(A) In SO₂, the bond angle is 119° whereas in SO₃, the bond angle is 120°.
(R) S atom in both SO₂ and SO₃ is sp²-hybridized.

 Both (A) and (R) are true and (R) is not the correct explanation of (A)

Explanation:

SO₂ (Sulfur Dioxide):

In SO₂, the sulfur atom is sp²-hybridized. This means that one 3s orbital and two 3p orbitals of sulfur combine to form three equivalent sp² hybrid orbitals. Two of these orbitals form sigma bonds with oxygen atoms, while the third contains a lone pair of electrons. The remaining unhybridized 3p orbital overlaps with an oxygen 2p orbital to form a pi bond, resulting in a bent molecular geometry. The bond angle in SO₂ is approximately 119°, slightly less than the ideal 120° for a perfect trigonal planar structure, due to the lone pair's greater electron-electron repulsion. :contentReference[oaicite:0]{index=0}

SO₃ (Sulfur Trioxide):

In SO₃, the sulfur atom is also sp²-hybridized. It forms three sigma bonds with three oxygen atoms, with no lone pairs on the sulfur atom. The molecule adopts a trigonal planar geometry with a bond angle of 120°, consistent with the ideal bond angle for sp² hybridization. The absence of lone pairs on the sulfur atom allows for equal distribution of electron density, resulting in a symmetrical structure. :contentReference[oaicite:1]{index=1}

Both statements are correct. The sulfur atom in both SO₂ and SO₃ is sp²-hybridized. The difference in bond angles arises from the presence of a lone pair in SO₂, which causes slightly more repulsion, reducing the bond angle compared to SO₃. Therefore, the reason correctly explains the observed bond angle difference.