Amongst the elements of group 14 the reducing power of the divalent species decreases in the order .

Options

A. GegtSngtPb
B. SngtGegtPb
C. PbgtSngtGe
D. SngtPbgtGe

Explanation

To determine the reducing power of the divalent species among the elements of group 14, we will analyze the elements in this group: Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb). The reducing power of these elements in their divalent state (i.e., +2 oxidation state) decreases in a specific order.

### Step-by-Step Solution:

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

2. **Understand the Oxidation States**:
- Carbon typically exhibits oxidation states of +4 and -4.
- Silicon can exhibit oxidation states of +4 and -4.
- Germanium can exhibit oxidation states of +4 and +2.
- Tin can exhibit oxidation states of +4 and +2.
- Lead can exhibit oxidation states of +4 and +2.

3. **Divalent Species**:
For the reducing power, we focus on the +2 oxidation state of these elements: Ge^2+, Sn^2+, and Pb^2+.

4. **Evaluate Reducing Power**:
The reducing power of these divalent species is influenced by their ability to lose electrons. As we move down the group from Carbon to Lead, the reducing power generally decreases due to the increasing stability of the +2 oxidation state and the inert pair effect.

5. **Order of Reducing Power**:
The order of reducing power of the divalent species in group 14 is:
- Carbon (C) > Silicon (Si) > Germanium (Ge) > Tin (Sn) > Lead (Pb).

6. **Conclusion**:
Therefore, the reducing power of the divalent species decreases in the order:
**C > Si > Ge > Sn > Pb**.