The stability of ions of Ge Sn and `Pb` will be in the order .

Options

A. `Ge^(2+) lt Sn^(2+) lt Pb^(2+)`
B. `Pb^(2+) gt Pb^(4+)`
C. `Sn^(4+) gt Pb^(2+)`
D. `Ge^(4+) lt Sn^(4+) lt Pb^(4+)`

Explanation

To determine the stability of the ions of Germanium (Ge), Tin (Sn), and Lead (Pb), we need to consider their positions in the periodic table and the factors that influence the stability of their oxidation states.

### Step-by-Step Solution:

1. **Identify the Group**:
- Germanium (Ge), Tin (Sn), and Lead (Pb) are all in Group 14 of the periodic table.

2. **Understand the Trend in Stability**:
- As we move down the group from Ge to Sn to Pb, the atomic size increases. This increase in size affects the stability of the oxidation states.

3. **Consider the Oxidation States**:
- The common oxidation states for these elements are +2 and +4. However, the +2 oxidation state becomes more stable as we move down the group due to the inert pair effect.

4. **Inert Pair Effect**:
- The inert pair effect refers to the tendency of the s-electrons (the two electrons in the outermost s orbital) to remain non-bonding or "inert" in heavier elements. This effect is more pronounced in heavier elements, leading to greater stability of the +2 oxidation state compared to the +4 state.

5. **Order of Stability**:
- For Ge, the +2 oxidation state is less stable compared to Sn and Pb.
- For Sn, the +2 oxidation state is more stable than for Ge but less stable than for Pb.
- For Pb, the +2 oxidation state is the most stable due to the inert pair effect being most pronounced.

6. **Final Order**:
- Therefore, the stability of the ions in order from least stable to most stable is:
- Ge < Sn < Pb

### Conclusion:
The stability of ions of Ge, Sn, and Pb will be in the order: **Ge < Sn < Pb**.