2. A. Electronegativity - The ability of an atom to attract electrons to itself in a bond 1.Periodic Trends (link to size) Metals – Low Electronegativity Non- Metals – High Electroneg The smaller the atom, the higher the electronegativity Types of Bonds

3. a.Molecular Compounds (non-metals) Sharing of electrons Covalent or polar covalent bonds Ex: H 2 b. Ionic Compounds (metal + non-metal) Exchange (stealing) of electrons Ex: NaCl Types of Bonds

7. 3. Types of bonds Electronegatvity Difference Example:Na-F Types of Bonds

8. Are the following bonds ionic, polar covalent or covalent? Ba – BrC – N Be – FB – H O – HBe – Cl P – HC – H O – O Types of Bonds

9. Ionic – Electron is completely removed from one atom and goes to another a. Metal – Low e-neg (loses e-) b. Non-metal – high e-neg (gains e-) Ionic

12. IAIIAIIIAIVAVAVIAVIIA Hydride H - Lithium Li + Beryllium Be 2+ Carbide C 4- Nitride N 3- Oxide O 2- Fluoride F - Sodium Na + Magnesium Mg 2+ Aluminum Al 3+ Phosphide P 3- Sulfide S 2- Chloride Cl - Potassium K + Calcium Ca 2+ Selenide Se 2- Bromide Br - Rubidium Rb + Strontium Sr 2+ Telluride Te 2- Iodide I - Cesium Cs + Barium Ba 2+ Common Charges

13. Complete the following chart: FormulaLewis Dot K and I Sr and F Ba and Cl Sr and N Ba and O

15. Complete the following chart: FormulaLewis Dot K and S Al and O Na and Br Ca and O

16. 1.Not Separate molecules 2.Crystal Lattice – Regular 3D pattern in an ionic solid Ionic Solids

18. at lattice pointsions at lattice points

19. 1.Water (molecule) dissolves salt (ionic crystal): Ions in Water

21. Molecules

22. Many ionic compounds are called salts CaCl 2 Calcium Chloride (Quik-Joe) NaHCO 3 Sodium bicarbonate(Baking soda) NaF Sodium Fluoride (toothpaste) CaCO 3 Calcium Carbonate(Chalk, antacid) NaOH Sodium Hydroxide (Drano) MgSO 4 Magnesium Sulfate(Epsom Salts) All big clumps (crystals) of Ions Other Salts

23. Group of atoms held together by covalent and polar covalent bonds (SHARING) Usually composed of non-metals Stronger than Ionic bonds Separate (discrete) groups of atoms What is a Molecule?

25. A. Single Bonds (LD and Stick) CH 4 H2OH2O (bonded versus lone pairs) Old School Lewis Dots

26. The Lone Pear(Pair) rides again!

27. N and H P and F Cl and O NH 2 CH 3 Old School Lewis Dots

28. You try: As and H N and Br CH 3 CH 2 OH NH 2 CH 2 SiCl 3 CH 3 OCH 3 Old School Lewis Dots

29. As and Cl C and Br CH 3 CH 2 NH 2 CH 3 OCH 2 CH 3

30. B. Multiple Bonds CO 2 C 2 H 2 Old School Lewis Dots

31. You Try: HCN N 2 Al N O 2 Old School Lewis Dots

32. Rules 1. Sum all valence electrons, including charges 2. Single Bonds 3. Outer atoms get an octet except H 4. Center gets rest even if it violates the octet 5. Double/triple bonds if center atom still does not have an octet Lewis Dots

33. NH 3 NCl 3 SF 6 Br 2 O ClF 5 Lewis Dots

34. You try: SF 4 KrF 4 Cl 2 O ClF 3 H 2 SO 4

35. Warm-Up: CH 3 CH 2 NH 2 SeF 4 KrCl 4 H 2 O 2 BaCl 2 (this is an ionic cmpd)

36. CO 2 HCN CN - ICl 4 - NO + Lewis Dots

37. CO 3 2- H 3 O + NH 4 + PO 4 3- SO 2

38. Hydrogenonly makes one bond Gr I, II and III Especially if with a halogen BeCl 2 BCl 3 AlCl 3 Less Than an Octet

39. Non-Metals starting with P More Than an Octet PSClAr AsSeBrKr TeIXe

40. PCl 5

41. Warm-Up:O 3 Definition – When a molecule can exist in more than one arrangement of electrons 1. Atoms don’t move 2. Only the electrons (double bonds) move 3. Also called “delocalized bonding” Resonance Structures

42. Si 2 H 4 AsO 4 3- CS 3 2- H 3 S + PH 4 +

43. SPECIAL NOTE: Oxygen rarely makes three bonds for resonance structures. Those structures are not common. Resonance Structures

44. PO 3 - HSO 3 +

45. Examples 1. NO 2 -, CO 3 2-, CHO 2 -, HNO 3 2. Which needs resonance, SO 3 or SO 3 2- Resonance Structures

46. Valence Shell Electron Pair Repulsion Theory (VSEPR) VSEPR – Valence electron pairs on the central atom push as far apart as possible. Shapes of Molecules

48. 1. Linear (180 o ) BeH 2 CO 2 Shapes of Molecules

50. 2. Trigonal Planar (120 o ) NO 3 - Shapes of Molecules

52. 3. Tetrahedral (109.5 o ) CH 4 Shapes of Molecules

56. 4. Trigonal Pyramidal (~107 o ) NH 3 Shapes of Molecules

58. 5. Bent (Type I, ~104.5 o ) H 2 O Shapes of Molecules

60. O HH

62. Bent (Type II, 120 o ) SO 2

63. Atoms are bent Bond angle = 120 o

64. 6. Trigonal Bipyramid (120 o, 90 o ) PCl 5 Shapes of Molecules

66. 7. Octahedral (90 o ) SF 6 Shapes of Molecules

68. DRAW LEWIS DOT STRUCTURES AND PREDICT THE BOND ANGLES FOR: PH 3 GeO 2 PCl 5 NCl 3 H 2 SSiH 4 CF 4 SO 3 2- SeCl 6 SO 3

69. Ex: All single bonds: PH 3 H 2 SSiH 4 SeCl 6 AsF 5 BeCl 2 CH 3 FHFBF 3 Shapes of Molecules

70. Ex: Multiple Bonds: N 2 HCN CO 2 H 2 CO Shapes of Molecules

71. SO 2 2+ SO 2 2- SO 2 SO 3 SF 6

72. Shapes of Molecules

73. 1. Examples: BeH 2 H2OH2O BH 3 NH 3 2. There is no relationship between formula and shape Shapes and Formula?

74. PO 2 - PO 3 - PO 3 3- PO 4 3- XeF 4

78. Household Molecules H 2 O HCl NH 3 H 2 SO 4

79. 1. Polar molecule – Overall, the electrons are attracted more to one end of an entire molecule 2. Non-Polar Molecule – The electrons are spread out evenly over the entire molecule  -/  + Partial (not full) charges Polar Molecules

80. H 2 H 2 O CH 4 H 2 CO (C is the center)

81. H 2 H 2 O CH 4 H 2 CO

82. BeCl 2 NH 3 CO 2 CSO HCN (triple bond)

84. CCl 4 CH 3 Cl CH 2 Cl 2 CHCl 3 HBeCl HBr

85. CH 3 ClCH 2 Cl 2 CHCl 3 HBeClHBr Polar Molecules

86. Lewis DotShapePolar or Non- polar molecule? H2OH2O NH 3 CH 3 Cl CH 3 CH 2 OH SO 2

87. Hydrogen Bonding a. Water Beading b. SurfaceTension c. Ice d. DNA e. Miscibility (NH 3, ethanol) f. Immiscibility (Water and Oil)

88. Water Beading

90. Surface Tension

92. Ice

96. Molecules Boiling Point Generally increases with increasing molar mass H 2 O unusually high - H-bonding

97. DNA

98. DNA is TWO molecules that are hydrogen bonded (like a zipper)

99. DNA Human Genome Project

100. DNA in one cell = 1 meter DNA in all your cells = 93,000,000 miles

101. Miscibility “Like dissolves like.” Polar dissolves Polar Water, ammonia

102. Miscibility

106. Water, alcohol

109. Miscibility Water, alcohol

110. Miscibility Non-Polar dissolves Non-Polar oil paint, thinner

112. Miscibility

113. Would acetone (shown below) dissolve in water? Acetone :O: || CH 3 CCH 3

114. Molecules London Dispersion Forces Very weak force Caused by temporary imbalances in electrons

115. Molecules London Forces: Inorganic Molecules More electrons, more chance for temporary dipole Boiling Point Table HalogenMolar Mass BP( o C)Noble Gas Atomic Mass BP( o C) F 2 (g)38.0-188He4.0-268 Cl 2 (g)71.0-35Ne20.2-246 Br 2 (l)159.859Ar39.9-186 I 2 (s)253.8185Kr83.8-152

116. Consider the following molecules: Te 2 S 2 O 2 Se 2 a.Rank them from weakest to strongest London forces b.Which should have the highest boiling point? Which should have the lowest? c.Would it take more energy to melt a sample of carbon or silicon?

117. Molecules London Forces: Organic Compounds The longer the carbon chain, the higher the London Dispersion Forces (the higher the melting point and boiling point) BP( o C) CH 4 -161.6 C 2 H 6 -88.63 C 3 H 8 -42.07 C 4 H 10 -0.5

118. Which should have a higher boiling point: C 6 H 14 or C 12 H 26

119. Using you knowledge of “like dissolves like”, explain the following trends in solubility. AlcoholSolubility in H 2 O (mol/100 g H 2 O at 20 o C) CH 3 OH∞ CH 3 CH 2 OH∞ CH 3 CH 2 CH 2 OH∞ CH 3 CH 2 CH 2 CH 2 OH0.11 CH 3 CH 2 CH 2 CH 2 CH 2 OH0.030 CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 OH0.0058 CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 CH 2 OH0.0008 Explain the following trends in solubility in water

121. Emulsifying agents – Mayonaise – Soap

123. The Key to the Universe

124. You Try: CCl 4 NO 3 - CH 3 ClH 2 CO CH 2 Cl 2 H 2 S Polar Molecules

125. KrCl 4 Si 2 H 4 BNCH 3 SiH 2 PH 2 SiS 2 H 2 SO 4 O HOSOH O

126. 9.(c) Sc 2+ (d) I 2- (e) As 2- 15. Rb + Ba 2+ Te 2- N 3- 16. Al 3+, Mg 2+, Na +, F -, O 2-, N 3- 20.RbFRb 2 TeRb 3 P MgF 2 MgTeMg 3 P 2 CrF 3 Cr 2 Te 3 CrP 22. BeSCs 2 SGa 2 S 3 SrS 24.a) Ir 8+ b) Sc 3+ c) Pt 6+ d) Co 3+ e) Tc 3+ f) Ag +

127. 27. a) HIb) SeBr 2 c) SiBr 4 d) H 3 As 49. a) PCb) Covc) PCd) Ionic 50. a) PCb) PCd) Ionicd) PC 52. a) N-Hb) Si-Oc) S-FP-Cl

129. 54.a) trigonal planarb) trigonal pyramid c) lineard) trigonal planar e) trigonal planar 56.a) H 2 Oc) NH 4 +

130. a)octahedralh) tetrahedral b)tetrahedrali) trigonal bipyramid c)linearj) trigonal pyramid d)trigonal planark) octahedral e)bentl) linear f)trigonal planarm) linear g)Linearn) linear

131. Assessing the Objectives (page 278) a)2, 3 b)Less than 109.5 o c)Trigonal Planar d)Bent e)Linear, 180 o bent, 120 o

132. Questions 1. Rank the three liquids from weakest to the strongest forces between their molecules. 2.Discuss how you chose your rankings from the results of the experiment. 3.Is isopropyl alcohol or hexane more like water? Explain, using the results from the experiments. 4.What information did the salt experiment provide about the molecules?

133. GAK – NEATNESS!!!!!!! 1.Glue 2.Food coloring 3.Borax solution

134. FormulaLewis Dot Ca and O Ca and Br P and H C and F N and F

135. Consider the following three chemical bonds: C-O Cl-BrRb-Cl a.Determine the type of bond present in each situation b.In which bond is an electron transferred? c.Draw the Lewis Dot structure of this ionic compound. d.In which bond are electrons unequally shared? e.Identify the element in that bond that the electron spends more time with.

136. The element chlorine forms compounds with both strontium and sulfur. a.Write the formula of the compound that forms between strontium and chlorine. b.Draw the Lewis Dot Structure of this compound, indicating whether it is ionic or molecular. c.Write the formula of the compound that forms between sulfur and chlorine. d.Draw the Lewis Dot Structure of this compound, indicating whether it is ionic or molecular. e.Is the structure you drew in (d) linear? Why or why not? f.State the bond angle of the structure in (d).

138. Draw the Lewis Dot Structure and predict whether it is a polar or non-polar molecule H 2 O CH 3 CH(OH)CH 3 CH 3 CH 2 CH 2 CH 2 CH 2 CH 3

139. WaterIsopropylHexane Alcohol

140. Draw Lewis Structures (Ionic) BaF 2 Li 2 O Draw Lewis Structures (Molecular) ClF 3 SiO 3 2- SO 2

141. CompoundCentral Atom BeH 2 Tan BH 3 Tan CH 4, NH 3, H 2 OBlack PCl 5 Tan SF 6 Yellow or silver

148. 7a. Octahedralh. Tetrahedral b.Tetrahedrali. Trigonal bipyramid c.Linearj. Trigonal pyramid d.Trigonal Planark. Octahedral e.Bent Il. Linear f.Trigonal Planarm. Linear g.Linearn. Linear

149. 1. Covalent, Ionic or Polar Covalent Bonds? a.Ionic b.Covalent c.Polar Covalent d.Ionic e.Ionic f.Polar Covalent g.Polar Covalent h.Ionic

150. 3a. K + Br - b.Al 3+ 3Cl - c.2Ga 3+ 3O 2- d.2Li + O 2- e.Ca 2+ 2Br - f.Na + OH - g.Ca 2+ 2NO 3 - h.2Na + CO 3 2- i.2Fe 3+ 3SO 4 2- j.Co 4+ 4NO 2 -

151. http://www.youtube.com/watch?v=WaPxTAeW 5e8