1. January 14, 2014 (E) 1. What did you do over winter break? 2. Write two things you know about chemistry and EXPLAIN. 3. Define the three trends: Atomic Radius Ionization Energy Electro-negativity 4. How many seconds are in 23 days?

2. January 16, 2014 (E) 1. The least reactive elements belong to this group 2. Lithium belongs to the group 3. Write both the FULL and SHORTCUT electron configuration for Lithium 4. How many valence electron(s) does Lithium have? 5. Sodium belongs to the group 6. How many valence electrons does Sodium have? 7. Based on #4 and #6, we can conclude that… 8. A football field is 100 yards in distance. How long is the field in INCHES? 1 yard is equal to 3 feet, and 1 foot is equal to 12 inches.

3. January 21, 2014 (E) 1. Normal atoms become ions when… 2. These metals want to become like Noble Gases 3. Ions with a positive charge are called… 4. Ions with a negative charge are called… 5. A couple wise guys used chemistry to make money. They sold bars of Tungsten covered with a thin layer of gold. Each bar is 10 ounces. Gold is valued at $1778 per ounce. They made 7 of these fake gold bars. How much money did these wise guys make?

4. January 23, 2014 (E) 1. Ions made up of more than one atoms are called… 2. An oxygen atom will become what type of ion with what amount of charge (+1, -1, etc.)? 3. An oxygen ion has how many electrons? 4. Aluminum ion has what amount of charge? 5. How many electrons does an Al ion have? 6. One dozen is equal to how many things? 7. You bought 2.5 dozen eggs. Each egg costs 17 cents. How much did you spend on eggs? 8. Pick up your work at the front

5. January 24, 2013 (O) AGENDA 1. Quiz 2. Significant Figures and Scientific Notation. 3. Lab 4. Naming Ionic Compounds Properties of salts 5. Prepare for exam HOMEWORK 1. Study 2. Wordproblems

6. January 27, 2014 (E) 1. Turn Fluorine into an ion 2. Turn Calcium into an ion 3. Turn Arsenic into an ion 4. Turn Aluminum into an ion 5. Which two groups are most reactive and unstable? 6. Why are these two groups so reactive and unstable? 7. How can each group become less reactive and more stable? 8. Review notes for quiz and pick up your work at the front.

7. January 27, 2014 (E) AGENDA 1. Review lab 2. How to name ionic compounds 3. Classwork 4. Properties of ionic compounds 5. Review for EXAM HOMEWORK 1. Study 2. Lab Questions

8. January 29, 2014 (E) 1. Turn Aluminum into an ion 2. Turn Oxygen into an ion 3. What is the formula for the Al cation and O anion? 4. What is the molar mass for #3? 5. How many grams of the compound are in 3.39 mol? 6. This element becomes an ion, but not by becoming like a Noble Gas. Which is it: F, Cl, Na, Fe 7. How will an element with e. config of 1s 2 2s 2 2p 6 3s 2 become stable like Noble Gas? Pick up work

9. January 31, 2014 (E) Predict the charge on the ion formed by each element. 1. selenium, used to make ruby-colored glass 2. yttrium, used to make high-performance spark plugs 3. calcium, used to prevent osteoporosis 4. iodine, required for the synthesis of thyroid hormones Write the formula for the ionic compound 5. potassium cation and cyanide anion 6. calcium cation and hypochlorite anion 7. sodium cation and bicarbonate anion 8. ammonium cation and sulfate anion Pick up work

10. January 31, 2014 (E) AGENDA 1. Notes on Naming Compounds Part II 2. Practice naming compounds part II 3. Notes on Properties of Ionic Compounds 4. Review for exam. HOMEWORK 1. Study 2. Section Review 5.3 #2, 3, 5-8

11. Periodic Table Important GROUPS 1. Alkali Metals 2. Alkali Earth Metals 3. Halogens 4. Noble Gases 5. Transition Metals 6. Lanthanides 7. Actinides 8. Metalloids

12. Periodic Table 1. Alkali Metals metals very reactive 2. Alkali Earth Metals metal does NOT dissolve quickly in water high melting point

13. Periodic Table 3. Halogens non-metal very reactive 4. Noble Gases gases stable not reactive – why?

14. Periodic Table 5. Metals conducts heat and electricity malleable – like Playdoh ductile

15. Periodic Table 6. Lanthanides extremely rare 7. Actinides also rare radioactive

16. Periodic Table 8. Metalloids solid, but not metal has properties of metals

17. Classwork page 131 #1,2,5,6,8,11,13 Answer in complete sentences

18. http://online.wsj.com/news/articles/SB100008723963904 43768804578035500956712628?mg=reno64- wsj&url=http%3A%2F%2Fonline.wsj.com%2Farticle%2FSB 10000872396390443768804578035500956712628.html http://www.npr.org/2011/03/28/134916924/Amherst- Admissions-Process http://www.npr.org/blogs/money/2013/12/20/255846145 /will-a-computer-decide-whether-you-get-your-next- job?utm_content=socialflow&utm_campaign=nprfacebook& utm_source=npr&utm_medium=facebook http://www.zerohedge.com/news/2012-09-23/gold- counterfeiting-goes-viral-10-tungsten-filled-gold-bars- are-discovered-manhattan

19. Ions OBJECTIVE: See connection between electron configuration and chemical properties

20. Ions What is an ION? an atom that gained or lost one or more electrons

21. Ions What is an ION? an atom that gained or lost one or more electrons 1. What determines if an atom gains or loses an electron 2. What determines how many electrons are gained or lost

22. Valence Electrons and Ions What are valence electrons? electrons in its outermost orbital

23. Valence Electrons and Ions Write FULL electron configuration for Silicon, Si

24. Valence Electrons and Ions Write FULL electron configuration for Silicon, Si

25. Valence Electrons and Ions Write FULL electron configuration for Silicon, Si Si = 1s 2 2s 2 2p 6 3s 2 3p 2

26. Valence Electrons and Ions Write FULL electron configuration for Silicon, Si Si = 1s 2 2s 2 2p 6 3s 2 3p 2

27. Valence Electron and Ions Write FULL electron configuration for Germanium, Ge

28. Valence Electron and Ions Write FULL electron configuration for Germanium, Ge Ge = 1s 2 2s 2 2p 6 3s 2 3p 2 4s 2 3d 10 4p 2 4 valence electrons

29. Valence Electron and Ions HeliumNeonArgonKryptonXenon 1.Write the electron configuration for the following elements 2.UNDERLINE valence electrons

30. Valence Electron and Ions The S orbital can hold how many electrons? TWO The P orbital can hold how many electrons? SIX Noble gases are stable and unreactive because their outer orbitals are FILLED 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

31. Valence Electron and 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

32. Textbook page 162 Ions with at POSTIVE charge, +, are called cations pronounced “cat – ions”

33. Ions IMPORTANT Ions and their parent atoms have different properties. Ex: a Li cation =/= a Li atom Why might this be the case? Just because ions have the same electron configuration as Noble Gases does not make them become Noble Gases. Ex: a Li cation =/= He atom Basic idea: ions not same as parent atom ions do not become Noble Gases

35. Textbook page 163

36. Valence Electron and 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 Non-Metals want to be noble by having the SAME electron configuration

37. Textbook page 162 Ions with at NEGATIVE charge called anions pronounced “an – ions”

38. Textbook page 162 Ions with at NEGATIVE charge called anions pronounced “an – ions”

39. 3. Trendy Table Periodic Trends Ionization Energy What is this? Energy needed to remove an electron from an atom

40. 3. Trendy Table Periodic Trends 2 nd Trend: First Ionization Energy What is this? Energy needed to remove an electron from an atom A FILLED orbital is a happy and stable orbital

41. 3. Trendy Table 2 nd Trend: First Ionization Energy

42. 3. Trendy Table 2 nd Trend: First Ionization Energy

43. 3. Trendy Table 2 nd Trend: First Ionization Energy

44. 3. Trendy Table Periodic Trends 3 Patterns 1.Atomic Radius 2.Ionization Energy 3.Electronegativity Atomic Radius Ionization Energy Electronegativity Period INCREASES Row INCREASES

45. http://online.wsj.com/news/articles/SB100008723963904 43768804578035500956712628?mg=reno64- wsj&url=http%3A%2F%2Fonline.wsj.com%2Farticle%2FSB 10000872396390443768804578035500956712628.html http://www.npr.org/2011/03/28/134916924/Amherst- Admissions-Process http://www.npr.org/blogs/money/2013/12/20/255846145 /will-a-computer-decide-whether-you-get-your-next- job?utm_content=socialflow&utm_campaign=nprfacebook& utm_source=npr&utm_medium=facebook http://www.zerohedge.com/news/2012-09-23/gold- counterfeiting-goes-viral-10-tungsten-filled-gold-bars- are-discovered-manhattan

46. 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 -

47. 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

48. Ions Because these ions are made from two or more atoms, they are called polyatomic ions -ite has less oxygen than -ate

49. Ions, Ionic Bonds, and Ionic Compounds OBJECTIVE: Understand how IONS join together to create IONIC COMPOUNDS

50. Ions, Ionic Bonds, and Ionic Compounds Ionic Bonding Ionic bonds form between cations and anions, ions with opposite charges Na + + Cl -  NaCl cation anionionic compound

51. Ions, Ionic Bonds, and Ionic Compounds Ionic bonds form between cations and anions, ions with opposite charges Na + + Cl -  NaCl cation anionionic compound Cu + + CH 3 COO -  CuCH 3 COO

52. Ions, Ionic Bonds, and Ionic Compounds Ionic bonds form between cations and anions, ions with opposite charges Cu + + CH 3 COO -  CuCH 3 COO cation anionionic compound NH 4 + + Cr 2 O 7 -  NH 4 Cr 2 O 7 cation anionionic compound

53. Ions, Ionic Bonds, and Ionic Compounds Ionic bonds form between cations and anions, ions with opposite charges NH 4 + + Cr 2 O 7 -  NH 4 Cr 2 O 7 cation anionionic compound CHARGES MUST CANCEL

54. Ions, Ionic Bonds, and Ionic Compounds 1. Make the following ionic compounds 2. Write formula 3. Calculate the molar mass 4. H+ and SO 4 2- 5. Al 3+ and O 2- 6. Mg 2+ and OH - 7. Ag + and Cl - 8. Na + and HCO 3 - 9. Ca 2+ and PO 4 3- 10. Na + and NO 2 - 11. NH 4 + and PO 4 3-

55. Complete table on separate paper 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 -

56. Complete table on separate paper 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 - KClFeCl 3 NH 4 ClBaCl 2 SO 4 2- K 2 SO 4 Fe 2 (SO 4 ) 3 (NH 4 ) 2 SO 4 BaSO 4 PO 4 3- K 3 PO 4 FePO 4 (NH 4 ) 3 PO 4 Ba 3 (PO 4 ) 2 NO 3 - KNO 3 Fe(NO 3 ) 3 NH 4 NO 3 Ba(NO 3 ) 2 OH - KOH Fe(OH) 3 NH 4 OH Ba(OH) 2

57. Calculating Moles for Ionic Compounds OBJECTIVE: Learn how to convert grams  moles, and moles  to grams for ionic compounds

58. Calculating Moles for Ionic Compounds A MOLE of something is equal to 602000000000000000000000 or 6.02 x 10 23

59. Calculating Moles for Ionic Compounds 1 MOLE of eggs = 602000000000000000000000 eggs 1 MOLE of donuts = 602000000000000000000000 donuts 1 MOLE of flowers = 602000000000000000000000 flowers 1 MOLE of Li atoms = 602000000000000000000000 Li atoms

60. Calculating Moles for Ionic Compounds How calculate GRAMS  MOLES Atomic Mass : 1 mol

61. Calculating Moles for Ionic Compounds How calculate GRAMS  MOLES How many moles are in 24 grams of C? 24 g1 mol= 12 g

62. Calculating Moles for Ionic Compounds How calculate GRAMS  MOLES How many moles are in 327 g of NaCl Na: 1 x 23 g = 23g + Cl: 1 x 35.45 g = 35.45g NaCl = 58.45 g 327 g NaCl 1 mol NaCl 58.45 g NaCl = 5.59 mol NaCl

63. Calculating Moles for Ionic Compounds How calculate MOLES  GRAMS How many grams are in 5.600 mol of NaCl? Na: 1 x 23 g = 23g + Cl: 1 x 35.45 g = 35.45g NaCl = 58.45 g 5.600 mol NaCl 58.45 g NaCl 1 mol NaCl = 327.3 g NaCl

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65. 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

66. Rules for Significant Figures 1. All nonzero #’s ARE significant. 2. Interior zeroes ARE significant. 3. Leading zeroes ARE NOT significant. 4. Trailing zeroes AFTER a decimal point ARE significant. 5. Trailing zeroes BEFORE a decimal point ARE significant 6. Trailing zeroes without a decimal point?

68. How many significant figures? 1. 218 kg 2. 0.025 L 3. 200 g 4. 1.05 cm 5. 200.0 mg

70. Naming Ionic Compounds

71. 1. Start with cation. 2. If cation is Transition Metal check table for roman numerals 3. Name the anion using the suffix “ IDE ”. If anion is polyatomic…

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

73. Cations with Roman Numerals in BOLD

74. 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.

75. 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

76. 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.

77. 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?

78. 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?

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

80. Properties of Ionic Compounds Ionic compounds are COMPOUNDS chemically joined Ions are joined by IONIC BONDS Ionic Bonds VERY STRONG!!

81. Properties of Ionic Compounds Strong bonds = high boiling point High boiling point = need lots of energy (heat) to break bond/connection between cation and anion.

82. Properties of Ionic Compounds bond strength depends on ion radius and ion charge

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

84. Properties of Ionic Compounds Ionic Compounds form crystals

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

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

87. Properties of Ionic Compounds Salts form crystals

88. Properties of Ionic Compounds

89. Mono Lake, CA

90. Properties of Ionic Compounds Mono Lake, CA

91. Properties of Ionic Compounds Mono Lake, CA

92. Properties of Ionic Compounds Mono Lake, CA

93. Properties of Ionic Compounds

95. calcium carbonate

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

97. Properties of Ionic Compounds calcium carbonate

98. Properties of Ionic Compounds Ionic Compounds conduct electricity

99. Properties of Ionic Compounds conduct electricity

100. Atoms Electron Configuration Valence Electrons Ions CationsAnions Ionic Compounds Calculations FormulaProperties Molar Mass Naming Grams   Moles