Naming Compounds Aim: To understand why it is necessary to have a system for naming compounds Binary compounds- Compounds composed of two elements Two classes o Compounds that contain metals and nonmetals o Compounds that contain two metals Naming Compounds that Contain a Metal and Nonmetals Aim: To learn to name binary compounds of a metal and nonmetal Metals lose electrons to become cations Nonmetals gain electrons to become an anion Metal + Nonmetal = Binary Ionic Compound (+) (-) Type I compounds-metals that form ONLY one type of cation Type II compounds- Metals that can form two or more cations that have different charges Rules for naming Type I Compounds 1. The cation is always named first and the anion second 2. A simple cation (obtained from a single atom) takes its name from the name of the element. Ex. Na + is called sodium in the names of compounds containing this ion. 3. A simple anion (obtained from a single atom) is named by taking the first part of the element name (the root) and adding ide. Thus Cl - ion is called chloride Noble gases are the least reactive; therefore they do not form compounds Octet rule-in most chemical reactions, atoms tend to match the s and p electron configuration of noble gases. The atoms want to have their p orbital filled. Type I Group 1 Group 2 Group 3 Charge 1 + 2 + 3 + Most reactive Most reactive When you form ionic compounds there is no net charge- Na + Cl - = NaCl Charge (+1) (-1) = 0 Sodium Chloride Al 3+ I - = AlI 3 Charge (+3) 3(-1) = 0 Aluminum iodide Remember to switch your charges and place as subscripts when you write your ionic compounds Nonmetals Group 15 Group 16 Group 17 Charge 3-2 - 1 - Common Simple Cations and Anions Cations Name Anion Name H +1 Hydrogen H -1 hydride Li +1 Lithium F -1 fluoride Na +1 Sodium Cl -1 chloride K +1 Potassium Br -1 bromide Cs +1 Cesium I -1 iodide Be 2+ Beryllium O 2- oxide Mg 2+ Magnesium S 2- sulfide Ca 2+ Calcium Ba 2+ Barium Al 3+ Aluminum Ag +1 Silver Zn 2+ zinc
Type II Ionic Compounds Type II Ions o Transition Metals and some other Metals o Typically they have several different ionic charges because electrons in d orbitals are very close in energy to the s and p valence electrons. As a result, these d electrons sometimes participate in ion formation. Some Common Type II Cations Ion Systematic Name Older Name Fe 3+ Iron (III) ferric Fe 2+ Iron (II) ferrous Cu 2+ Copper (II) cupric Cu +1 Copper (I) cuprous Co 3+ Cobalt (III) colbaltic Co 2+ Cobalt (II) cobaltous Sn 4+ Tin (IV) stannic Sn 2+ Tin (II) stannous Pb 4+ Lead (IV) plumbic Pb 2+ Lead (II) plumbous Hg 2+ Mercury (II) mercuric 2+ Hg 2 Mercury (I) mercurous 2+ Mercury (I) ions always occur bonded together in pairs to form Hg 2 Rules for Naming Type II Ionic Compounds 1. The cation is always named first and then the anion. 2. Because the cation can assume more than one charge, the charge is specified by a roman numeral in parentheses. What is the charge on the lead ion? Use the principle of charge balance to determine the cation charge. PbO 2 Remember Oxygen has a charge of -2. (?) 2(-2) = 0 +4 2(-2) = 0 Naming Binary Compounds that contain only Nonmetals (Type III) Aim: To learn how to name binary compounds containing only nonmetals Rules for naming Type III binary compounds 1. The first element in the formula is named first, and the full element name is used. 2. The second element is named as though it were an anion. 3. Prefixes are used to denote the numbers of atoms present. 4. The prefix mono- is never used for naming the first element. Ex. CO is called carbon monoxide not monocarbon monoxide. Prefixes used to indicate numbers in chemical names Prefix mono- di- tri- tetra- penta- hexa- hepta octa- nona- deca- Number indicated 1 2 3 4 5 6 7 8 9 10 NO nitrogen monoxide or N 2 O 5 dinitrogen pentoxide For easier pronunciation we often drop the o or a of the prefix when the second element is oxygen.
Chemistry: Binary Compounds List the oxidation numbers (charges) for each of the following elements. Ca 2+ N 3- Br 1- Be 2+ Ba 2+ Fr 1- K 1+ P 3- Al 3+ Group 1 1+ Group 2 2+ Group 13 3+ Group 15 3- Group 16 2- Group 17 1- Zn 2+ Ag 1+ Fe (III) 3+ Write the formulas for the following binary compounds. calcium oxide beryllium chloride iron (II) oxide CaO BeCl 2 FeO sodium fluoride potassium iodide copper (I) chloride NaF KI CuCl copper (II) chloride aluminum chloride lead (IV) nitride CuCl 2 AlCl 3 Pb 3 N 4 iron (III) oxide strontium oxide lead (II) nitride Fe 2 O 3 SrO Pb 3 N 2 Write the names of the following binary compounds. Cr 2 O 3 chromium (III) oxide NaBr sodium bromide PbI 2 lead (II) iodide HCl hydrogen chloride Al 2 O 3 aluminum oxide BN boron nitride RbI rubidium iodide BaF 2 barium fluoride H 2 S hydrogen sulfide NaCl sodium chloride
Chemistry: Ionic Binary Compounds: Single-Charge Cations Write the name of each of the following compounds. 1. Na 2 S 1. sodium sulfide 2. Al 2 O 3 2. aluminum oxide 3. NaCl 3. sodium chloride 4. RbI 4. rubidium iodide 5. ZnBr 2 5. zinc bromide 6. AgCl 6. silver chloride 7. BN 7. boron nitride 8. BaF 2 8. barium fluoride 9. Sr 3 N 2 9. strontium nitride_ 10. MgCl 2 10. magnesium chloride Write the chemical formula for each of the given names. 11. magnesium nitride 11. Mg 3 N 2 12. calcium oxide 12. CaO 13. silver fluoride 13. AgF 14. beryllium chloride 14. BeCl 2 15. potassium iodide 15. KI 16. aluminum chloride 16. AlCl 3 17. zinc oxide 17. ZnO 18. barium bromide 18. BaBr 2 19. lithium nitride 19. Li 3 N 20. potassium sulfide 20. K 2 S
Chemistry: Ionic Binary Compounds: Multiple-Charge Cations Write the name of each of the following compounds. 1. CuF 1. copper (I) fluoride 2. CuF 2 2. copper (II) fluoride 3. Cr 2 O 3 3. Chromium (III) oxide 4. PbI 2 4. lead (II) iodide 5. PbCl 4 5. lead (IV) chloride 6. CrO 3 6. chromium (VI) oxide_ 7. AuBr 7. gold (I) bromide 8. NiO 8. nickel (II) oxide 9. VI 3 9. vanadium (III) iodide 10. SnO 2 10. _tin (IV) oxide Write the chemical formula for each of the given names. 11. manganese (VII) oxide 11. Mn 2 O 7 12. niobium (V) chloride 12. NbCl 5 13. titanium (III) phosphide 13. TiP 14. palladium (IV) sulfide 14. PdS 2 15. platinum (II) fluoride 15. PtF 2 16. osmium (III) oxide 16. Os 2 O 3 17. iridium (IV) nitride 17. Ir 3 N 4 18. cobalt (II) chloride 18. CoCl 2 19. iron (III) sulfide 19. Fe 2 S 3 20. gold (III) iodide 20. AuI 3
Chemistry: Oxidation Numbers and Ionic Compounds Write the correct formula for the compound formed by each of the following pairs of ions. 1. Na 1+ F 1-1. NaF 2. K 1+ S 2- EXAMPLE 2. K 2 S 3. Ni 2+ SO 4 2-3. NiSO 4 4. Al 3+ O 2-4. Al 2 O 3 5. Ca 2+ ClO 3 1-5. Ca(ClO 3 ) 2 6. NH 4 1+ P 3-6. (NH 4 ) 3 P 7. Cu 1+ NO 3 1-8. Cu 2+ NO 3 1-7. _CuNO 3 8. Cu(NO 3 ) 2 9. Pb 4+ O 2-9. PbO 2 10. Li 1+ CO 3 2-10. Li 2 CO 3 For each of the following compounds, write A) the symbols of the ions in the compound, B) the number of each ion in one molecule of that compound and C) the name of the compound. 11. CaI 2 Example 11. one Ca 2+ and two I 1- Calcium Iodide 12. Na 2 CO 3 12. two Na + and one CO 3 2- sodium carbonate 13. Ga(ClO 3 ) 3 13. one Ga 3+ and three ClO 3 1- gallium chlorate 14. CuF 2 14. one Cu 2+ and two F - copper(ii) fluoride 15. (NH 4 ) 3 PO 4 15. three NH 4 1+ and one PO 4 3- ammonium phosphate 16. FeSO 4 16. one Fe 2+ and one SO 4 2- iron(ii) sulfate 17. Mg(NO 3 ) 2 17. one Mg 2+ and two NO 3 1- magnesium nitrate 18. NH 4 NO 2 18. one NH 4 1+ and one NO 2 1- ammonium nitrite 19. KC 2 H 3 O 2 19. one K + and one C 2 H 3 O 2 1- potassium acetate 20. Na 2 Cr 2 O 7 20. two Na + and one Cr 2 O 7 2- sodium dichromate
Chemistry: Covalent Binary Compounds: Nonmetal Nonmetal Combinations Write the name of each of the following compounds. 1. HF 1. hydrogen monofluoride 2. H 2 S 2. dihydrogen monosulfide 3. NO 3. nitrogen monoxide 4. N 2 O 4. dinitrogen monoxide 5. NO 2 5. nitrogen dioxide 6. N 2 O 5 6. dinitrogen pentoxide 7. SO 2 7. sulfur dioxide 8. CBr 4 8. carbon tetrabromide 9. C 2 H 6 9. dicarbon hexahydride (ethane) 10. C 4 H 10 10. tetra carbon decahydride (butane) Write the chemical formula for each of the given names. 11. nitrogen triiodide 11. NI 3 12. dinitrogen tetroxide 12. N 2 O 4 13. sulfur trioxide 13. SO 3 14. carbon monoxide 14. CO 15. dihydrogen monoxide 15. H 2 O 16. hydrogen monobromide 16. HBr 17. phosphorus trichloride 17. PCl 3 18. tricarbon octahydride 18. C 3 H 8 (propane) 19. carbon tetrahydride 19. CH 4 (methane)_ 20. dicarbon tetrahydride 20. C 2 H 4 (ethane)_
Chemistry: Errors in Chemical Formulas and Nomenclature Each of the following formulas or chemical names contains an error. Correct each example. 1. aluminum (III) iodide 1. aluminum iodide AlI 3 2. Al 3 O 2 2. Al 2 O 3 aluminum oxide 3. (NH 4 ) 3 Cl 2 3. NH 4 Cl ammonium chloride 4. lead (III) oxide 4. lead (II) or (IV) oxide PbO or PbO 2 5. leadic oxide 5. lead (IV) oxide PbO 2 6. stannous (II) bromide 6. tin (II) bromide SnBr 2 7. monocalcium dioxide 7. calcium oxide CaO 8. K(ClO 2 ) 8. KClO 2 Potassium chlorite 9. (OH) 3 Al 9. Al(OH) 3 aluminum hydroxide 10. Cr 4 (CN) 3 10. Cr(CN) 4 chromium (IV) cyanide 11. Pb(NO 3 ) 3 11. Pb(NO 3 ) 4 Lead (IV) nitrate 12. copper (I) chloric 12. copper (I) chloride CuCl 13. ferric (III) oxide 13. iron (III)oxide Fe2O3 14. NiNO 32 14. Ni(NO 3 ) 2 Nickel (II) nitrate 15. Mg 2 F 15. MgF 2 magnesium fluoride 16. ironic oxide 16. iron (III) oxide Fe 2 O 3 17. ClK 17. KCl potassium chloride 18. Ca 2 O 2 18. CaO calcium oxide 19. sodium (I) fluoride 19. sodium fluoride NaF 20. dititanium tetroxide 20. titanium (IV) oxide TiO 2 21. dihydrogen oxide 21. dihydrogen monoxide H 2 O 22. magnesium dihydroxide 22. magnesium hydroxide Mg(OH) 2 23. cuprous (I) sulfate 23. copper (I) sulfate Cu 2 SO 4 24. strontium difluoride 24. strontium fluoride SrF 2 25. NO 3 Na 25. NaNO 3 sodium nitrate