The boiling point of `D_(2)O` is greater than `H_(2)O_(2)` It is because

Options

A. `D_(2)O` has lower Kw value
B. `D_(2)O` has a lower dielectric constant
C. `D_(2)O` is a associated liquid
D. Inter molecular H-bonds are stronger in `D_(2)O` than in `H_(2)O_(2)`

Answer

To solve the question regarding why the boiling point of D₂O (deuterium oxide) is greater than that of H₂O₂ (hydrogen peroxide), we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Compounds**:
- D₂O (deuterium oxide) is a heavy isotope of water where hydrogen atoms are replaced by deuterium, which is a heavier isotope of hydrogen.
- H₂O₂ (hydrogen peroxide) is a compound consisting of two hydrogen atoms and two oxygen atoms.

2. **Analyzing the Molecular Structure**:
- D₂O has a similar molecular structure to H₂O, but the presence of deuterium makes it heavier.
- H₂O₂ has a different structure with a peroxy linkage (O-O bond) which affects its properties.

3. **Intermolecular Forces**:
- The boiling point of a substance is influenced by the strength of intermolecular forces. Stronger intermolecular forces lead to higher boiling points.
- D₂O exhibits strong hydrogen bonding due to the presence of O-H bonds, similar to H₂O, but the heavier deuterium leads to stronger interactions.

4. **Comparison of Hydrogen Bonding**:
- In H₂O₂, the hydrogen bonding is weaker compared to D₂O because of the presence of the O-O bond which does not participate in hydrogen bonding as effectively as the O-H bonds in D₂O.
- The hydrogen bonds in D₂O are stronger and more stable than those in H₂O₂.

5. **Conclusion**:
- Due to the stronger hydrogen bonding in D₂O compared to the weaker hydrogen bonding in H₂O₂, D₂O has a higher boiling point.

### Final Answer:
The boiling point of D₂O is greater than H₂O₂ because of stronger hydrogen bonding in D₂O compared to H₂O₂.

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