Which of the following molecules is non-polar in nature?

Options

A. `SbCl_5`
B. `NO_2`
C. `POCl_3`
D. `CH_2O`

Answer

To determine which of the following molecules is non-polar in nature, we will analyze each option based on the concept of dipole moment and molecular geometry. A molecule is considered non-polar if it has a dipole moment of zero, which typically occurs when the molecule has symmetrical geometry and the individual bond dipoles cancel each other out.

### Step-by-Step Solution:

1. **Identify the Molecules**: List the molecules provided in the options. For this example, we will consider the following:
- A) SbCl5
- B) NO2
- C) POCl3
- D) CH2O

2. **Analyze SbCl5**:
- **Hybridization**: The central atom is Antimony (Sb), which is in group 15 and has 5 valence electrons. The hybridization can be calculated as:
\[ \text{Hybridization} = \frac{(5 + 5)}{2} = 5 \quad \text{(5 bond pairs, no lone pairs)} \]
This gives us an sp³d hybridization.
- **Geometry**: The geometry of SbCl5 is trigonal bipyramidal.
- **Dipole Moment**: The dipole moments of the Sb-Cl bonds will cancel out due to symmetry, resulting in a net dipole moment of zero. Therefore, SbCl5 is **non-polar**.

3. **Analyze NO2**:
- **Hybridization**: The central atom is Nitrogen (N), which has 5 valence electrons. The hybridization is:
\[ \text{Hybridization} = \frac{(5 + 2)}{2} = 3.5 \quad \text{(1 lone pair, 2 bond pairs)} \]
- **Geometry**: The geometry of NO2 is bent due to the presence of a lone pair.
- **Dipole Moment**: The dipole moments do not cancel out due to the bent shape, resulting in a net dipole moment that is not zero. Therefore, NO2 is **polar**.

4. **Analyze POCl3**:
- **Hybridization**: The central atom is Phosphorus (P), which has 5 valence electrons. The hybridization is:
\[ \text{Hybridization} = \frac{(5 + 3)}{2} = 4 \quad \text{(4 bond pairs, 0 lone pairs)} \]
- **Geometry**: The geometry of POCl3 is tetrahedral.
- **Dipole Moment**: The different electronegativities of the atoms lead to a net dipole moment that is not zero. Therefore, POCl3 is **polar**.

5. **Analyze CH2O**:
- **Hybridization**: The central atom is Carbon (C), which has 4 valence electrons. The hybridization is:
\[ \text{Hybridization} = \frac{(4 + 2)}{2} = 3 \quad \text{(3 bond pairs, 0 lone pairs)} \]
- **Geometry**: The geometry of CH2O is trigonal planar.
- **Dipole Moment**: The dipole moments do not cancel out due to the presence of the polar C=O bond, resulting in a net dipole moment that is not zero. Therefore, CH2O is **polar**.

### Conclusion:
After analyzing all the molecules, we find that **SbCl5** is the only non-polar molecule among the options provided.

### Final Answer:
**A) SbCl5 is non-polar.**