Chemistry: Molecular Approach (4th Edition)

Published by Pearson
ISBN 10: 0134112830
ISBN 13: 978-0-13411-283-1

Chapter 8 - Section 8.3 - Electron Configurations: How Electrons Occupy Orbitals - For Practice: 8.1

Answer

The electron configurations are: a. $Cl$ : $1s^22s^22p^63s^23p^5$ or $[Ne] 3s^23p^5$ b. $Si$ : $1s^22s^22p^63s^23p^2$ or $ [Ne] 3s^23p^2$ c. $Sr$ : $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^2$ or $[Kr] 5s^2$ d. $O$ : $1s^22s^22p^4$ or $[He] 2s^2 2p^4$

Work Step by Step

a. $Cl$ has 17 electrons. It has 7 more electrons than its previous noble gas, $Ne$. The electrons are distributed in the orbitals to get the electronic configuration: $1s^22s^22p^63s^23p^5$ or $[Ne] 3s^23p^5$ b. $Si$ has 14 electrons. It has 4 more electrons than its previous noble gas, $Ne$. The electrons are distributed in the orbitals to get the electronic configuration: $1s^22s^22p^63s^23p^2$ or $ [Ne] 3s^23p^2$ c. $Sr$ has 38 electrons. It has 2 more electrons than its previous noble gas, $Kr$. The electrons are distributed in the orbitals to get the electronic configuration: $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^2$ or $[Kr] 5s^2$ d. $O$ has 8 electrons. It has 6 more electrons than its previous noble gas, $He$. The electrons are distributed in the orbitals to get the electronic configuration: $1s^22s^22p^4$ or $[He] 2s^2 2p^4$
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