Which has maximum dipole moment ?

Options

A.
B.
C.
D.

Answer

To determine which molecule has the maximum dipole moment among the given options, we will analyze each option step by step.

### Step 1: Understand Dipole Moment
The dipole moment (\( \mu \)) is a measure of the separation of positive and negative charges in a molecule. It is a vector quantity, which means it has both magnitude and direction. The dipole moment can be calculated using the formula:
\[ \mu = q \times d \]
where \( q \) is the charge and \( d \) is the distance between the charges.

### Step 2: Analyze Each Option
We will analyze the dipole moment of each molecule provided in the options.

#### Option A
- The molecule has C-Cl bonds.
- Chlorine (Cl) is more electronegative than carbon (C), so Cl will have a partial negative charge and C will have a partial positive charge.
- However, if the molecule is symmetrical, the dipole moments of the C-Cl bonds may cancel each other out.
- **Conclusion**: The dipole moment is equal to zero.

#### Option B
- Similar to Option A, this molecule has C-Cl bonds.
- The dipole moments from the C-Cl bonds do not cancel out because the molecule is not symmetrical.
- **Conclusion**: This molecule has a net dipole moment that is not equal to zero.

#### Option C
- This molecule also has C-Cl bonds.
- The dipole moments from the C-Cl bonds are arranged in such a way that they cancel each other out, resulting in no net dipole moment.
- **Conclusion**: The dipole moment is equal to zero.

#### Option D
- This molecule contains C-Cl bonds as well.
- The arrangement of the C-Cl bonds leads to cancellation of dipole moments.
- **Conclusion**: The dipole moment is equal to zero.

### Step 3: Compare the Results
From our analysis:
- Option A: Dipole moment = 0
- Option B: Dipole moment ≠ 0 (polar molecule)
- Option C: Dipole moment = 0
- Option D: Dipole moment = 0

### Final Answer
The molecule with the maximum dipole moment is **Option B**, which is a polar molecule.

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