The dipole moment of `H_(2)O_(2)` is more than that of `H_(2)O` but `H_(2)O_(2)` is not a good solvent because `:`

Options

A. It has a very high dielectric constant so that ionic compounds cannot be dissolved in it
B. It does not act as an oxidising agent
C. It acts as a reducing agent
D. It dissociates easily and acts as an oxidising agent in chemical reactions

Explanation

To solve the question regarding why the dipole moment of \( H_2O_2 \) (hydrogen peroxide) is more than that of \( H_2O \) (water) but \( H_2O_2 \) is not a good solvent, we can break it down into the following steps:

### Step 1: Understand the dipole moment
The dipole moment is a measure of the separation of positive and negative charges in a molecule. A higher dipole moment indicates a greater polarity.

### Step 2: Compare the dipole moments of \( H_2O \) and \( H_2O_2 \)
- \( H_2O \) has a bent shape due to the two lone pairs on the oxygen atom, leading to a significant dipole moment.
- \( H_2O_2 \) has a non-linear structure as well, but due to the presence of the O-O bond, it has a higher dipole moment than \( H_2O \).

### Step 3: Analyze the properties of \( H_2O_2 \)
Despite having a higher dipole moment, \( H_2O_2 \) is not a good solvent. The reasons for this include:
- **Thermal instability**: \( H_2O_2 \) decomposes easily into water and oxygen gas (reaction: \( 2 H_2O_2 \rightarrow 2 H_2O + O_2 \)).
- **Oxidizing agent**: \( H_2O_2 \) has strong oxidizing properties due to the weak O-O bond, which allows it to release radicals and participate in redox reactions.

### Step 4: Conclusion
The presence of weak bonds between the oxygen atoms in \( H_2O_2 \) makes it thermally unstable and a strong oxidizing agent. This instability and reactivity prevent \( H_2O_2 \) from being a good solvent, despite its higher dipole moment compared to \( H_2O \).

### Final Answer
The dipole moment of \( H_2O_2 \) is more than that of \( H_2O \) because of its structure, but \( H_2O_2 \) is not a good solvent because it is thermally unstable and acts as a strong oxidizing agent.

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