Orbital, Suborbital, and Subshell- how to calculate MAX e-?

[Dencology]

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For example:

N=4

what is the max # of e- that N=4 has in its orbital would be is 2n^2 which would be 32 e-

now for subshell it would be 4L +2 which would be 14 e-

then, what it suborbital. this is driving me crazy?

 

[chessxwizard]

Orbitals that have the same value of the principal quantum number form a shell. Orbitals within a shell are divided into subshells that have the same value of the angular quantum number. Chemists describe the shell and subshell in which an orbital belongs with a two-character code such as 2p or 4f. http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch6/quantum.html

I believe that a single orbital can hold a maximum of 2 electrons.... why don't you just draw it out if it gives you trouble?

N=1; s, 2 electrons (1 orbital)
N=2; s, 2 electrons (1 orbital); p, 6 electrons (3 orbitals)
N=3; s, 2 electrons (1 orbital); p, 6 electrons (3 orbitals); d, 10 electrons (5 orbitals)

etc...

 

[unitix]

an orbital can only hold 2 electrons. So,

1s ||
2s || 2p || || ||
3s || 3p || || || .....

Just draw it out with x's or arrows, each mark above is an electron, as you can see the p subshell has 3 orbitals px py and pz, each holdin 2 e-, therefore a total of 6 electrons in the p subshell and 2 electrons in the single orbital-s subshell etc etc etc same with d which holds 10 e- max and f which holds 14 e- max. Add all the electrons in the shell (N, row) to get the sum/quantify the maximum.

 

[unitix]

Your original post is confusing, but re reading it I believe you're asking how many electrons can be in a orbital, and that's 2, one electron with a different spin +1/2,-1/2 which is the quantum number Ms. Make sure to read up on Paulie's Exclusion Theory.