Correct order of vander waals radii among the following is:

Options

A. `N gt O gt F gt Ne`
B. `Ne gt N gt O gt F`
C. `N gt Ne gt O gt F`
D. `F gt Ne gt O gt N`

Answer

To determine the correct order of Van der Waals radii among nitrogen (N), oxygen (O), fluorine (F), and neon (Ne), we can follow these steps:

### Step 1: Understand the Concept of Van der Waals Radii
Van der Waals radii refer to the effective size of atoms when they are not bonded to each other. It is influenced by the atomic size and the effective nuclear charge experienced by the outermost electrons.

**Hint:** Remember that Van der Waals radii are larger for atoms with weaker effective nuclear charge.

### Step 2: Identify the Group and Period of Each Element
- Nitrogen (N) is in Group 15.
- Oxygen (O) is in Group 16.
- Fluorine (F) is in Group 17.
- Neon (Ne) is in Group 18.

All these elements are in the same period (Period 2).

**Hint:** Elements in the same period have similar electron configurations but different nuclear charges.

### Step 3: Analyze the Trend in Effective Nuclear Charge
As we move from left to right across a period, the effective nuclear charge increases. This means that the attraction between the nucleus and the outermost electrons becomes stronger, leading to a decrease in atomic size.

**Hint:** Higher effective nuclear charge results in smaller atomic size.

### Step 4: Compare the Sizes of the Atoms
- **Nitrogen (N)**: Has the largest Van der Waals radius because it has the lowest effective nuclear charge.
- **Oxygen (O)**: Smaller than nitrogen but larger than fluorine and neon.
- **Fluorine (F)**: Smaller than both nitrogen and oxygen due to higher effective nuclear charge.
- **Neon (Ne)**: Has the smallest Van der Waals radius as it has the highest effective nuclear charge and is a noble gas.

**Hint:** Remember that noble gases have a complete outer shell and thus have the smallest radii.

### Step 5: Establish the Correct Order
Based on the analysis:
- Nitrogen (largest)
- Oxygen
- Fluorine
- Neon (smallest)

Thus, the correct order of Van der Waals radii from largest to smallest is:
**N > O > F > Ne**

### Final Answer
The correct order of Van der Waals radii among nitrogen, oxygen, fluorine, and neon is:
**N > O > F > Ne**