If the ionic radii of each `K^(+)` and `F^(-)` are `1.34Å`, then tha atomic radii of `K` and `F` will be respectively:

Options

A. `1.34 Å, 1.34 Å`
B. `0.72Å, 1.96 Å`
C. `1.96 Å.0.72Å`
D. `1.96Å,1.34Å`

Answer

To find the atomic radii of potassium (K) and fluorine (F) based on the given ionic radii of their respective ions, we can follow these steps:

### Step 1: Understand Ionic vs. Atomic Radius
- The ionic radius of an atom changes when it gains or loses electrons.
- A cation (like K⁺) is formed when an atom loses electrons, resulting in a smaller radius compared to the neutral atom.
- An anion (like F⁻) is formed when an atom gains electrons, resulting in a larger radius compared to the neutral atom.

### Step 2: Analyze the Given Ionic Radii
- We are given that the ionic radii of K⁺ and F⁻ are both 1.34 Å.
- This means:
- Ionic radius of K⁺ = 1.34 Å
- Ionic radius of F⁻ = 1.34 Å

### Step 3: Determine the Relationship for Potassium (K)
- Since K⁺ is smaller than K (because K loses one electron to become K⁺), we can conclude:
- Atomic radius of K > Ionic radius of K⁺
- Therefore, Atomic radius of K > 1.34 Å

### Step 4: Determine the Relationship for Fluorine (F)
- Since F⁻ is larger than F (because F gains one electron to become F⁻), we can conclude:
- Atomic radius of F < Ionic radius of F⁻
- Therefore, Atomic radius of F < 1.34 Å

### Step 5: Conclusion
- Based on the above deductions:
- The atomic radius of potassium (K) is greater than 1.34 Å.
- The atomic radius of fluorine (F) is less than 1.34 Å.

### Final Answer
- The atomic radii of K and F will be respectively:
- K: > 1.34 Å
- F: < 1.34 Å