1. M.I.T. C.P. CHEMISTRY

2. Ionic compounds are two or more elements that are held together by opposite charge attraction. Oxygen-8 Magnesium-12 8 (+) 10 (-) -2 Charge 12 (+) 10 (-) +2 Charge Metal Non-metal

3. Metals combine with non-metals. Metals loose electrons to non-metals. They attract because their charges will be opposite.

4. -3 -2 Most of the negative ions have a set negative charge Negative Single Ion Nonmetals

5. IIA IIIAVIAVAIVA 2e - 3p + 4p + LiBe B 5p + 6p + C How do you know the charge? +1 +2 +3 +4 - 4

6. IIA IIIAVIAVAIVA How do you know the charge? +1 +2+3 +4 - 4 2e - NOF 7p + 8p + 9p + 10p + Ne 8e - Na 11p + -3 -2 0

7. Writing Ionic Formulas It is easier to write the formula of an ionic compound from its name than the reverse. The oxidation number of the negative ion must be memorized in all cases. Refer to the table of polyatomic ions.

8. Binary Ionic Formulas Type 1 Compounds Compounds that contain metals with fixed oxidation numbers from column 1, 2 and 3.

9. N Elements with Fixed Oxidation Numbers LaHfTaReOsCeBaTl Pb BiPoAtRnIrPtAuHg YZrNbMoTcRuRbSrInSnSbTeIXeRhPdAgCd ScTiVCrMnFeKCaGaGeAsSeBrKrCoNiCuZn AlSiPSClArNaMg BCOFNeLiBe HHHe AcRfDbSgRhHsFrRaMt +1+2+3 1A 2A 8A 0-4-3-2 7A 6A5A4A3A W NdPmSmEuGdTbCePrYbLuDyHoErTm NpAmCmBkThPaNoLrCfEsFmMdUPu Click on element to see its oxidation number(s)

10. Naming Binary Ionic Compounds Type 1 Compounds Compounds that contain metals with fixed oxidation numbers from column 1, 2 and 3.

11. Type 1 Compounds First comes the positive metal (cation). Take the element name. Second is the anion. Take the element name and add “ide.”

12. Sample Problem Chemical Formula to Name

13. Naming Binary Ionic Compounds Type 1 Compounds NaCl Sodium Chloride KCl Potassium Chloride K 2 O Potassium Oxide

14. Writing Binary Ionic Formulas Type 1 Compounds Compounds that contain metals with fixed oxidation numbers from column 1, 2 and 3.

15. “G” Method Aluminum Chloride Step 1: Write down, in order, the correct symbols. Al Cl

16. Aluminum Chloride Step 2: Write each oxidation number above each symbol. Al Cl 3 1

17. “G” Method Aluminum Chloride Step 2: Crisscross the oxidation numbers as you bring them down as subscript numbers. Al Cl 3 1

18. “G” Method Aluminum Chloride Step 3: Reduce if necessary. Cl 3 Al 1

19. Sample Problem Name to Chemical Formula

20. “G” Method Calcium Chloride Step 1: Ca Cl

21. Calcium Chloride Step 2: Ca Cl 2 1

22. “G” Method Calcium Chloride Step 3: Cl 2 Ca 1

23. Binary Ionic Formulas Type 2 Compounds Compounds that contain a metal cation that can have more than one oxidation number.

24. +1 +2 +3 +1 +2 -3 -2 Transitional Metals have multiple valence numbers

25. Writing Binary Ionic Formulas Type 2 Compounds Compounds that contain a metal cation that can have more than one oxidation number.

26. Naming Binary Ionic Compounds Type 2 Compounds Write the names of the ions. Determine the charge on the positive ion. This charge is expressed as a “Roman Numeral” in parenthesis that immediately follows the name of the metal.

27. “G” Method Tin II Fluoride Step 1: Sn F

28. Tin II Fluoride Step 2: Sn F 2 1

29. “G” Method Tin II Fluoride Step 2: Sn F 2 1

30. “G” Method Tin II Fluoride Step 3: F Sn 1 2

31. Naming Binary Ionic Formulas Type 2 Compounds Compounds that contain a metal cation that can have more than one oxidation number.

32. aluminum chloride What is the Lowest Common Multiple “LCM” of 3 and 1. Do not worry about the sign(+/-) Example #1: Name to Formula Al Cl 3 2. Determine number of ions 1. Write symbols of elements Final Formula (Al ) x (Cl -1 ) y = 0 1 If there is only one atom the “1” is not shown +3 If there is no Roman Numeral, you need to know the fixed oxidation number of the positive ion. Next

33. Sample Problems Chemical Formula to Name

34. SAMPLE PROBLEM #1 SnF 2 Tin 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name Fluoride (II) Sn x (F -1 ) 2 = 0 X + 2(-1) = 0 X = +2

35. SAMPLE PROBLEM #2 Cu 2 S Copper 1.Write the names of the ions Sulfide (I) x 2X + (- 2) = 0 2X = +2 (Cu ) 2 S You must know the charge on the sulfide ion is -2 The sum of the positive and negative charges must equal zero. 2. Determine the charge of the positive ion -2 +2 +1 2 X = +1 Final Name

36. SAMPLE PROBLEM #2 Cu 2 S copper I’m not a polyatomic ion 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name sulfide (I) 2Cu x (S) -2 = 0 2X + (-2) = 0 X = +1

37. Binary Ionic Formulas Type 3 Compounds Compounds that contain polyatomic ions.

38. Ions with -1 charge perbromate BrO 4 -1 bromate BrO 3 -1 bromite BrO 2 -1 hypobromite BrO -1 perchlorate ClO 4 -1 chlorate ClO 3 -1 chlorite ClO 2 -1 hypochlorite ClO -1 periodate IO 4 -1 iodate IO 3 -1 iodite IO 2 -1 hypoiodite IO -1 nitrateNO 3 -1 nitriteNO 2 -1 hydroxideOH -1 cyanideCN -1 acetateC 2 H 3 O 2 -1 PermanganateMnO 4 -1 bicarbonateHCO 3 -1 Ions with a -2 Charge carbonateCO 3 -2 sulfateSO 4 -2 sulfite SO 3 -2 chromate CrO 4 -2 dichromate Cr 2 O 7 -2 oxalate C 2 O 4 -2 Ions with a -3 Charge phosphate PO 4 -3 phosphite PO 3 -3 arsenate AsO 4 -3 Ions with +1 charge ammonium ion NH 4 +1 Polyatomic ions are mostly made of two non-metals. Polyatomic Ions

39. Ions with -1 charge perbromate BrO 4 -1 bromate BrO 3 -1 bromite BrO 2 -1 hypobromite BrO -1 perchlorate ClO 4 -1 chlorate ClO 3 -1 chlorite ClO 2 -1 hypochlorite ClO -1 periodate IO 4 -1 iodate IO 3 -1 iodite IO 2 -1 hypoiodite IO -1 These polyatomic ions match the charge of the single element

40. -2 These polyatomic ions match the charge of the single element Ions with a -2 Charge sulfateSO 4 -2 sulfite SO 3 -2

41. These polyatomic ions match the charge of the single element Ions with a -3 Charge phosphate PO 4 -3 phosphite PO 3 -3 -3

42. Writing Binary Ionic Formulas Type 3 Compounds Compounds that contain polyatomic ions.

43. “G” Method Carbon Sulfate Step 1: C SO 4

44. Carbon Sulfate Step 2: C SO 4 4 2

45. “G” Method Carbon Sulfate Step 2: C SO 4 4 2 ( )

46. “G” Method Carbon Sulfate Step 3: (SO 4 ) 4 C 2 2

47. N Oxidation Numbers (most common) LaHfTaReOsCeBaTl Pb BiPoAtRnIrPtAuHg YZrNbMoTcRuRbSrInSnSbTeIXeRhPdAgCd ScTiVCrMnFeKCaGaGeAsSeBrKrCoNiCuZn AlSiPSClArNaMg BCOFNeLiBe HHHe AcRfDbSgRhHsFrRaMt +1+2+3 1A 2A 8A 0-4-3-2 7A 6A5A4A3A W NdPmSmEuGdTbCePrYbLuDyHoErTm NpAmCmBkThPaNoLrCfEsFmMdUPu Click on element to see its oxidation number(s) +1+2 +3+2+4

48. Naming Binary Ionic Formulas Type 3 Compounds Compounds that contain polyatomic ions.

49. Naming Ionic Compounds CaSO 4 Calcium Sulfate Step 1: If the positive ion has a fixed oxidation number, then no Roman Numeral is used. Step 2: No Roman Numeral

50. The positive ion (usually a metal) is named first while the negative ion (a non-metal or a polyatomic ion) is named last. CuSO 4 Copper Sulfate Step 1: Write the Name of the Ions

51. The charge on the negative ion is used to determine the charge on the positive ion. In-order for the total oxidation state to be zero, the total positive charge must equal the total negative charge. A simple algebraic equation can be used to determine the charge on a single metal ion. CuSO 4 Cu ? SO 4 -2 x +(-2)=0 X = 2 Copper Sulfate Step 2: Determine the Charge of the Positive Ion

52. Naming Ionic Compounds This charge is expressed as a “Roman Numeral” in parenthesis that immediately follows the name of the metal. CuSO 4 Cu ? SO 4 -2 x +(-2)=0 X = 2 Copper (II) Sulfate

53. Naming Ionic Compounds Step 1: Cu 2 SO 4 Copper Sulfate

54. Step 2 Cu 2 SO 4 Cu 2 +x SO 4 -2 2x +(-2)=0 x = 1 Copper Sulfate

55. Naming Ionic Compounds Step 3 Cu 2 SO 4 Cu 2 +x SO 4 -2 2x +(-2)=0 x = 1 Copper (I) Sulfate

56. Sample Problems Chemical Formula to Name

57. SAMPLE PROBLEM #1 CuSO 3 copper I’m a polyatomic ion 1.Write the names of the ions Final Name sulfite (II) x X + (- 2) = 0 X = +2 Cu SO 3 = 0 You must know the charge on the sulfite ion is -2 The sum of the positive and negative charges must equal zero 2. Determine the charge of the positive ion -2 +2 Next +2

58. SAMPLE PROBLEM #2 KMnO 4 potassium I’m a polyatomic ion 1.Write the names of the ions Final Name permanganate If the positive ion has a fixed charge, you are finished.

59. SAMPLE PROBLEM #3 NH 4 NO 3 ammonium I’m a polyatomic ion 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name nitrate If the positive ion has a fixed charge, you are finished.

60. SAMPLE PROBLEM #4 Ba(ClO 4 ) 2 barium I’m a polyatomic ion 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name perchlorate If the positive ion has a fixed charge, you are finished.

61. SAMPLE PROBLEM #5 Na 2 Cr 2 O 7 sodium I’m a polyatomic ion 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name dichromate (I) 2(Na x )(Cr 2 O 7 ) -2 = 0 2X + (-2) = 0 X = +1 If the positive ion has a fixed charge, it is not shown

62. SAMPLE PROBLEM #6 LiCN lithium I’m a polyatomic ion 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name cyanide If the positive ion has a fixed charge, you are finished.

63. Binary Molecular Formulas Type 4 Covalent Compounds Compounds that contain two non-metals.

64. Prefixes denote the number of atoms present. 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa

65. “G” Method Carbon Tetrachloride Step 1: C Cl

66. Carbon Tetrachloride Step 2: C Cl 1 4

67. “G” Method Carbon Tetrachloride Step 3: C 1 4 Cl

68. Challenge Problems Chemical Formula to Name

69. Challenge Problem #1 Fe(NO 3 ) 3 Choose the correct name for the compound 1. Iron trinitrate 2. iron(I) nitrate 3. iron(III) nitrite 4. iron(III) nitrate 5. none of the above next problem Polyatomic IonsPeriodic Chart

70. Challenge Problem #2 sodium chlorite Choose the correct formula for the compound 1. NaCl 2. NaClO 3. NaClO 2 4. Na(ClO) 2 5. none of the above Prefixes Periodic Chart

71. POLYATOMIC IONS Ions with -1 charge perbromate BrO 4 -1 bromate BrO 3 -1 bromite BrO 2 -1 hypobromite BrO -1 perchlorate ClO 4 -1 chlorate ClO 3 -1 chlorite ClO 2 -1 hypochlorite ClO -1 periodate IO 4 -1 iodate IO 3 -1 iodite IO 2 -1 hypoiodite IO -1 nitrate NO 3 -1 nitrite NO 2 -1 hydroxide OH -1 cyanide CN -1 thiocyanate SCN -1 acetate C 2 H 3 O 2 -1 Permanganate MnO 4 -1 bicarbonate HCO 3 -1 Ions with a -2 Charge carbonate CO 3 -2 phthalate C 8 H 4 O 4 -2 sulfate SO 4 -2 sulfite SO 3 -2 chromate CrO 4 -2 dichromate Cr 2 O 7 -2 oxalate C 2 O 4 -2 peroxide O 2 -2 Ions with a -3 Charge phosphate PO 4 -3 phosphite PO 3 -3 arsenate AsO 4 -3 Ions with +1 charge ammonium ion NH 4 +1 return

72. N Oxidation Numbers (most common) LaHfTaReOsCeBaTl Pb BiPoAtRnIrPtAuHg YZrNbMoTcRuRbSrInSnSbTeIXeRhPdAgCd ScTiVCrMnFeKCaGaGeAsSeBrKrCoNiCuZn AlSiPSClArNaMg BCOFNeLiBe HHHe AcRfDbSgRhHsFrRaMt +1+2+3 1A 2A 8A 0-4-3-2 7A 6A5A4A3A W NdPmSmEuGdTbCePrYbLuDyHoErTm NpAmCmBkThPaNoLrCfEsFmMdUPu Click on element to see its oxidation number(s) +1+2 +3+2+4 return

73. Lab: Molecular Models

74. Linear

75. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear Bent Triangular Planar Triangular Pyramidal Tetrahedral

76. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear2 Bent Triangular Planar Triangular Pyramidal Tetrahedral

77. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20 Bent Triangular Planar Triangular Pyramidal Tetrahedral

78. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent Triangular Planar Triangular Pyramidal Tetrahedral

79. Bent

80. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent2 Triangular Planar Triangular Pyramidal Tetrahedral

81. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21 Triangular Planar Triangular Pyramidal Tetrahedral

82. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21AB 2 E Bent Triangular Planar Triangular Pyramidal Tetrahedral

83. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21AB 2 E Bent2 Triangular Planar Triangular Pyramidal Tetrahedral

84. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21AB 2 E Bent22 Triangular Planar Triangular Pyramidal Tetrahedral

85. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21AB 2 E Bent22AB 2 E 2 Triangular Planar Triangular Pyramidal Tetrahedral

86. Trigonal Planar

87. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21AB 2 E Bent22AB 2 E 2 Triangular Planar 30AB 3 Triangular Pyramidal Tetrahedral

88. Trigonal Pyramidal

89. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21AB 2 E Bent22AB 2 E 2 Triangular Planar 30AB 3 Triangular Pyramidal 31AB 3 E Tetrahedral

91. VSEPR Molecular Geometry Molecular Shape Diagram# of Attached Atoms Lone Electron Pairs Type of Molecule Linear20AB 2 Bent21AB 2 E Bent22AB 2 E 2 Triangular Planar 30AB 3 Triangular Pyramidal 31AB 3 E Tetrahedral40AB 4

92. Square Planar

93. VSEPR Theory V alence S hell E lectron P air R epulsion T heory Based on the number of high electron densities around a central atom. Can be used to predict structures of molecules or ions that contain only non-metals. Does fail in some cases.

94. VSEPR Rules & Examples Draw the Lewis dot diagram for the molecule or ion. Step 1 BeCl 2 NH 3 CH 4

95. Count the total number of regions of high electron density (bonding and unshared electron pairs) around the central atom. Step 2 Double and triple bonds count as ONE REGION OF HIGH ELECTRON DENSITY. An unpaired electron counts as ONE REGION OF HIGH ELECTRON DENSITY.

96. Step 2 BeCl 2 NH 3 CH 4 2 44

97. VSEPR Rules & Examples Identify the molecular structure based on the positions of the ATOMS ! STEP 3

98. Step 3 BeCl 2 NH 3 CH 4 Linear Triangular Pyramidal Tetrahedral

99. Resonance Structures When more than one Lewis structure can be drawn for a molecule or ion. Nitrate Polyatomic Ion NO3-

100. Resonance Hybrid Structure We can draw a Lewis-like structure that provides a better description of the actual character of the nitrate ion by blending the resonance structures into a single resonance hybrid. Nitrate Polyatomic Ion NO3-