Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 14 - Acids and Bases - Conceptual Exercise 14.25 - Lewis Acids and Bases - Page 645: c


$H_2S$ is a Lewis acid and a Lewis base.

Work Step by Step

$H_2S$ is a Lewis acid because, it can receive one pair of electrons and make a bond with one of its hydrogen. For example: $H_2S(aq) + H_2O(l) \lt -- \gt HS^-(aq) + H_3O^+(aq)$ - This only happens because the "S" is more electronegative, making the hydrogens slightly positive, so it can receive electrons from another molecule, and create a bond. $H_2S$ is a Lewis base because, normally the central atom $(S)$ has 6 electrons in its valence shell, and it is making 2 covalent bonds with the hydrogens, therefore: 6 - 2 = 4, and there are 4 free electrons (2 lone pairs) this molecule can give, making it a Lewis base.
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