Comment on below statement
In bcc lattice, the atoms at the corners of the unit cell are in contact with each other.

Explanation

To analyze the statement "In bcc lattice, the atoms at the corners of the unit cell are in contact with each other," we can follow these steps:

### Step 1: Understand the BCC Structure
The Body-Centered Cubic (BCC) lattice consists of atoms located at each of the eight corners of a cube and one atom at the center of the cube.

### Step 2: Visualize the Unit Cell
Draw a cube to represent the BCC unit cell. Mark the positions of the atoms:
- Place an atom at each of the eight corners of the cube.
- Place one atom at the center of the cube.

### Step 3: Analyze Atomic Contact
To determine if the corner atoms are in contact, consider the distance between two corner atoms along the edge of the cube. The distance between two corner atoms is equal to the length of the edge of the cube.

### Step 4: Calculate Edge Length and Atomic Radius
In a BCC lattice, the relationship between the edge length (a) and the atomic radius (r) can be derived from the geometry of the unit cell. The diagonal of the cube can be expressed in terms of the atomic radius:
- The body diagonal of the cube is \( \sqrt{3}a \).
- Along the body diagonal, there are two atomic radii from the corner atom to the center atom and one atomic radius from the center atom to the opposite corner atom, giving us the equation:
\[ \sqrt{3}a = 4r \]
- Therefore, the edge length \( a \) can be expressed as:
\[ a = \frac{4r}{\sqrt{3}} \]

### Step 5: Conclusion
Since the corner atoms do not touch each other (the distance between them is greater than the atomic radius), the statement is false. The corner atoms are separated by a distance equal to the edge length, which is greater than twice the atomic radius.

### Final Comment
Thus, the statement "In bcc lattice, the atoms at the corners of the unit cell are in contact with each other" is incorrect.

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