Created by StemPy LabTwo Lewis structures are drawn for . In structure I, sulphur forms two S=O double bonds and two S-OH single bonds. In structure II, all four bonds from sulphur are single, and the two oxygen atoms without hydrogen carry three lone pairs each. Judged by the formal-charge rule that NCERT uses to choose between Lewis structures, which statement is correct?
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← Match each species in List-I with its bond order and magnetic nature in List-II. Use the correct energy order of the molecular orbitals for each species. List-I (Species) A. N₂⁺ B. O₂²⁻ C. B₂ D. C₂²⁻ List-II (Bond order and magnetic nature) I. Bond order 3, diamagnetic II. Bond order 1, paramagnetic III. Bond order 2.5, paramagnetic IV. Bond order 1, diamagneticSome ionic compounds show partial covalent character, because the cation distorts the electron cloud of the anion. Read two statements on what makes this distortion larger. Statement I: For cations of similar size and the same charge, a cation with the configuration (n-1)dⁿ ns⁰ polarises an anion more than one with the noble gas configuration ns²np⁶. Statement II: A larger anion holds its outer electrons more tightly, so the covalent character falls as the anion becomes larger. →
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