2.4: CHEMICAL NOMENCLATURE
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2.4: CHEMICAL NOMENCLATURE 1. MOLECULAR COMPOUNDS Naming: • Put the appropriate prefix IN FRONT of the element name • Exception: Do not use mono- on the FIRST element • Change the ending of the second element to “ide” • Many also have common names Formulas: • Use the prefix to determine the subscript • DO NOT reduce. Prefixes 1 – mono 2 – di 3 – tri 4 – tetra 5 – penta 6 – hexa 7 – hepta 8 – octa 9 – nona 10 -- deca 1. MOLECULAR COMPOUNDS Common Names Common Name Ammonia Methane Water Ozone Formula 1. MOLECULAR COMPOUNDS Common Names Common Name Formula Ammonia NH3 Methane Water Ozone 1. MOLECULAR COMPOUNDS Common Names Common Name Formula Ammonia NH3 Methane CH4 Water Ozone 1. MOLECULAR COMPOUNDS Common Names Common Name Formula Ammonia NH3 Methane CH4 Water H2O Ozone 1. MOLECULAR COMPOUNDS Common Names Common Name Formula Ammonia NH3 Methane CH4 Water H2O Ozone O3 1. MOLECULAR COMPOUNDS Practice Trinitrogen hexasulfide Carbon dioxide Tetrafluorine octachloride NO P2Br9 SI3 1. MOLECULAR COMPOUNDS Practice Trinitrogen hexasulfide N3S6 Carbon dioxide Tetrafluorine octachloride NO P2Br9 SI3 1. MOLECULAR COMPOUNDS Practice Trinitrogen hexasulfide N3S6 Carbon dioxide CO2 Tetrafluorine octachloride NO P2Br9 SI3 1. MOLECULAR COMPOUNDS Practice Trinitrogen hexasulfide N3S6 Carbon dioxide CO2 Tetrafluorine octachloride F4Cl8 NO P2Br9 SI3 1. MOLECULAR COMPOUNDS Practice Trinitrogen hexasulfide N3S6 Carbon dioxide CO2 Tetrafluorine octachloride F4Cl8 Nitrogen monoxide NO P2Br9 SI3 1. MOLECULAR COMPOUNDS Practice Trinitrogen hexasulfide N3S6 Carbon dioxide CO2 Tetrafluorine octachloride F4Cl8 Nitrogen monoxide NO Diphosphorus nonabromide P2Br9 SI3 1. MOLECULAR COMPOUNDS Practice Trinitrogen hexasulfide N3S6 Carbon dioxide CO2 Tetrafluorine octachloride F4Cl8 Nitrogen monoxide NO Diphosphorus nonabromide P2Br9 Sulfur triiodide SI3 2. IONIC COMPOUNDS a) Simple Binary Compounds (2 different elements – metal and non-metal) Naming: • Write the metal first, then the non-metal • Change the ending of the non metal to –ide Formulas: • Write the symbol for each element in the correct order (metal first) • Write the ionic charge above each symbol • Note: Zn2+ and Ag+ • Criss-cross the numbers from the charges to the opposite element • Simplify (reduce) if necessary 2. IONIC COMPOUNDS Practice Beryllium fluoride Calcium sulfide Aluminum oxide CaCl2 MgO KP3 2. IONIC COMPOUNDS Practice Beryllium fluoride BeF2 Calcium sulfide Aluminum oxide CaCl2 MgO KP3 2. IONIC COMPOUNDS Practice Beryllium fluoride BeF2 Calcium sulfide CaS Aluminum oxide CaCl2 MgO KP3 2. IONIC COMPOUNDS Practice Beryllium fluoride BeF2 Calcium sulfide CaS Aluminum oxide Al2O3 CaCl2 MgO KP3 2. IONIC COMPOUNDS Practice Beryllium fluoride BeF2 Calcium sulfide CaS Aluminum oxide Al2O3 Calcium chloride CaCl2 MgO KP3 2. IONIC COMPOUNDS Practice Beryllium fluoride BeF2 Calcium sulfide CaS Aluminum oxide Al2O3 Calcium chloride CaCl2 Magnesium oxide MgO K3P 2. IONIC COMPOUNDS Practice Beryllium fluoride BeF2 Calcium sulfide CaS Aluminum oxide Al2O3 Calcium chloride CaCl2 Magnesium oxide MgO Potassium phosphide K3P 2. IONIC COMPOUNDS b) Multivalent Binary Compounds (the metal has more than one ionic charge) Naming • Two methods to name these: a) Stock method – uses roman numerals • Write the roman number that corresponds with the correct charge AFTER the metal name (I, II, III, IV, V) Multivalent metals Charges b) Classical method – the “ous-ic” system • uses latin names of elements Copper Cu+ Cu2+ • “ous” = lowest valence Tin Sn2+ Sn4+ • “ic” = highest valence Iron Fe2+ Fe3+ Nickel Ni2+ Ni3+ Formulas Manganese Mn2+ Mn4+ • Use the criss-cross method and reduce Gold Au+ Au3+ Lead Pb2+ Pb4+ Mercury Hg+ Hg2+ 2. IONIC COMPOUNDS b) Multivalent Binary Compounds (the metal has more than one ionic charge) Latin Name Cuprum (Cu) Ferrum (Fe) Stannum (Sn) Plumbum (Pb) Remove “um” ending Lower Valence Lower Valence Name (ous) Higher Valence Higher valence Name (ic) 2. IONIC COMPOUNDS b) Multivalent Binary Compounds (the metal has more than one ionic charge) Latin Name Remove “um” ending Lower Valence Lower Valence Name (ous) Higher Valence Higher valence Name (ic) Cuprum (Cu) Cupr 1+ Cuprous 2+ Cupric Ferrum (Fe) Stannum (Sn) Plumbum (Pb) 2. IONIC COMPOUNDS b) Multivalent Binary Compounds (the metal has more than one ionic charge) Latin Name Remove “um” ending Lower Valence Lower Valence Name (ous) Higher Valence Higher valence Name (ic) Cuprum (Cu) Cupr 1+ Cuprous 2+ Cupric Ferrum (Fe) Ferr 2+ Ferrous 3+ Ferric Stannum (Sn) Plumbum (Pb) 2. IONIC COMPOUNDS b) Multivalent Binary Compounds (the metal has more than one ionic charge) Latin Name Remove “um” ending Lower Valence Lower Valence Name (ous) Higher Valence Higher valence Name (ic) Cuprum (Cu) Cupr 1+ Cuprous 2+ Cupric Ferrum (Fe) Ferr 2+ Ferrous 3+ Ferric Stannum (Sn) Stann 2+ Stannous 4+ Stannic Plumbum (Pb) plumb 2+ plumbous 4+ Plumbic 2. IONIC COMPOUNDS Practice Copper (II) fluoride Tin (IV) sulfide Mercury (I) oxide Stannic phosphide Ferrous oxide SnCl2 FeO PbS2 2. IONIC COMPOUNDS Practice Copper (II) fluoride Cupric fluoride CuF2 Tin (IV) sulfide Mercury (I) oxide Stannic phosphide Ferrous oxide SnCl2 FeO PbS2 2. IONIC COMPOUNDS Practice Copper (II) fluoride Cupric fluoride CuF2 Tin (IV) sulfide Stannic sulfide SnS2 Mercury (I) oxide Stannic phosphide Ferrous oxide SnCl2 FeO PbS2 2. IONIC COMPOUNDS Practice Copper (II) fluoride Cupric fluoride CuF2 Tin (IV) sulfide Stannic sulfide SnS2 Mercury (I) oxide ----- Hg2O Tin (IV) phosphide Stannic phosphide Sn3P4 Iron (II) oxide Ferrous oxide FeO Tin (II) chloride Stannous chloride SnCl2 Iron (III) sulfide Ferric sulfide Fe2S3 Lead (IV) sulfide Plumbic sulfide PbS2 2. IONIC COMPOUNDS c) Polyatomic Compounds • Polyatomic ions: ions that contain more than one type of atom • Can be + or – charged • Will combine with an oppositely charged ion to make a compound • See chart for polyatomic ions Naming • Do not change endings of polyatomic ions. Otherwise, same ionic naming rules apply Formulas • Use criss-cross method • DO NOT alter the subscripts of the polyatomic ion • Put the polyatomic in brackets, criss-cross the number to the OUTSIDE of these brackets • Simplify if necessary 2. IONIC COMPOUNDS Practice Copper (II) chlorate Zinc sulfate Magnesium hydroxide NaCN Fe(NO3)3 NH4OH 2. IONIC COMPOUNDS Practice Copper (II) chlorate Cu(ClO3)2 Zinc sulfate Magnesium hydroxide NaCN Fe(NO3)3 NH4OH 2. IONIC COMPOUNDS Practice Copper (II) chlorate Cu(ClO3)2 Zinc sulfate ZnSO4 Magnesium hydroxide NaCN Fe(NO3)3 NH4OH 2. IONIC COMPOUNDS Practice Copper (II) chlorate Cu(ClO3)2 Zinc sulfate ZnSO4 Magnesium hydroxide Mg(OH)2 NaCN Fe(NO3)3 NH4OH 2. IONIC COMPOUNDS Practice Copper (II) chlorate Cu(ClO3)2 Zinc sulfate ZnSO4 Magnesium hydroxide Mg(OH)2 Sodium cyanide NaCN Fe(NO3)3 NH4OH 2. IONIC COMPOUNDS Practice Copper (II) chlorate Cu(ClO3)2 Zinc sulfate ZnSO4 Magnesium hydroxide Mg(OH)2 Sodium cyanide NaCN Iron (III) nitrate Fe(NO3)3 NH4OH 2. IONIC COMPOUNDS Practice Copper (II) chlorate Cu(ClO3)2 Zinc sulfate ZnSO4 Magnesium hydroxide Mg(OH)2 Sodium cyanide NaCN Iron (III) nitrate Fe(NO3)3 Ammonium hydroxide NH4OH 2. IONIC COMPOUNDS d) Derivatives of Polyatomic Ions • Other polyatomic ions may have different amounts of oxygen atoms Naming • Name the original ion • Add prefix “per-” if there is 1 MORE oxygen • Change suffix to “-ite” if there is 1 LESS oxygen • Add prefix “hypo-” and change suffix to “-ite” if there are 2 LESS oxygen Formulas • Add or subtract the appropriate number of oxygen from the original ion • Overall charge of ion does NOT change 2. IONIC COMPOUNDS Example Chlorate ClO3- 2. IONIC COMPOUNDS Example perchlorate ClO4- Chlorate ClO3- 2. IONIC COMPOUNDS Example perchlorate ClO4- Chlorate ClO3- chlorite ClO2- 2. IONIC COMPOUNDS Example perchlorate ClO4- Chlorate ClO3- chlorite ClO2- hypochlorite ClO- 2. IONIC COMPOUNDS Practice (ions only) Iodite Hypophosphite persulfite BrO2Practice (compounds) Iron (II) hyposulfite Lithium chlorite NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite persulfite BrO2Practice (compounds) Iron (II) hyposulfite Lithium chlorite NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite PO23- persulfate BrO2Practice (compounds) Iron (II) hyposulfite Lithium chlorite NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite PO23- persulfate SO52BrO2- Practice (compounds) Iron (II) hyposulfite Lithium chlorite NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite PO23- persulfate SO52- Bromite BrO2- Practice (compounds) Iron (II) hyposulfite Lithium chlorite NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite PO23- persulfate SO52- Bromite BrO2- Practice (compounds) Iron (II) hyposulfite FeSO2 Lithium chlorite NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite PO23- persulfate SO52- Bromite BrO2- Practice (compounds) Iron (II) hyposulfite FeSO2 Lithium chlorite LiClO2 NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite PO23- persulfate SO52- Bromite BrO2- Practice (compounds) Iron (II) hyposulfite FeSO2 Lithium chlorite LiClO2 Sodium hypoiodite NaIO K3PO5 2. IONIC COMPOUNDS Practice (ions only) Iodite IO2- Hypophosphite PO23- persulfate SO52- Bromite BrO2- Practice (compounds) Iron (II) hyposulfite FeSO2 Lithium chlorite LiClO2 Sodium hypoiodite NaIO Potassium perphosphate K3PO5 3. ACIDS a) Binary Acids • An acid which is made by dissolving certain gases in water • Acids always start with a hydrogen that acts like a metal • A binary acid is formed from a binary compound • The subscript (aq) is used to denote the acid • (aq) = aqueous = dissolved in water Naming • Has the same formula as the gas, but a different name (hydro_______ic acid) Formulas • Use “criss-cross” – H+ is the cation (H acts like a metal) 3. ACIDS a) Binary Acids Name of Gas Formula Name of Acid Formula Hydrogen chloride HCl (g) Hydrochloric acid HCl (aq) HBr (g) Hydroiodic acid Hydrogen fluoride H2S (aq) 3. ACIDS a) Binary Acids Name of Gas Formula Name of Acid Formula Hydrogen chloride HCl (g) Hydrochloric acid HCl (aq) Hydrogen bromide HBr (g) Hydrobromic acid HBr (aq) Hydroiodic acid Hydrogen fluoride H2S (aq) 3. ACIDS a) Binary Acids Name of Gas Formula Name of Acid Formula Hydrogen chloride HCl (g) Hydrochloric acid HCl (aq) Hydrogen bromide HBr (g) Hydrobromic acid HBr (aq) Hydrogen iodide HI (g) Hydroiodic acid HI (aq) Hydrogen fluoride HF (g) Hydrofluoric acid HF (aq) Hydrogen sulfide H2S (g) Hydrosulfuric acid H2S (aq) 3. ACIDS b) Oxyacids • Contain oxygen, hydrogen, plus another element Naming • Remove “-ate” and add “-ic acid” Formulas • Combine hydrogen with the corresponding polyatomic ion 3. ACIDS b) Oxyacids Original Polyatomic Ion Acid Name Nitrate Nitric Acid Chlorate Chloric Acid Sulfate Sulfuric Acid Carbonate Carbonic Acid Phosphate Phosphoric Acid Acetate Acetic acid Chromate Chromic Acid Dichromate Dichromic Acid Acid Formula 3. ACIDS b) Oxyacids Original Polyatomic Ion Acid Name Acid Formula Nitrate Nitric Acid HNO3 Chlorate Chloric Acid Sulfate Sulfuric Acid Carbonate Carbonic Acid Phosphate Phosphoric Acid Acetate Acetic acid Chromate Chromic Acid Dichromate Dichromic Acid 3. ACIDS b) Oxyacids Original Polyatomic Ion Acid Name Acid Formula Nitrate Nitric Acid HNO3 Chlorate Chloric Acid HClO3 Sulfate Sulfuric Acid Carbonate Carbonic Acid Phosphate Phosphoric Acid Acetate Acetic acid Chromate Chromic Acid Dichromate Dichromic Acid 3. ACIDS b) Oxyacids Original Polyatomic Ion Acid Name Acid Formula Nitrate Nitric Acid HNO3 Chlorate Chloric Acid HClO3 Sulfate Sulfuric Acid H2SO4 Carbonate Carbonic Acid H2CO3 Phosphate Phosphoric Acid H3PO4 Acetate Acetic acid CH3COOH Chromate Chromic Acid H2CrO4 Dichromate Dichromic Acid H2Cr2O7 3. ACIDS c) Derivatives of Oxyacids • Many of the oxyacids have various forms, or derivatives Naming • Similar to derivatives of polyatomic ions and “ous/ic” system • • • • Start with original acid ( - ic acid) Add prefix “per-” if there is 1 MORE oxygen Change suffix “-ic” to “-ous” if there is 1 LESS oxygen Add prefix “hypo-” and change suffix “ic” to “-ous” if there are 2 LESS oxygen Formulas • Use prefixes and suffixes to determine the correct number of oxygen atoms 3. ACIDS Practice Chloric Acid HClO3 Nitrous Acid Percarbonic Acid H3PO2 H2CO 3. ACIDS Practice Perchloric acid HClO4 Chloric Acid HClO3 Nitrous Acid Percarbonic Acid H3PO2 H2CO 3. ACIDS Practice Perchloric acid HClO4 Chloric Acid HClO3 Chlorous acid HClO2 Nitrous Acid Percarbonic Acid H3PO2 H2CO 3. ACIDS Practice Perchloric acid HClO4 Chloric Acid HClO3 Chlorous acid HClO2 Hypochlorous acid HClO Nitrous Acid Percarbonic Acid H3PO2 H2CO 3. ACIDS Practice Perchloric acid HClO4 Chloric Acid HClO3 Chlorous acid HClO2 Hypochlorous acid HClO Nitrous Acid HNO2 Percarbonic Acid H3PO2 H2CO 3. ACIDS Practice Perchloric acid HClO4 Chloric Acid HClO3 Chlorous acid HClO2 Hypochlorous acid HClO Nitrous Acid HNO2 Percarbonic Acid H2CO4 H3PO2 H2CO 3. ACIDS Practice Perchloric acid HClO4 Chloric Acid HClO3 Chlorous acid HClO2 Hypochlorous acid HClO Nitrous Acid HNO2 Percarbonic Acid H2CO4 Hypophosphorous acid H3PO2 H2CO 3. ACIDS Practice Perchloric acid HClO4 Chloric Acid HClO3 Chlorous acid HClO2 Hypochlorous acid HClO Nitrous Acid HNO2 Percarbonic Acid H2CO4 Hypophosphorous acid H3PO2 Hypocarbonous acid H2CO 3. ACIDS d) Acid Salts • Formed when only some of the hydrogen atoms in an acid are replaced by a metal Naming • If 1 hydrogen replaced – use hydrogen or bi • If more than 1 hydrogen replaced – use a prefix to indicate the number of hydrogen atoms that are present Formulas • Will see hydrogen in the middle of the name – this is a part of a polyatomic ion (see chart) • Use criss-cross 3. ACIDS Practice Sodium hydrogen carbonate (OR sodium bicarbonate) Calcium dihydrogen phosphate Potassium biphosphate LiHSO3 Ba(HSO4)2 3. ACIDS Practice Sodium hydrogen carbonate (OR sodium bicarbonate) NaHCO3 Calcium dihydrogen phosphate Potassium biphosphate LiHSO3 Ba(HSO4)2 3. ACIDS Practice Sodium hydrogen carbonate (OR sodium bicarbonate) NaHCO3 Calcium dihydrogen phosphate Ca(H2PO4)2 Potassium biphosphate LiHSO3 Ba(HSO4)2 3. ACIDS Practice Sodium hydrogen carbonate (OR sodium bicarbonate) NaHCO3 Calcium dihydrogen phosphate Ca(H2PO4)2 Potassium biphosphate K2HPO4 LiHSO3 Ba(HSO4)2 3. ACIDS Practice Sodium hydrogen carbonate (OR sodium bicarbonate) NaHCO3 Calcium dihydrogen phosphate Ca(H2PO4)2 Potassium biphosphate K2HPO4 Lithium hydrogen sulfite (OR lithium bisulfite) LiHSO3 Ba(HSO4)2 3. ACIDS Practice Sodium hydrogen carbonate (OR sodium bicarbonate) NaHCO3 Calcium dihydrogen phosphate Ca(H2PO4)2 Potassium biphosphate K2HPO4 Lithium hydrogen sulfite (OR lithium bisulfite) LiHSO3 Barium hydrogen sulfate (OR barium bisulfate) Ba(HSO4)2 4. HYDRATES • Not all substances are “dry” – many have traces of water in them • Even if we try to evaporate certain substances, some of the water remains Naming • Name the compound normally, followed by _______hydrate (use the appropriate prefix for the number of water molecules) Formulas • Write the formula for the compound first, followed by a dot and the number of water molecules present 4. HYDRATES Practice Copper (II) sulfate pentahydrate Barium hydroxide octahydrate CoCl2 6 H2O Na3PO3 2 H2O 4. HYDRATES Practice Copper (II) sulfate pentahydrate CuSO4 5 H2O Barium hydroxide octahydrate CoCl2 6 H2O Na3PO3 2 H2O 4. HYDRATES Practice Copper (II) sulfate pentahydrate CuSO4 5 H2O Barium hydroxide octahydrate Ba(OH)2 8 H2O CoCl2 6 H2O Na3PO3 2 H2O 4. HYDRATES Practice Copper (II) sulfate pentahydrate CuSO4 5 H2O Barium hydroxide octahydrate Ba(OH)2 8 H2O Cobalt (II) chloride hexahydrate CoCl2 6 H2O Na3PO3 2 H2O 4. HYDRATES Practice Copper (II) sulfate pentahydrate CuSO4 5 H2O Barium hydroxide octahydrate Ba(OH)2 8 H2O Cobalt (II) chloride hexahydrate CoCl2 6 H2O Sodium phosphite dihydrate Na3PO3 2 H2O
