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RULES OF CHEMICAL NOMENCLATURE I. Elements (periodic table) A. Symbols: First letter or first two letters of the elements name. 1. Some use latin name for symbol, ex. gold (latin name= aurum or Au). 2. Learn all on page 166 that have an* plus Sb, As, Bi, Ce, Cs, Au, Kr, Mo,Pt, Ra, Rn, Rb, Sc, Se, Te, Tl, Ti, W, U & Xe. II. Formula: Represents composition of a compound. A. Tells proportions of elements in a compound relative to each other. 1. Subscripts are used to indicate number of atoms of each element in a compound. (whole numbers) 2. The subscript follows the atom or atoms it refers to. If subscript follows a “( )” then everything inside the “( )” is multiplied by the subscript. B. All atoms have oxidation numbers (valence). This is the combining power of the atom. C. Polyatomic ions or “radicals” are groups of atoms that behave as if they are single atoms. They also have oxidation numbers. ( we will show these later). D. We will use the concept of valence to write formulas. 1. Valence is either “+” or “-“. 2. In ALL compounds, the sum of the valences adds up to zero. 3. Metals are always “+”. 4. Non-metals can be “+” or “-“. 5. Most radicals are “-“ , only common “+” radical is NH4+1 (ammonium). E. Atoms that have a constant valence 1. Always +1 (H, Li, Na, K, Rb, Cs, Ag) 2. Always +2 ( Be, Mg, Ca, Sr, Ba, Zn,Cd) 3. Always + 3 (Al) (H can be –1 in some special cases) III. Binary Salts: a compound of a metal and a non-metal. (2 elements) A. Metal is always written first (because ‘+’ is always first), nonmetal is last. B. Named by adding name of first element (metal) to second element (non-metal) whose name is modified to end in “ide.” (metals are to the left of the staircase; non-metals are to the right in periodic table.) (oxygen becomes “oxide,” chlorine becomes “chloride,” sulfur becomes “sulfide,” etc.) C. Most metals have a variable valence and this must be indicated in the name of the compound. 1. The stock system: the valence (+) of the metal is given as a Roman numeral. a. Iron (Fe) can be either Fe +2 or Fe +3; therefore, both forms exist in compounds. (ex. Iron (II) Chloride = FeCl2 while Iron (III) Chloride = FeCl3) b. Can also be named Ferrous Chloride and Ferric Chloride. (This is the old way, but is still valid). IV. Salts: Those with Polyatomic ion or “radical” (see radical sheet) A. Four ways to identify salts: 1. metal + non-metal (binary) 2. metal + radical 3. radical (ammonium) + non-metal 4. radical (ammonium) + radical B. Naming salts (other than binary) 1. name of metal plus name of radical 2. name of radical (ammonium) plus name of non-metal or other radical. C. The “common form” of the radical must be memorized (see radical sheet) 1. common form has “ate” ending 2. other endings are based on the “ate” ending a. if there is one less oxygen, then the name ends in “ite” b. if there are two less oxygen, then the name starts with “hypo” and ends in “ite” c. if there is one more oxygen then the common form starts with “per” and ends in “ate” (ex. NaNO3 = Sodium Nitrate, NaNO2 = Sodium Nitrite, NaNO = Sodium Hyponitrite, NaNO4 = Sodium Pernitrate) V. Acids: All have H as the first element and are disolved in water (aqueous or “aq”) 1. Can be named as salts if not dissolved in water 2. Binary Acids: hydrogen + non-metal a. named by changing hydrogen to “hydro” b. change non-metal ending to “ic” (change “ide” to “ic”) c. followed by the word “acid” (ex: HCl = hydrochloric acid) 3. Ternary acids – hydrogen + radical a. named for the radical; “ate” changes to “ic” and is followed by “acid” (ex: HNO3 = Nitric Acid) b. “ite” changes to “ous” c. also uses “hypo” and “per” VI. Molecular Compounds: Non-metal plus non-metal A. Greek system of naming 1. only used for two non-metals 2. ends in “ide” 3. number of each kind of atom is indicated by a greek numerical prefix. a. mono = 1 b. di = 2 c. tri = 3 d. tetra = 4 e. penta = 5 f. hexa = 6 (ex: CO2 is Carbon Dioxide) • mono is usually omitted except in carbon monoxide (CO) • some names for compounds don’t fit the rules (ex: H2O = water, NH3 = ammonia)