On moving down the group, acidic nature of oxides of group 14.

Options

A. Decreases
B. Increases
C. Remains same
D. Increases then decreases

Answer

To analyze the acidic nature of oxides of group 14 elements as we move down the group, we can follow these steps:

### Step 1: Identify the Group 14 Elements
Group 14 of the periodic table includes the following elements:
- Carbon (C)
- Silicon (Si)
- Germanium (Ge)
- Tin (Sn)
- Lead (Pb)

### Step 2: Understand the Nature of Oxides
The oxides of these elements can be classified based on their acidic or basic nature:
- **Non-metal oxides** (like CO2) are generally **acidic**.
- **Metalloid oxides** (like SiO2 and GeO2) can be **acidic** or **amphoteric** (showing both acidic and basic properties).
- **Metal oxides** (like SnO2 and PbO) are generally **basic**.

### Step 3: Analyze the Trend in Acidic Nature
As we move down the group from carbon to lead:
- The non-metal character decreases, and the metallic character increases.
- Carbon (C) has a strong acidic oxide (CO2).
- Silicon (Si) has an oxide (SiO2) that is acidic.
- Germanium (Ge) has oxides that can be amphoteric.
- Tin (Sn) and Lead (Pb) have oxides that are more basic in nature.

### Step 4: Conclusion on Acidic Nature
As we progress down the group:
- The acidic nature of the oxides decreases.
- The basic character of the oxides increases.

Thus, the overall trend is that the acidic nature of the oxides of group 14 **decreases** as we move down the group.

### Final Answer:
The acidic nature of the oxides of group 14 decreases as we move down the group.

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