Explain how the charges of group a metal and nonmetal ions are related to their positions in the periodic table.

See explanation below

Explanation:

In the old nomenclature,.the periodic table is classified like this:

IA, IIA, IB, and such.

New nomenclature only name it like the number of columns the periodic table has, like group 1, 2, 3, 4 and so

Now using the old nomenclature, the groups with the "A" are:

Group 1: group IA

Group 2: IIA

Group 13 - 18: IIIA - VIIIA

These last groups are the non metal elements.

Now according to this, the relation is pretty easy to explain. Any element of group IA, IIA or IIIA when they lose electrons for any reason, they will always form cations, in other words, positive charges, and the number of these charges is equal to their group number, for example, if you take Sodium (Na) which is in group IA, and lose electrons, it's ion is Na+1 (the plus 1, is equal to the number of it's group). Same thing happen with an element of group IIA like Calcium, when it loses electrons, it becomes Ca+2.

On the other hand, any element of group IVA through VIIIA, which are the non metals, the charge of it's respective ion, is always determined substracting 8 from the group where they are. For example, if we take Carbon, which is in group IVA (Group 14), if we substract 8 from 4, we'll have -4, so it's charge would be -4.

In the case of Fluorine (Group VIIA), if we substract 8 from 7, we have -1, so the charge of fluorine is -1.

This is the relation between the charges of group A metals and non metals ions.

its first and third is your answer i did the qustion the fourth isnt right