Given this set of quantum numbers for a multielectron atom, n=2, l=0, ml =0, ms =+1⁄2...
Given this set of quantum numbers for a multielectron atom, n=2, l=0, ml =0, ms =+1⁄2 and n=2, l=0, ml =0, ms =–1⁄2 which set of n and l quantum numbers corresponds to the lowest-energy configuration for the next additional electron?
Homework Answers
n = 2 means the shell is 2
l = 0 means the subshell is s
ml = 0 for l = 0 shubshell or s-subshell.
ms = +1/2 and -1/2 suggests that there are two electrons in the subshell. Thus, the given configuration is 2s2. The next lowest energy subshell is 2p. For p-subshell l = 1. Hence, the set of n and l quantum numbers that corresponds to the lowest energy for the next additional electron will be:
n = 2 and l = 1
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