Sulfur Trioxide (SO₃):
* Hybridization: The sulfur atom in SO₃ undergoes sp² hybridization, which means its valence electrons are arranged in three sp² hybrid orbitals and one unhybridized p orbital.
* Bonding: These sp² orbitals form three sigma bonds with three oxygen atoms, creating a trigonal planar geometry.
* Shape: The three oxygen atoms are positioned at 120-degree angles around the central sulfur, resulting in a triangular planar shape.
* No lone pairs: The sulfur atom has no lone pairs of electrons.
Sulfur Dioxide (SO₂):
* Hybridization: The sulfur atom in SO₂ undergoes sp³ hybridization, which means its valence electrons are arranged in four sp³ hybrid orbitals.
* Bonding: These sp³ orbitals form two sigma bonds with two oxygen atoms.
* Lone pairs: The sulfur atom has one lone pair of electrons remaining.
* Shape: The two oxygen atoms and the lone pair of electrons are positioned around the central sulfur, creating a bent or V-shaped geometry. The lone pair exerts a stronger repulsive force than the bonding pairs, pushing the two oxygen atoms closer together.
In summary:
* The difference in shape is primarily due to the presence of a lone pair on the sulfur atom in SO₂ but not in SO₃.
* Lone pairs have a greater repulsive force than bonding pairs, causing a distortion in the geometry.
* In SO₃, the absence of a lone pair allows the three oxygen atoms to arrange themselves in a symmetrical triangular planar structure.
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