1. Covalent Bonding Chap. 9

2. I.Why does it form?

3. A.Octet rule An atom will gain, lose, or share electrons in order to get a full set

4. I.Why does it form? A.Octet rule B.Stability/Minimum energy

5. I.Why does it form? II. What is a molecule? Molecule = covalent compound

6. I.Why does it form? II. What is a molecule? A.Non-metal with a non-metal

7. I.Why does it form? II. What is a molecule? A.Non-metal with a non-metal B.Some molecules are diatomic Molecules made of two of the same atom

8. I.Why does it form? II. What is a molecule? A.Non-metal with a non-metal B.Some molecules are diatomic C.Properties

9. 1. Often are gases or liquids Properties of Covalent Compounds

10. 1. Often are gases or liquids 2. Tend to have lower M.P. Properties of Covalent Compounds

11. 1. Often are gases or liquids 2. Tend to have lower M.P. 3. Often are soft Properties of Covalent Compounds

12. 1. Often are gases or liquids 2. Tend to have lower M.P. 3. Often are soft 4. Many are non-electrolytes Properties of Covalent Compounds

13. III. Representing Molecules Lewis structure uses dots and dashes to represent electrons and bonds

14. III. Representing Molecules IV. Covalent Bond types

15. III. Representing Molecules IV. Covalent Bond types A.Single bond Bond made of one pair of shared electrons

16. III. Representing Molecules IV. Covalent Bond types A.Single bond B.Double bond Bond made of two pairs of shared electrons

17. III. Representing Molecules IV. Covalent Bond types A.Single bond B.Double bond C.Triple bond Bond made of three pairs of shared electrons

18. III. Representing Molecules IV. Covalent Bond types A.Single bond B.Double bond C.Triple bond D.Quadruple bond?

19. III. Representing Molecules IV. Covalent Bond types V. Bond strength Bond energy measures the bond strength.

20. III. Representing Molecules IV. Covalent Bond types V. Bond strength A.The longer the bond the ______ the bond energy

21. III. Representing Molecules IV. Covalent Bond types V. Bond strength A.The longer the bond the ______ the bond energy B.Double bonds require _____ energy to break than single bonds.

22. Bond energy example H 2 + Cl 2 2HCl H-H436 kJ Cl-Cl242 kJ HCl431 kJ What is the energy change for this reaction? Is it exothermic?

23. VI. Naming Covalent Compounds

24. A.Binary Inorganic Molecules

25. Rules for Naming Covalent Compounds

26. 1. Name the first...

27. Rules for Naming Covalent Compounds 1. Name the first... 2. Name the second with... 1. Name the first... 2. Name the second with...

28. Rules for Naming Covalent Compounds 1. Name the first... 2. Name the second with... 3. Use prefixes to tell... 1. Name the first... 2. Name the second with... 3. Use prefixes to tell...

29. Rules for Naming Covalent Compounds 1. Name the first... 2. Name the second with... 3. Use prefixes to tell... 4. Never begin name with... 1. Name the first... 2. Name the second with... 3. Use prefixes to tell... 4. Never begin name with...

30. Prefixes for Numbers of Atoms

31. 1. mono-

32. Prefixes for Numbers of Atoms 1. mono- 2. di- 1. mono- 2. di-

33. Prefixes for Numbers of Atoms 1. mono- 2. di- 3. tri- 1. mono- 2. di- 3. tri-

34. Prefixes for Numbers of Atoms 1. mono- 2. di- 3. tri- 4. tetra- 1. mono- 2. di- 3. tri- 4. tetra-

35. Prefixes for Numbers of Atoms 1. mono- 2. di- 3. tri- 4. tetra- 5. penta- 1. mono- 2. di- 3. tri- 4. tetra- 5. penta-

36. Prefixes for Numbers of Atoms 1. mono-6. hexa- 2. di- 3. tri- 4. tetra- 5. penta- 1. mono-6. hexa- 2. di- 3. tri- 4. tetra- 5. penta-

37. Prefixes for Numbers of Atoms 1. mono-6. hexa- 2. di-7. hepta- 3. tri- 4. tetra- 5. penta- 1. mono-6. hexa- 2. di-7. hepta- 3. tri- 4. tetra- 5. penta-

38. Prefixes for Numbers of Atoms 1. mono-6. hexa- 2. di-7. hepta- 3. tri-8. octa- 4. tetra- 5. penta- 1. mono-6. hexa- 2. di-7. hepta- 3. tri-8. octa- 4. tetra- 5. penta-

39. Prefixes for Numbers of Atoms 1. mono-6. hexa- 2. di-7. hepta- 3. tri-8. octa- 4. tetra-9. nona- 5. penta- 1. mono-6. hexa- 2. di-7. hepta- 3. tri-8. octa- 4. tetra-9. nona- 5. penta-

40. Prefixes for Numbers of Atoms 1. mono-6. hexa- 2. di-7. hepta- 3. tri-8. octa- 4. tetra-9. nona- 5. penta-10. deca- 1. mono-6. hexa- 2. di-7. hepta- 3. tri-8. octa- 4. tetra-9. nona- 5. penta-10. deca-

41. Rules for Naming Covalent Compounds 1. Name the first... 2. Name the second with... 3. Use prefixes to tell... 4. Never begin name with... 1. Name the first... 2. Name the second with... 3. Use prefixes to tell... 4. Never begin name with...

42. VI. Naming Covalent Compounds A.Binary Inorganic Molecules B.Common Names

43. Covalent compounds with carbon VI. Naming Covalent Compounds A.Binary Inorganic Molecules B.Common Names C.Organic Molecules

44. Names for organic hydrocarbons

45. CH 4 methane

46. Names for organic hydrocarbons CH 4 methane C 2 H 6 ethane CH 4 methane C 2 H 6 ethane

47. Names for organic hydrocarbons CH 4 methane C 2 H 6 ethane C 3 H 8 propane CH 4 methane C 2 H 6 ethane C 3 H 8 propane

48. Names for organic hydrocarbons CH 4 methane C 2 H 6 ethane C 3 H 8 propane C 4 H 10 butane CH 4 methane C 2 H 6 ethane C 3 H 8 propane C 4 H 10 butane

49. Names for organic hydrocarbons CH 4 methane C 2 H 6 ethane C 3 H 8 propane C 4 H 10 butane C 5 H 12 pentane CH 4 methane C 2 H 6 ethane C 3 H 8 propane C 4 H 10 butane C 5 H 12 pentane

50. Names for organic hydrocarbons C 6 H 14 C 7 H 16 C 8 H 18 C 9 H 20 C 10 H 22 C 6 H 14 C 7 H 16 C 8 H 18 C 9 H 20 C 10 H 22

51. Names for organic hydrocarbons C 6 H 14 hexane C 7 H 16 C 8 H 18 C 9 H 20 C 10 H 22 C 6 H 14 hexane C 7 H 16 C 8 H 18 C 9 H 20 C 10 H 22

52. Names for organic hydrocarbons C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 C 9 H 20 C 10 H 22 C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 C 9 H 20 C 10 H 22

53. Names for organic hydrocarbons C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 octane C 9 H 20 C 10 H 22 C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 octane C 9 H 20 C 10 H 22

54. Names for organic hydrocarbons C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 octane C 9 H 20 nonane C 10 H 22 C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 octane C 9 H 20 nonane C 10 H 22

55. Names for organic hydrocarbons C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 octane C 9 H 20 nonane C 10 H 22 decane C 6 H 14 hexane C 7 H 16 heptane C 8 H 18 octane C 9 H 20 nonane C 10 H 22 decane

56. Self Check 1 PF 3 SF 6 CS 2 SiH 4 Write the names for these compounds

57. Self Check 2 Carbon tetrachloride Diphosphorus decachloride Write the formulas for these compounds

58. Acids are hydrogen-donating compounds VI. Naming Covalent Compounds D.Naming acids

59. Acids composed of H + ion and a monatomic anion. VI. Naming Covalent Compounds D.Naming acids 1. Binary Acids

60. Rules for Naming Acids Anion Name Acid Name chloride Hydrochloric acid Formula

61. Rules for Naming Acids Anion Name Acid Name chloride fluoride chloride fluoride Hydrochloric acid Hydrofluoric acid Hydrochloric acid Hydrofluoric acid Formula

62. Rules for Naming Acids Anion Name Acid Name chloride fluoride bromide chloride fluoride bromide Hydrochloric acid Hydrofluoric acid ?? Hydrochloric acid Hydrofluoric acid ?? Formula

63. Rules for Naming Acids Anion Name Acid Name chloride fluoride bromide chloride fluoride bromide Hydrochloric acid Hydrofluoric acid Hydrobromic acid Hydrochloric acid Hydrofluoric acid Hydrobromic acid Formula

64. Rules for Naming Acids Anion Name Acid Name chloride fluoride bromide ____-ide chloride fluoride bromide ____-ide Hydrochloric acid Hydrofluoric acid Hydrobromic acid Hydro____ic acid Hydrochloric acid Hydrofluoric acid Hydrobromic acid Hydro____ic acid Formula

65. VI. Naming Covalent Compounds D.Naming acids 1. Binary Acids 2. Oxyacids Acids composed of H + ion and a polyatomic anion containing oxygen.

66. Rules for Naming Oxyacids Anion Name Acid Name chlorate Chloric acid Formula

67. Rules for Naming Oxyacids Anion Name Acid Name chlorate nitrate chlorate nitrate Chloric acid Nitric acid Chloric acid Nitric acid Formula

68. Rules for Naming Oxyacids Anion Name Acid Name chlorate nitrate sulfate chlorate nitrate sulfate Chloric acid Nitric acid ?? Chloric acid Nitric acid ?? Formula

69. Rules for Naming Oxyacids Anion Name Acid Name chlorate nitrate Sulfate chlorate nitrate Sulfate Chloric acid Nitric acid Sulfuric acid Chloric acid Nitric acid Sulfuric acid Formula

70. Rules for Naming Oxyacids Anion Name Acid Name chlorate nitrate Sulfate ______ate chlorate nitrate Sulfate ______ate Chloric acid Nitric acid Sulfuric acid ______ic acid Chloric acid Nitric acid Sulfuric acid ______ic acid Formula

71. Rules for Naming Oxyacids Anion Name Acid Name chlorite Chlorous acid Formula

72. Rules for Naming Oxyacids Anion Name Acid Name chlorite nitrite chlorite nitrite Chlorous acid Nitrous acid Chlorous acid Nitrous acid Formula

73. Rules for Naming Oxyacids Anion Name Acid Name chlorite nitrite sulfite chlorite nitrite sulfite Chlorous acid Nitrous acid ?? Chlorous acid Nitrous acid ?? Formula

74. Rules for Naming Oxyacids Anion Name Acid Name chlorite nitrite sulfite chlorite nitrite sulfite Chlorous acid Nitrous acid Sulfurous acid Chlorous acid Nitrous acid Sulfurous acid Formula

75. Rules for Naming Oxyacids Anion Name Acid Name chlorite nitrite sulfite ____ite chlorite nitrite sulfite ____ite Chlorous acid Nitrous acid Sulfurous acid ______ous acid Chlorous acid Nitrous acid Sulfurous acid ______ous acid Formula

76. Self Check 3 Carbonic acid Phosphoric acid Acetic acid Write the formulas for these compounds

77. VII. Structural Formulas A Lewis structure shows which atoms are bonded to which.

78. Valence electrons = outermost electrons. VII. Structural Formulas A.Valence electrons important

79. Pair of electrons shared between two elements. VII. Structural Formulas A.Valence electrons important 1. Bonding Electrons

80. Pair of electrons not being shared. VII. Structural Formulas A.Valence electrons important 1. Bonding Electrons 2. Lone pairs

81. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure

82. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure 1. for molecules

83. Rules for Lewis Structures 1. Determine the total...

84. Rules for Lewis Structures 1. Determine the total... 2. Join all elements with...

85. Rules for Lewis Structures 1. Determine the total... 2. Join all elements with... 3. Arrange remaining...

86. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure 1. for molecules 2. for molecules with multiple bonds

87. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure 1. for molecules 2. for molecules with multiple bonds 3. for ions

88. Self Check 4 CH 3 Cl CS 2 Phosphorus trifluoride Dichlorine monoxide Draw a Lewis structure for:

89. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure 1. for molecules 2. for molecules with multiple bonds 3. for ions 4. resonance structures

90. Concept that a molecule is described by more than one structure Resonance

91. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure C.Exceptions

92. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure C.Exceptions 1. odd number of electrons

93. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure C.Exceptions 1. odd number of electrons 2. less than an octet

94. VII. Structural Formulas A.Valence electrons important B.Drawing a Lewis structure C.Exceptions 1. odd number of electrons 2. less than an octet 3. more than an octet

95. VIII. Molecular Shape

96. A.VSEPR Theory Valence shell electron pair repulsion theory: electrons are placed at maximum distances from other electrons

97. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes

98. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes 1. Linear (BeCl 2 )

99. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes 1. Linear (BeCl 2 ) 2. Trigonal planar (BF 3 )

100. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes 1. Linear (BeCl 2 ) 2. Trigonal planar (BF 3 ) 3. Tetrahedral (CH 4 )

101. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes 1. Linear (BeCl 2 ) 2. Trigonal planar (BF 3 ) 3. Tetrahedral (CH 4 ) a. trigonal pyramidal (NH 3 )

102. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes 1. Linear (BeCl 2 ) 2. Trigonal planar (BF 3 ) 3. Tetrahedral (CH 4 ) a. trigonal pyramidal b. bent

103. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes 1. Linear (BeCl 2 ) 2. Trigonal planar (BF 3 ) 3. Tetrahedral (CH 4 ) 4. Trigonal bipyramidal

104. VIII. Molecular Shape A.VSEPR Theory B.Molecular Shapes 1. Linear (BeCl 2 ) 2. Trigonal planar (BF 3 ) 3. Tetrahedral (CH 4 ) 4. Trigonal bipyramidal 5. Octahedral

105. IX. Polarity

106. A.When is a bond polar? Polar bonds occur when electrons are shared unequally.

107. Bond types ElectronegativityBond DifferenceType

108. Bond types ElectronegativityBond DifferenceType 0.0 – 0.4non-polar covalent

109. Bond types ElectronegativityBond DifferenceType 0.0 – 0.4non-polar covalent 0.5 – 1.9polar covalent

110. Bond types ElectronegativityBond DifferenceType 0.0 – 0.4non-polar covalent 0.5 – 1.9polar covalent 1.9 -ionic

111. “COVALENT” Electronegativity Difference 0.51.01.52.02.53.03.5 Bond types

112. IX. Polarity A.When is a bond polar? B.When is a molecule polar? Polar molecules contain polar bonds and are NOT symmetrical.

114. Self Check 5 Are the bonds in ammonia (NH 3 ) polar? Is the molecule polar?

116. The End