# Chapter 6 - Electronic Structure of Atoms - Exercises: 6.79c

After filling the subshell $3s$, the electrons must move to the next lowest-energy subshell, the $3p$, not the $3d$.

#### Work Step by Step

$[Ne]3s^23d^5$ The problem here is quite similar to part a). After completely filling the orbital in subshell $3s$ with 2 electrons, the electrons must move to the next lowest-energy subshell, which is the $3p$ subshell, not the $3d$ one. Therefore, one correct electron configuration must be $[Ne]3s^23p^5$

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