The reducing nature of any metal in aqueous solution depends upon
a.Enthalpy of atomisation
b. Ionisation enthalpies
c. Hydration energy

Options

A. a & b only
B. Only b
C. b & c only
D. a,b & c

Answer

To determine the reducing nature of any metal in aqueous solution, we need to analyze how each of the given factors—enthalpy of atomization, ionization enthalpy, and hydration energy—contributes to the ability of the metal to lose electrons. Here’s a step-by-step breakdown:

### Step 1: Understanding Reducing Nature
The reducing nature of a metal refers to its ability to lose electrons and thus oxidize itself. This is crucial in aqueous solutions where metals often participate in redox reactions.

**Hint:** Remember that reducing agents donate electrons in chemical reactions.

### Step 2: Enthalpy of Atomization
The first factor is the enthalpy of atomization. This is the energy required to convert a solid metal into gaseous atoms. For a metal to lose electrons, it must first be in the gaseous state. Therefore, a lower enthalpy of atomization means that it is easier for the metal to convert from solid to gaseous state, facilitating the reduction process.

**Hint:** Think of this as the energy barrier to break the solid structure of the metal.

### Step 3: Ionization Enthalpy
The second factor is ionization enthalpy, which is the energy required to remove the most loosely bound electron from a gaseous atom. A lower ionization enthalpy means that the metal can more easily lose electrons, which is essential for its reducing ability. If the ionization energy is high, the metal will not readily lose electrons, thus reducing its reducing power.

**Hint:** Consider how tightly the electrons are held by the nucleus of the metal.

### Step 4: Hydration Energy
The third factor is hydration energy. After the metal loses an electron and forms a cation, this cation must interact with water molecules in the solution. Hydration energy is the energy released when the cation is surrounded by water molecules. A higher hydration energy stabilizes the cation in solution, making the overall process more favorable.

**Hint:** This is about how well the cation interacts with water after losing an electron.

### Conclusion
In summary, the reducing nature of a metal in aqueous solution depends on:
- **Enthalpy of Atomization:** Lower values are favorable.
- **Ionization Enthalpy:** Lower values are favorable.
- **Hydration Energy:** Higher values are favorable.

Therefore, the reducing nature of any metal in aqueous solution depends on all three factors: enthalpy of atomization, ionization enthalpy, and hydration energy.

### Final Answer
The correct answer is **a, b, and c**.

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