State whether the statement is true or false. In water two O–H bond dissociation enthalpies are not identical.

Answer

To determine whether the statement "In water, two O–H bond dissociation enthalpies are not identical" is true or false, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Bond Dissociation Enthalpy**:
- Bond dissociation enthalpy is defined as the amount of energy required to break a bond in a molecule. In the case of water (H₂O), there are two O–H bonds.

2. **Analyzing the Water Molecule Structure**:
- The water molecule has a bent shape due to the presence of two lone pairs of electrons on the oxygen atom. This geometry affects the bond angles and the distribution of electron density around the molecule.

3. **Breaking the Bonds**:
- When one O–H bond is broken, the remaining structure has one O–H bond and two lone pairs of electrons on the oxygen atom. This change in structure alters the electronic environment around the remaining bond.

4. **Effect of the Change in Environment**:
- After breaking the first O–H bond, the remaining bond experiences a different electronic environment. The oxygen atom now has a different charge distribution and steric effects due to the presence of lone pairs and the remaining hydrogen atom.

5. **Conclusion on Bond Dissociation Energies**:
- Because the environment around the bonds changes after one bond is broken, the energy required to break the second O–H bond will differ from the first. Therefore, the two O–H bond dissociation enthalpies are not identical.

6. **Final Answer**:
- The statement "In water, two O–H bond dissociation enthalpies are not identical" is **True**.