Discussion Overview
The discussion centers on the atomic radius of Boron (B) compared to Beryllium (Be), exploring the reasons behind the observed size difference despite Boron having an additional p orbital. The scope includes theoretical considerations of electron configurations, ionization energies, and shielding effects.
Discussion Character
- Exploratory, Technical explanation, Debate/contested
Main Points Raised
- One participant notes that the first ionization energy decreases from Be to B, suggesting that the outermost electron in B is held more loosely, yet this does not correlate with an expected increase in atomic radius.
- Another participant proposes that the atomic radius of B is smaller due to a higher nuclear charge, despite its additional p orbital.
- A participant expresses confusion about the initial question, reiterating the inquiry regarding the smaller atomic radius of B despite having an extra p orbital shielded by full 1s and 2s orbitals.
- It is mentioned that the radius of the B+ ion is smaller than that of neutral Be, attributing this to the higher nuclear charge in B.
- One participant raises a point about the non-spherical nature of p orbitals, questioning how the size of Boron is defined in terms of dimensions.
Areas of Agreement / Disagreement
Participants express differing views on the factors influencing the atomic radius of Boron compared to Beryllium, indicating that the discussion remains unresolved with multiple competing explanations.
Contextual Notes
There are limitations in the assumptions made regarding electron shielding and the influence of nuclear charge on atomic size, which are not fully explored or agreed upon.
that isn't how it is... Now.. the universal question: WHY?