Molecule having non-polar as well as polar bonds but the molecule as a whole is polar

Options

A. `S_(2)F_(2)`
B. `N_(2)O_(4)`
C. `Si_(2)H_(6)`
D. `I_(2)Cl_(6)`

Explanation

To solve the question regarding a molecule that has both non-polar and polar bonds but is overall polar, we will analyze the given options step by step.

### Step-by-Step Solution:

1. **Understanding the Question**: We need to identify a molecule that contains both polar and non-polar bonds, yet has an overall polar character. A polar molecule has a net dipole moment, meaning that the dipoles do not cancel each other out.

2. **Analyzing the First Option: \( \text{S}_2\text{F}_2 \)**:
- **Structure**: The molecule consists of two sulfur atoms and two fluorine atoms. The structure can be represented as \( \text{S-F} \) bonds.
- **Bond Polarity**: The \( \text{S-F} \) bonds are polar due to the difference in electronegativity between sulfur and fluorine. The \( \text{S-S} \) bond is non-polar since both sulfur atoms have the same electronegativity.
- **Overall Polarity**: The dipole moments from the \( \text{S-F} \) bonds do not cancel out because the molecule is asymmetrical. Therefore, \( \text{S}_2\text{F}_2 \) is a polar molecule.

3. **Analyzing the Second Option: \( \text{N}_2\text{O}_4 \)**:
- **Structure**: The molecule consists of two nitrogen atoms and four oxygen atoms.
- **Bond Polarity**: The \( \text{N-N} \) bond is non-polar, while the \( \text{N=O} \) bonds are polar.
- **Overall Polarity**: The molecule has a symmetrical structure, leading to the cancellation of dipole moments. Thus, \( \text{N}_2\text{O}_4 \) is a non-polar molecule.

4. **Analyzing the Third Option: \( \text{SiH}_6 \)**:
- **Structure**: This molecule has a tetrahedral geometry with silicon at the center and hydrogen atoms surrounding it.
- **Bond Polarity**: The \( \text{Si-H} \) bonds are polar, while the \( \text{Si-Si} \) bond is non-polar.
- **Overall Polarity**: The symmetrical arrangement of the hydrogen atoms around silicon results in the cancellation of dipole moments, making \( \text{SiH}_6 \) a non-polar molecule.

5. **Analyzing the Fourth Option: \( \text{I}_2\text{Cl}_6 \)**:
- **Structure**: This molecule consists of iodine and chlorine atoms.
- **Bond Polarity**: The \( \text{I-Cl} \) bonds are polar, while the \( \text{I-I} \) bond is non-polar.
- **Overall Polarity**: The symmetrical structure leads to cancellation of dipole moments, making \( \text{I}_2\text{Cl}_6 \) a non-polar molecule.

6. **Conclusion**: The only molecule that fits the criteria of having both polar and non-polar bonds while being overall polar is \( \text{S}_2\text{F}_2 \). Thus, the correct answer is option A.

### Final Answer:
The molecule that has non-polar as well as polar bonds but is overall polar is \( \text{S}_2\text{F}_2 \).