Select correct statement about radius of an atom:

Options

A. Values of Vander waal's radii are larger than those of convalent radii because the Vander waal's forces are much weaker than the forces operating between atoms in a covalently bonded molecule.
B. The matallic radii are smaller than the Vander waal's radii, since the bonding forces in the metallic crystal lattice are much stronger than the Vander waal's forces.
C. Both `(A)` & `(B)`
D. None of these

Answer

To solve the question regarding the correct statements about the radius of an atom, we will analyze the provided options step by step.

### Step 1: Understanding Atomic Radii
Atomic radii can be classified into different types based on the bonding and interactions between atoms. The main types include:
- **Covalent Radius**: The radius of an atom when it is covalently bonded to another atom.
- **Van der Waals Radius**: The radius of an atom when it is not bonded but is in close proximity to another atom, influenced by weak Van der Waals forces.
- **Metallic Radius**: The radius of an atom in a metallic crystal lattice.

### Step 2: Analyzing Option A
**Statement A**: "The value of Van der Waals radii are larger than those of covalent radii because Van der Waals forces are much weaker than the forces operating between atoms in covalently bonded molecules."

- **Analysis**: This statement is correct. Van der Waals radii are indeed larger than covalent radii. This is because, in covalent bonding, atoms are closely packed due to strong covalent bonds, resulting in a smaller radius. In contrast, Van der Waals interactions are weaker, allowing atoms to be further apart, resulting in a larger radius.

### Step 3: Analyzing Option B
**Statement B**: "The metallic radii are smaller than covalent and Van der Waals radii since the bonding forces in metallic crystal lattices are much stronger than Van der Waals forces."

- **Analysis**: This statement is also correct. In metallic bonding, atoms are held together by a sea of delocalized electrons, which creates a strong bonding force. However, the metallic radius is generally larger than the covalent radius but can be comparable to or sometimes larger than the Van der Waals radius, depending on the specific elements involved. Therefore, this statement needs clarification; while metallic bonding is strong, it does not necessarily mean metallic radii are smaller than both covalent and Van der Waals radii in all cases.

### Conclusion
Both options A and B contain elements of truth, but the interpretation of B needs careful consideration.

### Final Answer
- The correct interpretation is that **Option A is correct**, while **Option B is partially correct** but requires clarification regarding the comparison of radii.