Select the correct statement.

Options

A. Both lattice energy and hydration energy decrease with ionic size
B. Lattice energy can be calculated using Born-Haber cycle
C. If the cation is large compared to the anion, the lattice energy will remain almost constant within a particular group
D. All of the above are correct statements

Explanation

To solve the question regarding the correct statements about lattice energy and hydration energy, we will analyze each option provided in the context of the definitions and principles discussed in the video transcript.

### Step-by-Step Solution:

1. **Understanding Lattice Energy**:
- Lattice energy is defined as the amount of energy required to break a solid ionic lattice into its gaseous ions. It is inversely proportional to the sum of the ionic radii of the cation and anion (1/(R+ + R-)). As the size of the ions increases, the lattice energy decreases.

2. **Understanding Hydration Energy**:
- Hydration energy is the energy released when gaseous ions are solvated by water molecules. It is also inversely proportional to the size of the ions. Larger ions have lower hydration energy due to decreased charge density.

3. **Evaluating Option A**:
- The statement claims that lattice energy and hydration energy decrease with ionic size. This is correct based on the definitions provided. As the ionic size increases, both energies decrease.

4. **Evaluating Option B**:
- This option states that lattice energy can be calculated using the Born-Haber Cycle. This is also correct. The Born-Haber Cycle allows us to calculate lattice energy by considering various energy changes involved in the formation of an ionic compound.

5. **Evaluating Option C**:
- The statement mentions that if the cation is large compared to the anion, the lattice energy will remain almost constant within a group. This is true because if the cation size remains constant and only the anion size increases, the overall effect on lattice energy is minimal, as it primarily depends on the cation size.

6. **Conclusion**:
- Since all three options (A, B, and C) are correct, the final answer is that option D, which states that all the above statements are correct, is the correct choice.

### Final Answer:
**Option D: All the above are correct statements.**