Which of the following statement is true ?

Options

A. The dipole moment of `NF_(3)` is more than `NH_(3)`
B. trans `-2,3-`dichloro`-2-`pentene does not have net permanent dipole moment.
C. Carbono tetrachloride has no net dipole moment because of its regular tetrahedral strcture.
D. Dipole moment is zero for sulphurdioxide molecule.

Explanation

To determine which of the given statements is true, we will analyze each statement regarding the dipole moments of the respective molecules mentioned.

### Step 1: Analyze Statement A
**Statement A:** The dipole moment of NF3 is more than that of ammonia (NH3).

- **Structure of NH3:** Ammonia has a pyramidal structure due to the presence of a lone pair of electrons on nitrogen. The dipole moment is directed from the hydrogen atoms towards the nitrogen atom.
- **Dipole Moment of NH3:** The dipole moment of ammonia is approximately 1.47 Debye.

- **Structure of NF3:** NF3 also has a pyramidal structure, but the electronegativity of fluorine is higher than that of hydrogen. The dipole moments from the N-F bonds point towards the fluorine atoms.
- **Dipole Moment of NF3:** The dipole moments from the N-F bonds partially cancel the dipole moment due to the lone pair on nitrogen, resulting in a lower dipole moment of about 0.24 Debye.

**Conclusion for Statement A:** This statement is false since the dipole moment of NF3 is less than that of NH3.

### Step 2: Analyze Statement B
**Statement B:** Trans-2,3-dichloro-2-pentene does not have a permanent dipole moment.

- **Structure of Trans-2,3-dichloro-2-pentene:** The structure has a double bond between the second and third carbon atoms, with chlorine atoms attached to the second and third carbons.
- **Dipole Moment Analysis:** In the trans configuration, the dipole moments from the chlorine atoms do not cancel each other out completely, leading to a net dipole moment.

**Conclusion for Statement B:** This statement is false since the molecule does have a permanent dipole moment.

### Step 3: Analyze Statement C
**Statement C:** Carbon tetrachloride (CCl4) has no net dipole moment because of its regular tetrahedral structure.

- **Structure of CCl4:** The carbon atom is at the center with four chlorine atoms at the corners of a tetrahedron.
- **Dipole Moment Analysis:** The individual dipole moments of the C-Cl bonds cancel each other out due to symmetry.

**Conclusion for Statement C:** This statement is true since CCl4 has a net dipole moment of zero.

### Step 4: Analyze Statement D
**Statement D:** The dipole moment is zero for sulfur dioxide (SO2).

- **Structure of SO2:** The molecule has a bent shape due to the presence of a lone pair on sulfur.
- **Dipole Moment Analysis:** The bent structure leads to a net dipole moment because the dipole moments do not cancel out.

**Conclusion for Statement D:** This statement is false since SO2 has a dipole moment of approximately 1.61 Debye.

### Final Conclusion
The only true statement among the options provided is **Statement C**: Carbon tetrachloride has no net dipole moment because of its regular tetrahedral structure.