The molecular shapes of SF$$_4$$, CF$$_4$$ and XeF$$_4$$ are

To decide whether the three molecules have identical or different shapes and to count the lone-pairs present on their central atoms, we use the VSEPR (Valence Shell Electron Pair Repulsion) model.

Case 1: $$SF_4$$
• Central atom = S. Its valence-shell configuration is $$3s^2\,3p^4$$, so it brings 6 valence electrons.
• Four $$F$$ atoms contribute $$4 \times 1 = 4$$ electrons (one from each for the S-F σ-bonds).
• Total electron pairs around S $$= \frac{6+4}{2} = 5$$ pairs → AX$$_4$$E (4 bonding + 1 lone pair).
• Geometry of 5 electron pairs is trigonal bipyramidal; the presence of one lone pair gives a see-saw (disphenoidal) molecular shape.

Case 2: $$CF_4$$
• Central atom = C. Valence electrons = 4.
• Four $$F$$ atoms contribute 4 electrons for bonding.
• Total electron pairs around C $$= \frac{4+4}{2} = 4$$ pairs → AX$$_4$$ (4 bonding + 0 lone pairs).
• Geometry of 4 electron pairs is tetrahedral and, with no lone pair, the molecular shape is also tetrahedral.

Case 3: $$XeF_4$$
• Central atom = Xe. Valence electrons = 8.
• Four $$F$$ atoms give 4 electrons for bonding.
• Total electron pairs around Xe $$= \frac{8+4}{2} = 6$$ pairs → AX$$_4$$E$$_2$$ (4 bonding + 2 lone pairs).
• Geometry of 6 electron pairs is octahedral; two lone pairs occupy trans axial positions, leaving a square-planar molecular shape.

Summary:
• $$SF_4$$: 1 lone pair, see-saw shape.
• $$CF_4$$: 0 lone pairs, tetrahedral shape.
• $$XeF_4$$: 2 lone pairs, square-planar shape.
Thus the molecules have different shapes and possess 1, 0 and 2 lone pairs on the central atoms, respectively.

Option D which is: different with 1, 0 and 2 lone pairs of electron on the central atoms respectively