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

  • Thread starter Thread starter no name
  • Start date Start date
Click For Summary
SUMMARY

The electron configuration 1s2 2s2 2p5 3s2 3p5 is theoretically possible for a non-ground state atom, but it exists only for an extremely brief duration, typically no longer than nanoseconds. This configuration arises when an electron is ejected from the 2p subshell, allowing an electron from the 3s subshell to occupy the vacancy. While the configuration can occur in an excited state, it is not a stable arrangement and should not be considered a general possibility.

PREREQUISITES
  • Understanding of electron configurations and subshells
  • Knowledge of atomic orbitals and their filling order
  • Familiarity with concepts of excited states in quantum chemistry
  • Basic principles of electron transitions and lifetimes
NEXT STEPS
  • Research the principles of electron configurations in excited states
  • Study quantum mechanics related to atomic orbitals and electron transitions
  • Explore the concept of electron lifetimes in excited states
  • Learn about the implications of electron configurations on chemical properties
USEFUL FOR

Chemistry students, educators, and anyone interested in atomic structure and quantum mechanics.

no name
Messages
48
Reaction score
0
is this electron configuration possible for non ground state atom:
1s2 2s2 2p5 3s2 3p5
Thannx in advance
 
Chemistry news on Phys.org
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.
 

Similar threads

Finding the g-value in the Boltzmann distribution
  • · Replies 7 ·
Replies
7
Views
2K
Chemistry: Electron Configurations & Reactivity
  • · Replies 4 ·
Replies
4
Views
3K
Electron Configuration Exceptions
  • · Replies 4 ·
Replies
4
Views
27K
3d orbital after 3p?Why not 4s?
  • · Replies 16 ·
Replies
16
Views
16K
What is the Correct Electron Configuration for Fe(2+)?
  • · Replies 5 ·
Replies
5
Views
4K
Principal Quantum Number of the Excited Oxygen atom.
  • · Replies 3 ·
Replies
3
Views
13K
Doubt regarding removing of electrons from shells
  • · Replies 3 ·
Replies
3
Views
4K
Which Electron Configurations of Phosphorus Are Correct?
  • · Replies 5 ·
Replies
5
Views
7K
Hybridized orbitals (can't understand diagram)
  • · Replies 14 ·
Replies
14
Views
3K
Why doesn;t Carbon show deviation from electron configuration
  • · Replies 1 ·
Replies
1
Views
6K