To practice naming and writing chemical formulas for many inorganic compounds, both ionic and molecular. In this exercise you will practice naming and writing chemical formulas for many inorganic compounds, both ionic and molecular. Before beginning the exercise you should carefully read all the sections of your text (or notes) on the names and formulas of ionic compounds, simple covalent compounds, and acids. The following is a brief summary of the Nomenclature rules for each of these types of compounds. Ionic Compounds Ionic compounds are composed of metal cations and non-metal anions, or, of polyatomic ions. Names and formulas always start with the positively charged cation. Ions are combined in ratios so that the final ionic compound is neutral. Never use prefixes in the names of ionic compounds. The cation name is simply combined with the anion name only. If the cation is capable of having more than one possible charge, the cation charge is included in the name as a Roman numeral in brackets (Stock system). Several ion names, charges and formulas are provided in the following tables. They must be memorized as soon as possible. Names of Selected Cations (names are in alphabetical order) 0 1 2 3 \(\ce{Al^{3+}}\) Aluminum \(\ce{Pb^{2+}}\) Lead(II); Plumbous \(\ce{NH4^{+}}\) Ammonium \(\ce{Pb^{4+}}\) Lead(IV); Plumbic \(\ce{As^{3+}}\) Arsenic(III) \(\ce{Li^{+}}\) Lithium \(\ce{Ba^{2+}}\) Barium \(\ce{Mg^{2+}}\) Magnesium \(\ce{Cd^{2+}}\) Cadmium \(\ce{Mn^{2+}}\) Manganese(II) \(\ce{Ca^{2+}}\) Calcium \(\ce{Mn^{4+}}\) Manganese(IV) \(\ce{Cr^{2+}}\) Chromium(II) \(\ce{Hg2^{2+}}\) Mercury(I); Mercurous \(\ce{Cr^{3+}}\) Chromium(III) \(\ce{Hg^{2+}}\) Mercury(II); Mercuric \(\ce{Cr^{6+}}\) Chromium(VI) \(\ce{Ni^{2+}}\) Nickel(II); Nickelous \(\ce{Co^{2+}}\) Cobalt(II); Cobaltous \(\ce{K^{+}}\) Potassium \(\ce{Co^{3+}}\) Cobalt(III); Cobaltic \(\ce{Ag^{+}}\) Silver \(\ce{Cu^{+}}\) Copper(I); Cuprous \(\ce{Na^{+}}\) Sodium \(\ce{Cu^{2+}}\) Copper(II); Cupric \(\ce{Rb^{+}}\) Rubidium \(\ce{Au^{3+}}\) Gold(III); Auric \(\ce{Sr^{2+}}\) Strontium \(\ce{H^{+}}\) Hydrogen \(\ce{Sn^{2+}}\) Tin(II); Stannous \(\ce{Fe^{2+}}\) Iron(II); Ferrous \(\ce{Sn^{4+}}\) Tin(IV); Stannic \(\ce{Fe^{3+}}\) Iron(III); Ferric \(\ce{Zn^{2+}}\) Zinc Names of Selected Anions (names are in alphabetical order, but with oxyanions grouped together) 0 1 2 3 \(\ce{C2H3O2^{-}}\) Acetate \(\ce{I^{-}}\) Iodide \(\ce{AsO4^{3-}}\) Arsenate \(\ce{IO4^{-}}\) Periodate \(\ce{BO3^{3-}}\) Borate \(\ce{MoO4^{2-}}\) Molybdate \(\ce{B4O7^{2-}}\) Tetraborate \(\ce{N^{3-}}\) Nitride \(\ce{Br^{-}}\) Bromide \(\ce{NO2^{-}}\) Nitrite \(\ce{BrO^{-}}\) Hypobromite \(\ce{NO3^{-}}\) Nitrate \(\ce{BrO3^{-}}\) Bromate \(\ce{C2O4^{2-}}\) Oxalate \(\ce{CO3^{2-}}\) Carbonate \(\ce{O^{2-}}\) Oxide \(\ce{HCO3^{-}}\) Bicarbonate; Hydrogen carbonate \(\ce{O2^{2-}}\) Peroxide \(\ce{Cl^{-}}\) Chloride \(\ce{MnO4^{-}}\) Permanganate \(\ce{ClO^{-}}\) Hypochlorite \(\ce{P^{3-}}\) Phosphide \(\ce{ClO2^{-}}\) Chlorite \(\ce{PO4^{3-}}\) Phosphate \(\ce{ClO3^{-}}\) Chlorate \(\ce{HPO4^{2-}}\) Hydrogen phosphate \(\ce{ClO4^{-}}\) Perchlorate \(\ce{H2PO4^{-}}\) Dihydrogen phosphate \(\ce{CrO4^{2-}}\) Chromate \(\ce{Se^{2-}}\) Selenide \(\ce{Cr2O7^{2-}}\) Dichromate \(\ce{S^{2-}}\) Sulfide \(\ce{C6H5O7^{3-}}\) Citrate \(\ce{SO3^{2-}}\) Sulfite \(\ce{CN^{-}}\) Cyanide \(\ce{SO4^{2-}}\) Sulfate \(\ce{F^{-}}\) Fluoride \(\ce{HSO3^{-}}\) Bisulfite; Hydrogen sulfite \(\ce{H^{-}}\) Hydride \(\ce{HSO4^{-}}\) Bisulfate; Hydrogen sulfate \(\ce{OH^{-}}\) Hydroxide \(\ce{S2O3^{2-}}\) Thiosulfate NaN NaN \(\ce{SCN^{-}}\) Thiocyanate Examples \(\ce{K2S}\) 2 \(\ce{K^{1+}}\) cations and 1 \(\ce{S^{2-}}\) anion potassium sulfide \(\ce{FeCl3}\) 1 \(\ce{Fe^{3+}}\) cation and 3 \(\ce{Cl^{1-}}\) anions iron(III) chloride, or ferric chloride \(\ce{Mg3(PO4)2}\) 3 \(\ce{Mg^{2+}}\) cations and 2 \(\ce{PO4^{3-}}\) anions magnesium phosphate Simple Covalent (Molecular) Compounds Simple covalent (molecular) compounds are composed of non-metal atoms only. The more metallic non-metal is written first. Prefixes are used in the name to indicate the number of each atom present. A list of prefixes 1-10 (and 12) is provided below, which must be memorized. The prefix “mono” is dropped if there is only one of the first element. The name of the second element always ends in "-ide." Prefixes for Covalent Compounds 0 1 1 Mono 2 Di 3 Tri 4 Tetra 5 Penta 6 Hexa 7 Hepta 8 Octa 9 Nona 10 Deca 12 Dodeca Examples \(\ce{P4S3}\) 4 \(\ce{P}\) atoms and 3 \(\ce{S}\) atoms tetraphosphorus trisulfide \(\ce{N2O}\) 2 \(\ce{N}\) atoms and 1 \(\ce{O}\) atom dinitrogen monoxide \(\ce{BrCl5}\) 1 \(\ce{Br}\) atom and 5 \(\ce{Cl}\) atoms bromine pentachloride Acids Acids are composed of hydrogen cations and non-metal anions or polyatomic anions. H always leads the formula. Acids are in the aqueous state. Ions are combined in ratios so that the final acid is neutral. The acid name depends on the name of the anion involved: \[ \ce{H^{1+}} + \text{Anion} \ce{->} \text{Acid}\] \[ \ce{H^{+}} + \text{___ide} \ce{->} \text{Hydro___ic Acid}\] \[ \ce{H^{+}} + \text{___ate} \ce{->} \text{___ic Acid}\] \[ \ce{H^{+}} + \text{___ite} \ce{->} \text{___ous Acid}\] Examples \(\ce{HBr}\) ( aq ) 1 \(\ce{H^{1+}}\) cation and 1 \(\ce{Br^{1-}}\) anion (bromide) hydrobromic acid \(\ce{HNO3}\) ( aq ) 1 \(\ce{H^{1+}}\) cation and 1 \(\ce{NO3^{1-}}\) anion (nitrate) nitric acid \(\ce{H2SO3}\) ( aq ) 2 \(\ce{H^{1+}}\) cations and 1 \(\ce{SO3^{2-}}\) anion (sulfite) sulfurous acid Hydrates Hydrates are solid substances that also contain water molecules in their crystal structure. The number of water molecules for each formula unit is fixed. The formula is written the same as any other compound, but then we add a dot (\(\ce{*}\)), (note that this is NOT a multiplication sign!) followed by the number of water molecules per ionic formula unit and the symbol \(\ce{H2O}\). The name is the same as for any other compound, but we add the word “hydrate” at the end with a Latin prefix to indicate the number of water molecules per ionic formula unit. Examples \(\ce{CuSO4*5H2O}\) 1 \(\ce{Cu^{2+}}\) ion, 1 \(\ce{SO4^{2-}}\) ion, and 5 water molecules Copper (II) sulfate pentahydrat sodium carbonate decahydrate \(\ce{Na^{+}}\) ion(s), \(\ce{CO3^{2-}}\) ions(s), and 10 water molecules \(\ce{Na2CO3*10H2O}\) Lab Report: Inorganic Nomenclature Part A: Naming Practice Name each of the compounds in the following table. Compounds marked with a star (*) should be named using both the Stock and the “ic/ous” naming systems. 0 1 2 1 *\(\ce{Au(NO3)3}\) NaN 2 \(\ce{Ca3(PO4)2}\) NaN 3 \(\ce{Cl2O}\) NaN 4 \(\ce{LiH}\) NaN 5 \(\ce{NaClO3}\) NaN 6 \(\ce{H2C2O4}\) (aq) NaN 7 \(\ce{AlCl3}\) NaN 8 \(\ce{Ni(CN)2}\) NaN 9 \(\ce{P4O10}\) NaN 10 *\(\ce{SnSO3}\) NaN 11 \(\ce{(NH4)2CO3}\) NaN 12 \(\ce{HF}\) (aq) NaN 13 \(\ce{CrO3}\) NaN 14 \(\ce{Ba(C2H3O2)2}\) NaN 15 \(\ce{ICl5}\) NaN 16 \(\ce{Fe(NH4)2(SO4)2*6H2O}\) NaN 17 *\(\ce{PbS2}\) NaN 18 \(\ce{HBrO}\) (aq) NaN 19 \(\ce{ZnCr2O7}\) NaN 20 \(\ce{Na2S2O3*5H2O}\) NaN Part B: Formula Practice Write the formulas for each of the compounds in the following table. 0 1 2 1 Ferric sulfate NaN 2 Strontium oxalate NaN 3 Chromic acid NaN 4 Nickel(III) carbonate NaN 5 Silver bromate NaN 6 Dinitrogen difluoride NaN 7 Magnesium molybdate NaN 8 Sodium hydrogen phosphate NaN 9 Hydrocyanic acid NaN 10 Cuprous nitrite NaN 11 Nickelous nitrate hexahydrate NaN 12 Manganese(II) periodate NaN 13 Sulfur trioxide NaN 14 Mercury(I) iodide NaN 15 Lithium thiosulfate NaN 16 Chlorous acid NaN 17 Plumbic bicarbonate NaN 18 Barium chloride dihydrate NaN 19 Aluminum chromate NaN 20 Rubidium peroxide NaN Part C: Formulas and Names If the name of the compound is given, write its formula. If the formula is given, write its name. You may use either the Stock system or “ic/ous” system for naming, where relevant. 0 1 2 1 \(\ce{Ca(ClO2)2}\) NaN 2 Stannic fluoride NaN 3 Silicon tetrabromide NaN 4 \(\ce{Cr(BrO)2}\) NaN 5 Potassium tetraborate tetrahydrate NaN 6 Gallium arsenate NaN 7 \(\ce{HNO2}\) (aq) NaN 8 \(\ce{LiH2PO4}\) NaN 9 Magnesium tetraborate NaN 10 \(\ce{Br3O8}\) NaN 11 \(\ce{MnO2}\) NaN 12 Silver thiocyanate NaN 13 Citric acid NaN 14 \(\ce{AlN}\) NaN 15 \(\ce{Cu(NO3)2*3H2O}\) NaN 16 Titanium(II) bisulfate NaN 17 Sulfur hexafluoride NaN 18 \(\ce{(NH4)3PO4}\) NaN 19 Cuprous hydroxide NaN 20 \(\ce{HClO4}\) (aq) NaN 21 Plumbous oxalate NaN 22 \(\ce{NO2}\) NaN 23 \(\ce{CdCO3}\) NaN 24 Bismuth(V) oxide NaN 25 Permanganic acid NaN 26 \(\ce{Ag2SO4}\) NaN 27 Strontium phosphide NaN 28 Tricarbon disulfide NaN 29 \(\ce{Au2O3}\) NaN 30 Sodium dichromate NaN 31 \(\ce{HI}\) (aq) NaN 32 \(\ce{NH4HSO3}\) NaN 33 Mercuric cyanide NaN 34 \(\ce{Cl2O7}\) NaN 35 Vanadium(III) nitrate NaN 36 Sulfurous acid NaN 37 \(\ce{KF}\) NaN 38 Zinc hypochlorite NaN 39 \(\ce{CO}\) NaN 40 Nickelous acetate NaN