Electron Configuration of Filled Valence Electron Orbitals

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SUMMARY

The discussion centers on the electron configuration of elements such as Beryllium (Be) and Calcium (Ca), which have fully filled 2s orbitals but unfilled p orbitals. Participants clarify that these elements can participate in chemical bonding despite having no unpaired electrons by promoting an s electron to a p orbital, allowing for bonding through an excited state configuration (e.g., Be 2s2 to Be 2s12p1). This mechanism contrasts with elements like Sodium (Na) and Chlorine (Cl), which bond using unpaired electrons in their outer orbitals.

PREREQUISITES
  • Understanding of electron configurations in atomic theory
  • Familiarity with concepts of ionic and covalent bonding
  • Knowledge of excited states in quantum mechanics
  • Basic grasp of periodic table trends and orbital filling
NEXT STEPS
  • Study the principles of electron promotion in atomic orbitals
  • Learn about the differences in bonding mechanisms between main group elements
  • Explore the concept of excited states and their role in chemical reactions
  • Investigate the properties of alkaline earth metals and their bonding behavior
USEFUL FOR

Chemistry students, educators, and professionals interested in atomic structure, bonding theories, and the behavior of alkaline earth metals in chemical reactions.

Dong Aleta
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Hi!

I have understood how elements such as Be and Ca, with fully filled 2s orbitals, are not to be considered "noble" because they still have unfilled p orbitals. But I'm having trouble understanding how these elements participate in chemical reactions without having any unpaired electrons.

My understanding is that for an atom to bond (ionically or covalently) it has to have an unpaired electron. Is that incorrect? If yes, can you please explain how? Thanks so much!
 
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The energetic difference between s and p orbitals is quite low in these elements so that the energy required to promote an s electron to a p orbital before bonding is made up by the energy gained in bonding.
 
DrDu said:
The energetic difference between s and p orbitals is quite low in these elements so that the energy required to promote an s electron to a p orbital before bonding is made up by the energy gained in bonding.
Does that mean that elements such as Be and Ca have a different mechanism for forming bonds, different than those of, say Na with an unpaired 3s1 electron and Cl with another unpaired 3p5 electron?
 
Not really. But in Be or Ca, you have to start (at least conceptually) from an excited state of the atom, i.e. Be 2s##^2## -> Be 2s##^1##2p##^1##.
 
DrDu said:
Not really. But in Be or Ca, you have to start (at least conceptually) from an excited state of the atom, i.e. Be 2s##^2## -> Be 2s##^1##2p##^1##.
Oh I see! I get it now. Thank you so much! I really appreciate the assistance. :D
 

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