Amongst the elements of group 14 the oxidising power of the tetravalent species increases in the order

Options

A. `GeltPbltSn`
B. `GeltSnltPb`
C. `PbltGeltSn`
D. None of the above

Explanation

To determine the order of oxidizing power of the tetravalent species in Group 14 elements (carbon, silicon, germanium, tin, and lead), we need to analyze the oxidation states and their stability as we move down the group.

### Step-by-Step Solution:

1. **Identify the Group 14 Elements**: The elements in Group 14 are Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb).

2. **Determine the Common Oxidation States**: The tetravalent species in this group typically exhibit +4 oxidation states. However, as we move down the group, the +2 oxidation state becomes more stable due to the inert pair effect.

3. **Understand the Concept of Oxidizing Power**: The oxidizing power of a species refers to its ability to gain electrons (or be reduced). A higher oxidizing power indicates a greater tendency to undergo reduction, which corresponds to a decrease in oxidation state.

4. **Analyze the Stability of Oxidation States**:
- **Carbon (C)**: +4 is stable but does not readily reduce to +2.
- **Silicon (Si)**: +4 is stable but less so than carbon.
- **Germanium (Ge)**: +4 is stable, but +2 is more stable than in silicon.
- **Tin (Sn)**: +4 is less stable than +2, showing a greater tendency to reduce.
- **Lead (Pb)**: +4 is the least stable, and +2 is the most stable, showing the highest tendency to reduce.

5. **Establish the Order of Oxidizing Power**: As the stability of the +2 oxidation state increases down the group, the oxidizing power increases. Thus, the order of oxidizing power from least to most is:
- Carbon (C) < Silicon (Si) < Germanium (Ge) < Tin (Sn) < Lead (Pb)

6. **Final Conclusion**: Therefore, the oxidizing power of the tetravalent species in Group 14 increases in the order:
- C < Si < Ge < Sn < Pb