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Rules for Naming Compounds 1. When combining ions or atoms to form a compound, always write the metal first, then the nonmetal. Ions with positive oxidation numbers (+) are considered to be metals. Ions with negative oxidation numbers (-)are considered to be nonmetals. ex. Chart 1 – Metals and Nonmetals Metal Nonmetal Formula H+1 O-2 H2O Ba+2 S-2 BaS NH4 +1 CO3 Ca+2 -2 (NH4)2CO3 F-1 CaF2 2. When naming a compound, the atom representing the metal remains the same; however, the atom representing the nonmetal is changed by dropping the suffix or ending and adding –ide. ex. Chart 2 – Suffixes for Nonmetals Metal Nonmetal Name Formula Hydrogen Oxygen Hydrogen oxide H2O Barium Sulfur Barium sulfide BaS Lithium Iodine Lithium iodide LiI Calcium Fluorine Calcium fluoride CaF2 The exceptions to this rule pertain to polyatomic ions. Do not change the suffix or ending of the polyatomic ion that represents a nonmetal. ex. Metal Chart 3 – Polyatomic Ions as Nonmetals Nonmetal Name Formula Cesium Carbonate Cesium carbonate Ce2CO3 Lithium Sulfate Lithium sulfate Li2SO4 Hydrogen Peroxide Hydrogen peroxide H2O2 Strontium Nitrate Strontium nitrate Sr(NO3)2 3. When naming a compound, use Roman Numerals to identify the oxidation state of the metal, not the nonmetal. This method is usually used with atoms of multiple oxidation states. Copper, Tin, Lead, Mercury, and Iron 1 Do not use the Roman numeral with the nonmetal. ex. Metal Cu +2 Chart 4 – Roman Numerals for Metals Nonmetal Name -2 O Formula Copper II Oxide CuO Sn+4 O-2 Tin IV Oxide SnO2 Pb +4 O2 -2 Lead IV Peroxide Pb(O2)2 Hg+2 O-2 Mercury II Oxide HgO 4. When naming a compound, use –ic and –ous suffix to identify the oxidation state of the metal, not the nonmetal. This method is usually used with atoms of multiple oxidation states. Copper, Tin, Lead, Mercury, and Iron Do not use the –ic and –ous ending as a suffix on the nonmetal. ex. Metal Cu +2 +4 Chart 5 – The Metals ends :-ic and –ous Nonmetal Name Formula -2 Cupric Oxide CuO -2 O Sn O Stannic Oxide SnO2 Pb+4 O2-2 Plumbic Peroxide Pb(O2)2 +2 -2 Mercuric Oxide HgO -2 Ferrous Oxide FeO Hg +2 Fe Atom O O Chart 6 – Summary of Rules 3 and 4 -ic or -ous Roman Numeral Chemical Symbol Copper Cupric Copper II Cu+2 Copper Cuprous Copper I Cu+1 Mercury Mercuric Mercury II Hg+2 Mercury Mercurous Mercury I Hg+1 Iron Ferric Iron III Fe+3 Iron Ferrous Iron II Fe+2 Tin Stannic Tin IV Sn+4 Tin Stannous Tin II Sn+2 Lead Plumbic Lead IV Pb+4 Lead Plumbous Lead II Pb+2 2 5. When naming a compound, use the prefixes below to identify the number of atoms in the metal or nonmetal. The prefix can be used with the metal and the nonmetal or with just the metal or with just the nonmetal. The prefix usually identifies the atom in the compound with the subscript See charts 7-8 Chart 7 – Prefixes for Compounds Number Prefix 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca- Chart 8 – Naming Compounds with Prefixes Chemical Formula Name CO2 carbon dioxide H2O dihydrogen oxide CO carbon monoxide CCl4 carbon tetrachloride CS2 carbon disulfide SF6 sulfur hexafluoride BaCl2 barium dichloride NaI monosodium iodide 6. When metals are combined with oxygen, many compounds are formed depending upon the oxidation state of the metals. -ate -ite hypo…ite hyper…ate Roman Numerals are used prefixes are used See charts 9-10 below 3 Chart 9 - Nitrogen Oxides Chemical Formula Name N2O nitrogen I oxide, dinitrogen oxide, nitrous oxide NO nitrogen II oxide, nitrogen oxide, nitric oxide N2O3 nitrogen III oxide, dinitrogen trioxide NO2 nitrogen IV oxide, nitrogen dioxide, nitrite N2O4 nitrogen IV oxide, dinitrogen tetraoxide N2O5 nitrogen V oxide, dinitrogen pentoxide Chart 10 – hypo, hyper, -ate, -ite prefixes and suffixes Chemical Formula Name HClO4 hydrogen perchlorate HClO3 hydrogen chlorate HClO2 hydrogen chlorite HClO hydrogen hypochlorite H3PO4 hydrogen phosphate H3PO3 hydrogen phosphite H3PO2 hydrogen hypophosphite H2SO4 hydrogen sulfate H2SO3 hydrogen sulfite H2SO2 hydrogen hyposulfite HNO3 hydrogen nitrate HNO2 hydrogen nitrite HNO hydrogen hyponitrite 7. Acids are formed by adding a hydrogen ion to an ionic compound. The subscript (aq) is added to the compound to designate the compound is an acid. see Chart 11 (aq) means aqueous or dissolved in water The hydrogen or hydronium ion is key to forming the acid 4 Ion Chart 11 - Ionic Compounds Forming Acids + H+ Compound Acid ClO4- (perchlorate) + H+ HClO4 (hydrogen perchlorate) HClO4(aq) (perchloric acid) ClO3- (chlorate) + H+ HClO3 (hydrogen chlorate) HClO3(aq) (chloric acid) ClO2- (chlorite) + H+ HClO2 (hydrogen chlorite) HClO2(aq) (chlorous acid) ClO- (hypochlorite) + H+ HClO (hydrogen hypochlorite) HClO(aq) (hypochlorous acid) Cl- + H+ HCl (hydrogen chloride) HCl(aq) C2H3O2- (acetate) + H+ HC2H3O2 (hydrogen acetate) HC2H3O2(aq) (acetic acid) CO3-2 (carbonate) + H+ H2CO3 (hydrogen carbonate) H2CO3(aq) (carbonic acid) C2O4-2 (oxalate) + H+ HC2O4-2 (hydrogen oxalate) HC2O4-2(aq) (oxalic acid) PO4-3 (phosphate) + H+ H3PO4 (hydrogen phosphate) H3PO4(aq) (phosphoric acid) PO3-3 (phosphite) + H+ H3PO3 (hydrogen phosphite) H3PO3(aq) (phosphorous acid) PO2-3 (hypophosphite) + H+ H3PO2 (hydrogen hypophosphite) H3PO2(aq) (hypophosphorous acid) SO4-2 (sulfate) + H+ H2SO4 (hydrogen sulfate) H2SO4(aq) (sulfuric acid) SO3-2 (sulfite) + H+ H2SO3 (hydrogen sulfite) H2SO3(aq) (sulfurous acid) SO2-2 (hyposulfite) + H+ H2SO2 (hydrogen hyposulfite) H2SO2(aq) (hyposulfurous acid) NO3- (nitrate) + H+ HNO3 (hydrogen nitrate) HNO3(aq) (nitric acid) NO2- (nitrite) + H+ HNO2 (hydrogen nitrite) HNO2(aq) (nitrous acid) NO- (hyponitrite) + H+ HNO (hydrogen hyponitrite) HNO(aq) (hyponitrous acid) (chlorine) (hydrochloric acid) 5 Chart 12 - Common Acids Binary Acids (2 elements) Monoprotic Chemical Formula Acid HF(aq) hydrofluoric acid HCl(aq) hydrochloric acid HBr(aq) hydrobromic acid HI(aq) hydroiodic acid Polyprotic H2S(aq) hydrosulfuric acid Ternary Acids (3 elements) HNO3(aq) nitric acid HNO2(aq) nitrous acid H2SO4(aq) sulfuric acid H2SO3(aq) sulfurous acid HClO4(aq) perchloric acid HClO3(aq) chloric acid HClO2(aq) chlorous acid HClO(aq) hypochlorous acid HC2H3O2(aq) acetic acid H3PO4(aq) phosphoric acid H2CO3(aq) carbonic acid H2BO3(aq) boric acid 8. When naming organic compounds, use the prefix that designates the number of carbons in the compound. See chart 13 6 Chart 13 – Prefixes for organic compounds Number of Carbons Prefix 1 meth- 2 eth- 3 prop- 4 but- 5 pent- 6 hex- 7 hept- 8 oct- 9 non- 10 dec- 9. When naming organic compounds, use the suffix that designates the number of single bonds in the compound. If the compound has all single bonds which cause the compound to be saturated with hydrogen atoms. The suffix is –ane. If the compound has all single bonds and 1 double bond, the suffix used is –ene. If the compound has all single bonds and 1 triple bond, the suffix used is –yne. See chart 14-17 Chart 14 – Suffixes for organic compounds Types of Bonds Suffix Single Bonds -ane Double Bonds -ene Triple Bonds -yne 7 Chart 15 – Suffixes for Saturated Hydrocarbons Saturated Hydrocarbons Name Chemical Formula methane CH4 ethane C2H6 propane C3H8 butane C4H10 pentane C5H12 hexane C6H14 heptane C7H16 octane C8H18 nonane C9H20 decane C10H22 equation CnH2n+2 Chart 16 – Suffixes for Unsaturated Hydrocarbons Unsaturated Hydrocarbons Name Chemical Formula ethene C2H4 propene C3H6 butene C4H8 pentene C5H10 hexene C6H12 heptene C7H14 octene C8H16 nonene C9H18 decene C10H20 equation CnH2n 8 Chart 17 – Suffixes for Unsaturated Hydrocarbons Polyunsaturated Hydrocarbons Name Chemical Formula ethyne C2H2 propyne C3H4 butyne C4H6 pentyne C5H8 hexyne C6H10 heptyne C7H12 octyne C8H14 nonyne C9H16 decyne C10H18 equation CnH2n-2 9 Chart 18 – Summary of the Hydrocarbons Name Chemical Formula ethyne C2H2 propyne C3H4 butyne C4H6 pentyne C5H8 hexyne C6H10 heptyne C7H12 octyne C8H14 nonyne C9H16 decyne C10H18 equation CnH2n-2 ethene C2H4 propene C3H6 butene C4H8 pentene C5H10 hexene C6H12 heptene C7H14 octene C8H16 nonene C9H18 decene C10H20 equation CnH2n methane CH4 ethane C2H6 propane C3H8 butane C4H10 pentane C5H12 hexane C6H14 heptane C7H16 octane C8H18 nonane C9H20 decane C10H22 equation CnH2n+2 10 Structure Formulas for 11 12 Works Cited Smoot, Robert C., et al. Chemistry A Modern Course. Columbus: Merrill, 1990. 13