General, Organic, and Biological Chemistry: Structures of Life (5th Edition)

Published by Pearson
ISBN 10: 0321967461
ISBN 13: 978-0-32196-746-6

Chapter 4 - Atoms - 4.7 Electron Configurations - Questions and Problems: 4.56

Answer

a) Magnesium: [Ne]$3s^2$ b) Oxygen: [He]$2s^2$$2p^4$ c) Sulfur: [Ne]$3s^2$$3p^4$ d) Nitrogen: [He]$2s^2$$2p^3$

Work Step by Step

Abbreviated electron configurations begin with the Noble gas from Group 8A from the period BEFORE the one your element is in and work outward from there. a) Magnesium: Period 3, Group 2A. Begins with [Ne] because Neon is the Noble gas in period 2. The electron configuration after [Ne] then beings with the 3rd s sublevel until all the electrons are accounted for. Thus, Mg, with 12 electrons, begins with [Ne] (10 electrons), the $3s^2$, to equal 12 total, represented like so: [Ne]$3s^2$. b) Oxygen: 8 electrons. Period 2, Group 6A, so n=2, with 6 valence electrons. Noble gas for period 1 is Helium (He), so the abbreviated electron configuration is [He]$2s^2$$2p^4$. c) Sulfur: 16 electrons. Period 3, Group 6A, n=3, with 6 valence electrons. The noble gas for period 2 is Neon (Ne), so the abbreviated electron configuration is [Ne]$3s^2$$3p^4$. d) Nitrogen: 7 electrons. Period 2, Group 5A, n=2, with 5 valence electrons. The noble gas for period 1 is Helium (He), so the abbreviated electron configuration is [He]$2s^2$$2p^3$.
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.