2. Catalyst – November 10-5, 2009 1. What has the higher 1 st ionization energy Calcium or Oxygen? 2. Which has a higher melting point Potassium Iodide or Hydrogen Disulfide?

3. Today’s Agenda  Catalyst  Going over some things/Whiteboard Practice  Practice Quiz  Exit Question

4. Today’s Objectives  SWBAT get ready to DOMINATE the Unit 4 Test!

5. Today…  We are going to review some things and practice on the whiteboards. Please ask questions where you might be confused!!  Then, we will take a practice quiz to get you in the mood!

6. Ionization Energy  Ionization Energy is the ENERGY it takes to remove an electron.  There are two types of questions:  1 st ionization energy- know the trend!  2 nd, 3 rd, 4 th - does it break into a new shell? LET’S PRACTICE!

7. First Ionization Energy!

8. Multiple Ionization Energies  There is a gigantic increase in ionization energy if you break into a full valence shell!  Why???

9. Ionization Energy Can you figure out why there is such an increase in the red numbers? Use your BOHR models!! (10 mins) LiBe B C IE 1 520 900 801 1086 IE 2 7,298 1757 2427 2353 IE 3 14,849 3660 4621 IE 4 25,026 6223 IE 5 37,830

10. Practice  *First, draw a Bohr Model for both elements  Which has the highest 2 nd ionization energy?  Boron  Sodium

11. Practice  Which has the highest 3 rd ionization energy?  Calcium  Nitrogen

12. Practice  Which has the highest 1 st ionization energy?  Selenium  Polonium

13. Bond Type Chart/Differences in EN  Man, I wish there was an easy way to use electronegativity to figure out what bond type I have between two elements…  OH WAIT! There is! Pull out your book and turn to page 263.

14. All you do is take the difference of the two elements…  That sounds easy!  What type of bond is formed between Oxygen and Sulfur?  Find electronegativities, subtract the higher one from the lower one. Then, look at the chart!

15. Bond Type Chart DEN RangeBond Type 0.0 – 0.39Nonpolar Covalent 0.4 – 0.89Moderately Polar Covalent 0.9 – 1.69Very Polar Covalent 1.7 or greaterIonic

16. Example 2  Determine the type of bond in MgO

17. Electronegativity Chart

18. Example 2  Determine the type of bond in MgO 1. Find electronegativity of each atom Mg = 1.3 Paulings, O = 3.4 Paulings

19. Example 2  Determine the type of bond in O 2 1. Find electronegativity of each atom Mg = 1.3 Paulings, O = 3.4 Paulings 2. Find Electronegativity Difference (∆EN) DEN = 3.4 – 1.3 = 2.1 3. Look at chart to determine bond type.

20. Bond Type Chart DEN RangeBond Type 0.0 – 0.39Nonpolar Covalent 0.4 – 0.89Moderately Polar Covalent 0.9 – 1.69Very Polar Covalent 1.7 or greaterIonic

21. Your Turn!  NaF  F 2  CH 4  AlN

22. Lewis Structure/Bond Formation  HF  P 2  SiO 2  CO

23. Your Turn!  H 2 S  HCN  Se 2  SiOH 2

24. Kriss Krossing/Straight Naming  Kriss Krossing will make you get a good grade on this test!  Then, name the compounds.

25. Kris Kross Method! Ca 3 As 2 Ca 2+ As 3-

26. Which charge ALWAYS comes first? POSITIVE!!!

27. Which type of element ALWAYS comes first? METAL!!!

28. K F Ba N Ga O Ca Cl K Si Co I

29. Using the Polyatomic Sheet!  Find formula:  Potassium Carbonate  Calcium Phosphate  Ammonium Hydroxide  Sodium Sulfate

30. Covalent Naming  PH 3  CO  N 2 O 3

31. From the name! Write the formula  Nitrogen Trifluoride  Silicon Monoxide  Phosphorous Pentachloride  Antimony Dibromide

32. Put everything away except a piece of paper and a pencil/pen

33. 1.Non-metals tend to _________ electrons when forming an ionic bond because they have more than 4 valence electrons. Gain

34. 2. Which of the following is NOT a covalent compound? a. CH 4 b. CO c. NaF d. H 2 O NaF

35. 3. What is the stable ion for Cesium? Cs 1+

36. 4. In which direction does ionization energy decrease on the periodic table? Why? Going down a group/family, because it is easier to steal electrons from higher energy levels

37. 5. Show the formation of the ionic bond between Sodium and Chlorine Na  Na + Cl  Cl - + 1e- Na + + Cl -  NaCl

38. 6. What element will have the highest 3 rd Ionization energy? Why? a. Carbon b. Aluminum c. Fluorine d. Magnesium Mg, because its 3 rd electron is in a full (happy) shell.

39. 7. What is the stable ion for Arsenic? As 3-

40. 8. What element will have the lowest 3 rd Ionization energy? Why? a. Carbon b. Aluminum c. Fluorine d. Magnesium Aluminum, because it wants to get rid of its 3 rd electron so it can have a full outer shell

41.  What is the correct Lewis Dot structure for Xenon? Xe

42.  What kind of bonds do noble gases make? None, they already have a full outer shell

43. 9. What is the correct Lewis Dot Structure for Phosphorus? P

44. 10. Show the formation of the ionic bond between Aluminum and Oxygen Al  Al 3+ O  O 2- + 3e- + 2e-

45. 11. Which element will have the lowest 1 st Ionization energy? Why? a. Magnesium b. Carbon c. Fluorine d. Potassium Potassium, because it wants to get rid of its 1 st electron so it can have a full outer shell

46. 12. Show the formation of the ionic bond between Magnesium and Fluorine Mg  Mg 2+ F  F - + 2e- + 1e-

47. 13. Name the following compound: Mg 3 N 2 Ionic: Magnesium Nitride

48. 14. Name the following compound: H 3 (PO 4 ) Ionic: Hydrogen Phosphate

49. 15. Name the following compound: N 3 P 5 Covalent: Trinitrogen pentaphosphate

50. 16. What is the chemical formula for the following compound?  Dinitrogen pentachloride N 2 Cl 5

51. 17. What is the chemical formula for the following compound?  Aluminum bromide Ionic, so kriss kross AlBr 3

52. 18. What is the chemical formula for the following compound?  Lead (IV) Hydroxide Ionic, so kriss kross Pb(OH) 4

53. 19. Draw the lewis dot structure for the following compound:  C 3 H 8

54. 20. Draw the lewis dot structure for the following compound:  HCP  What kind of bond is between C and P?

55. 21. Draw the lewis dot structure for the following compound:  HNO

56. 22. Draw the lewis dot structure for the following compound:  HCN

57. Exit Question  How do you plan to make sure you DOMINATE the Unit 4 Test?