Why is the ion charge of iodine -1?

Answer 1

Iodine is a halogen (group 7 of the Periodic Table), and halogens are supposed to have seven valenced electrons to match the amount of protons in their nucleus. However, in order to form a full octet of valence electrons, iodine atoms are willing to accept one more electron. This electron brings iodine's charge down to -1. And unlike other halogens that are smaller than iodine (fluorine, chlorine, and bromine), iodine is large enough so that its negative charge can be distributed more evenly. This makes iodine stable with a negative charge, and a good leaving group in chemical reactions (something you will probably learn later on in organic chemistry).

Answer 2

It isn't - it is neutral - but when ionized becomes -2. This is because of its position in the periodic table. It wants to become a stable Neon type structure - 10 electrons - to do this it needs to acquire 2 electorns and hence it will become -2 charge when ionized

Answer 3

Iodine typically gains one electron to achieve a stable electron configuration of eight valence electrons, resulting in a negative charge of -1. This configuration allows iodine to achieve a stable noble gas configuration similar to its nearest noble gas, xenon.

Answer 4

Oxygen's charge is -2, NOT -1 Oxygen's charge is -2, NOT -1

Answer 5

A lone, neutral oxygen atom has 6 electrons in its outer shell, but this is not very stable, so oxygen will tend to gain 2 more electrons in order to get a full, stable shell of 8 electrons.