How many electrons occupy P orbitals in a chlorine atom?

1 Answer
Nov 8, 2015

Answer:

#11#

Explanation:

Your tool of choice here will be chlorine's electron configuration.

Chlorine, #"Cl"#, is located in period 3, group 17 of the periodic table, and has an atomic number equal to #17#. This tells you that a neutral chlorine atom will have a total of #17# electrons surrounding its nucleus.

Chlorine's electron configuration looks like this

#"Cl: " 1s^2 2s^2 2p^color(red)(6) 3s^2 3p^color(green)(5)#

Now, notice that the first energy level doesn't not contain a p-subshell, and implicitly any p-orbitals.

The second energy level, on the other hand, contains two subshells, the 2s-subshell, which contains #2# electrons, and the 2p-subshell, which contains three 2p-orbitals and a total of #color(red)(6)# electrons, #2# per orbital.

Finally, the third energy level contains two occupied subshells, the 3s-subshell, which once again contains #2# electrons, and the 3p-subshell, which contains #color(green)(5)# electrons.

Therefore, the number of electrons you get in p-orbitals will be equal to #11#

  • 6 electrons in the 2p-subshell
  • 5 electrons in the 3p-subshell