Created by StemPy LabAssertion (A): The O-O bond in is shorter than the O-O bond in , although has one electron fewer than to hold the two oxygen nuclei together. Reason (R): When loses an electron to form , the electron is removed from a bonding molecular orbital, so fewer bonding electrons remain.
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← Match each species in List-I with the hybridisation of its central atom in List-II. Count every region of electron density on the central atom: a bonded atom counts as one region, whatever the bond order, and so does a lone pair. List-I (Species) A. NO₂⁺ B. CO₃²⁻ C. SO₄²⁻ D. SF₄ List-II (Hybridisation of the central atom) I. sp³ II. sp III. sp³d IV. sp²A student writes six statements about dipole moments. (i) SF₄ has zero dipole moment, because its four S-F bond dipoles cancel. (ii) BF₃ has zero dipole moment, although each B-F bond is polar. (iii) CCl₄ has zero dipole moment, but CHCl₃ does not. (iv) In the crossed arrow for a bond dipole, the cross is at the negative end. (v) 1 D equals 3.33564 × 10⁻³⁰ C m. (vi) CO₂ has zero dipole moment, but H₂O does not. How many of these statements are correct? →
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