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How many core electrons are in Iodine?
##46##
Iodine, ##"I"##, is located in period 5, group 17 of the , and has an equal to ##53##.
That means that a neutral iodine atom will have a total of ##53## electrons surrounding its nucleus.
Now, out of these ##53## electrons, some are considered core electrons and some areconsidered .
##n_"total" = n_"valence" + n_"core"##
But how would you distinguish between the two types of electrons?
To do that, you need to look at the of iodine, which looks like this
##"I: " 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5 52^2 4d^10 5p^5##
You know that the are defined as being the electrons located on the highest energy level of that atom, which is given by the principal quantum number, ##n##.
Notice that, in iodine's case, the highest energy level is ##n=5##. You have two subshells occupied with electrons on this energy level, ##5s^2## and ##5p^5##.
This means that iodine has a total of
##underbrace(2e^(-))_(color(blue)("from 5s subshell")) + overbrace(5e^(-))^(color(red)("from 5p subshell")) = "7 valence " e^(-)##
The rest of the electrons will thus be core electrons.
##n_"core" = n_"total" - n_"valence"##
##n_"core" = 53 - 7 = color(green)("46 core "e^(-))##
Therefore, a neutral iodine atom has ##46## core electrons and ##7## .