The heavier members of `13` and `14` groups besides the group
oxidation state also show another oxidation state. Down the group `(darr)`, the stability of higher oxidation state increases. This concept which is commonly called inert pair effect has been used to explain many physical and chemical properties of the element of these
groups.
The strongest reductant amoung the following is

Options

A. `SnCl_(2)`
B. `SnCl_(4)`
C. `PbCl_(2)`
D. `GeCl_(2)`

Explanation

To solve the question regarding the strongest reductant among the given compounds (SnCl2, SnCl4, PbCl2, and GeCl2), we will follow these steps:

### Step 1: Understand the Concept of Oxidation States
The question mentions oxidation states and the inert pair effect. In group 13 and 14 elements, as we move down the group, the stability of the higher oxidation state increases due to the inert pair effect. This means that heavier elements tend to exhibit a more stable lower oxidation state.

**Hint:** Remember that the inert pair effect refers to the tendency of the s-electrons to remain non-bonding in heavier elements.

### Step 2: Identify the Oxidation States of Each Compound
- **SnCl2**: Tin (Sn) has an oxidation state of +2.
- **SnCl4**: Tin (Sn) has an oxidation state of +4.
- **PbCl2**: Lead (Pb) has an oxidation state of +2.
- **GeCl2**: Germanium (Ge) has an oxidation state of +2.

**Hint:** Write down the oxidation states of each element in the compounds to compare them.

### Step 3: Analyze the Stability of Oxidation States
For group 14 elements:
- The +2 oxidation state becomes more stable as we move down the group (from C to Pb).
- The +4 oxidation state is less stable for heavier elements like Pb and Sn.

**Hint:** Consider how the stability of oxidation states changes as you go down the group.

### Step 4: Determine the Reducing Agent
A reducing agent is a species that donates electrons and is oxidized in the process. The strongest reductant will be the one that can easily convert from a lower oxidation state to a higher one.

- **SnCl4** cannot be a reductant because it is already in a +4 state.
- **PbCl2** is in a +2 state, but as we noted, Pb prefers to stay in the +2 state.
- **GeCl2** is also in a +2 state, but Ge can be oxidized to +4.

Since GeCl2 can be oxidized to GeCl4, it can act as a stronger reductant compared to SnCl2 and PbCl2.

**Hint:** Identify which compounds can be oxidized to a higher oxidation state to determine their reducing ability.

### Step 5: Conclusion
Based on the analysis, GeCl2 is the strongest reductant among the given options because it can easily transition from +2 to +4 oxidation state, while the others either cannot or are less favorable.

**Final Answer:** The strongest reductant among the following is **GeCl2**.