Question:
The number of possible aromatic benzenoid isomers for \(C_6H_4Cl_2\) are
The number of possible aromatic benzenoid isomers for \(C_6H_4Cl_2\) are
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For disubstituted benzene with two identical substituents, only three positional isomers are possible:
\[
\text{ortho }(1,2),\quad \text{meta }(1,3),\quad \text{para }(1,4)
\]
Updated On: Jul 18, 2026
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The Correct Option is B
Solution and Explanation
Step 1: Identify the compound.
The molecular formula is \[ C_6H_4Cl_2 \] This represents dichlorobenzene, which is formed by replacing two hydrogen atoms of benzene with two chlorine atoms.
Step 2: Understand possible positions of two chlorine atoms.
In benzene, when two identical substituents are attached, only three different relative positions are possible due to symmetry.
These are: \[ \text{ortho }(1,2) \] \[ \text{meta }(1,3) \] \[ \text{para }(1,4) \]
Step 3: List the possible isomers.
The three aromatic benzenoid isomers of \(C_6H_4Cl_2\) are: \[ 1,2\text{-dichlorobenzene} \] \[ 1,3\text{-dichlorobenzene} \] \[ 1,4\text{-dichlorobenzene} \]
Step 4: Count the total number of isomers.
Therefore, the total number of possible aromatic benzenoid isomers is \[ 3 \]
Step 5: Final conclusion.
Hence, \[ \boxed{3} \] Therefore, option (2) is correct.
The molecular formula is \[ C_6H_4Cl_2 \] This represents dichlorobenzene, which is formed by replacing two hydrogen atoms of benzene with two chlorine atoms.
Step 2: Understand possible positions of two chlorine atoms.
In benzene, when two identical substituents are attached, only three different relative positions are possible due to symmetry.
These are: \[ \text{ortho }(1,2) \] \[ \text{meta }(1,3) \] \[ \text{para }(1,4) \]
Step 3: List the possible isomers.
The three aromatic benzenoid isomers of \(C_6H_4Cl_2\) are: \[ 1,2\text{-dichlorobenzene} \] \[ 1,3\text{-dichlorobenzene} \] \[ 1,4\text{-dichlorobenzene} \]
Step 4: Count the total number of isomers.
Therefore, the total number of possible aromatic benzenoid isomers is \[ 3 \]
Step 5: Final conclusion.
Hence, \[ \boxed{3} \] Therefore, option (2) is correct.
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