The freezing of any liquid to a solid is expected to have:

Options

A. a positive `DeltaH` and a positive `DeltaS`
B. a negative `DeltaH` and a positive `DeltaS`
C. a positive `DeltaH` and a negative `Delta S`
D. a negative `DeltaH` and a negative `DeltaS`.

Explanation

To analyze the freezing of any liquid to a solid, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Process**: Freezing is the process where a liquid turns into a solid. This involves a change in the state of matter.

2. **Entropy Change (ΔS)**: When a liquid freezes, the molecules become more ordered as they transition from a disordered liquid state to a more ordered solid state. This means the randomness of the system decreases.
- **Conclusion**: Therefore, the change in entropy (ΔS) is negative (ΔS < 0).

3. **Enthalpy Change (ΔH)**: During freezing, energy is released as the molecules come together to form a solid. This release of energy indicates that the system is losing heat.
- **Conclusion**: Hence, the change in enthalpy (ΔH) is also negative (ΔH < 0).

4. **Final Evaluation**: Based on the analysis:
- ΔH < 0 (enthalpy is negative)
- ΔS < 0 (entropy is negative)

5. **Selecting the Correct Option**: The correct option that describes the changes during the freezing of a liquid to a solid is option 4, which states that both ΔH and ΔS are negative.

### Summary of Results:
- **ΔH**: Negative (ΔH < 0)
- **ΔS**: Negative (ΔS < 0)