Density is highest for :

Options

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

Explanation

To determine which element has the highest density among the given options (Si, Ge, Sn, Pb), we can follow these steps:

### Step 1: Identify the Elements
The elements provided are:
- Si (Silicon)
- Ge (Germanium)
- Sn (Tin)
- Pb (Lead)

### Step 2: Understand the Group
All these elements belong to the carbon family (Group 14 of the periodic table).

### Step 3: Recall the Density Formula
Density is defined as:
\[ \text{Density} = \frac{\text{Mass}}{\text{Volume}} \]

### Step 4: Analyze Trends in the Periodic Table
As we move down a group in the periodic table:
- Atomic size increases.
- Atomic mass increases.

### Step 5: Relate Density to Atomic Mass and Volume
Since density is directly proportional to mass and inversely proportional to volume, we can infer that:
- As atomic mass increases (going down the group), density tends to increase as well, assuming the volume does not increase disproportionately.

### Step 6: Compare the Elements
- Si has a lower atomic mass and size compared to Ge, Sn, and Pb.
- Ge has a higher atomic mass and size than Si but lower than Sn and Pb.
- Sn has a higher atomic mass and size than both Si and Ge but lower than Pb.
- Pb has the highest atomic mass and size among these elements.

### Step 7: Conclusion
Since Pb (Lead) has the highest atomic mass and size, it will also have the highest density among the given options.

Thus, the correct answer is:
**Option D: Pb (Lead)**

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