(Two Elements) 1. Metals (One Oxidation State) +

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N-1 NOMENCLATURE OF SIMPLE INORGANIC COMPOUNDS A. Binary Ionic Compounds (two elements) 1. Metals (one oxidation state) + Non-metal Metal element name + non-metal element “stem” + “ide” Examples: LiBr Lithium Bromide CaO Calcium Oxide Al2O3 Aluminum Oxide Mg3N2 Magnesium Nitride Common Monatomic Cations and Anions Cation Name Anion Name H+ hydrogen H– hydride Li+ lithium F– fluoride Na+ sodium Cl– chloride K+ potassium Br– bromide Cs+ cesium I– iodide Be2+ berillium O2– oxide Mg2+ magnesium S2– sulfide Ca2+ calcium N3– nitride Ba2+ barium P3– phosphide Al3+ aluminum Ag+ silver Zn2+ zinc 2. Metals ( > one oxidation state) + Non-metal Roman numeral → oxidation state Examples: FeCl2 Iron (II) Chloride FeCl3 Iron (III) Chloride CuBr Copper (I) Bromide CuBr2 Copper (II) Bromide SnO Tin (II) Oxide SnO2 Tin (IV) Oxide TiCl2 Titanium (II) Chloride TiCl3 Titanium (III) Chloride TiCl4 Titanium (IV) Chloride N-2 NOMENCLATURE OF SIMPLE INORGANIC COMPOUNDS 3. Stems for Non-metals III IV V VI VII B - bor C - carb N - nitr O - ox F - fluor Si - silic P - phosph S - sulf Cl - chlor As - arsen Se - selen Br - brom Sb - antimon Te - tellur I - iod N-3 4. Binary Compounds Containing Two Non-Metals (E1 and E2) No. of + +No. of + + Name E1 "Stem" of E2 -ide E1 E2 Examples: HBr Hydrogen Bromide BeCl2 Berylium (di) chloride H2S (di) Hydrogen Sulfide BN Boron Nitride H2O di hydrogen oxide → water NH3 Nitrogen tri hydride → ammonia PH3 Phosphorous tri hydride → phosphine CO Carbon Monoxide CO2 Carbon Dioxide SO2 Sulfur Dioxide OF2 Oxygen di fluoride AsCl3 Arsenic tri chloride P4O6 Tetra Phosphorous Hex Oxide N2O Di Nitrogen Oxide NO Nitrogen Oxide N2O3 Di Nitrogen Tri Oxide NO2 Nitrogen Di Oxide (Place more metallic element first) N-4 Binary Acids: Compound (g) Name (g) Aqueous Solution HF (g) Hydrogen Fluoride Hydrofluoric Acid HCl (g) Hydrogen Chloride Hydrochloric Acid + + H + H2O → H3O Hydro + “stem” + ic Acid Ternary Acids – “Common oxidation state” – “ic” 13 14 15 16 17 III IV V VI VII +1 -2 H3BO3 H2CO3 HNO3 boric acid carbonic acid nitric acid H2SIO4 H3PO4 H2SO4 HClO3 IN ACIDS silicic acid phosphoric acid sulfuric acid chloric acid Ox No H = +1 “ “ O = -2 H3AsO4 H2SeO4 HBrO3 arsenic acid selenic acid bromic acid H3 B O3 3(+1) + x +3(-2)=0 H6TeO6 HIO3 x = +3 telluric acid iodic acid N-5 B. Ternary Compounds (three elements) 1. Ternary Acids a. Oxyacids (two ox. states) “Stem” + ic → Higher ox. state “Stem” + ous → Lower ox. state HNO2 – Nitrous Acid H2SO3 – Sulfurous Acid HNO3 – Nitric Acid H2SO4 – Sulfuric Acid b. Oxyacids – more than two ox. states. Use prefixes (hypo-, per-) and suffixes (-ous, -ic). Acid Name Ox. State HClO Hypochlorous Acid H=+1, Cl=+1, O=-2 HClO2 Chlorous Acid H=+1, Cl=+2, O=-2 Common ⇒ HClO3 Chloric Acid H=+1, Cl=+5, O=-2 HClO4 Perchloric Acid H=+1, Cl=+7, O=-2 Sodium Salt (-ite, -ate) NaClO Sodium hypochlorite NaClO2 Sodium chlorite NaClO3 Sodium chlorate NaClO3 Sodium perchlorate .

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Preparation of Telluric Acid from Tellurium Dioxide by Oxidation with Potassium Permanganate Frank C. Mathers, Charles M. Rice, Howard Broderick, and Robert Forney, Indiana University General Statement Tellurium dioxide, Te0 2 , although periodically similar to sulfur dioxide, cannot be oxidized by nitric acid to the valence of six, i.e., to telluric acid, H 2 Te04.2H 2 0. Among the many stronger oxidizing agents that will produce this oxidation, potassium permanganate in a nitric acid solution is quite satisfactory. This paper gives directions and data for the preparation of telluric acid by this reaction. The making of telluric acid is a desirable laboratory experiment because (1) tellurim dioxide is available in large quantities and is easily obtained, (2) the telluric acid is a stable compound, easily purified, easily crystallized, and non-corrosive, and (3) students are interested in experimenting with the rarer elements. The small soluibility of telluric acid and the high solubility of both manganese and potassium nitrates in nitric acidi gives a sufficient differ- ence in properties for successful purification by crystallization of the telluric acid. Methods of Analyses Tellurium dioxide can be volumetrically 2 titrated in a sulfuric acid solution by an excess of standard potassium permanganate, followed by enough standard oxalic acid to decolorize the excess of permanganate. The excess of oxalic acid must then be titrated by more of the perman- ganate. The telluric acid can be titrated, like any ordinary monobasic acid, 3 (1911). with standard sodium hydroxide using phenolphthalein as an indicator, if an equal volume of glycerine is added. If any nitric acid is present, it must be neutralized first with sodium hydroxide, using methyl orange as indicator.
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