The Correct Answer and Explanation is:
Let’s analyze each compound one by one with Lewis structures, molecular geometry, bond angles, hybridization, and polarity.
a. SF₄
- Lewis Structure: S is central with 4 single bonds to F and 1 lone pair.
- Electron Groups: 5 (4 bonding + 1 lone pair)
- Geometry: Seesaw
- Bond Angles: Approximately 102° (equatorial) and 173° (axial)
- Hybridization: sp³d
- Polarity: Polar (asymmetrical shape causes dipole moment)
b. AlCl₄⁻
- Lewis Structure: Al is central with 4 single bonds to Cl; gains one electron to complete octet
- Electron Groups: 4 (no lone pairs)
- Geometry: Tetrahedral
- Bond Angles: 109.5°
- Hybridization: sp³
- Polarity: Nonpolar (symmetrical charge distribution)
c. SF₆
- Lewis Structure: S is central with 6 single bonds to F
- Electron Groups: 6 (no lone pairs)
- Geometry: Octahedral
- Bond Angles: 90°
- Hybridization: sp³d²
- Polarity: Nonpolar (symmetrical)
d. POCl₃
- Lewis Structure: P is central with double bond to O and single bonds to 3 Cl
- Electron Groups: 4 (no lone pairs)
- Geometry: Tetrahedral
- Bond Angles: 109.5°
- Hybridization: sp³
- Polarity: Polar (due to differing atoms and dipole moments)
e. SOCl₂
- Lewis Structure: S is central, double bond to O, single bonds to 2 Cl, and 1 lone pair
- Electron Groups: 4 (3 bonding + 1 lone pair)
- Geometry: Trigonal pyramidal
- Bond Angles: Around 107°
- Hybridization: sp³
- Polarity: Polar
f. IBr₂⁺
- Lewis Structure: I is central with 2 single bonds to Br and 2 lone pairs
- Electron Groups: 4 (2 bonding + 2 lone pairs)
- Geometry: Bent
- Bond Angles: Less than 109.5°
- Hybridization: sp³
- Polarity: Polar
g. IF₅
- Lewis Structure: I is central with 5 single bonds to F and 1 lone pair
- Electron Groups: 6 (5 bonding + 1 lone pair)
- Geometry: Square pyramidal
- Bond Angles: 90° and <90°
- Hybridization: sp³d²
- Polarity: Polar
Each structure involves determining electron domains, geometry, and molecular symmetry to predict polarity and hybridization accurately.
