1. OUTLINE OF TOPICS 1. Bonding & Compounds 2. Covalent Bonding & Compounds 3. Lewis Structures & VSEPR 4. Nomenclature 5. Ions 6. Ionic Bonds & Compounds 7. Nomenclature II

2. 1. Bonding and Compounds OBJECTIVE: How bonds are made

3. 1. Bonding and Compounds H 2 OCO 2 C 2 H 2 subscripts tell how many atoms

4. 1. Bonding and Compounds atoms share or give away electrons to form COMPOUNDS

5. 1. Bonding and Compounds compounds are formed by BONDS

6. 1. Bonding and Compounds bonds are formed when atoms share or give away VALENCE ELECTRONS

7. 1. Bonding and Compounds valence electrons electrons in the outermost orbital

8. 1. Bonding and Compounds How do we know which are the valence electrons? valence electrons are in the HIGHEST ENERGY LEVEL (largest numbers)

9. 1. Bonding and Compounds Write electron configuration for Silicon, Si Si = 1s 2 2s 2 2p 6 3s 2 3p 2

10. 1. Bonding and Compounds Write electron configuration for Gallium, Ga Ga = 1s 2 2s 2 2p 6 3s 2 3p 2 4s 2 3d 10 4p 1 Ge has 3 valence electrons

11. 1. Bonding and Compounds 1.Write electron configurations 2.Underline and count valence electrons Do you notice a pattern? LithiumMgBoronSulfurFluorineNeon SodiumCaAluminumSeleniumChlorineKrypton

12. 1. Bonding and Compounds EXAMPLE: Lithium 1s 2 2s 1 Sodium 1s 2 2s 2 2p 6 3s 1 This pattern is seen in groups 1-2 and 13-18 What did groups have in common?

13. 1. Bonding and Compounds Summary & Review 1. What do the subscripts in a compound tell you? 2. How many atoms of EACH in the following compounds: NaCl, H 2 O, CO 2, H 2 O 2, C 6 H 12 O 11 3. How do you know which electrons are the valence electrons?

14. 2. Covalent Bonds & Compounds OBJECTIVE: Bonds when atoms SHARE electrons

15. 2. Covalent Bonds & Compounds 2 types of bonds Covalent Ionic

16. 2. Covalent Bonds & Compounds co-valent So which electrons are the atoms sharing?? sharing VALENCE electrons

17. 2. Covalent Bonds & Compounds Covalent Bond/Compounds = when atoms SHARE valence electrons video

18. 2. Covalent Bonds & Compounds Some examples of covalent compounds

19. 2. Covalent Bonds & Compounds Some example of covalent compounds

20. 6. Covalent Bonds & Compounds Most compounds = covalent bonds

21. 2. Covalent Bonds 2 types Nonpolar Covalent valence electrons EQUALLY shared Polar Covalent valence electrons NOT equally shared

22. 2. Covalent Bonds Electronegativity how much an element wants an electron Higher the number, the more “selfish”

23. 2. Covalent Bonds Electronegativity determines type 0 – 0.49 Nonpolar C 0.50 – 2.0 Polar C above 2.0 Ionic

24. 3. Types of Covalent Bonds weaker stronger 0 – 0.49 Nonpolar C 0.50 – 2.0 Polar C above 2.0 Ionic

25. 3. Types of Covalent Bonds

26. 2. Covalent Bonds H 2, NaCl, Cl 2, KCl, HBr OF 2, F 2, N 2, NO, NH 3 Subtract electronegativity values to determine bond type.

27. 2. Covalent Bonds & Compounds Summary & Review 1. What is shared in a covalent bond/compound? 2. What are the two types of covalent bonds? 3. How can you tell if a covalent bond is nonpolar or polar polar? 4. What does a high electronegativity value mean? 5. If a bond is polar, what are the two signs you use? 6. How do you know where put the signs? 7. What do those signs mean?

28. CLASSWORK: #3, 6, 11, 12,14 11. Order from most to least polar

29. 3. Lewis Structures & VSEPR How many valence electrons do the each of the Noble Gases have? He Ne Ar Kr Xe Rn

30. 3. Lewis Structures & VSEPR OBJECTIVE: How bonds are made

31. 3. Lewis Structures & VSEPR Most elements want 8 valence electrons Octet Rule

32. 3. Lewis Structures & VSEPR dot = valence electron

33. 3. Lewis Structures & VSEPR blue line = bond

34. 3. Lewis Structures & VSEPR Elements that do not want 8 dots Group 1 H, Li, Na, K, etc. Only wants 2 dots more exceptions later

35. 3. Lewis Structures & VSEPR Draw the following Lewis Structures H 2 Cl 2 H 2 SHBr OF 2 H 2 O NH 3 CH 2 F 2 CH 4 C 2 H 6

36. 3. Lewis Structures & VSEPR Draw the following structures O2N2O2N2 COCO 2 HCNSO 3 C 2 Cl 4 COCl 2

37. 3. Lewis Structures & VSEPR 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

38. 3. Lewis Structures & VSEPR

39. Most elements will want 8 valence electrons dot = valence electron

40. 3. Lewis Structures & VSEPR Exceptions to the Octet Rule 1.Less than 8 2.More than 8 3.Polyatomic Ions

41. 3. Lewis Structures & VSEPR Exceptions to the Octet Rule 1.Less than 8 Beryllium and Boron BeCl 2 BCl 3

42. 3. Lewis Structures & VSEPR Exceptions to the Octet Rule 2. More than 8 Sulfur and Xenon SF 6 XeF 4

43. 3. Lewis Structures & VSEPR Exceptions to the Octet Rule 3. Polyatomic Ions CationsAnions REMOVE electrons ADD electrons add brackets [ ]

44. 3. Lewis Structures & VSEPR Resonance = 2 or more possible Lewis Dot Structures

45. 3. Lewis Structures & VSEPR Resonance = 2 or more possible Lewis Dot Structures

46. 3. Lewis Structures & VSEPR Summary & Review 1. What element goes in the middle of a Lewis Structure? 2. Which group does not need 8 dots? 3. Which element is NEVER in the center

47. 3. Lewis Structures & VSEPR OBJECTIVE: Determine Shape of Compounds

48. 3. Lewis Structures & VSEPR How to determine shape? VSEPR Valence Shell Electron Pair Repulsion

49. 3. Lewis Structures & VSEPR VSEPR Main Idea: Electrons around atoms REPEL each other

50. we will learn 5 shapes Linear 3. Lewis Structures & VSEPR

51. we will learn 5 shapes Bent 3. Lewis Structures & VSEPR

52. we will learn 5 shapes Triagonal Planar 3. Lewis Structures & VSEPR

53. we will learn 5 shapes Pyramidal 3. Lewis Structures & VSEPR

54. we will learn 5 shapes Tetrahedral 3. Lewis Structures & VSEPR

56. How to determine shape? Lewis Structures

57. 3. Lewis Structures & VSEPR VSEPRLewis SHAPE # of bonds

60. 3. Lewis Structures & VSEPR Determine shape by 1. Draw Lewis Structure 2. How many things around the center atom? 3. How many lone pairs?

61. 3. Lewis Structures & VSEPR Determine shape by 1. Draw Lewis Structure 2. How many things around the center atom? 3. How many lone pairs? IMPORTANT Things like: charges, single, double, triple bonds do NOT matter

62. 3. Lewis Structures & VSEPR 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

63. 4. 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?

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

65. 4. Naming Covalent Compounds Numbers MATTER! CO CO 2 SO SO 2

66. 4. 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 ”

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

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

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

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

71. 4. Naming Covalent Compounds 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

72. 4. Naming Covalent Compounds Summary & Review 1. How can you tell the difference between ionic and covalent compounds 2. How is hydrogen different?

73. 4. Naming 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

74. 5. IONS 5 + - 2 = 5 + - 3 = 5 + - 4 = 5 + - 6 =

75. 5. IONS OBJECTIVE: When atoms give away electrons

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

77. 5. IONS How do we know if an atom GAINS or LOSES electrons? and How MANY electrons is it going to gain or lose?

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

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

80. 5. IONS All metals become CATIONS

81. 5. IONS Transition Metals do not care about being NOBLE They have their own thing going one. DO NOT HAVE TO MEMORIZE…kind of

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

83. 5. IONS Ions with at NEGATIVE charge called anions pronounced “an – ions”

84. 5. IONS Helium Neon Argon Krypton 1.Write the electron configuration for the following elements 2.UNDERLINE valence electrons The S orbital can hold how many electrons MAX? TWO The P orbital can hold how many electrons MAX? SIX Noble Gases do not become ions because their orbitals are FILLED THEY have all the VALENCE ELECTRONS THEY NEED

85. 5. IONS Helium 1s 2 Neon [He]2s 2 2p 6 Argon [Ne]3s 2 3p 6 Krypton [Ar]4s 2 3d 10 4p 6 Xenon [Kr]5s 2 4d 10 5p 6 Alkali and Alkali Earth Metals want to be noble by having the SAME electron configuration as the nearest noble gas Non-Metals want to be noble by having the SAME electron configuration as the nearest noble gas

86. 5. IONS So far we learned how a “normal” atom becomes an ion Li  Li + + 1electron Mg  Mg 2+ + 2electrons N + 3electrons  N 3- O + 2electrons  O 2- F + electron  F -

87. 5. 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

88. 5. IONS Because these ions are made from two or more atoms, they are called polyatomic ions -ite has less oxygen than –ate Memorize? Kind of

89. 5. IONS Summary & Review 1.What is an ion? 2.What are the two types of ions? 3.Metals form these types of ions, and non-metals form these types of ions. 4.Why do Noble Gases not become ions? 5.Predict the charge of each atom if it were to become an ion: Ca, Cl, Cu, F, Fe, Li, Na, N, O

90. 6. Ionic Compounds 4x + -16 = 0 2x + -8 = 0 3x + -12 = 0 2 + -x = 0 10 + -2x = 0 12 + -3x = 0

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

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

93. 6. 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

94. 1. Separate into cations and anions 2. Separate into Alkali, Alkali Earth, Halogens, Transition Metals, and Polyatomic Ions 3. Make the following compounds 6. Ionic Compounds H + + Cl -  Na + + Cl -  Mg 2+ + Cl -  Mg 2+ + SO 4 2-  Mg 2+ + SO 3 2-  Fe 2+ + Cr 2 O 7 2-  NH 4 + + Cl -  Fe 2+ + O 2-  Na + + O 2-  Na + + OH -  Fe 3+ + OH -  NH 4 + + SO 4 2- 

95. 6. 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

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

97. Summary & Review What is the correct formula for magnesium hydroxide: MgOH 2, MgO 2 H 2 or Mg(OH) 2 ? K+K+ Fe 3+ NH 4 + Ba 2+ Cl - KCl SO 4 2- PO 4 3- NO 3 - OH -

98. Properties of Ionic Compounds OBJECTIVE: A quick look at salts SALTS

99. Properties of Ionic Compounds Ionic Bonds very strong bonds!! metal cation + non-metal anion Ionic compounds are generally called SALTs

100. Properties of Ionic Compounds Ionic Compounds form crystals

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

102. Properties of Ionic Compounds Shape depends on radius of ions crystal lattice (lattice = repeating pattern)

103. Properties of Ionic Compounds Salts form crystals

104. Properties of Ionic Compounds

105. Mono Lake, CA

106. Properties of Ionic Compounds Mono Lake, CA

107. Properties of Ionic Compounds Mono Lake, CA

108. Properties of Ionic Compounds Mono Lake, CA

109. Properties of Ionic Compounds

111. calcium carbonate

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

113. Properties of Ionic Compounds calcium carbonate

114. Properties of Ionic Compounds Ionic Compounds conduct electricity

115. Properties of Ionic Compounds conduct electricity

116. Complete table on separte paper ? mols ? grams K+K+ Fe 3+ NH 4 + Ba 2+ Cl - 12g 3.27 mol SO 4 2- 79.3g 65.30 mol PO 4 3- 123.4g 2.31 mol NO 3 - 423.1g 3.27 mol OH - 1.497g 1.985 mol

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

118. 6. Naming Ionic Compounds OBJECTIVE: Learn how to name compounds like NaHCO 3

119. 6. Naming Ionic Compounds only TRANSITION METALS will have roman numerals

120. 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!

121. Naming Ionic Compounds IMPORTANT Roman Numeral =/= Subscript copper(I) oxide Cu 2 O Roman Numeral = CHARGE of Cu +

122. Cations with Roman Numerals in BOLD

123. Naming Ionic Compounds II Writing formulas from names of ionic compounds 1. Write anion and charge. -ATE-ITE 2. Write cation and charge. Table 2.5? 3. Cross charges and write formula.

124. Naming Ionic Compounds A. Ca 2+ CN - Ca(CN) 2 B. Rb + S 2 O 3 2- Rb 2 S 2 O 3 C. Ca 2+ CH3COO - Ca(CH 3 COO) 2 D. NH 4 + SO 4 2- (NH 4 ) 2 SO 4

125. Naming Ionic Compounds Writing formulas from names of ionic compounds 1. Write anion and charge. -ATE-ITE 2. Write cation and charge. Table 2.5? 3. Cross charges and write formula.

126. Ammonium phosphate is used by firefighters to extinguish and slow down fires. Local firefighters used over 10000.00 g of this compound when fighting the 1700-acre fire near Glendora, CA. This ionic compound works by “suffocating” the fire. Fire requires oxygen, but ammonium phosphate is a dry powder that covers and blankets fires thereby “suffocating” it. Much more of this compound was needed to combat the recent fire that burned an area that is almost equivalent to 29 football fields. 1. What is the formula for the compound? 2. Which is the cation, and what is its charge? 3. Which is the anion, and what is its charge? 4. What is the molar mass of the compound? 5. How many moles were used by the firefighters?

127. Ammonium phosphate is used by firefighters to extinguish and slow down fires. Local firefighters used over 10000.00 g of this compound when fighting the 1700- acre fire near Glendora, CA. This ionic compound works by “suffocating” the fire. Fire requires oxygen, but ammonium phosphate is a dry powder that covers and blankets fires thereby “suffocating” it. Much more of this compound was needed to combat the recent fire that burned an area that is almost equivalent to 29 football fields. A. What is the formula for the compound? B. Which is the cation, and what is its charge? C. Which is the anion, and what is its charge? D. What is the molar mass of the compound? E. How many moles were used by the firefighters?