Which of the following compound (s) is/are non-polar?

Options

A. `NO_(2)`
B. `B_(2)H_(6)`
C. `PF_(3)Cl_(2)`
D. `B_(3)N_(3)H_(6)`

Answer

To determine which of the given compounds are non-polar, we will analyze each compound one by one based on their molecular structure and dipole moments.

### Step 1: Analyze NO2 (Nitrogen Dioxide)
1. **Structure**: NO2 has a nitrogen atom bonded to two oxygen atoms, with one of the bonds being a double bond and the other a coordinate bond.
2. **Lone Pair**: The nitrogen atom has one lone pair of electrons.
3. **Electronegativity**: Oxygen is more electronegative than nitrogen, which means the dipole moment will point towards the oxygen atoms.
4. **Resultant Dipole Moment**: Due to the bent shape of the molecule and the presence of a lone pair, the dipole moments do not cancel out, resulting in a net dipole moment.
5. **Conclusion**: NO2 is a polar molecule.

### Step 2: Analyze B2H6 (Diborane)
1. **Structure**: B2H6 has a dimeric structure with boron and hydrogen atoms.
2. **Electronegativity**: Hydrogen is more electronegative than boron, but the molecule is symmetrical.
3. **Dipole Moments**: The dipole moments from the hydrogen atoms point towards the hydrogen atoms, but they cancel each other out due to the symmetrical arrangement.
4. **Resultant Dipole Moment**: The net dipole moment is zero.
5. **Conclusion**: B2H6 is a non-polar molecule.

### Step 3: Analyze PF3Cl2 (Phosphorus Trifluoride Dichloride)
1. **Structure**: PF3Cl2 has a phosphorus atom bonded to three fluorine atoms and two chlorine atoms.
2. **Electronegativity**: Fluorine is the most electronegative atom, followed by chlorine.
3. **Dipole Moments**: The dipole moments from the fluorine atoms point towards them, while the dipole moments from the chlorine atoms also point towards them.
4. **Resultant Dipole Moment**: The dipole moments do not cancel out completely due to the different electronegativities and the asymmetrical shape of the molecule.
5. **Conclusion**: PF3Cl2 is a polar molecule.

### Step 4: Analyze B3N3H6 (Borosine)
1. **Structure**: B3N3H6 consists of alternating boron and nitrogen atoms in a cyclic structure with hydrogen atoms attached.
2. **Electronegativity**: Nitrogen is more electronegative than boron.
3. **Dipole Moments**: The difference in electronegativity creates dipole moments that do not cancel out.
4. **Resultant Dipole Moment**: The dipole moments result in a net dipole moment that does not equal zero.
5. **Conclusion**: B3N3H6 is a polar molecule.

### Final Conclusion:
From the analysis of the compounds:
- **NO2**: Polar
- **B2H6**: Non-polar
- **PF3Cl2**: Polar
- **B3N3H6**: Polar

**The only non-polar compound among the options is B2H6.**