Electronic configuration for ions

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SUMMARY

The discussion centers on the electronic configuration of ions, specifically addressing the order of electron addition and removal in relation to the building-up principle. For principal quantum numbers n ≥ 4, electrons are added to the (n-1)d orbitals before the p-orbitals. When forming cations, electrons are removed first from the np-orbitals, then from the ns-orbitals, and finally from the (n-1)d orbitals. The participants seek clarification on the energy level calculations that dictate these configurations, particularly the relationship between E((n-1)d) and E(ns) for n ≥ 4, and how ionization affects orbital splitting.

PREREQUISITES
  • Understanding of the Aufbau principle in electron configuration
  • Familiarity with quantum numbers and orbital types (s, p, d)
  • Knowledge of ionization processes and their effects on electron configurations
  • Basic principles of atomic structure and energy levels
NEXT STEPS
  • Research the Aufbau principle and its implications for electron configurations
  • Study the differences in energy levels between ns and (n-1)d orbitals for n ≥ 4
  • Explore the concept of ionization energy and its impact on orbital arrangement
  • Investigate advanced topics in quantum mechanics related to atomic structure
USEFUL FOR

Chemistry students, educators, and professionals seeking a deeper understanding of electronic configurations in ions, particularly those studying advanced atomic theory and quantum mechanics.

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When we try to predict electronic configurations by the building up principle we add electrons to the d-orbitals before the p-orbitals for principal quantum numbers n ≥ 4.

What I don't understand is why, according to my textbook, we're supposed to remove electrons from np-orbitals first, then ns-orbitals and then (n-1)d-orbitals when predicting the configuration for cations.

Why do we add electrons to (n-1)d-orbitals after ns-orbitals but remove electrons from ns-orbitals before (n-1)d-orbitals? - makes no sense.

Furthermore, if someone could explain or point me somewhere to an explanation as to how the energy levels are calculated (why E((n-1)d) > E(ns) for n ≥ 4) that would be great.
 
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Because it makes a difference whether you are comparing neutral atoms or an atom and an ion.
On ionization the ordering of the orbitals becomes more hydrogen like, i.e. the splitting of the s, p, and d orbitals decreases.
 
I see, thanks - for the answer to my other question as well!

I'm guessing this is beyond undergraduate courses?
 

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