than single bonds due to the increased attraction between the two nuclei, resulting in a shorter bond length.

### Step 3: Compare Bond Lengths
Based on the analysis:
- C=C will have the shortest bond length due to the double bond.
- C-H will have a shorter bond length than C-C but longer than C=C.
- C-O will have a bond length that is shorter than C-C but longer than C-H.
- C-C will have the longest bond length among these bonds.

### Step 4: Order the Bonds
From shortest to longest bond length, we can summarize:
1. C=C (shortest)
2. C-H
3. C-O
4. C-C (longest)

### Final Answer
The correct order of increasing bond length is: **C=C < C-H < C-O < C-C**.

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