What are the electron configurations for I and N3?

Question

Mateo Aguilar · Accepted Answer

#I : [Kr] 5p^5 # and #N^(3-) : 1s^2 2s^2 2p^6#

The atomic number—the total number of electrons in the ground state—and oxidation state of an element determine the electron configurations.

Ground state Iodine has an atomic number of 53. Simply use this information to obtain its electronic configuration. #I : 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^5# or simply #I : [Kr] 5p^5 #.

When considering oxidation states for elements that are not in the ground state, one can simply use the notation "n+" to indicate the removal of n electrons from the total number of electrons of the ground state element, or "n-" to indicate the addition of n electrons.

For example, #N^(3-)#. "3-" means adding 3 more electrons to its number of electrons in ground state. Nitrogen has 7 electrons in the ground state with electron configuration of #N : 1s^2 2s^2 2p^3#. Adding 3 more electrons would give us a total of 10 electrons. Therefore, #N^(3-) : 1s^2 2s^2 2p^6#

Kai Bowman · Answer

undefined Iodine (I) has the following electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^5. The nitride ion (N3-) has the following electron configuration: 1s^2 2s^2 2p^6.