Waiting for answer This question has not been answered yet. You can hire a professional tutor to get the answer.

QUESTION

# 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 .