What will be the shape of the compound `MB_(4)L_(2)`? Here B is bond pair and L is lone pair.

Options

A. Square planar
B. Octahedral
C. Square pyramid
D. Tetrahedral

Explanation

To determine the shape of the compound \( MB_4L_2 \), where \( B \) represents bond pairs and \( L \) represents lone pairs, we can follow these steps:

### Step 1: Identify the Central Atom and Count Bond and Lone Pairs
- The central atom is \( M \).
- There are 4 bond pairs (\( B_4 \)) and 2 lone pairs (\( L_2 \)).

### Step 2: Calculate the Steric Number
- The steric number is calculated as the sum of the number of bond pairs and lone pairs:
\[ \text{Steric Number} = \text{Number of Bond Pairs} + \text{Number of Lone Pairs} = 4 + 2 = 6 \]

### Step 3: Determine the Electron Geometry
- According to VSEPR (Valence Shell Electron Pair Repulsion) theory, a steric number of 6 corresponds to an octahedral electron geometry.

### Step 4: Determine the Molecular Geometry
- In the case of \( MB_4L_2 \), we have 4 bond pairs and 2 lone pairs. The lone pairs will occupy positions that minimize their repulsion, which are typically opposite each other in an octahedral arrangement.
- This arrangement leads to a molecular geometry that excludes the lone pairs, resulting in a square planar shape.

### Step 5: Draw the Structure
- Visualizing the structure, we place \( M \) at the center and the 4 surrounding atoms (let's call them \( X \)) at the corners of a square, with the 2 lone pairs positioned above and below the plane of the square.

### Conclusion
- The shape of the compound \( MB_4L_2 \) is **square planar**.

### Final Answer
- The shape of the compound \( MB_4L_2 \) is **square planar**.

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