The tendency of Ge, Sn, Pb to show `+2` oxidation state, increases in the sequence

Options

A. `Ge=SnltPb`
B. `GeltSnltPb`
C. `GegtSngtPb`
D. `GegtSn=Pb`

Explanation

To determine the increasing tendency of Germanium (Ge), Tin (Sn), and Lead (Pb) to show a +2 oxidation state, we can analyze the properties of these elements in relation to their position in the periodic table and their atomic sizes.

### Step-by-Step Solution:

1. **Identify the Elements**: We are considering three elements: Germanium (Ge), Tin (Sn), and Lead (Pb). These elements belong to Group 14 of the periodic table.

2. **Understand Oxidation States**: The +2 oxidation state is common for these elements, but the tendency to exhibit this state can vary. Generally, as we move down a group in the periodic table, the tendency to lose electrons and show a +2 oxidation state increases due to the increase in atomic size and the shielding effect.

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