Consider the following dioxide of group 14
1. `CO_2`
2. `SiO_2`
3. `GeO_2`
4. `SnO_2`
5. `PbO_2`
The basicity of the dioxide alters in the order

Options

A. `CO_2 gt SiO_2 gt GeO_2 gt SnO_2 gt PbO_2`
B. `CO_2 lt SiO_2 lt GeO_2 lt SnO_2 lt PbO_2`
C. `CO_2 lt SiO_2 lt GeO_2 lt PbO_2 lt SnO_2`
D. `CO_2 lt SiO_2 lt SnO_2 lt PbO_2 lt GeO_2`

Answer

To determine the order of basicity of the dioxides of Group 14 elements, we need to analyze the properties of each compound listed: CO₂, SiO₂, GeO₂, SnO₂, and PbO₂.

### Step-by-Step Solution:

1. **Identify the Nature of Each Oxide:**
- CO₂ (Carbon Dioxide): Non-metal oxide, acidic in nature.
- SiO₂ (Silicon Dioxide): Non-metal oxide, generally considered to be acidic or amphoteric.
- GeO₂ (Germanium Dioxide): Can exhibit amphoteric behavior.
- SnO₂ (Tin Dioxide): More metallic than GeO₂, generally amphoteric but can show basic character.
- PbO₂ (Lead Dioxide): More metallic, shows basic character.

2. **Understand the Trend Across the Group:**
- As we move from top to bottom in Group 14 (from C to Pb), the metallic character increases. This is because the elements become larger and more metallic in nature.
- The basicity of oxides generally increases down the group due to this increase in metallic character.

3. **Order the Basicity:**
- CO₂ is the least basic (acidic).
- SiO₂ is slightly more basic than CO₂ but still acidic.
- GeO₂ is amphoteric, so it is more basic than SiO₂.
- SnO₂ is more basic than GeO₂ due to its metallic character.
- PbO₂ is the most basic among these oxides.

4. **Final Order of Basicity:**
- The order of basicity from least to most basic is:
- CO₂ < SiO₂ < GeO₂ < SnO₂ < PbO₂

### Conclusion:
The basicity of the dioxides alters in the order:
**CO₂ < SiO₂ < GeO₂ < SnO₂ < PbO₂**