Chemical Formula Writing & Nomenclature Binary Acids Naming Binary Acids

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Chemical Formula Writing & Nomenclature Binary Acids Naming Binary Acids

© Mr. D. Scott; CHS Chemical Formula Writing & Nomenclature Binary Acids Ternary Acids Basic Rules for acids All formulas begin with hydrogen, H Those hydrogens listed first are the ones capable of being ionized when in solution and/or reacted with bases. Hydrogens listed later in the formula are not capable of being ionized. Binary Acids These follow the format HxAy where A represents some non-metal element covalently bonded to hydrogen. Naming Binary Acids hydro- -ic acid add prefix root of non-metal name This naming approach assumes that the acid compound in aqueous (dissolved in water). When these compounds are pure, the naming rules follow those of the binary molecules that we will cover later. Until further notice, we will name these compounds as acids in aqueous solution. © Mr. D. Scott; CHS The oxidation state of the non-metal follows the same rule as it does when it is combining with a metal. It will be the first one listed and negative. Examples: +1 -3 H + P H + P H3P hydrophosphoric acid +1 -2 H + S H + S H2S hydrosulfuric acid +1 -2 H + Se H + Se H2Se hydroselenic acid H + F H+1 + F-1 HF hydrofluoric acid H + Cl H+1 + Cl-1 HCl hydrochloric acid H + Br H+1 + Br-1 HBr hydrobromic acid H + I H+1 + I-1 HI hydroiodic acid © Mr. D. Scott; CHS Ternary Acids These follow the format Hx(polyatomic ion)y An important consideration – All acids are molecules. While we are using our PAL to combine various polyatomic ions with hydrogen, these are NOT IONIC COMPOUNDS. The hydrogen is covalently bonding somewhere on the polyatomic ion and producing a molecular substance. Naming Ternary Acids -ate -ic -ite -ous acid root of polyatomic name The ending of the polyatomic name is changed when naming these acids as indicated above. The rest of the polyatomic name is not changed. Not every polyatomic ion will make an acid when combined with hydrogen. Your knowledge about these will be gained through experience. © Mr. D. Scott; CHS Examples: H + nitrate HNO3 nitric acid H + nitrite HNO2 nitrous acid H + hypochlorite HClO hypochlorous acid H + chlorite HClO2 chlorous acid H + chlorate HClO3 chloric acid H + perchlorate HClO4 perchloric acid H + acetate HC2H3O2 acetic acid H + carbonate H2CO3 carbonic acid H + oxalate H2C2O4 oxalic acid H + citrate H3C6H5O7 citric acid .

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Group 17 (Halogens)
Sodium, Na Gallium, Ga CHEMISTRY 1000 Topic #2: The Chemical Alphabet Fall 2020 Dr. Susan Findlay See Exercises 11.1 to 11.4 Forms of Carbon The Halogens (Group 17) What is a halogen? Any element in Group 17 (the only group containing Cl2 solids, liquids and gases at room temperature) Exists as diatomic molecules ( , , , ) Melting Boiling 2State2 2 2Density Point Point (at 20 °C) (at 20 °C) Fluorine -220 °C -188 °C Gas 0.0017 g/cm3 Chlorine -101 °C -34 °C Gas 0.0032 g/cm3 Br2 Bromine -7.25 °C 58.8 °C Liquid 3.123 g/cm3 Iodine 114 °C 185 °C Solid 4.93 g/cm3 A nonmetal I2 Volatile (evaporates easily) with corrosive fumes Does not occur in nature as a pure element. Electronegative; , and are strong acids; is one of the stronger weak acids 2 The Halogens (Group 17) What is a halogen? Only forms one monoatomic anion (-1) and no free cations Has seven valence electrons (valence electron configuration . ) and a large electron affinity 2 5 A good oxidizing agent (good at gaining electrons so that other elements can be oxidized) First Ionization Electron Affinity Standard Reduction Energy (kJ/mol) Potential (kJ/mol) (V = J/C) Fluorine 1681 328.0 +2.866 Chlorine 1251 349.0 +1.358 Bromine 1140 324.6 +1.065 Iodine 1008 295.2 +0.535 3 The Halogens (Group 17) Fluorine, chlorine and bromine are strong enough oxidizing agents that they can oxidize the oxygen in water! When fluorine is bubbled through water, hydrogen fluoride and oxygen gas are produced.
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United States Patent Office
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