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

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Discussion Overview

The discussion revolves around the possibility of the electron configuration 1s2 2s2 2p5 3s2 3p5 for a non-ground state atom. Participants explore the implications of this configuration in terms of stability and the conditions under which it might exist, focusing on theoretical and conceptual aspects.

Discussion Character

  • Debate/contested, Conceptual clarification

Main Points Raised

  • Some participants assert that the configuration is not possible, citing that it would have a very short lifetime, likely no longer than nanoseconds.
  • Others question the feasibility of filling the 3s orbital while the 2p subshell is not full, suggesting that a full 2p subshell is a prerequisite for such configurations.
  • A participant mentions a personal experience from a chemistry quiz where they answered negatively regarding the configuration's possibility, but received a different evaluation from their teacher.
  • One participant proposes that the configuration could exist temporarily if an electron is knocked out from the 2p subshell, allowing an electron from the 3s subshell to occupy the vacancy, although they caution against labeling it as generally "possible."

Areas of Agreement / Disagreement

Participants generally disagree on the possibility of the electron configuration being valid for a non-ground state atom, with multiple competing views on its stability and the conditions required for its existence.

Contextual Notes

There are unresolved questions regarding the assumptions about electron configurations and the definitions of "possible" in this context. The discussion reflects varying interpretations of excited states and the criteria for electron filling in subshells.

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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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