1. Use VSEPR theory to determine shape

A pyramidal shape generally arises when the central atom has:

• three bond pairs and one lone pair  trigonal pyramidal, or
• four bond pairs and one lone pair in a trigonal bipyramidal arrangement  see-saw / T-shaped, not simply pyramidal.

So we examine each species carefully.

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2. Option A: $SO_3$

In $SO_3$, sulfur is the central atom bonded to three oxygens.

• Number of electron domains around $S = 3$
• No lone pair on sulfur in the usual VSEPR description

Hence the geometry is: $\text{trigonal planar}$

So, $SO_3$ is not pyramidal.

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3. Option B: $BrF_3$

For $BrF_3$, bromine has 7 valence electrons.

• 3 bond pairs with fluorine
• 2 lone pairs on bromine

Thus total electron pairs around Br = 5, giving: $\text{trigonal bipyramidal electron pair geometry}$

With two equatorial lone pairs, the molecular shape becomes: $\text{T-shaped}$

So, $BrF_3$ is not pyramidal.

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4. Option C: $SiO_3^{2-}$

For $SiO_3^{2-}$, silicon is bonded to three oxygens.

Using VSEPR, silicon has 3 regions of electron density around it and no lone pair.

Hence shape is: $\text{trigonal planar}$

So, $SiO_3^{2-}$ is not pyramidal.

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5. Option D: $OSF_2$

This is thionyl fluoride, with sulfur as the central atom.

Structure: one $S=O$ bond and two $S-F$ bonds.

Now count electron domains around sulfur:

• one $S=O$ double bond  counts as one electron domain
• two $S-F$ single bonds  two electron domains
• one lone pair on sulfur

Total electron domains around sulfur = 4.

So electron pair geometry is: $\text{tetrahedral}$

With one lone pair and three bonded atoms, molecular shape is: $\text{trigonal pyramidal}$

Thus, $OSF_2$ has pyramidal shape.

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6. Final answer

The species having pyramidal shape is: $\boxed{D\;:\;OSF_2}$

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7. Comparison with stored correct answer

Stored correct answer: $D$

My derived answer is also $D$, so they agree.