For the processes `K^+(g) overset(I)(to)K(g) overset(II)(to)K(s) `

Options

A. energy is released in (I) and absorbed in (II)
B. energy is absorbed in (I) and released in (II)
C. energy is absorbed in both the processes
D. energy is released in both the processes

Answer

To solve the question regarding the processes \( K^+(g) \overset{(I)}{\to} K(g) \overset{(II)}{\to} K(s) \), we need to analyze each step in terms of energy changes.

### Step 1: Analyze Process I
- **Process I**: \( K^+(g) \to K(g) \)
- In this step, potassium in the +1 oxidation state (K\(^+\)) is gaining an electron to become neutral potassium (K).
- The electronic configuration of K is \( [Ar] 4s^1 \), and for K\(^+\), it is \( [Ar] 4s^0 \).
- When K\(^+\) gains an electron, it transitions to a more stable state (neutral K).
- Since energy is required to add an electron to a stable configuration, this process **absorbs energy**.

### Step 2: Analyze Process II
- **Process II**: \( K(g) \to K(s) \)
- In this step, potassium in the gaseous state is converting to solid potassium.
- This process is known as deposition.
- When a gas converts to a solid, the thermal energy of the gas is released as the particles lose energy and come together to form a solid structure.
- Therefore, this process **releases energy**.

### Summary of Energy Changes
- **Process I**: Energy is **absorbed** (endothermic).
- **Process II**: Energy is **released** (exothermic).

### Conclusion
The correct answer is that energy is absorbed in the first process and released in the second process.