1. Outline of Topics 1. REVIEW Ions, Ionic Compounds 2. Naming Ionic Compounds 3. Properties of Ionic Compounds 4. Naming Covalent Compounds 5. VSEPR

2. REVIEW of IONS OBJECTIVE: When atoms give away electrons

3. IONS ION What is it? An atom that LOST/GAINED electron(s)

4. IONS Goal is to get to the NEAREST Noble Gas RULES 1.If you go LEFT, you become POSITIVE. 2.If you go RIGHT, you become NEGATIVE

5. IONS Ions that LOSE electrons have a POSTIVE charge called cations pronounced “cat – ions”

6. IONS All metals become CATIONS

7. IONS USE HALF SHEET FOR TRANSITION METALS

8. IONS Ions that GAINS electrons have a NEGATIVE charge called anions pronounced “an – ions”

9. IONS Ex: CN - NH 4 + CO 3 2- Because these ions are made from two or more atoms, they are called polyatomic ions Some ions are made from two or more atoms

10. IONS -ite has less oxygen than –ate Memorize? Kind of

11. IONS Summary & Review 1.What is an ion? 2.What are the two types of ions? 3.Which ions gains electrons: cations or anions? 4.Predict the charge of each atom if it were to become an ion: Ca, Cl, Cu, F, Fe, Li, Na, N, O

12. Ionic Compounds OBJECTIVE: Joining Cations + Anions to make compounds

13. Ionic Compounds Na + + Cl -  NaCl cation anionionic compound forumula NaCl joined by IONIC BOND IONIC BOND = giving away/gaining electrons

14. Ionic Compounds Li + + Cl -  K + + Cl -  Ca 2+ + Cl -  Li + + O 2-  Ca 2+ + O 2-  LiCl KCl CaCl 2 Li 2 O CaO Charges must cancel and = 0

15. Ionic Compounds Cu + + CH 3 COO -  NH 4 + + Cr 2 O 7 -  Mg 2+ + OH -  CuCH 3 COO NH 4 Cr 2 O 7 Mg ( OH ) 2 Parenthesis for POLYATOMIC

16. Ionic Compounds Write formula for ionic compounds 1. Al 3+ + O 2-  2. Fe 2+ + Cl -  3. Na + + HCO 3 -  4. Na + + NO 2 -  5. Ca 2+ + PO 4 3-  6. H + + SO 4 2-  7. Mg 2+ + OH -  8. NH 4 + + PO 4 3- 

17. Ionic Compounds Write formula for ionic compounds 1. Al 3+ + O 2-  2. Fe 2+ + Cl -  3. Na + + HCO 3 -  4. Na + + NO 2 -  5. Ca 2+ + PO 4 3-  6. H + + SO 4 2-  7. Mg 2+ + OH -  8. Fe 3+ + Cl -  9. NH 4 + + PO 4 3- 

18. 1. Naming Ionic Compounds Write from 1 to 5 in Roman Numerals I II

19. 1. Naming Ionic Compounds OBJECTIVE: Learn how to name compounds like NaHCO 3

20. 1. Naming Ionic Compounds First Name + Last Name = Full Name only TRANSITION METALS have roman numerals

21. Cations with Roman Numerals in BOLD

22. 1. Naming Ionic Compounds 1. Start with CATION, always 2. Name the anion using the suffix “ IDE ”. If anion is polyatomic…

23. 1. Naming Ionic Compounds “uncross” numbers to figure our roman numeral for cation FeCl 3 Cr 2 O 3 Cu 2 OMn 3 N 2 Mn(NO 2 ) 3 Mn(NO 3 ) 3 Mn(NO 3 ) 2 If no numbers then 1. Figure out charge of anion FeOCrO MnOCoN CrPO 4 ZnCrO 7 CuSO 4 CuNO 3

24. 1. Naming Ionic Compounds 1. Start with CATION, always 2. If cation is Transition Metal check table for roman numerals 3. Name the anion using the suffix “ IDE ”. If anion is polyatomic… 4. That’s it!

25. 1. Naming Ionic Compounds Writing formulas from names of ionic compounds 1. Write anion and charge. 2. Write cation and charge. 3. Cross charges and write formula. -ATE-ITE half sheet

26. Naming Ionic Compounds 1. Sodium Chloride 2. Lithium Fluoride 3. Iron(II) Chloride 4. Sodium Nitrate 5. Magnesium Hydroxide 6. Sodium Acetate 7. Ammonium Chloride 8. Hydrogen Peroxide 9. Sodium Carbonate 10. Ammonium Phosphate

27. 1. Naming Ionic Compounds SUMMARY & REVIEW Formula to Name 1. Start with cation 2. When to use roman numerals? 3. Then add…to anion 4. What about polyatomic ions? Name to Formula 1. Start with anion – LAST NAME 2. What if anion ends in ATE or ITE? 3. Write symbol for cation – FIRST NAME 4. Roman numerals?

28. 2. Properties of Ionic Compounds What are some properties of salt?

29. 2. Properties of Ionic Compounds OBJECTIVE: Properties of salts

30. 2. Properties of Ionic Compounds Ionic compounds are chemically joined by IONIC BONDS Ionic Bonds VERY STRONG!!

31. 2. Properties of Ionic Compounds Ionic compounds are generally called SALTs metal cation + non-metal anion

32. 2. Properties of Ionic Compounds Ionic Bonds metal cation + non-metal anion Ionic compounds are generally called SALTs

33. 2. Properties of Ionic Compounds High boiling point = STRONG BONDS

34. 2. Properties of Ionic Compounds High boiling point = need lots of energy (heat) to break ionic bond between cation and anion.

35. 2. Properties of Ionic Compounds Ionic Compounds form crystals

36. 2. Properties of Ionic Compounds Ionic Compounds form crystals Copper (II) sulfate

37. 2. Properties of Ionic Compounds Ionic Compounds Brittle (break, not bend)

38. 2. Properties of Ionic Compounds Ionic Compounds conducts electricity Used to make batteries

39. 2. Properties of Ionic Compounds conduct electricity

40. 2. Properties of Ionic Compounds

41. Mono Lake, CA

42. 2. Properties of Ionic Compounds Mono Lake, CA

43. 2. Properties of Ionic Compounds Mono Lake, CA

44. 2. Properties of Ionic Compounds Mono Lake, CA

45. 2. Properties of Ionic Compounds

47. Properties of Ionic Compounds calcium carbonate

48. Properties of Ionic Compounds calcium carbonate

49. 2. Properties of Ionic Compounds SUMMARY & REVIEW 1. Ionic compounds are generally called… 2. Ionic compounds have… 3. Ionic compounds forms 4. Ionic compounds are… 5. Ionic compounds can…

50. 3. Naming Covalent Compounds How many wheels on a bicycle? How many wheels on a tricycle? How many sides on a pentagon? How many sides on a hexagon? How many sides on an octagon?

51. 3. Naming Covalent Compounds OBJECTIVE: Learn how to name compounds like H 2 O & CO 2

52. 3. Naming Covalent Compounds Numbers MATTER! CO CO 2 SO SO 2

53. 3. Naming Covalent Compounds FIRST ELEMENT 1. Name the element 2. If more than one, use prefix 3. “mono” NEVER used for first name SECOND ELEMENT 1. Name element 2. If more than one, use prefix 3. Add “ IDE ”

54. 3. Naming Covalent Compounds Name the compounds 1. CS 2 2. NF 3 3. SF 6 4. CO 5. N 2 O 3

55. 3. Naming Covalent Compounds Write the formula 1. Silicon tetrafluoride 2. Arsenic trichloride 3. Carbon dioxide 4. Boron tribromide 5. Dihydrogen monoxide

56. 3. Naming Covalent Compounds How to know if compound is ionic or covalent? IONIC: between metal and non-metal COVALENT: between non-metals

57. 3. Naming Covalent Compounds IONIC: RED + BLUE COVALENT: YELLOW/BLUE + BLUE

58. Covalent Compound Calculations A. Name each compound/write formula 1. BF 3 2. BrCl 3. IF 4 4. SF 6 5. carbon dioxide 6. boron tribromide 7. oxygen difluoride 8. xenon tetrafluoride

59. Properties of Covalent Bonds 2 types of covalent bonds Polar Electron shared UNEQUALLY Non-Polar Electrons shared EQUALLY

60. Properties of Covalent Bonds Polar Covalent have dipoles

61. Properties of Covalent Bonds Bond Type Determines Properties of Things

62. Properties of Covalent Bonds

63. 3. Namine Covalent Compounds Summary & Review 1. How can you tell the difference between ionic and covalent compounds 2. How is hydrogen different?

64. 3. Namine Covalent Compounds Summary & Review 1. How can you tell the difference between ionic and covalent compounds 2. Name/write formula for the following 1. P 4 S 5 2. SeF 6 3. Si 2 Br 6 4. SCl 4 5. B 2 Si 6. antimony tribromide 7. hexaboron silicide 8. chlorine dioxide 9. hydrogen iodide 10. iodine pentafluoride

65. 3. Namine Covalent Compounds 1. P 4 S 5 2. SeF 6 3. Si 2 Br 6 4. SCl 4 5. B 2 Si 6. antimony tribromide 7. hexaboron silicide 8. chlorine dioxide 9. hydrogen tri-iodide 10. iodine pentafluoride

66. 4. Lewis Structures OBJECTIVE: How bonds are made

67. 4. Lewis Structures Most elements want 8 valence electrons Octet Rule

68. 4. Lewis Structures dot = valence electron

69. 4. Lewis Structures blue line = bond

70. 4. Lewis Structures 1. Write elements 2. Count total number of valence e 3. LEAST electronegative is in the center (usually CARBON) 4. Draw bond 5. Then draw dots until you run out 6. Make double/triple bonds if necessary

71. 4. Lewis Dot Structures Exceptions to the Octet Rule 1.Less than 8 2.More than 8 3.Polyatomic Ions

72. 4. Lewis Dot Structures Exceptions to the Octet Rule 1.Less than 8 Hydrogen Beryllium and Boron BeCl 2 BCl 3

73. 4. Lewis Dot Structures Exceptions to the Octet Rule 2. More than 8 Phosphorus,Sulfur, Chlorine Xenon PCl 5 SF 6 XeF 4

74. 4. Lewis Dot Structures Exceptions to the Octet Rule 3. Polyatomic Ions CationsAnions SUBTRACT electrons ADD electrons add brackets [ ]

75. 4. Lewis Dot Structures Resonance = 2 or more possible Lewis Dot Structures

76. 4. Lewis Dot Structures Resonance = 2 or more possible Lewis Dot Structures

77. 4. Lewis Structures Summary & Review 1. Which elements have less than 8? 2. Which elements have more than 8?

78. 4. Lewis Structures Summary & Review 1. Which element goes in the middle of a Lewis Structure? 2. Which is NEVER in the center? 3. Which elements do not need 8 dots? 4. Which elements can have more than 8? 5. What do you add to non polyatomic ions? 6. What is a resonance?

79. 5. VSPER 1.Draw a triangle 2.Draw a square 3.Draw a pyramid

80. 5. VSPER OBJECTIVE: Lewis Structures in 3D

81. 5. VSPER How to determine shape? VSEPR Valence Shell Electron Pair Repulsion

82. 5. VSPER How is VSEPR different from Lewis? VSEPRLewis Lewis in 3D shows bonds

83. 5 main shapes Linear 5. VSPER

84. Triagonal Planar 5. VSPER

85. Tetrahedral 5. VSPER

86. Triagonal bipyramidal

87. 5. VSPER Octahedral

88. 5. VSPER More shapes derived from the 5 main ones

89. 5. VSPER

94. Bent 5. VSPER

95. Triagonal Pyramidal 5. VSPER

96. T-shape

97. 5. VSPER Seesaw

98. 5. VSPER Square Pyramidal

99. 5. VSPER Square Planar

100. 5. VSPER How to determine shape?? 1. Draw Lewis Structure 2. Count how many THINGS around the center atom? 3. How many LONE PAIRS? 4. Axial & Equatorial

102. 5. VSPER VSEPR Main Idea: Electrons around atoms REPEL each other

103. 5. VSPER Determine shape by 1. Draw Lewis Structure 2. Add marshmallows around the center 3. Remove marshmallow that represent lone pairs IMPORTANT Things like: charges, single, double, triple bonds do NOT matter

104. 5. VSPER Summary & Review 1. What is the main idea of VSEPR 2. How is VSEPR different from Lewis Structures 3. How do you determine the VSEPR shape?

105. Sample Problem Charles Goodyear accidently created rubber by heating atoms of carbon and sulfur together. The resulting covalent compound is named carbon disulfide. This covalent compound is extremely useful because of its elastic ability. A. What is the formula for this compound? B. Draw the Lewis Structure for this compound. C. What is the VSEPR shape?