According to VBT the extent of overlapping depends upon types of orbitals involved in overlapping and nature of overlapping. More will be the overlapping and the bond energy will also be high.
The incorrect order of bond dissociation energy will be :

Options

A. `H-H gt Cl - Cl gt Br - Br`
B. `Si - Si gt P- P gt Cl- Cl`
C. `C-C gt N -N gt O-O`
D. `H-Cl gt H- Br gt H -I`

Explanation

To determine the incorrect order of bond dissociation energy, we need to analyze the bond energies of different types of bonds based on the principles of valence bond theory (VBT). The bond dissociation energy is the energy required to break a bond between two atoms, and it is influenced by the type of bond (single, double, triple) and the size of the atoms involved.

### Step-by-Step Solution:

1. **Understanding Bond Types**:
- Single bonds (sigma bonds) are weaker than double bonds (one sigma and one pi bond), which in turn are weaker than triple bonds (one sigma and two pi bonds).
- Therefore, the general order of bond strength is: Triple bond > Double bond > Single bond.

2. **Analyzing Atomic Size and Electronegativity**:
- As we move down a group in the periodic table, the atomic size increases due to the addition of electron shells. This leads to longer bond lengths and, consequently, lower bond dissociation energies.
- For example, in the halogen group (F, Cl, Br, I), the bond dissociation energy decreases as we move from fluorine to iodine due to increasing atomic size.

3. **Evaluating Given Bonds**:
- Let's consider the bonds mentioned in the question:
- **C≡C** (triple bond), **C=C** (double bond), and **C-C** (single bond) will have bond energies in the order: C≡C > C=C > C-C.
- For bonds involving halogens, the order of bond strength will be: H-F > H-Cl > H-Br > H-I.

4. **Identifying the Incorrect Order**:
- The question asks for the incorrect order of bond dissociation energies. We need to compare the bond energies of different pairs or groups of bonds.
- For example, if the order presented is: P-P > Si-Si > Cl-Cl, this would be incorrect because:
- P-P (single bond) is weaker than Si-Si (single bond) due to the larger atomic size of phosphorus compared to silicon.
- Cl-Cl (single bond) is weaker than both Si-Si and P-P due to the larger size of chlorine.

5. **Conclusion**:
- After evaluating the bond types and their corresponding energies, we can conclude that the incorrect order of bond dissociation energy is likely to be the one that does not follow the expected trend based on bond type and atomic size.

### Final Answer:
The incorrect order of bond dissociation energy is **B option**.