Predicting charges of an ion.?

Question

Each of the following elements is able to form an ion. Using the periodic table, predict the charge of the ion.

(a) Mg

(b) Al

(c) K

(d) S

can anyone explain how im supposed to do this. im new to chem and i was wondering if the charge of an ion is the same as its first oxidation state or.. what???

Answer 1

Mg (group 2) = 2+
Al (group 3) = 3+
K (group 1) = 1+

S (group 6) = 6-8 = 2- (octet rule)

Octet rule, gain or lose electrons to make the outermost shell with 8 electrons. those metals lose group-number of electrons, the next outermost shell become the outermost.

Answer 2

For cations (positively charged ions), look at the column number. This has to do with the number of electrons. Column I forms singly charged cations.
Column II forms doubly charged cations.
Column III (for Al), etc.
Think of anions as coming from the opposite direction.
Halides would be ionic column I.
Sulfur is in the next column (II).

Answer 3

ok rather plenty no count number if this is low style of valance electrons then it's going to be a possitive ion because of the fact it loses electrons and vice versa. Be=2+(valance=2) F=a million- (valance=7) Na=a million+ (valance=a million) S=2-(valance=6) Ca=2+(valance=2) Cl=a million-(valance=7) valance of a million-4 is + valance of four-8 is - 4 is impartial!! sturdy luck!!

Answer 4

For a metal: Group Number followed by +.
For a non-metal: 8 - Group Number followed by -.

Don't write any figure 1s.

K is therefore K+ and so on.