Binary Ionic Compounds (Type I)
1. The cation (positively charged ion; Na+, Al3+) is always named first and the anion (negatively chargedion; Cl-, O2-) second.
2. A monatomic (meaning one-atom) cation takes its name from the name of the element. For example, Na+ is called sodium in the names of compounds containing this ion.3. A monatomic anion is named by taking the root of the element name and adding -ide. Thus, the Cl- ion is called chloride, the S2- ion is called sulfide, and the O2- ion is called oxide.
Somecommon monatomic cations and anions are shown below |
Cation | Name | Cation | Name | | Anion | Name | Anion | Name |
H+ | Hydrogen | Li+ | Lithium | | H- | Hydride | F- | Fluoride |
Na+ |Sodium | K+ | Potassium | | Cl- | Chloride | Br- | Bromide |
Cs+ | Cesium | Be2+ | Beryllium | | I- | Iodide | O2- | Oxide |
Mg2+ | Magnesium | Ca2+ | Calcium | | S2- | Sulfide | Se2- |Selenide |
Ba2+ | Barium | Al3+ | Aluminum | | N3- | Nitride | P3- | Phosphide |
Zn2+ | Zinc | Ag+ | Silver | | As3- | Arsenide | C4- | Carbide |
Binary Ionic Compounds (Type II)
1. The cationof a transition metal is always named first (like any cation) and the anion second.
2. A monatomic (meaning one-atom) cation takes its name from the name of the element. For example, Cu+ iscalled Copper(I) and Cu2+ is called Copper(II) in the names of compounds containing these ions. The number in parentheses is the charge of the cation.
3. All transition metal cations, except Zn2+,Cd2+, and Ag+ (which always have the charges shown here), must show the oxidation number (charge) in parantheses following the English spelling of the element, such as Iron(III), Copper(I), orVanadium(V), whenever a compound containing these ions, which have multiple charges, is named.
4. For the cations in Groups IIIA-VIA (including, Sn, Pb, Ga, Bi, etc.) also have multiple charges, even...