According to VSEPR theory, the most probable shape of the molecule having 4 electrons pairs in the outer shell of the central atom is

Options

A. Linear
B. Tetrhedral
C. Hexahedral
D. Octahedral

Answer

To determine the most probable shape of a molecule with 4 electron pairs in the outer shell of the central atom according to VSEPR (Valence Shell Electron Pair Repulsion) theory, follow these steps:

### Step 1: Identify the Number of Electron Pairs
The question states that there are 4 electron pairs around the central atom. These can be either bonding pairs (shared between atoms) or lone pairs (non-bonding pairs).

### Step 2: Determine the Arrangement of Electron Pairs
According to VSEPR theory, the arrangement of electron pairs around a central atom is based on minimizing repulsion between them. For 4 electron pairs, the arrangement that minimizes repulsion is tetrahedral.

### Step 3: Identify the Shape of the Molecule
When there are 4 bonding pairs and no lone pairs, the shape of the molecule is also tetrahedral. This means that the atoms bonded to the central atom will be positioned at the corners of a tetrahedron.

### Step 4: Provide Examples
Common examples of molecules that exhibit this tetrahedral shape include methane (CH₄) and silicon tetrafluoride (SiF₄). In these molecules, the central atom is bonded to four other atoms, forming a tetrahedral geometry.

### Conclusion
Thus, according to VSEPR theory, the most probable shape of a molecule having 4 electron pairs in the outer shell of the central atom is **tetrahedral**.