NOMENCLATURE

Inorganic Nomenclature Using different oxidation states Potassium + oxygen K O K 2 O potassium oxide

Inorganics Using the same oxidation states Calcium + oxygen Ca O CaO calcium oxide

Inorganics Using polyatomic ions calcium + bromate Ca(BrO 3 ) 2

Sample Problems Beryllium iodide (beryllium + iodine) BeI 2 Calcium carbide (calcium + carbon) Ca 2 C

More Problems Aluminum sulfate Al 2 (SO 4 ) 3 Ammonium hydroxide NH 4 OH

Stock Formulas Iron (III) Chloride FeCl 3 Tin (II) Nitride Sn 3 N 2

Naming Compounds The nonmetal name in a BINARY COMPOUND (two compounds – a metal and nonmetal bonded ionically) has the nonmetal name end in “ide”. BaBr 2 barium bromide Mg 3 N 2 magnesium nitride K 2 S potassium sulfide

Naming using Stock formulas Fe(OH) 2 Iron (II) hydroxide CuSO 4 Copper (II) sulfate

Practice Problems  Writing Formulas: 1, 2, 4, 5, 10, 15, 25, 31, 34, 43, 53, 70 Naming Compounds: 154, 160, 163, 166, 172, 179, 181, 201, 228, 234, 242, 280

Now to the additions: An older system used in place of the Stock system uses suffixes on the metal to indicate a lower or higher oxidation state. * metals with lower oxidation state: “ous” ending * metals with higher oxidation state: “ic” ending Metals use Latin names

Examples: Iron (II) = ferrous Iron (III) = ferric Copper (1) = cuprous copper (II) = cupric Tin (II) = stannous tin (IV) = stannic Lead (II) = plumbous lead (IV) = plumbic Mercury (I) = mercurous Mercury (II) = mercuric Chromium (II) = chromous chromium (III) chromic Cobalt (II) = cobaltous cobalt (III) = cobaltic Manganese (II) = manganous manganese (III) = manganaic

Binary Covalent Compounds For binary compounds whose first element is a nonmetal (covalent bonding) use the following prefixes for the number of atoms. The first element will have its normal ending, the second will end in “ide” 1 = mono, 2 = di, 3 = tri, 4 = tetra, 5 = penta, 6 = hexa, 7 = hepta, 8 = octa, 9 = nona, 10 = deca, 11 = undeca, 12 = dodeca

Binary Covalent Examples: SO 2 sulfur dioxide Cl 2 O 7 dichlorine tetrachloride P 2 O 3 diphosphorus trioxide P 2 O 5 diphosphorus pentaoxide

Hydrogen Exceptions For compounds with hydrogen in the middle use either the “bi” prefix or the word “hydrogen” Examples: NaHSO 4 sodium bisulfate or sodium hydrogen sulfate Ca(HSO 4 ) 2 calcium bisulfate or calcium hydrogen sulfate

Another Problem For phosphate salts with more than 1 type ion, one of which is hydrogen, use the following format: NaH 2 PO 4 sodium dihydrogen phospate K 2 HPO 4 potassium monohydrogen phosphate

No Reduction Formulas Certain formulas are not reduced: The most common one is mercury (I) which is Hg 2 2+ Example: Mercury (I) nitrate = Hg 2 (NO 3 ) 2 Mercury (I) chloride = Hg 2 Cl 2

Peroxide Another example of no reduction is peroxide which is O 2 2- hydrogen peroxide = H 2 O 2 sodium peroxide = Na 2 O 2

Inorganic Acids Standard “ate” polyatomic ion acids with “ic” HBrO 3 Bromic acid HClO 3 Chloric acid HNO 3 Nitric acid H 3 PO 4 Phosphoric acid H 2 SO 4 Sulfuric acid H 2 CO 3 Carbonic acid

Removing all oxygens When all oxygens are removed, add a “hydro” prefix (along with “ic” ending) HBrO 3 Bromic acid HBrO Hydrobromic acid HNO 3 Nitric acid HNO Hydronitric acid

Adding an extra oxygen When an extra oxygen is added, add a “per” prefix, along with “ic” ending H 2 CO 3 carbonic acid H 2 CO 4 percarbonic acid HClO 3 chloric acid HClO 4 perchloric acid

Taking 1 oxygen away When 1 oxygen is taken away from the normal “ic” ending formula, change “ic” to “ous” H 2 SO 4 sulfuric acid H 2 SO 3 sulfurous acid H 3 PO 4 phosphoric acid H 3 PO 3 phosphorous acid

Taking 2 oxygens away When 2 oxygens are taken away from normal “ic” ending, change “ic” to “ous” and add a “hypo” prefix” HNO 3 Nitric acid HNO hyponitrous acid HClO 3 chloric acid HClO hypochlorous acid H 3 PO 2 hypophosphorous acid

Final Homework Problems 3, 6, 16, 22, 44, 50, 55, 67, 89, 96, 100, 113, 120, 127, 135, 147, , 165, 175, 187, 204, 210, 223, 236, 243, 291, 306, 333, 341, 324