Question #03743

1 Answer
Jun 29, 2017

Answer:

#6# electrons per energy level starting with the second energy level.

Explanation:

The angular momentum quantum number, #l#, describes the energy subshell in which an electron is located inside an atom.

In your case, #l=1# describes the #p# subshell.

Now, in order to figure out the number of electrons that can have #l=1#, i.e. the number of electrons that can occupy a #p# subshell, you must first determine the number of orbitals that are present in this subshell.

The number of orbitals present in a given subshell can be calculated by using

#"no. of orbitals" = 2l + 1#

In your case, you have

#"no. of orbitals" = 2 * 1 +1 = 3#

This means that a #p# subshell, regardless of the energy level on which it is located (for energy levels that are #>1#, of course), can hold #3# orbitals.

According to Pauli's Exclusion Principle, each orbital can hold a maximum of #2# electrons, one having spin-up and one having spin-down.

You can thus say that a #p# subshell can hold a maximum of

#3 color(red)(cancel(color(black)("orbitals"))) * "2 e"^(-)/(1color(red)(cancel(color(black)("orbital")))) = "6 e"^(-)#

Therefore, you can say that #6# electrons can share #l=1# per energy level.