Question

The correct order of atomic radii of N, F, Al, Si is:

• A. \( F > N > Si > Al \)
• B. \( F > N > Al > Si \)
• C. \( Al > Si > F > N \)
• D. \( Al > Si > N > F \)

Hint:

Atomic radius increases down a group and decreases across a period due to increasing nuclear charge.

Answer 1

The Correct Option is D

Step 1: Periodic Trends of Atomic Radius - Across a period: Atomic radius decreases. - Down a group: Atomic radius increases. Step 2: Apply the Trends - \( N \) and \( F \) are in the same period, but \( F \) has a smaller radius. - \( Si \) and \( Al \) are in the same period, but \( Al \) has a slightly larger radius. - Down the group, radius increases. Step 3: Correct Order \[ Al > Si > N > F \]

Answer 2

The atomic radius of elements depends on their position in the periodic table.

Given elements: Nitrogen (N), Fluorine (F), Aluminum (Al), and Silicon (Si).

Explanation:
1. All these elements are in the second and third periods of the periodic table.
2. Moving from left to right across a period, atomic radius decreases due to increasing nuclear charge pulling electrons closer.
3. Moving down a group, atomic radius increases due to addition of electron shells.

Positions of elements:
- Al and Si are in period 3 (third period).
- N and F are in period 2 (second period).

Therefore, atomic radius trend is:
- Among Al and Si (period 3), Al is to the left of Si, so Al > Si.
- Among N and F (period 2), N is to the left of F, so N > F.
- Period 3 elements have larger atomic radii than period 2 elements.

Hence, the correct order of atomic radii is:
\[ Al > Si > N > F \]