![]() For example, on the label of your dentist’s fluoride rinse, the compound chemists call tin(II) fluoride is usually listed as stannous fluoride. Even though this text uses the systematic names with roman numerals, you should be able to recognize these common names because they are still often used. The names of Fe 3 +, Fe 2 +, Sn 4 +, and Sn 2 + are therefore ferric, ferrous, stannic, and stannous, respectively. The name of the cation with the higher charge is formed from the root of the element’s Latin name with the suffix - ic attached, and the name of the cation with the lower charge has the same root with the suffix - ous. Thus Cu + is copper(I) (read as “copper one”), Fe 2 + is iron(II), Fe 3 + is iron(III), Sn 2 + is tin(II), and Sn 4 + is tin(IV).Īn older system of nomenclature for such cations is still widely used, however. In such cases, the positive charge on the metal is indicated by a roman numeral in parentheses immediately following the name of the metal. ![]() In particular, transition metals tend to lose electrons in the ns orbitals before they lose electrons in the (n-1)d orbitals. This behavior is observed for most transition metals, many actinides, and the heaviest elements of groups 13–15. As shown in Figure 10.3.2, many metals can form more than one cation. For example, Na + is the sodium ion, Ca 2 + is the calcium ion, and Al 3 + is the aluminum ion. The name of the cation of a metal that forms only one cation is the same as the name of the metal (with the word ion added if the cation is by itself). As noted in Section 3.3, these metals are usually in groups 1–3, 12, and 13.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |