OXIDATION NUMBERS oxidation number
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1 OXIDATION NUMBERS The oxidation number or state refers to the charge an atom would have if the pairs of electrons in each bond of the compound belonged to the atom with the most electronegative charge, as if the electrons had been transferred and not shared. For ionic compounds this is already the case, so the oxidation number and the ionic charge are the same. For a covalently bonded compound the oxidation number is a hypothetical charge. Ionic charges are differentiated from oxidation numbers by the placement of the charge and the number. Ionic charges are written with the charge following the number, however, oxidation numbers are written with the charge is written before the number. There are several rules that apply to oxidation numbers: 1. The sum of all oxidation numbers in a compound must equal zero. - For example: What are the oxidation numbers for sodium and chlorine in NaCL? Na is +1 and Cl is 1 for a total of zero. 2. The sum of all oxidation numbers in a polyatomic ion must be equal to the charge of the ion. - For example: What is the charge on the sulfur in the polyatomic ion SO 4-2? Each oxygen carries an oxidation number of 2, for a total of 8. The overall charge must be 2, therefore the sulfur must have an oxidation number of When there is a combination of non-metals, the less electronegative atom will have a positive oxidation number, and the higher electronegative atom will have a negative oxidation number. - For example: What are the oxidation numbers of CO 2? Carbon will have an oxidation number of +4 and oxygen will have an oxidation number of The oxidation number of an elementary substance is zero, this also applies to diatomic molecules. **Review the seven diatomic molecules! - For example: What is the oxidation number for the chlorine in Cl 2? Each chlorine is zero, because the atoms have identical electronegativities the electrons will be shared equally. 5. The oxidation number of any one atom ion is equal to its ionic charge. - For example: What is the oxidation number for a sodium ion? The sodium ion s oxidation number is Oxygen s oxidation number is always equal to 2, except when it is in peroxide, then it is equal to 1. - For example: What is the oxidation number of oxygen in water? Water is H 2 O, the hydrogen each have +1 oxidation numbers totaling +2. The molecule must have a zero total, therefore, oxygen s oxidation number is 2. - What is the oxidation number in hydrogen peroxide, H 2 O 2? H 2 has a total of +2, therefore O 2 must have a value of 2 leaving each oxygen with a 1 oxidation number. 7. Hydrogen has a oxidation number of +1, except when it is in a hydride, then it is equal to 1. - For example: What is the oxidation number for hydrogen in HCl? The chlorine atom has an oxidation number of 1, therefore the hydrogen must be What is the oxidation number of hydrogen in Lithium hydride, LiH? Lithium has an oxidation number of +1, therefore hydrogen must have an oxidation number of 1.
2 Practice: Determine the oxidation number for each of the elements in the following molecules and ions. 1. Ag Ag= 11. Ag 2 S Ag= S= 2. CdS Cd= S= 12. HgCl Hg= Cl= 3. CdCl 2 Cd= Cl= 13. HgCl 2 Hg= Cl= 4. I 2 I= 14. H(NO 3 ) H= N= O= 5. SnCl 2 Sn= Cl= 15. NaOH Na= O= H= 6. SnCl 4 Sn= Cl= 16. H 2 O 2 H= O= 7. FeCl 2 Fe= Cl= 17. LiH Li= H= 8. FeCl 3 Fe= Cl= 18. K(ClO 3 ) K= Cl= O= 9. NO 2-1 N= O= 19. H 2 (SO 4 ) H= S= O= 10. N 2 O N= O= 20. Fe(NO 3 ) 3 Fe= N= O=
3 NOMENCLATURE Nomenclature is the process of naming a compound or molecule. I. Ionic Compounds The name of the compound consists of the name of the metal followed by the ide form of the non-metal. Ex. NaCl sodium chloride Ca(C 2 H 3 O 2 ) 2 calcium acetate MgO magnesium oxide Practice: Name the following compounds. 1. CaO 4.. BaCl 2 2. Al 2 (CO 3 ) 3 5. Na(MnO 4 ) 3. (NH 4 ) 2 SO 4 6. FeS 1. Potassium bicarbonate 4. Ammonium nitrate 2. Zinc acetate 5. Zinc phosphate 3. Silver dichromate 6. Lithium chloride II. Compounds Having Metals with more than one Oxidation State The compound is written as normal with the oxidation number in Roman Numerals in parentheses after the name of the metal. Ex. FeCl 2 Iron (II) chloride Cl = -1 so then Fe = +2, written Iron (II) FeCl 3 Iron (III) chloride Cl = -1 so then Fe = +3, written Iron (III) CrO 2 Chromium (IV) oxide O = -2 so then Cr = +4, written Chromium (IV) CrO 3 Chromium (VI) oxide O = -2 so then Cr = +6, written Chromiun (VI) An alternate method uses the Latin and Greek names of the metals. Add ous to the lower charge and ic to the higher charge. We will not use this method, but most of the world does! Ex. FeCl 2 Ferrous chloride FeCl 3 Ferric chloride Reminders about Polyatomic Ions Rule: The prefix per- denotes the greatest number of oxygen (if more than two forms). The suffix ate denotes the most oxygen.*** The suffix ite denotes fewer oxygen. The prefix hypo- denotes the least number of oxygen. Ex. ClO 4 perchlorate ClO 3 chlorate ***the one we memorize ClO 2 chlorite ClO hypochlorite Practice: Name the following compounds. 1. Fe(OH) 3 4. Cr(C 2 H 3 O 2 ) 2 2. Cu 2 (SO 4 ) 5. FeS 3. Pb(NO 3 ) 2 6. Pb(SO 4 ) 1. Iron (III) oxide 4. Copper (II) hydroxide 2. Copper (II) iodide 5. Lead (II) dichromate 3. Iron (II) phosphate 6. Mercury (I) chloride
4 II. Binary Compounds containing Two Non-Metals The name consists of the non-metal that is further toward the left and bottom of the periodic table, followed by the ide form of the second non-metal. Compounds containing more than one of the non-metal elements can be distinguished by: Mono one Penta five Octa eight Di two Hexa six Nona nine Tri three Hepta seven Deca ten Tetra four Ex. CO CO 2 Carbon monoxide Carbon dioxide Practice: Name the following compounds. 1. PBr 3 4. SiO 2 2. CS 2 5. N 2 O 5 3. Cl 2 O 7 6. XeF 4 1. Dibromine tetraoxide 4. Tetrasulfur tetranitride 2. Diiodine tetraoxide 5. Sulfur hexafluoride 3. Phosphorous triiodide 6. Oxygen dibromide V. Binary Inorganic Compounds (Acids) Containing a hydrogen and an non-metal. Start with hydrogen then the ide form of the non-metal. When this type of compound is in an aqueous solution it will form an acid, then state hydro for the hydrogen and add the suffix ic to the non-metal. An acid is a molecular substance that when dissolved in water produces hydrogen ions (H + ). Ex. HCl(aq) hydrochloric acid H 2 S (aq) hydrosulfuric acid If the combination is hydrogen and a polyatomic ion change the ate of the polyatomic ion to ic. Ex. C 2 H 3 O 2 - acetate HC 2 H 3 O 2 acetic acid PO 4 3- phosphate H 3 PO 4 phosphoric acid VI. Ternary Compounds (Acids) Chlorine, nitrogen, sulfur, phophorus, and others form oxyacids. Oxyacids are ternary compounds with hydrogen and oxygen. If the acid has the most oxygen then it has the suffix ic. If the acid has fewer oxygen then it has the suffix ous. If the acid has the greatest number of oxygen it has the prefix per-. If the acid has the least number of oxygen it has the prefix hypo-. Ex. HClO 4 HClO 3 HClO 2 HClO Perchloric acid Chloric acid Chlorous acid Hypochlorous acid
5 Practice: Name the following compounds. 1. HI(aq) 4. H(C 2 H 3 O 2 )(aq) 2. HBr(aq) 5. HF(aq) 3. H(ClO 3 )(aq) 6. H(NO 2 )(aq) 1. Sulfurous acid 4. Nitric acid 2. Hydrochloric acid 5. Phosphoric acid 3. Hydrosulfuric acid 6. Chlorous acid VII. Hydrates Compounds that contain water molecules weakly bound in their crystals. When the compound loses the water molecules it is referred to as anhydrous. To name state the name of the binary compound and then list the number of water molecules attached. Ex. Copper (II) sulfate is a white powdery substance. When associated with water CuSO 4 5 H 2 O copper (II) sulfate pentahydrate is a blue crystal. Practice: Name the following compounds. 1. Na 2 CO 3 10 H 2 O 2. BaCl 2 2 H 2 O 3. CuSO 4 5 H 2 O 1. Magnesium sulfate heptahydrate 2. Ferric nitrate trihydrate
6 Name: Period: Date: Homework: Oxidation Numbers Determine the oxidation number for each of the elements in the following molecules and ions. 1. Ca(OH) 2 Ca= O= H= 11. Ba(BrO 3 ) 2 Ba= Br= O= 2. Bi(NO 3 ) 3 Bi= N= O= 12. NaAsO 2 Na= As= O= 3. Ca(ClO) 2 Ca= Cl= O= 13. Pb(Cr 2 O 7 ) Pb= Cr= O= 4. K(MnO 4 ) K= Mn= O= 14. Na(ClO 4 ) Na= Cl= O= 5. Na 2 (CrO 4 ) Na= Cr= O= 15. MnO 2 Mn= O= 6. Cu 2 (SO 4 ) Cu= S= O= 16. O 2 O= 7. Fe 2 O 3 Fe= O= 17. Al 2 (Cr 2 O 7 ) 3 Al= Cr= O= 8. Na(MnO 4 ) Na= Mn= O= 18. Mn(NO 3 ) 2 Mn= N= O= 9. Cl 2 Cl= 19. KClO K= Cl= O= 10. Sb 2 (SO 4 ) 3 Sb= S= O= 20. FeCO 3 Fe= C= O= 21. What is the oxidation number of chromium in K 2 Cr 2 O 7? (1) +12 (3) +3 (2) +2 (4) In which substance is the oxidation number of Cl equal to +l? (1) Cl 2 (3) AlCl 3 (2) Cl 2 O (4) HClO In which substance does hydrogen have an oxidation number of zero? (1) LiH (3) H 2 S (2) H 2 O (4)H In which compound does carbon have an oxidation state of -4? (1) CO (3) CCl (2) CO 2 (4) CH What is the oxidation number of carbon in Na(HCO 3 )? (1) 2 (3) 4 (2) +2 (4) +4
7 Write the name for the following ionic compounds. 26. Mg 3 N Ag 2 S 27. Ca 3 (PO 4 ) Fe(NO 3 ) Al 2 (SO 4 ) Ba(CO 3 ) 29. (NH 4 )Cl 34. Li 2 (C 2 O 4 ) 30. K 2 O 35. CuI 2 Write the formula for the following ionic compounds. 36. Calcium sulfide 41. Barium phosphate 37. Magnesium phosphide 42. Ammonium nitrite 38. Sodium sulfate 43. Aluminium chloride 39. Potassium bicarbonate 44. Cesium bromide 40. Zinc bromide 45. Potassium permanganate Write the names for the following metallic compounds. 46. CuCl 48. Fe 2 O HgO 49. Bi 2 O 3 Write the formula for the following metallic compounds. 50. Tin (IV) chloride 55. Mercury (I) nitride 51. Cobalt (II) fluoride 56. Iron (II) oxide 52. Chromium (II) sulfide 57. Copper (II) hydroxide 53. Lead (II) sulfide 58. Iron (III) nitrate 54. Tin (II) bromide 59. Copper (II) iodide Write the name for the following covalent compounds. 60. NO 65. N 2 O P 2 O S 2 Br PCl CS IF ClF CBr SO 3
8 Write the formula for the following covalent compounds. 70. Sulfur trioxide 75. Sulfur hexafluoride 71. Phosphorous trioxide 76. Carbon disulfide 72. Dinitrogen pentoxide 77. Dinitrogen trioxide 73. Oxygen dibromide 78. Phosphorous pentoxide 74. Tetrasulfur tetranitride 79. Carbon dioxide Write the names of the following acids. 80. HCl(aq) 85. HNO 2 (aq) 81. H 2 SO 4 (aq) 86. H 2 CO 3 (aq) 82. HClO 2 (aq) 87. H 3 PO 5 (aq) 83. HBr(aq) 88. H 3 PO 4 (aq) 84. H 2 S(aq) 89. HI(aq) Write the formula for the following acids. 90. Nitric acid 95. Hydrosulfuric acid 91. Hydrofluoric acid 96. Sulfurous acid 92. Hypoclhorous acid 97. Cyanic acid 94. Acetic acid 98. Perchloric acid Write the name of the following hydrates. 99. MgSO4 7 H 2 O 100. Ba(OH) 2 8 H 2 O 101. CaCl 2 2 H 2 O Write the formula for the following hydrates Sodium sulfate decahydrate 103. Potassium aluminum sulfate dodecahydrate 104. Sodium tetraborate decahydrate
9
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