Match Molecular Shapes of Chemical Species with Number of Occurrences

To determine the correct match between List-I (molecular shapes) and List-II (number of occurrences), we analyze the hybridization, electron-pair geometry, and molecular shape of each given chemical species using the Valence Shell Electron Pair Repulsion (VSEPR) theory:

1. $\text{SOCl}_2$:

   • Central atom: Sulfur ($\text{S}$, 6 valence electrons).
   • Bonding: $1 \times \text{S=O}$ double bond (1 $\sigma$-bond) and $2 \times \text{S-Cl}$ single bonds (2 $\sigma$-bonds).
   • Lone pairs: $1$ lone pair on $\text{S}$.
   • Steric Number = $3$ ($\sigma$-bonds) + 1 (lone pair) = $4$.
   • Molecular Shape: Trigonal Pyramidal.

2. $\text{XeOF}_4$:

   • Central atom: Xenon ($\text{Xe}$, 8 valence electrons).
   • Bonding: $1 \times \text{Xe=O}$ double bond (1 $\sigma$-bond) and $4 \times \text{Xe-F}$ single bonds (4 $\sigma$-bonds).
   • Lone pairs: $\frac{8 - 2 - 4}{2} = 1$ lone pair on $\text{Xe}$.
   • Steric Number = $5$ ($\sigma$-bonds) + 1 (lone pair) = $6$.
   • Molecular Shape: Square Pyramidal.

3. $\text{ClF}_3$:

   • Central atom: Chlorine ($\text{Cl}$, 7 valence electrons).
   • Bonding: $3 \times \text{Cl-F}$ single bonds (3 $\sigma$-bonds).
   • Lone pairs: $\frac{7 - 3}{2} = 2$ lone pairs on $\text{Cl}$.
   • Steric Number = $3$ ($\sigma$-bonds) + $2$ (lone pairs) = $5$.
   • Molecular Shape: T-Shaped.

4. $\text{ClF}_5$:

   • Central atom: Chlorine ($\text{Cl}$, 7 valence electrons).
   • Bonding: $5 \times \text{Cl-F}$ single bonds (5 $\sigma$-bonds).
   • Lone pairs: $\frac{7 - 5}{2} = 1$ lone pair on $\text{Cl}$.
   • Steric Number = $5$ ($\sigma$-bonds) + 1 (lone pair) = $6$.
   • Molecular Shape: Square Pyramidal.

5. $\text{XeF}_5^+$:

   • Central atom: Xenon ($\text{Xe}^+$, $8 - 1 = 7$ valence electrons).
   • Bonding: $5 \times \text{Xe-F}$ single bonds (5 $\sigma$-bonds).
   • Lone pairs: $\frac{7 - 5}{2} = 1$ lone pair on $\text{Xe}$.
   • Steric Number = $5$ ($\sigma$-bonds) + 1 (lone pair) = $6$.
   • Molecular Shape: Square Pyramidal.

6. $\text{SO}_3^{2-}$:

   • Central atom: Sulfur ($\text{S}$, 6 valence electrons $+ 2$ electrons from charge $= 8$ valence electrons).
   • Bonding: $3 \times \text{S-O}$ bonds (3 $\sigma$-bonds).
   • Lone pairs: $\frac{8 - 6}{2} = 1$ lone pair on $\text{S}$.
   • Steric Number = $3$ ($\sigma$-bonds) + 1 (lone pair) = $4$.
   • Molecular Shape: Trigonal Pyramidal.

7. $\text{XeF}_3^+$:

   • Central atom: Xenon ($\text{Xe}^+$, $8 - 1 = 7$ valence electrons).
   • Bonding: $3 \times \text{Xe-F}$ single bonds (3 $\sigma$-bonds).
   • Lone pairs: $\frac{7 - 3}{2} = 2$ lone pairs on $\text{Xe}$.
   • Steric Number = $3$ ($\sigma$-bonds) + 2 (lone pairs) = $5$.
   • Molecular Shape: T-Shaped.

8. $\text{SF}_4$:

   • Central atom: Sulfur ($\text{S}$, 6 valence electrons).
   • Bonding: $4 \times \text{S-F}$ single bonds (4 $\sigma$-bonds).
   • Lone pairs: $\frac{6 - 4}{2} = 1$ lone pair on $\text{S}$.
   • Steric Number = $4$ ($\sigma$-bonds) + 1 (lone pair) = $5$.
   • Molecular Shape: See-saw.

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Counting the Species per Molecular Shape:

• (P) See-saw: $\text{SF}_4$ $\rightarrow$ 1 species (one) $\implies \text{P} \rightarrow 1$
• (Q) T-Shaped: $\text{ClF}_3, \text{XeF}_3^+$ $\rightarrow$ 2 species (two) $\implies \text{Q} \rightarrow 2$
• (R) Trigonal Planar: None $\rightarrow$ 0 species (zero) $\implies \text{R} \rightarrow 5$
• (S) Square Pyramidal: $\text{XeOF}_4, \text{ClF}_5, \text{XeF}_5^+$ $\rightarrow$ 3 species (three) $\implies \text{S} \rightarrow 3$

Thus, the correct matching is: $\text{P} \rightarrow 1; \quad \text{Q} \rightarrow 2; \quad \text{R} \rightarrow 5; \quad \text{S} \rightarrow 3$

Hence, the correct option is A.