IIIIIIIV Chemical Nomenclature I. Ions to Know II. Molecular Compounds III. Ionic Compounds IV.Acids

I. Ions to Know NH 4 + Ammonium ionOH - Hydroxide ionC 2 O 4 -2 Oxalate ionPO 4 -3 Phosphate ion H3O+H3O+ Hydronium ionCN - Cyanide ionCrO 4 -2 Chromate ionPO 3 -3 Phosphite ion Hg 2 +2 Mercury (I) ionHCO 3 - Bicarbonate ionCr 2 O 7 -2 Dichromate ionAsO 4 -3 Arsenate ion C2H3O2-C2H3O2- Acetate ionO 2 -2 Peroxide ion NO 3 - Nitrate ionCO 3 -2 Carbonate ion NO 2 - Nitrite ionSO 4 -2 Sulfate ion ClO 4 - Perchlorate ionSO 3 -2 Sulfite ion ClO 3 - Chlorate ion ClO 2 - Chlorite ion ClO - Hypochlorite ion BrO 4 - Perbromate ion BrO 3 - Bromate ion BrO 2 - Bromite ion BrO - Hypobromite ion IO 4 - Periodate ion IO3 - Iodate ion IO 2 - Iodite ion IO - Hypoiodite ion

II. Molecular Nomenclature zPrefix System (binary compounds) 1.Less e - neg atom comes first. 2.Add prefixes to indicate # of atoms. Omit mono- prefix on first element. 3.Change the ending of the second element to -ide.

PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER II. Molecular Nomenclature

zCCl 4 zN 2 O zSF 6 ycarbon tetrachloride ydinitrogen monoxide ysulfur hexafluoride II. Molecular Nomenclature

zarsenic trichloride zdinitrogen pentoxide ztetraphosphorus decoxide yAsCl 3 yN2O5yN2O5 yP 4 O 10 II. Molecular Nomenclature

NOF Cl Br I H II. Molecular Nomenclature zThe Seven Diatomic Elements Br 2 I 2 N 2 Cl 2 H 2 O 2 F 2

III. Ionic Nomenclature Ionic Formulas zWrite each ion, cation first. Don’t show charges in the final formula. zOverall charge must equal zero. yIf charges cancel, just write symbols. yIf not, use subscripts to balance charges. zUse parentheses to show more than one polyatomic ion. zStock System - Roman numerals indicate the ion’s charge.

III. Ionic Nomenclature Ionic Names zWrite the names of both ions, cation first. zChange ending of monatomic ions to -ide. zPolyatomic ions have special names. zStock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

III. Ionic Nomenclature zConsider the following: yDoes it contain a polyatomic ion? x-ide, 2 elements  no x-ate, -ite, 3+ elements  yes yDoes it contain a Roman numeral? xCheck the table for metals not in Groups 1 or 2. yNo prefixes!

Common Ion Charges NA III. Ionic Nomenclature

zpotassium chloride zmagnesium nitrate zcopper(II) chloride  K + Cl   Mg 2+ NO 3   Cu 2+ Cl   KCl  Mg(NO 3 ) 2  CuCl 2 III. Ionic Nomenclature

zNaBr zNa 2 CO 3 zFeCl 3 ysodium bromide ysodium carbonate yiron(III) chloride III. Ionic Nomenclature

IV. Acid Nomenclature zAcids – What are they? yCompounds that form H + in water. yFormulas usually begin with ‘H’. zExamples: yHCl (aq)– hydrochloric acid yHNO 3 (aq)– nitric acid yH 2 SO 4 (aq)– sulfuric acid

IV. Acid Nomenclature

zHBr zH 2 CO 3 zH 2 SO 3 y2 elements, -ide y3 elements, -ate y3 elements, -ite  hydrobromic acid  carbonic acid  sulfurous acid IV. Acid Nomenclature

zhydrofluoric acid zsulfuric acid znitrous acid y2 elements y3 elements, -ic y3 elements, -ous  HF (aq)  H 2 SO 4  HNO 2 IV. Acid Nomenclature  H + F-  H + SO 4 2-  H + NO 2 - (aq)