Non-Ground State Atom: 1s2 2s2 2p5 3s2 3p5 - Possible?

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The discussion centers on the feasibility of the electron configuration 1s2 2s2 2p5 3s2 3p5 for a non-ground state atom. Participants agree that while this configuration is theoretically possible for a very brief moment—likely no longer than nanoseconds—it is not stable or typical. The conversation highlights the confusion surrounding the filling of the 3s orbital before the 2p subshell is fully occupied. One explanation provided is that an electron from the 2p subshell can be excited and subsequently replaced by an electron from the 3s subshell, leading to the temporary existence of the stated configuration. However, it is emphasized that such configurations are not generally considered valid in standard chemistry contexts. The original poster expresses frustration over being marked wrong on a quiz for stating that this configuration is not possible, prompting suggestions to seek clarification from the teacher.
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is this electron configuration possible for non ground state atom:
1s2 2s2 2p5 3s2 3p5
Thannx in advance
 
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It will have a very tiny lifetime, probably no longer than nanoseconds - in other words, "NO".

Why do you ask ?
 
Gokul43201 said:
It will have a very tiny lifetime, probably no longer than nanoseconds - in other words, "NO".

Why do you ask ?

How is it even possible to fill up the 3s orbital when the 2p isn't full?
 
in my chem quiz there was a question like this ' is it possible to have this electron configuration for an excited atom' ..
i wrote no ... but the teacher marked me wrong ...
wut do u think ..?
 
anyone has any clue?
 
Bladibla said:
How is it even possible to fill up the 3s orbital when the 2p isn't full?
You start with a full 2p subshell. Then an electron or photon comes by and knocks out one of the 2p electrons. Very soon, an electron from the 3s subshell falls to occupy the vacancy created. But for a very tiny length of time, the stated configuration exists (but it's unfair to say that such a configuration is, in general, "possible").
 
no name said:
in my chem quiz there was a question like this ' is it possible to have this electron configuration for an excited atom' ..
i wrote no ... but the teacher marked me wrong ...
wut do u think ..?
You should ask your teacher for his/her reasoning is...and do come back and let us know what it is.
 

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