Pz.-The fourth quantum number (spin quantum number) will matter for Nitrogens ground state configuration. The three electrons that are to fill up the Px, Py, & Pz orbitals of the 2P subshell must fill each orbital with the SAME spin quantum number (+1/2 or -1/2) & unpaired (b/c of Hunds rule).Report Abuse-1s+- 2s+- 2py+- 2px+ 2pz+ for a ground state Oxygen would be correct because there were initially +1/2 spins in each Px,......
The possible combinations would result in: (1s^2) (2s^2) (2p^2) ---> (with the orbitals within the 1s and 2s subshells completely filled) The "2p" shell has the three orbitals of Px, Py, and Pz. The two remaining electrons that will go in the "2p" subshell can decide to be in a combination of either the Px, Py or Px, Pz or Py, Pz.
The fourth quantum number (spin quantum number) will matter for Nitrogen's ground state configuration. The three electrons that are to fill up the Px, Py, & Pz orbitals of the 2P subshell must fill each orbital with the SAME spin quantum number (+1/2 or -1/2) & unpaired (b/c of Hund's rule).
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1s+- 2s+- 2py+- 2px+ 2pz+ for a ground state Oxygen would be correct because there were initially +1/2 spins in each Px, Py, & Pz. Then the fourth electron would have to have a -1/2 spin regardless of which orbital (either Px, Py, or Pz) it was placed it.
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Filling of electronic covers occurs so that total backs was maximum.
The order of filling electronic orbital is confirmed experiment.(Hund rule)
In much electronic atoms electron move in the field of a kernel and others electrons and consequently there are exceptions at sequence of filling electronic orbital (will accept d-elements 39-48).
I don't think so, since these three orbitals are degenerate, that is, they have same energies.
