The metallic character of element of group 14

Options

A. Decreses from top to bottom
B. Increases from top to bottom
C. Does not change gradually
D. Metallic character is not seen

Answer

To determine the metallic character of elements in Group 14, we can follow these steps:

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

### Step 2: Classify the Elements
Next, we classify these elements based on their metallic character:
- Carbon (C) is a nonmetal.
- Silicon (Si) and Germanium (Ge) are metalloids.
- Tin (Sn) and Lead (Pb) are metals.

### Step 3: Observe the Trend in Metallic Character
As we move down the group from Carbon to Lead, we observe the following trend:
- The metallic character increases as we go down the group.
- Carbon, being at the top, is a nonmetal, while Lead at the bottom is a metal.

### Step 4: Explain the Reason for the Trend
The increase in metallic character down the group can be attributed to the following reasons:
- The atomic size increases down the group, which leads to a decrease in ionization energy.
- Lower ionization energy makes it easier for the atoms to lose electrons and exhibit metallic properties.

### Step 5: Conclusion
Thus, the metallic character of elements in Group 14 increases from Carbon to Lead. Therefore, the correct statement is that the metallic character increases from top to bottom in Group 14.

### Summary
- **Group 14 Elements**: C, Si, Ge, Sn, Pb
- **Trend**: Metallic character increases from Carbon (nonmetal) to Lead (metal).
- **Reason**: Increasing atomic size and decreasing ionization energy.