The tendency of group 14 elements to show +2 oxidation state increases in the order of

Options

A. `C lt Si lt Sn lt Pb lt Ge`
B. `C lt Si lt Ge lt Sn lt Pb`
C. `Ge lt Sn lt Pb lt C lt Si`
D. `Pb lt Sn lt Ge lt C lt Si`

Explanation

To determine the order of the tendency of group 14 elements to show a +2 oxidation state, we can analyze the elements in this group, which are Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb).

### Step-by-Step Solution:

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

2. **Understand Oxidation States**: Group 14 elements can exhibit oxidation states of +4 and +2. The +4 oxidation state is due to the involvement of all four valence electrons, while the +2 state arises when only the two p electrons are involved.

3. **Inert Pair Effect**: The tendency to show the +2 oxidation state increases down the group due to the inert pair effect. This effect refers to the reluctance of the s-electrons (ns²) to participate in bonding as we move down the group.

4. **Analyze Each Element**:
- **Carbon (C)**: The +2 oxidation state is less stable because it prefers to form covalent bonds and typically exhibits a +4 state.
- **Silicon (Si)**: Similar to Carbon, Silicon can show +2 but prefers +4.
- **Germanium (Ge)**: Shows a more pronounced +2 state compared to Si and C due to the inert pair effect starting to take place.
- **Tin (Sn)**: More stable in the +2 state due to the inert pair effect being more significant.
- **Lead (Pb)**: The +2 oxidation state is quite stable due to the inert pair effect being fully realized.

5. **Order of Increasing Tendency**: Based on the above analysis, the order of increasing tendency to show the +2 oxidation state is:
- Carbon (C) < Silicon (Si) < Germanium (Ge) < Tin (Sn) < Lead (Pb)

### Final Order:
The tendency of group 14 elements to show +2 oxidation state increases in the order:
**C < Si < Ge < Sn < Pb**