Naming inorganic compounds Chemical nomenclature 命名法 1. Naming ionic compounds 2. Naming acids 3. Naming binary 二元的 molecular compounds 4. Naming hydrates

particular substance particular substance chemical formula and name chemical formula and name essential vocabulary essential vocabulary

individual, traditional names individual, traditional names systematic 系统的 method systematic 系统的 method chemical nomenclature 化学物质命名法 chemical nomenclature 化学物质命名法 systematic name systematic name

the division of substance the division of substance two categories 种类 : organic compounds two categories 种类 : organic compounds inorganic compounds inorganic compounds Inorganic compounds: Inorganic compounds: ionic compounds ionic compounds acids acids binary molecular compounds binary molecular compounds hydrates hydrates

Naming ionic compounds Ionic compounds usually consist of chemical combinations of metals and nonmetals. Ionic compounds usually consist of chemical combinations of metals and nonmetals. The metals form the positive ions, and the nonmetals form the negative ions. The metals form the positive ions, and the nonmetals form the negative ions. 1. Positive ions(Cations) 2. Negative ions(Anions) 3. Ionic compounds

Positive ⑴ When cations are formed from metal atoms, cations have the same name as the metals. ⑴ When cations are formed from metal atoms, cations have the same name as the metals. ⑵ When a metal can form cations of differing charges, cations have the name of metal followed by the positive charge which is given by a Roman numeral in parentheses 圆括号. ⑵ When a metal can form cations of differing charges, cations have the name of metal followed by the positive charge which is given by a Roman numeral in parentheses 圆括号. ⑶ When cations are formed from nonmetal atom, cations have names that end in –ium. ⑶ When cations are formed from nonmetal atom, cations have names that end in –ium.

Names of some common cations (1) Charge 1+ Charge 1+ H + Hydrogen ion Li + Lithium ion Na + Sodium ion K + Potassium ion Cs + Cesium ion Ag + Silver ion NH 4 + Ammonium ion Cu + Copper( Ⅰ ) ion or Cuprous ion Charge 2+ Charge 2+ Mg 2+ Magnesium ion Ca 2+ Calcium ion Sr 2+ Strontium ion Ba 2+ Barium ion Zn 2+ Zinc ion Cd 2+ Cadmium ion

Names of some common cations(2) Co 2+ Cobalt( Ⅱ ) ion or Cobaltous ion Co 2+ Cobalt( Ⅱ ) ion or Cobaltous ion Cu 2+ Copper( Ⅱ ) ion or Cupric ion Cu 2+ Copper( Ⅱ ) ion or Cupric ion Fe 2+ Iron( Ⅱ ) ion or Ferrous ion Fe 2+ Iron( Ⅱ ) ion or Ferrous ion Mn 2+ Manganese( Ⅱ ) ion or Manganous ion Mn 2+ Manganese( Ⅱ ) ion or Manganous ion Hg 2 2+ Mercury( Ⅰ ) ion or Mercurous ion Hg 2 2+ Mercury( Ⅰ ) ion or Mercurous ion Hg 2+ Mercury( Ⅱ ) ion or Mercuric ion Hg 2+ Mercury( Ⅱ ) ion or Mercuric ion Ni 2+ Nickel( Ⅱ ) ion or Nickelous ion Ni 2+ Nickel( Ⅱ ) ion or Nickelous ion Pb 2+ Lead( Ⅱ ) ion or Plumbous ion Pb 2+ Lead( Ⅱ ) ion or Plumbous ion Sn 2+ Tin( Ⅱ ) ion or Stannous ion Sn 2+ Tin( Ⅱ ) ion or Stannous ion

Names of some common cations(3) Charge 3+ Charge 3+ Al 3+ Aluminum ion Al 3+ Aluminum ion Cr 3+ Chromium( Ⅲ ) ion or Chromic ion Cr 3+ Chromium( Ⅲ ) ion or Chromic ion Fe 3+ Iron( Ⅲ ) ion or ferric ion Fe 3+ Iron( Ⅲ ) ion or ferric ion

Negative ions (Anions) ⑴ Monatomic anions have names formed by dropping the ending of the name of the element and adding the A few simple polyatomic anions also have names ending in A few simple polyatomic anions also have names ending (2) Polyatomic anions containing oxygen have names ending in –ate or –ite, or have prefix of pre- or hypo-. Oxyanion （含氧阴离子 Oxyanion (3) when the anion is an oxyanion with H +, the anion is named by adding a prefix as hydrogen

Common anions(1) H - H - Hydride ion Hydride ion F - F - Fluoride ion Fluoride ion Cl - Cl - Chloride ion Chloride ion Br - Br - Bromide ion Bromide ion I - I - Iodide ion Iodide ion S - S - Sulfide ion Sulfide ion OH - Hydroxide ion N 3- Nitride ion C 4- Carbide ion P 3- Phosphide ion O 2- Oxide ion O 2 2- Peroxide ion

Common anions(2) CN - CN - Cyanide ion Cyanide ion SCN - SCN - Thiocyanate ion Thiocyanate ion CH 3 COO - CH 3 COO - Acetate ion Acetate ion C 2 O 4 2- C 2 O 4 2- Oxalate ion Oxalate ion CrO 4 2- CrO 4 2- Chromate ion Chromate ion Cr 2 O 7 2- Cr 2 O 7 2- Dichromate ion Dichromate ion SO 4 2- Sulfate ion SO 3 2- Sulfite ion S 2 O 3 2- Thiosulphate ion PO 4 3- Phosphate ion PO 3 3- phosphite ion PO 2 3- hypophosphite ion

Common anions(3) HPO 4 2- HPO 4 2- hydrogen phosphate ion hydrogen phosphate ion H 2 PO 4 - H 2 PO 4 - dihydrogen phosphate ion dihydrogen phosphate ion CO 3 2- CO 3 2- carbonate ion carbonate ion HCO 3 2- HCO 3 2- hydrogen carbonate ion hydrogen carbonate ion NO 3 - NO 3 - Nitrate ion Nitrate ion NO 2 - NO 2 - Nitrite ion Nitrite ion ClO 4 - perchlorate ion ClO 3 - chlorate ion ClO 2 - chlorite ion ClO - hypochlorite ion MnO 4 - permanganate ion MnO 3 - manganate ion

Exercise 1 Write down symbols, including charge, for each of the following ions. Write down symbols, including charge, for each of the following ions. 1. Ammonium ion 2. Bisulfate ion 3. Bisulfite ion 4. Permanganate ion 5. Hydroxide ion 6. Dichromate ion 7. Hypochlorite ion 8. Perchlorate ion

Exercise 2 Write symbols, including charge, for each of the following ions. Write symbols, including charge, for each of the following ions. 1. Bicarbonate ion 2. Carbonate ion 3. Thiosulfate ion 4. Chromate ion 5. Acetate ion 6. Phosphate ion 7. Phosphite ion 8. Phosphide ion

Exercise 3 Write names for each of the following ions. Write names for each of the following ions. 1. ClO 3 – 2. ClO 4 – 3. CO SCN - 5. SO 4 2-

Exercise 4 Write names for each of the following ions. Write names for each of the following ions. 1. Br - 2. N O P OH -

Ionic compounds Names of ionic compounds are the cation name followed by the anion name. Names of ionic compounds are the cation name followed by the anion name. For example, For example, BaBr 2 Barium bromide BaBr 2 Barium bromide Al(NO 3 ) 3 Aluminum nitrate Al(NO 3 ) 3 Aluminum nitrate Cu(ClO 4 ) 2 Copper( Ⅱ ) perchlorate Cu(ClO 4 ) 2 Copper( Ⅱ ) perchlorate or cupric perchlorate or cupric perchlorate

Exercise 1 Name the following compounds: Name the following compounds: K 2 SO 4, Ba(OH) 2, FeCl 3. K 2 SO 4, Ba(OH) 2, FeCl 3.Solution Potassium sulfate Potassium sulfate Barium hydroxide Barium hydroxide Iron( Ⅲ ) chloride Iron( Ⅲ ) chloride

Exercise2 Give the chemical formula for Give the chemical formula for ( a ) magnesium sulfate ( a ) magnesium sulfate ( b ) silver sulfate ( b ) silver sulfate ( c ) lead( Ⅱ ) nitrate ( c ) lead( Ⅱ ) nitrateSolution ( a ) MgSO 4 ( a ) MgSO 4 ( b ) Ag 2 SO 4 ( b ) Ag 2 SO 4 ( c ) Pb(NO 3 ) 2 ( c ) Pb(NO 3 ) 2

Exercise 3 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. Barium hydroxide 2. Chromium( Ⅲ ) nitrate 3. Ammonium carbonate 4. Cupric cyanide 5. Calcium phosphate

Exercise 4 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. Cadmium nitrate 2. Nickel ( Ⅲ ) hydroxide 3. Ammonium dichromate 4. Calcium hypochlorite 5. Ammonium oxalate

Exercise 5 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. Stannic chromate 2. Lead sulfide 3. Ferrous acetate 4. Ammonium thiocyanate 5. Nickel ( Ⅲ ) hydroxide

Exercise 6 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. lead ( Ⅱ ) phosphate 2. Ferric chromate 3. Cuprous cyanide 4. Ammonium sulfide 5. Silver nitride

Exercise 7 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. Sodium peroxide 2. Ferric oxide 3. Cobalt( Ⅲ ) nitrate 4. Chromium( Ⅲ ) sulfate 5. Potassium permanganate

Exercise 8 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. Aluminum chloride 2. Aluminum hydroxide 3. Ammonium sulfate 4. Ferrous phosphate 5. Antimony ( Ⅲ ) sulfide

Exercise 9 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. Calcium hydroxide 2. Stannous fluoride 3. Ammonium phosphate 4. Calcium carbonate 5. Calcium hypochlorite

Exercise 10 Write formulas for each of the following compounds. Write formulas for each of the following compounds. 1. Potassium carbonate 2. Calcium acetate 3. Magnesium hydroxide 4. Sodium thiosulfate 5. Sodium carbonate

Exercise 11 Write names for each of the following compounds. Write names for each of the following compounds. 1. SnCl 4 2. Hg 2 Cl 2 3. FeO 4. MnCl 2 5. CuS 6. Co(NO 3 ) 3

Exercise 12 Write names for each of the following compounds. Write names for each of the following compounds. 1. Cr 2 O 3 2. CuCH 3 COO 3. Pb(NO 3 ) 2 4. HgS 5. Fe 2 (SO 4 ) 3 6. Cu(OH) 2

Naming acids ⑴ Acids based on anions whose names end in –ide. ⑴ Acids based on anions whose names end in –ide. Anions whose names end in –ide have associated acids that have the hydro- prefix and an –ic ending. Anions whose names end in –ide have associated acids that have the hydro- prefix and an –ic ending. For example, For example, Cl - (chloride)HCl(hydrochloric acid) S 2- (sulfide) H2SH2S (hydrosulfuric acid) I-I- (iodide)HI(hydroiodic acid)

Example F - F - Fluoride ion Fluoride ion HF Hydrofluoric acid HF Hydrofluoric acid Br - Br - Bromide ion Bromide ion HBr Hydrobromic acid HBr Hydrobromic acid CN - CN - Cyanide ion Cyanide ion HCN Hydrocyanic acid HCN Hydrocyanic acid

⑵ Acids based on anions whose names end in –ate or –ite. ⑵ Acids based on anions whose names end in –ate or –ite. * Anions whose names end in –ate have associated acids with an –ic ending. * Anions whose names end in –ate have associated acids with an –ic ending. * Anions whose names end in –ite have acids with an –ous ending. * Anions whose names end in –ite have acids with an –ous ending. For example, For example, ClO - (hypochlorite) HClO (hypochlorous acid) ClO 2 - (chlorite)HClO 2 (chlorous acid) ClO 3 - (chlorate)HClO 3 (chloric acid) ClO 4 - (perchlorate)HClO 4 (perchloric acid)

Summary AnionAcid -idehydro___ic acid -ate ____ic acid -ite ___ous acid

Important Acids and their anions Ⅰ Binary Acids of halogen Binary Acids of halogen HF Hydrofluoric acid Fluoride ion HF Hydrofluoric acid Fluoride ion HCl Hydrochloric acid Chloride ion HCl Hydrochloric acid Chloride ion HBr Hydrobromic acid Bromide ion HBr Hydrobromic acid Bromide ion HI Hydroiodic acid Iodide ion HI Hydroiodic acid Iodide ion Acid Containing Sulfur Acid Containing Sulfur H 2 SO 4 Sulfuric acid Sulfate ion H 2 SO 4 Sulfuric acid Sulfate ion H 2 SO 3 Sulfurous acid Sulfite ion H 2 SO 3 Sulfurous acid Sulfite ion H 2 S Hydrosulfuric acid Sulfide ion H 2 S Hydrosulfuric acid Sulfide ion

Important Acids and their anions Ⅱ Acids Containing Nitrogen or Phosphorus Acids Containing Nitrogen or Phosphorus HNO 3 Nitric acid Nitrate ion HNO 3 Nitric acid Nitrate ion HNO 2 Nitrous acid Nitrite ion HNO 2 Nitrous acid Nitrite ion H 3 PO 4 Phosphoric acid Phosphate ion H 3 PO 4 Phosphoric acid Phosphate ion H 3 PO 3 Phosphorous acid Phosphite ion H 3 PO 3 Phosphorous acid Phosphite ion Important Acids Containing Carbon Important Acids Containing Carbon H 2 CO 3 Carbonic acid Carbonate ion H 2 CO 3 Carbonic acid Carbonate ion CH 3 COOH Acetic acid Acetate ion CH 3 COOH Acetic acid Acetate ion HCN Hydrocyanic acid Cyanide ion HCN Hydrocyanic acid Cyanide ion

Important Acids and their anions Ⅲ Oxyacids Containing Halogen Oxyacids Containing Halogen HClO 4 Perchloric acid Perchlorate ion HClO 4 Perchloric acid Perchlorate ion HClO 3 Chloric acid Chlorate ion HClO 3 Chloric acid Chlorate ion HClO 2 Chlorous acid Chlorite ion HClO 2 Chlorous acid Chlorite ion HClO Hypochlorous acid Hypochlorite ion HClO Hypochlorous acid Hypochlorite ion HBrO 3 Bromic acid Bromate ion HBrO 3 Bromic acid Bromate ion HIO 3 Iodic acid Iodate ion HIO 3 Iodic acid Iodate ion

Exercise1 Name the following acids: Name the following acids: (a) HCN (b)HNO 3 (c) H 2 SO 4 (d) H 2 SO 3 (a) HCN (b)HNO 3 (c) H 2 SO 4 (d) H 2 SO 3Solution (a) Hydrocyanic acid (b) Nitric acid (c) Sulfuric acid (d) Sulfurous acid

Exercise 2 Give the chemical formulas for Give the chemical formulas for (a) hydrobromic acid (a) hydrobromic acid (b) carbonic acid (b) carbonic acid (c) sulfurous acid (c) sulfurous acid (d) periodic acid (d) periodic acidSolution (a) HBr (b) H 2 CO 3 (c) H 2 SO 3 (d) HIO 4

Exercise Give names or chemical formulas for the following compounds. Give names or chemical formulas for the following compounds. 1. Sodium hydrogen carbonate 2. Potassium dihydrogen phosphate 3. Periodic acid 4. HBr(gas) 5. HBr(in water) 6. HIO 7. HNO 2 8. HBrO 4

Naming binary molecular compounds The rules: The rules: 1. The element in the compound that is further from fluorine in the periodic table is usually named first. B >Si >C >P >N >H >S >I >Br >Cl >O >F B >Si >C >P >N >H >S >I >Br >Cl >O >F 2. The name of the second element is given an -ide ending. -ide ending. 3. Greek are used to indicate the number of atoms of each -notice -notice -notice

Examples Cl 2 O Cl 2 O dichlorine monoxide dichlorine monoxide N 2 O 4 N 2 O 4 dinitrogen tetroxide dinitrogen tetroxide NF 3 NF 3 nitrogen trifluoride nitrogen trifluoride P 4 S 10 P 4 S 10 tetraphosphorus decasulfide tetraphosphorus decasulfide

Exercise1 Naming the following compounds: Naming the following compounds: 1. SO 2 2. PCl 5 3. N 2 O 3 1. SO 2 2. PCl 5 3. N 2 O 3Solution 1. Sulfur dioxide 1. Sulfur dioxide 2. Phosphorus pentachloride 2. Phosphorus pentachloride 3. Dinitrogen trioxide 3. Dinitrogen trioxide

Exercise2 Give the chemical formula for Give the chemical formula for 1. Silicon tetrabromide 1. Silicon tetrabromide 2. Disulfur dichloride 2. Disulfur dichloride 3. Hydrogen cyanide 3. Hydrogen cyanide 4. Dinitrogen tetroxide 4. Dinitrogen tetroxide 5. Tetraphosphorus hexasulfide 5. Tetraphosphorus hexasulfide Solution 1. SiBr 4 2. S 2 Cl 2 3. HCN 4. N 2 O 4 5. P 4 S 6

Exercise3 Write the chemical formula for each substance mentioned in the following word descriptions. Write the chemical formula for each substance mentioned in the following word descriptions. 1. Zinc carbonate can be heated to form zinc oxide and carbon dioxide. 2. On treatment with hydrofluoric acid, silicon dioxide forms silicon tetrafluoride and water. 3. Sulfur dioxide reacts with water to form sulfurous acid. 4. The substance hydrogen phosphide, commonly called phosphine, is a toxic gas 毒气. 5. Perchloric acid reacts with cadmium to form cadmium( Ⅱ ) perchlorate. 6. Vanadium( Ⅲ ) bromide is a colored solid. 7. Sodium hydrogen carbonate is used as a deodorant 除溴剂.

Hydrates Hydrates are compounds that have a specific number of water molecules attached to them. Hydrates are compounds that have a specific number of water molecules attached to them. for example, for example, CuSO 4 5H 2 O CuSO 4 5H 2 O copper( Ⅱ ) sulfate pentahydrate copper( Ⅱ ) sulfate pentahydrate anhydrous copper( Ⅱ ) sulfate anhydrous copper( Ⅱ ) sulfate BaCl 2 2H 2 O barium chloride dihydrate BaCl 2 2H 2 O barium chloride dihydrate LiCl H 2 O lithium chloride monohydrate LiCl H 2 O lithium chloride monohydrate MgSO 4 7H 2 O magnesium sulfate hepahydrate MgSO 4 7H 2 O magnesium sulfate hepahydrate Sr(NO 3 ) 2 4H 2 O strontium nitrate tetrahydrate Sr(NO 3 ) 2 4H 2 O strontium nitrate tetrahydrate

Common and Systematic Names of Some Compound Ⅰ Formula Common name Systematic Name Formula Common name Systematic Name H 2 O H 2 O WaterDihydrogen monoxide NH 3 AmmoniaTrihydrogen nitride CO 2 Dry iceSolid carbon dioxide NaClTable saltSodium chloride N2ON2O Laughing gasDinitrogen monoxide CaCO 3 Marble, chalk, limestone Calcium carbonate

Common and Systematic Names of Some Compound Ⅱ Formula Common name Systematic Name Formula Common name Systematic Name CaO QuicklimeCalcium oxide Ca(OH) 2 Slaked limeCalcium hydroxide NaHCO 3 Baking soda Sodium hydrogen carbonate Na 2 CO 3 ·10H 2 OWashing soda Sodium carbonate decahydrate MgSO 4 ·7H 2 OEpson salt Magnesium sulfate heptahydrate Mg(OH) 2 Milk of magnesia Magnesium hydroxide CaSO 4 ·2H 2 O gypsum Calcium sulfate dihydrate

For example -ate -ite -ate -ite NO 3 3- Nitrate ion PO 4 3- Phosphate ion NO 3 3- Nitrate ion PO 4 3- Phosphate ion NO 2 2- Nitrite ion PO 3 3- Phosphite ion NO 2 2- Nitrite ion PO 3 3- Phosphite ion SO 4 2- Sulfate ion ClO 3 - Chlorate ion SO 4 2- Sulfate ion ClO 3 - Chlorate ion SO 3 2- Sulfite ion ClO 2 - Chlorite ion End SO 3 2- Sulfite ion ClO 2 - Chlorite ion End End

For example ClO 4 - perchlorate ion (one more O than chlorate) ClO 4 - perchlorate ion (one more O than chlorate) ClO 3 - chlorate ion ClO 3 - chlorate ion ClO 2 - chlorite ion (one less O than chlorate) ClO 2 - chlorite ion (one less O than chlorate) ClO - hypochlorite ion (one less O than chlorite) End ClO - hypochlorite ion (one less O than chlorite) EndEnd

Prefix Meaning Prefix Meaning Mono- 1 Mono- 1 Di- 2 Di- 2 Tri- 3 Tri- 3 Tetra- 4 Tetra- 4 Penta- 5 Penta- 5 Hexa- 6 Hexa- 6 Hepta- 7 Hepta- 7 Octa- 8 Octa- 8 Nona- 9 Nona- 9 Deca- 10 End Deca- 10 End End

Notice : -- The prefix mono- is never used with the first element. -- When the prefix ends in a or o and the name of the second element begins with a vowel 元音, the a or o is often dropped. End End

Example of positive ions End End 1) Na + Sodium ion Zn 2+ Zinc ion 1) Na + Sodium ion Zn 2+ Zinc ion Al 3+ Aluminium ion Al 3+ Aluminium ion 2) Fe 2+ iron( Ⅱ ) ion or ferrous ion Fe 3+ iron( Ⅲ ) ion or ferric ion Fe 3+ iron( Ⅲ ) ion or ferric ion Cu + copper( Ⅰ ) ion or cuprous ion Cu + copper( Ⅰ ) ion or cuprous ion Cu 2+ copper( Ⅱ ) ion or cupric ion Cu 2+ copper( Ⅱ ) ion or cupric ion 3) NH 4 + Ammonium ion H 3 O + Hydronium ion H 3 O + Hydronium ion

Case 1 of anions End End For example, For example, H - Hydride ion H - Hydride ion O 2- Oxide ion O 2- Oxide ion N 3- Nitride ion N 3- Nitride ion For example, For example, OH - Hydroxide ion OH - Hydroxide ion CN - Cyanide ion CN - Cyanide ion O 2 2- Peroxide ion O 2 2- Peroxide ion

Case 2 of anions End End Ending: -ate for the most common oxyanion of element -ate for the most common oxyanion of element -ite for an oxyanion that has the same charge -ite for an oxyanion that has the same charge but one less O but one less Prefix: (for a series of oxyanions of the same element) per- indicates one more O atom than the oxyanion per- indicates one more O atom than the oxyanion ending in –ate. ending in –ate. hypo- indicates one less O atom than the oxyanion hypo- indicates one less O atom than the oxyanion ending in ending

Case 3 of anions End End For example, CO 3 2- Carbonate ion CO 3 2- Carbonate ion HCO 3 - Hydrogen carbonate ion HCO 3 - Hydrogen carbonate ion ( bicarbonate ion ) ( bicarbonate ion ) PO 4 3- Phosphate ion PO 4 3- Phosphate ion H PO 4 2- Hydrogen phosphate ion H PO 4 2- Hydrogen phosphate ion ( biphosphate ion ) ( biphosphate ion ) H 2 PO 4 - Dihydrogen phosphate ion H 2 PO 4 - Dihydrogen phosphate ion