Naming Inorganic Compounds
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- Ethelbert Ellis
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1 Naming Inorganic Compounds yes Metal or NH 4? no yes Group I or II; Al, Ag, Zn, NH 4? no yes H in front? no yes O is present, but not H 2 O or H 2 O 2? no yes (aq) is written? no Type I Ionic Compound Type II Ionic Compound Oxyacid Nonoxyacid Binary Covalent Compound Al 2O 3 (s) CuCl(s) HClO(aq) HCl(aq) HCl(g) aluminum oxide copper(i) chloride hypochlorous acid hydrochloric acid hydrogen chloride P 2O 5(s) LiOH (s) CuCl 2 (s) HClO 2 (aq) H 2 S(aq) H 2 S(g) lithium hydroxide copper(ii) chloride chlorous acid hydrosulfuric acid hydrogen sulfide AgNO 3 (s) Fe 2 O 3 (s) HClO 3 (aq) HCN(aq) HCN(g) silver nitrate iron(iii) oxide chloric acid hydrocyanic acid hydrogen cyanide Na 2 O 2 (s) sodium peroxide CaCO 3 (s) calcium carbonate NH 4 NO 3 (s) ammonium nitrate FeO(s) iron(ii) oxide Cr 2 (SO 4 ) 3 (s) chromium(iii) sulfate MnS(s) manganese(ii) sulfide Sn(NO 3 ) 2 (s) tin(ii) nitrate HClO 4 (aq) or (l) perchloric acid H 2 SO 3 (aq) sulfurous acid H 2 SO 4 (aq) or (l) sulfuric acid H 2 O 2 (l) hydrogen peroxide H 2 O(l) water diphosphorus pentoxide NO 2 (g) nitrogen dioxide S 2 Cl 2 (l) disulfur dichloride CO(g) carbon monoxide PF 5 (g) phosphorus pentafluoride XeF 4 (s) xenon tetrafluoride NH 3 (g) ammonia CH 4 (g) methane
2 Intentionally Blank
3 CHEMICAL SYMBOLS AND FORMULAS Al 1) Element aluminum 2) Elementary substance (aluminum metal) 3) One atom of aluminum 2Al Two atoms of Aluminum 2H Two atoms of hydrogen H 2 1) Molecular hydrogen; substance (hydrogen gas) 2) One molecule of hydrogen H 2 O 1) Water as a substance ( a covalent compound) 2) One molecule of water 2H 2 O Two molecules of water 2Al + 3O 2 Two atoms of aluminum and (mixed with) three molecules of oxygen Al 2 (SO 4 ) 3 1) Aluminum sulfate as a substance (an ionic compound) 2) One formula unit of aluminum sulfate: per each 2 atoms of aluminum there are 3 SO 4 groups OR 2 atoms of aluminum, 3 atoms of sulfur and 12 atoms of oxygen per one formula unit of aluminum sulfate
4 Greek Prefixes for Naming Compounds Number Prefix 1 mono- 2 di- bicycle 3 tri- tricycle 4 tetra- 5 penta- the Pentagon 6 hexa- 7 hepta- September 8 octa- October 9 nona- (Latin) November 10 deca- December 11 undeca- (Latin) 12 dodeca- 13 trideca- 20 icosa-
5 Names and Formulas of Common Ions Positive Ions (cations) The charges of these ions can be figured out using the periodic table: Negative Ions (anions) The charges of these ions can be figured out using the periodic table: Hydrogen H + Hydride H Lithium Li + Fluoride F Sodium Na + Chloride Cl Potassium K + Bromide Br Rubidium Rb + Iodide I Cesium Cs + Oxide 2 O Beryllium Be 2+ Sulfide 2 S Magnesium Mg 2+ Nitride 3 N Calcium Ca 2+ Phosphide P Strontium Sr 2+ Barium Ba 2+ Aluminum Al 3+ 3 These ions must be memorized: These ions must be memorized: Hydronium H 3 O + Acetate C 2 H 3 O 2 Ammonium NH 4 Hydroxide OH Silver Ag + Cyanide CN Cadmium Cd 2+ Cyanate OCN Zinc Zn 2+ Thiocyanate SCN Copper (I) or cuprous Cu + Hypochlorite ClO Copper (II) or cupric Cu 2+ Chlorite ClO 2 Mercury (I) or mercurous 2 Hg 2 Chlorate ClO 3 Mercury (II) or mercuric Hg 2+ Perchlorate ClO 4 Lead (II) or plumbus Pb 2+ Nitrate NO 3 Lead (IV) or plumbic Pb 4+ Nitrite NO 2 Iron (II) or ferrous Fe 2+ Permanganate MnO 4 Iron (III) or ferric Fe 3+ Carbonate CO 2 3 Manganese (II) Mn 2+ Hydrogen carbonate or bicarbnate HCO 3 Nickel (II) Ni 2+ Chromate 2 CrO 4 Tin (II) or stannous Sn 2+ 2 Dichromate Cr 2 O 7 Tin (IV) or stannic Sn 4+ 2 Peroxide O 2 Chromium (II) Cr 2+ Sulfate 2 SO 4 Chromium (III) Cr 3+ Hydrogen sulfate or bisulfate HSO 4 Cobalt (II) Co 2+ Sulfite SO 2 3 Cobalt (III) Co 3+ Hydrogen sulfite or bisulfite HSO 3 Bismuth (III) Bi 3+ Phosphate PO 3 4 Hydrogen phosphate 2 HPO 4 Dihydrogen phosphate H 2 PO 4 3 Borate BO 3 Oxalate 2 C 2 O Note: Ions in bold type are very common and must be memorized first!!! 4
6 I A MONATOMIC IONS VII A VIII A II A III A IV A V A VI A H - C 4- N 3- O 2- F - III B IV B V B VI B VII B VIII B VIII B VIII B I B II B Si 4- P 3- S 2- Cl - Cr 2+ Cr 3+ Fe2+ Co 2+ Cu+ Mn2+ Fe 3+ Ni2+ As 3- Se 2- Br - Co3+ Cu 2+ Sn 2+ Sn 4+ Te 2- I - Pb 2+ Au + 2 Hg 2 Bi 3+ Au 3+ Hg 2+ Pb 4+ E metallic elements that form several stable monatomic cations: 2 Cr 3+ is chromium (III) ion, Hg 2+ is mercury (II) ion, etc.; Hg is a polyatomic ion called mercury (I) ion 2 E nonmetallic elements; each forms a single stable monatomic anion: F - is fluoride ion, Si 4- is silicide ion, etc. ions that do not exist in aqueous solutions; they react with water by accepting either H + or OH - ions (small amounts of H + and OH - ions are always present in water: H2O H + + OH - )
7 Oxyacids and Oxyanions SO 3 2 sulfite ion NO 2 nitrite ion HSO 3 hydrogen sulfite ion HNO 2 nitrous acid H 2 SO 3 sulfurous acid minus O minus O HNO 3 nitric acid H 2 CO 3 carbonic acid H 2 SO 4 sulfuric acid H 3 PO 4 phosphoric acid NO 3 nitrate ion HCO 3 hydrogen carbonate ion HSO 4 hydrogen sulfate ion H 2 PO 4 dihydrogen phosphate ion CO 3 2 carbonate ion SO 4 2 sulfate ion HPO 4 2 hydrogen phosphate ion PO 4 3 phosphate ion
8 OXYACIDS * OXYANIONS H 2 O (HOH) water OH hydroxide ion HC 2 H 3 O 2 (aq) acetic acid C 2 H 3 O 2 acetate ion HClO 4 (aq) perchloric acid ClO 4 HClO 3 (aq) chloric acid ClO 3 HClO 2 (aq) chlorous acid ClO 2 perchlorate ion chlorate ion chlorite ion HClO (aq) hypochlorous acid ClO hypochlorite ion HNO 3 (aq) nitric acid NO 3 HNO 2 (aq) nitrous acid NO 2 nitrate ion nitrite ion H 2 CO 3 (aq) carbonic acid CO 2 3 carbonate ion HCO 3 hydrogen carbonate ion (bicarbonate ion) H 2 SO 4 (aq) sulfuric acid SO 2 4 sulfate ion HSO 4 hydrogen sulfate (bisulfate ion) H 2 SO 3 (aq) sulfurous acid SO 2 3 sulfite ion HSO 3 hydrogen sulfite ion (bisulfite ion) H 3 PO 4 (aq) phosphoric acid PO 3 4 phosphate ion HPO 2 4 H 2 PO 4 hydrogen phosphate ion dihydrogen phosphate ion * Pure covalent molecular compounds or their aqueous solutions. Usually, only acids with the highest number of oxygen atoms (HClO 4, HNO 3, H 3 PO 4, H 2 SO 4 ) can be obtained in pure form. They are also stable in aqueous solutions. All other acids exist only as aqueous solutions. Organic acids, such as acetic acid, are stable in pure form and in aqueous solutions.
9 NONOXYACIDS AND NONOXYANIONS COMPOUNDS ACIDS ANIONS pure substances: aqueous solutions: exist in ionic crystals only HX molecules HX dissolved in H 2 O or as X (aq) in aqueous solutions HF(g) hydrogen fluoride HF(aq) hydrofluoric acid F fluoride ion HCl(g) hydrogen chloride HCl(aq) hydrochloric acid Cl chloride ion HBr(g) hydrogen bromide HBr(aq) hydrobromic acid Br bromide ion HI(g) hydrogen iodide HI(aq) hydroiodic acid I iodide ion H 2 S(g) hydrogen sulfide H 2 S(aq) hydrosulfuric acid S sulfide ion HS hydrogen sulfide ion HCN(g) hydrogen cyanide HCN(aq) hydrocyanic acid CN cyanide ion
10 PREFIXES AND SUFFIXES IN THE NAMES OF ACIDS AND CORRESPONDING ANIONS Number of Oxygen Atoms Acid Anion Greatest per... ic acid per... ate ion Greater... ic acid... ate ion Smaller... ous acid... ite ion Smallest hypo... ous acid hypo... ite ion None hydro... ic acid... ide ion EXAMPLE: HClO 4 (aq) perchloric acid ClO 4 HClO 3 (aq) chloric acid ClO 3 HClO 2 (aq) chlorous acid ClO 2 perchlorate ion chlorate ion chlorite ion HClO(aq) hypochlorous acid ClO hypochlorite ion HCl(aq) hydrochloric acid Cl chloride ion
11 Formulas and Names of Binary Ionic Compounds (1) Write the formula for each ion below the ion s name. (2) Fill in the blanks with the correct formula and name of the compound formed by the combination of ions. Chloride ion Cl Oxide ion Bromide ion Sulfide ion Nitride ion Sodium ion Na + NaCl sodium chloride Copper (I) ion Calcium ion Iron (II) ion Iron (III) ion Aluminum ion
12 Formulas and Names of Binary Covalent Compounds Fill the blanks in the following table. Formula Name Formula Name CO tetraphosphorus decaoxide carbon disulfide NH 3 SO 2 sulfur hexafluoride SiC N 2 O 3 dinitrogen monoxide OF 2 P 4 S 3 silicon tetrachloride IF 7 CH 4 H 2 O sulfur trioxide dihydrogen disulfide KrF 2 Cl 2 O 7 dinitrogen pentaoxide
13 Formula Writing Exercise A For each box write the chemical formula of the compound formed by the cation at the head of the column and the anion at the left of the row. Li 2 Mg NH 4 Al 3 Na 2 Ba K 2 Ca Br LiBr 2 SO 4 OH F 2 O NO 3 3 PO 4 Cl 2 S I CO 2 3
14 FORMULA WRITING EXERCISE 1 Give a correct chemical name for each of the following compounds: 1. MgO magnesium oxide 2. PbI 2 3. FeS 4. ZnSO 4 5. Li 2 CO 3 6. Ba(NO 3 ) 2 7. NH 4 NO 2 8. K 2 SO 3 9. CrCl Sr(C 2 H 3 O 2 ) Mg 3 N Ca 3 (PO 4 ) SnO KMnO Hg 2 Cl NaHCO CCl NO N 2 O PBr CaO HCl(aq) 23. HNO 3 (aq) 24. H 2 SO 3 (aq) 25. H 3 PO 4 (aq)
15 FORMULA WRITING EXERCISE 2 Write chemical formulas for the following compounds: 1. Potassium iodide 2. Barium sulfate 3. Aluminum nitrate 4. Copper (II) carbonate 5. Gold (III) chloride 6. Ferric hydroxide 7. Lead (II) chromate 8. Nickel (II) hydroxide 9. Mercury (II) bromide 10. Silver acetate 11. Magnesium chlorate 12. Sodium peroxide 13. Manganese (II) phosphate 14. Ammonium sulfide 15. Platinum (IV) fluoride 16. Chromium (III) hydroxide 17. Calcium oxalate 18. Antimony trichloride 19. Ammonia 20. Silicon dioxide 21. Carbon monoxide 22. Hydrobromic acid 23. Nitrous acid 24. Acetic acid 25. Sulfuric acid
16 FORMULA AND NAME EXERCISES Indicate the covalent compounds below with *. Write the complete chemical formulas for each of the compounds (ionic or covalent). 1. Barium sulfate 2. Calcium chloride 3. Potassium oxide 4. Lithium hydroxide 5. Aluminum iodide 6. Carbon disulfide 7. Tin (IV) fluoride 8. Manganese (II) phosphide 9. Iron (III) sulfite 10. Beryllium acetate 11. Mercury (II) nitrite 12. Copper (I) phosphate 13. Dinitrogen pentoxide 14. Hydrogen peroxide 15. Boron tribromide 16. Nickel (II) chromate 17. Sodium hydrogen carbonate 18. Hydrocyanic acid (sodium bicarbonate) 19. Nitrous acid 20. Silver hypochlorite Indicate covalent compounds below with *. Write the complete name formulas for each of the compounds (ionic or covalent). 1. Mg(CN) 2 2. Li 3 PO 4 3. P 4 O KMnO 4 5. (NH 4 ) 2 CO 3 6. Hg(OH) 2 7. CdSe 10. OF N 2 (g) 12. HBrO 3 (aq) 13. CsHS 14. SiCl KH 2 PO HBr(aq) 17. Cd(NO 3 ) 2 7H 2 O 17. AsH 3
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