Chapter 8 Bonding and Molecular Structure - Study Questions - Page 337b: 35

Work Step by Step

a) Valence electrons C: 4, H: 1, O: 6, N:5 Bicarbonate: $3×6+1+4+1=24$ Nitric acid: $1+5+3×6=24$ They are isoelectronic. b) Two ressonance structures each, alternating the O= with the O- group. c) The nitrogen in nitric acid has a formal charge of +1, the oxygen making a single bond only in both cases has a formal charge of -1, but due to ressonance, they have a -1/2 charge along with the one making a double bond. d) It's harder to remove/easier to add a $H^+$ from/to a negatively charged anion like bicarbonate than nitric acid, therefore it's more acidic.

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