The species having pyramidal shape is

Options

A. `SO_(3)`
B. `BrF_(3)`
C. `SiO_(3)^(2-)`
D. `OSF_(2)`

Explanation

To determine which species has a pyramidal shape from the given options (SO3, BRF3, SiO3, OSF2), we will analyze each compound step by step.

### Step 1: Analyze SO3
- **Hybridization**: SO3 has sulfur in the center bonded to three oxygen atoms.
- **Shape**: The shape of SO3 is trigonal planar due to sp² hybridization. There are no lone pairs on the sulfur atom.
- **Conclusion**: SO3 is not pyramidal.

### Step 2: Analyze BRF3
- **Hybridization**: In BRF3, bromine is bonded to three fluorine atoms and has two lone pairs of electrons.
- **Shape**: The presence of lone pairs leads to a T-shaped geometry, which is not pyramidal.
- **Conclusion**: BRF3 is not pyramidal.

### Step 3: Analyze SiO3
- **Hybridization**: SiO3 has silicon in the center bonded to three oxygen atoms.
- **Shape**: Similar to SO3, SiO3 is also trigonal planar due to sp² hybridization. There are no lone pairs on silicon.
- **Conclusion**: SiO3 is not pyramidal.

### Step 4: Analyze OSF2
- **Hybridization**: In OSF2, oxygen is bonded to one sulfur atom and two fluorine atoms.
- **Shape**: The presence of one lone pair on the oxygen leads to a pyramidal shape (specifically, a bent or angular shape).
- **Conclusion**: OSF2 has a pyramidal shape.

### Final Answer
The species having a pyramidal shape is **OSF2**.

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