Share with your friends
Call
This may seem a bit confusing when one looks at , since chlorine is the seventh element in its row, but iodine is the seventeenth.
However, in the case of iodine, ten of the electrons that were added as we moved across the fifth row of the table belong to the fourth shell (the same one that is the valence shell for bromine), and not to the fifth.
The reason for this is rather lengthy, but suffice to say that it gives rise to the transition metals - these ten that make up columns 3 through 12. The electrons are filling energy levels based on the lowest available energy (as opposed to furthest from the nucleus, which is not quite the same thing).
Because these ten electrons are not in the outermost shell, they are not .
Specifically, with iodine, the fifth shell begins with two electrons, then ten go into the fourth shell as already mentioned, before the next five occupy the fifth shell again, for a total of seven valence electrons (just like chlorine).
Talk Doctor Online in Bissoy App