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 determine the trend in 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 elements in the periodic table include Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb).

### Step 2: Understand the Nature of Oxides
The oxides of these elements can be classified based on their acidic or basic nature. Generally, oxides can be acidic, basic, or amphoteric.

### Step 3: Analyze the Trend in Electronegativity
As we move down the group from Carbon to Lead, the electronegativity of the elements decreases. Electronegativity is the ability of an atom to attract electrons towards itself.

### Step 4: Relate Electronegativity to Acidity
The acidic nature of oxides is influenced by the electronegativity of the element forming the oxide. Higher electronegativity typically leads to more acidic oxides because the element can better stabilize the negative charge of the oxide ion (O²⁻) when it reacts with water to form acids.

### Step 5: Determine the Trend in Acidity
Since the electronegativity decreases down the group, the acidic nature of the oxides also decreases. Therefore, the oxides of Carbon (CO₂) are more acidic compared to those of Silicon (SiO₂), Germanium (GeO₂), Tin (SnO₂), and Lead (PbO).

### Conclusion
Thus, the acidic nature of oxides of Group 14 elements decreases as we move down the group. Therefore, the correct answer to the question is that the acidic nature of oxides decreases down the group.

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