A chemistry reference book lists the following Pauling electronegativity values: H = 2.2, O = 3.5, N = 3.0, S = 2.5. Consider the four heteronuclear single bonds H–O, H–N, H–S, and H–H (for comparison purposes, treat the last as having zero electronegativity difference).
(a) Calculate ΔEN (the absolute electronegativity difference) for each of the four bonds.
(b) Rank the bonds from smallest to largest bond-dipole magnitude.
(c) Identify which bond is approximately twice as polar as the H–S bond and justify your choice quantitatively.