Arrange the following atoms in the order of increasing atomic radius : N, B, C, S

Options

A. C, S, N, B
B. S, N, B, C
C. C, B, S, N
D. N, C, B, S

Explanation

To arrange the atoms N (Nitrogen), B (Boron), C (Carbon), and S (Sulfur) in the order of increasing atomic radius, we need to consider their positions in the periodic table and the trends in atomic radius.

### Step-by-Step Solution:

1. **Identify the Group and Period of Each Element:**
- Boron (B) is in Group 13, Period 2.
- Carbon (C) is in Group 14, Period 2.
- Nitrogen (N) is in Group 15, Period 2.
- Sulfur (S) is in Group 16, Period 3.

2. **Understand the Trend of Atomic Radius:**
- Atomic radius generally decreases across a period (from left to right) due to the increase in nuclear charge, which pulls the electrons closer to the nucleus.
- Atomic radius increases down a group due to the addition of electron shells.

3. **Compare the Elements:**
- Since B, C, and N are in the same period (Period 2), we can compare their atomic radii directly:
- Boron (B) has the largest atomic radius among B, C, and N because it is the furthest left in the period.
- Carbon (C) is smaller than Boron but larger than Nitrogen (N).
- Nitrogen (N) has the smallest atomic radius among these three.
- Sulfur (S) is in Period 3 and has a larger atomic radius than all the elements in Period 2 due to the addition of a new electron shell.

4. **Arrange in Order of Increasing Atomic Radius:**
- From the analysis, we have:
- Nitrogen (N) < Carbon (C) < Boron (B) < Sulfur (S)
- Therefore, the order of increasing atomic radius is:
- N < C < B < S

### Final Answer:
The order of increasing atomic radius is: **N < C < B < S**