![]() ![]() (2) These formulas are always written with hydrogenįirst. Two points should be noted: (1) The acid name has the prefix hydroĪnd the suffix ic. One for the pure state and one for the compound dissolved in water (see TableĦ.5). Therefore, these compounds have two sets of names, Because this property identifies an acid ( Section 5.7D ), these compounds When these compounds are dissolved in water, the solution contains hydrogen The binary nonmetallic compounds discussed in the preceding section. Group 6 of the periodic table combines with hydrogen can be named as were The binary compound formed when a halogen or any element, except oxygen, from The prefix mono is often omitted for the first element but never omitted for the second. In both the formula and the name of these compounds, the most nonmetallic element comes first (see The name of the second element is modified to the root of its name followed by the ending ide. TABLE 6.4 Prefixes used in naming binary compounds of two nonmetals Number They are named using prefixes to state how many atoms of an element are in one Carbon dioxide (CO 2)Īnd phosphorus trichloride (PCl 3) are examples of such compounds. Binary compounds containing two nonmetalsīinary compounds of two nonmetals, neither of which is hydrogen, are molecular TABLE 6.3 Some elements with non-English rootnames (root is italicized) ElementĢ. These elements that use Latin roots are shown in Table 6.3. Thus, in this system, Fe 2+ is ferrous and Fe 3+ is ferric Pb 2+ is plumbous and Pb 4+ is plumbic. Often this system also uses the Latin root of the name of the element. This older method gives the ending ous to the ion of lower oxidation state and the ending ic to the ion of higher oxidation state. Thus,īefore leaving this group of compounds, we should mention again the second and less-preferred method of naming cations of the same element in different oxidation states. The cation is named first and the anion second. In these examples, the root name of the element is italicized. The sulfide ion is S 2-, and the oxide ion is O 2. In binary compounds are named by using the root name of the element, followedīy the suffix ide for example, bromide ion is Br -, The proper names for these ions are chromium(II) and chromium(III). Ion does not say whether the ion is Cr 2+ or Cr 3+ According to IUPAC rules, the names of all other metallicĬations contain the name of the element followed by its oxidation state (in For example, the sodium ion can only be Na +, the calcium ion Only ions with a +2 charge, and aluminum forms only the ion Al 3+.įor these ions, the name of the element followed by the term ion is an unambiguous The names and formulas of cations and anions were introduced in SectionĪlkali metals form only ions with a +1 charge, the alkaline earth metals form Binaryīinary compounds of a metal and a nonmetal contain a metallic cation and a nonmetallicĪnion. Many chemical compounds are binary that is, they contain two elements. Number of nitrogen in the nitrate ion, NO 3 -, by setting We can use this rule to calculate the oxidation In a polyatomic ion, the net charge on the ion is the sum of the oxidation.(+2 for zinc and -2 for the two chloride ions) is 0. In the compound ZnCl 2, the oxidation number of the zinc ion is The sum of the oxidation numbers of the atoms in a compound is 0.Peroxides areĪn exception to this rule: In hydrogen peroxide, H 2O 2,įor example, the oxidation number of oxygen is -1. Oxygen in a compound usually has the oxidation number -2.To this rule occurs when hydrogen is bonded to a metal. Hydrogen in a compound usually has the oxidation number +1.In Ag 2S, the oxidation number of silverĪs Ag + is +1 and that of sulfur as S 2- is -2. The oxidation number of chlorine as Cl - is -1 and that of zincĪs Zn 2+ is +2. The oxidation number of a monatomic ion is the charge on that ion.Oxidation number of hydrogen in H 2 is 0. The oxidation number of zinc (Zn) as an uncombined atom is 0, and the The oxidation number of an uncombined element is 0.Oxidation numbers are assigned according to the following rules: Of an element represents the positive or negative character (nature) of an atom of that element in a particular bonding situation. Many of the rules by which names are assigned are based on the concept of oxidation numbers. TABLE 6.2 Names and formulas of some common ionic Several ionic compounds are listed in TableĦ.2, with both their common and systematic names. AlthoughĪll compounds have systematic names, many also have trivial, or common, names. Systematic names and are based on a set of rules drawn up by IUPAC. Of the compound and perhaps something of its properties. Ideally, this name should indicate the composition ![]()
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