Two displayed structures are I: F–Xe–N[SO₂Cl]₂ and II: F–Xe–O–S(=O)₂–Cl. Assume the N and its three neighbours in I are coplanar; every S has four σ-bond directions; each Xe has two bonds and three lone pairs. Use only the supplied Lewis/local-domain model, not a literal d-orbital bonding theory. Which statements are correct?

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Each sulfur has two S=O directions, one S–Cl and one S–N or S–O direction, hence four σ domains. N in I is explicitly planar. Linking O in II has two bonds and two lone pairs, not no lone pairs. A Xe AX₂E₃ model puts the three lone pairs equatorial and two bonds axial. Every S=O double bond contains one σ bond, so I has four S–O σ bonds, not six. These domain and bond-component counts give A, C.

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