You use the periodic table to assign standard charges to ions.
To assign charges to ions, you must recognize these rules apply to main group elements. The other elements correspond to transition metals and post transition metals. You can not transfer the same rules to transition metals.
The main group comprises IA(1)-IIA(2), and IIIA(13)-XVIIA(18).
Figure 1 shows the main group elements in white. The grayed out areas show the transition metals.
The ability to predict charges resides in the main group elements. Any elements between IB(3)-VIIIB(12) are transition metal elements. You can not predict the charge in the same simple straight forward way.
In another way to see the periodic table, elements are divided into metals and nonmetals. Ionic compounds form from a metal and nonmetal (or nonmetal polyatomic ion). Both a metal and a nonmetal must be present.
You can do this when you divide the periodic table into metal and nonmetal elements, shown in Figure 2.
On the left side of Figure 2 the gray shaded area shows which elements are metals. Next to the metals on the right, a zig-zag region with a marbled texture shows metalloids. The far right of the periodic table shows white elements which correspond to nonmetals.
Metalloids are elements between metals and nonmetals. These elements have properties of both metals and nonmetals, but are not completely either one.
The way an ion forms from an element, whether it loses electrons or gains electrons depends on whether an element is a metal or nonmetal, Figure 3.
How many electrons (negative charges) does an atom lose to become a cation or gain to become an anion? The answer depends on how many valence electrons an element has when it is neutral.
The number of charges an element gains or loses, must in the end, equal eight valence electrons in its outer most electron shell. This is the same number of electrons in the valence electron shell of as the inert noble gases.
Whether an element gains or loses electrons in order to conform to the octet rules is a characteristic which makes an element a metal or nonmetal.
Figure 4 shows both a metal and nonmetal in a gray neutral state. Their path to obtain an octet of valence electrons are opposites. Nonmetals gain electrons to become anions. Metals lose electrons to reach a state where they mimic the valence electrons of the noble gases.
When a metal forms an ion, it gives up its valence electrons and becomes a positively charge atom, cation.
For instance sodium has one valence electron. It gives up its electron because it is a metal. That gives it a +1 charge. The electron shell below its outermost electron shell has a full octet. Sodium has sacrificed its outer electron to resemble the electron configuration of neon.
In contrast to metals, nonmetals gain electrons. When a neutral atom gains electrons it becomes negative, an anion.
For example sulfur has six valence electrons in its outer most electron shell. That's two fewer electrons than argon. When sulfur gains two electrons to become an anion, it now has eight electrons in its valence shell. This makes the sulfide -2 anion have the same stable configuration as argon.
Main group elements have predictable charges they assume when they become ions. The charge they most frequently assume depends on which column an element is found in. Figure 5 shows which elements assume which charge by the family of element.
Notice carbon and group 14 (IVA) does not have a charge assigned to it. This is because carbon can take a +4 or -4 charge depending on who its bonding partner is.
The other main group elements however follow predictable patterns when they form ions.
Bare in mind an element only becomes an ion under the influence of a near by complimentary element. Metals and nonmetals in their native state always have a charge of zero (or neutral).
For example sodium metal has a charge of 0. When sodium (Na) encounters a nonmetal like chlorine (Cl2) which also has a charge of zero, the sodium loses and electron while chlorine gains an electron. That is the moment when an element takes on the identity of an ion.
In language you will often hear: "what charge does calcium have?" The element itself does not have a charge. The question stated more correctly would be: "What charge does calcium take when it becomes an ion due to its interaction with an element which can accept its electrons?"
The first question is the more common one, but it usually means the second question. Just keep the idea straight that elements do not have charges, but ions of the elements do have charges.Tags: anion, cation, ionic compounds, ions