Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 7 - Periodic Properties of the Elements - Exercises - Page 293: 7.45d


The electron configuration for $Ag^{+}$ is $$Ag^{+}: [Kr]4d^{10}$$ $Ag^+$ does not have noble-gas configuration.

Work Step by Step

*RULES TO WRITE ELECTRON CONFIGURATIONS FOR IONS: - When electrons are removed to form cations, those of the orbitals that have the largest principal quantum number $n$ will be removed first. - If there are more than one subshell for a given $n$, electrons of the subshell with the highest value of $l$ will be removed first. - When electrons are added to form anions, they would be added to the empty or partially occupied orbital with the lowest value of $n$. 1) The electron configuration of a neutral $Ag$ atom is $$Ag: [Kr]4d^{10}5s^1$$ 2) Here we need to find the electron configuration for $Ag^{+}$, an ion having 1 electron removed from a neutral $Ag$ atom. Therefore, according to the rules, when electrons are removed, we would look for the orbital with the largest $n$ first. Here, subshell $5s$, with $n=5$, have the largest $n$. There are 1 electron occupying subshell $5s$ in a neutral $Ag$ atom. So that electron would be removed to created ion $Ag^+$. That means the electron configuration for $Ag^{+}$ is $$Ag^{+}: [Kr]4d^{10}$$ The above configuration is not the configuration of any noble gases, so $Ag^{+}$ does not have noble-gas configuration.
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