0
$\begingroup$

Do the outermost s1 and s2 electrons block an outside observer from measuring the larger inner group orbitals for elements heavier than Nitrogen (for instance, would Chromium's 4s1 electron or Manganese's 4s2 electrons prevent you from detecting the spin of the 3d5 electrons in either case?)

I edited this into an individual question from the original list of them per moderator instruction.

$\endgroup$
  • 1
    $\begingroup$ Have you heard about Aufbau principle? $\endgroup$ – Pritt Balagopal Aug 3 '17 at 13:09
  • $\begingroup$ @PrittBalagopal The Aufbau principle doesn't seem to hold up for the description of Vanadium, Chromium, Maganese and most other elements beyond group 2 (that is, inner orbitals get partially filled then jump to filling the next group of orbitals before going back downward.) $\endgroup$ – CoryG Aug 3 '17 at 14:37
  • 1
    $\begingroup$ It does hold for vanadium. Ot doesn't hold for chromium because $\mathrm{3d^5}$ is exceptionally stable due to being half filled. $\endgroup$ – Pritt Balagopal Aug 4 '17 at 0:42
  • $\begingroup$ @PrittBalagopal Vanadium is [Ar] 3d3 4s2 - meaning the 4s subshell gets filled before the 3d subshell. $\endgroup$ – CoryG Aug 4 '17 at 9:00
  • 1
    $\begingroup$ Well yeah? 4s does come before 3d in the Aufbau series. Look here. $\endgroup$ – Pritt Balagopal Aug 4 '17 at 11:07
1
$\begingroup$

With regards to your first question, as you get to higher energy levels, the distance between each one increases and as a consequence the shells get closer together and begin to overlap. This is also seen with 5s and 4d iirc.

$\endgroup$

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.