Dipole moment of `H_(2)O_(2)` is non-zero as

Options

A. Two dipole moments are opposite but unequal
B. Two dipole moments are opposite and equal
C. Two dipole moments are equal but not at `180^(@)`
D. Two dipole moments are equal but non-planar.

Answer

To determine why the dipole moment of hydrogen peroxide (H₂O₂) is non-zero, we can analyze the molecular structure and the arrangement of its bonds step by step.

### Step-by-Step Solution:

1. **Understanding the Molecular Structure of H₂O₂**:
- Hydrogen peroxide (H₂O₂) consists of two hydrogen atoms and two oxygen atoms. The molecular structure can be visualized as having an open book-like shape due to the arrangement of the atoms.

2. **Identifying the Bond Polarities**:
- Each O-H bond in H₂O₂ is polar because oxygen is more electronegative than hydrogen. This means that the electrons in the O-H bond are drawn closer to the oxygen atom, creating a dipole moment (a vector quantity pointing from the less electronegative atom to the more electronegative atom).

3. **Analyzing the Geometry**:
- The two O-H bonds are not in the same plane; they are oriented at an angle to each other. This non-planarity is crucial because it means that the dipole moments of the individual O-H bonds do not cancel each other out.

4. **Resultant Dipole Moment**:
- Since the dipole moments of the two O-H bonds are equal in magnitude but are oriented in different directions (due to the non-planar arrangement), they do not cancel each other completely. This results in a net dipole moment for the molecule.

5. **Conclusion**:
- Therefore, the dipole moment of H₂O₂ is non-zero because the two dipole moments are equal in magnitude but are non-planar, leading to a resultant dipole moment.

### Final Answer:
The dipole moment of H₂O₂ is non-zero because the two dipole moments are equal but non-planar.