Exploring Energy Levels and Electron Configurations in Atomic Models

Click For Summary
SUMMARY

The discussion focuses on the electron configurations in atomic models, specifically addressing the distribution of electrons across different shells and sub-shells. The K, L, M, and N shells correspond to electron capacities of 2, 8, 18, and 32, respectively, based on their sub-shell compositions: s (2), p (6), d (10), and f (14). The inquiry also highlights the energy dynamics of electrons in outer shells, noting that electrons in the outermost shell require less energy to remove despite being farther from the nucleus.

PREREQUISITES
  • Understanding of atomic structure and electron shells
  • Familiarity with quantum numbers and their significance
  • Knowledge of sub-shell types: s, p, d, f
  • Basic principles of electron energy levels
NEXT STEPS
  • Research the Pauli Exclusion Principle and its impact on electron configurations
  • Learn about the Aufbau principle for filling electron shells
  • Explore Hund's Rule in relation to electron distribution in sub-shells
  • Investigate the relationship between electron energy levels and ionization energy
USEFUL FOR

Students of chemistry, educators teaching atomic theory, and anyone interested in the principles of electron configurations and energy levels in atomic models.

scientifico
Messages
181
Reaction score
0
Hello, why in the normal atomic configuration every layer except the second can contain only up to 8 electrons if for example the level with quantic number 3 contain up to 18 electrons?
What relation is there between this two models?

Thank you!
 
Physics news on Phys.org
You have the K,L,M,N (and so on) shells, which contain 2,8,18,32.. electrons.

Those numbers come from the sub-shells which make up the shells, which are denoted s,p,d,f.
The sub-shells contain 2, 6, 10, 14 electrons, respectively. (twice the odd numbers 1,3,5,7)

The K shell contains only an s sub-shell, so it has two electrons in total. The L shell has one s and one p, giving 2+6=8 electrons in total.
The M shell has an s,p and d, so 2+6+10 = 18, and the N shell has an f sub-shell as well, so 2+6+10+14 = 32 electrons.
 
An electron in the last layer require less energy to be removed, so why the last layer has more energy than the layer nearest the nucleum?
 

Similar threads

Undergrad Amount of electrons in nuclei
  • · Replies 10 ·
Replies
10
Views
2K
Undergrad Electromagnetic radiation, photons, quantized energy levels
  • · Replies 1 ·
Replies
1
Views
2K
Undergrad Weakly interacting electrons in an atom
  • · Replies 2 ·
Replies
2
Views
2K
Undergrad Electron configuration vs. Lewis dot structure?
  • · Replies 1 ·
Replies
1
Views
1K
High School Are electrons in atoms always in eigenstates?
  • · Replies 6 ·
Replies
6
Views
2K
Undergrad Why does the energy level of an electron in an atom have a width?
  • · Replies 3 ·
Replies
3
Views
2K
Undergrad Continuous Spectrum and Energy levels of Electrons (Energy Bands)
  • · Replies 7 ·
Replies
7
Views
3K
High School Energy needed for electron's change in energy level in an atom
  • · Replies 15 ·
Replies
15
Views
3K
Help with Atomic Calcium Electron Configurations
  • · Replies 11 ·
Replies
11
Views
3K
Undergrad Calculate the energy of the electron in a non-H like atom
  • · Replies 6 ·
Replies
6
Views
2K