I. Introduction to Bonding

1. I. Introduction to Bonding

2. Do Now: • Write down these dates for the Science Fair Project: • By Friday (for bonus points) and Monday (at the latest) send me your Experimental Design (Procedure) and Background Information Slides • Your weeks for experimentation are: 10/31 – 11/05; 11/06 – 11/10 • Due date for Data slide (a quiz grade) is 11/11/2016 • Due date for Analysis, Conclusion, and Reference Slides are 11/18/2016 • Your entire project (which is worth 5 grades (2 HW, 1 Quiz, 1 Lab, and 1 Test)) MUST be turned in prior to Thanksgiving Break!

3. Let’s start thinking… • How many ways can you combine the black pieces with the blue pieces?

4. Student Answers:

5. Rapid Recall: • What are the two things that elements can do with electrons? • Think of several substances you interact with daily, list those that are compounds:

6. A bonding party… • Think back to all you already know about elements (their trends, properties, etc.)—see how many things you can spot that make sense in the video…

7. Exit Card: • What is a bond? • What is a question you have about how elements bond?

8. Do Now: • Take the elements Aluminum (Al) and Sulfur (S) and determine the number of valence electrons each has (use their electron configuration for this) • Identify if each is a cation or anion (Cations have 1-3 VE and Anions have 5-7 VE) • Put them together using puzzle pieces like yesterday! • Congratulations, you’ve created Aluminum Sulfide!

9. A. Vocabulary Q1: Chemical Bond attractive force between atoms or ions that binds them together as a unit bonds form in order to… decrease potential energy (PE) increase stability

10. A. Vocabulary CHEMICAL FORMULA IONIC COVALENT Formula Unit Molecular Formula NaCl CO2

11. A. What are the differences? CHEMICAL FORMULA IONIC COVALENT Formula Unit Molecular Formula NaCl CO2

12. A. Vocabulary COMPOUND more than 2 elements 2 elements Binary Compound Ternary Compound NaCl NaNO3

13. A. Vocabulary ION 2 or more atoms 1 atom Monatomic Ion Polyatomic Ion Na+ NO3-

14. Quick Write • Create TWO questions for all the diagrams you just took down that begins with If I have…and How…

15. Dogs teaching Chemistry… • See if these dogs can answer your questions…if not (don’t worry) I will!

16. Exit Card: • Write down one thing from the video that I haven’t said in class today.

17. Do Now: Ionic or Covalent? • Hint: I (M-NM) and C (NM-NM) • HCl • NaCl • Mg3Al2 • H2O2 • Na(CH3OO)

18. B. Types of Bonds COVALENT IONIC e- are transferred from metal to nonmetal e-aresharedbetweentwononmetals Bond Formation Type of Structure truemolecules crystal lattice Physical State liquidorgas solid Melting Point low high Solubility in Water yes usuallynot yes (solution or liquid) Electrical Conductivity no Other Properties odorous

19. B. Types of Bonds METALLIC e- are delocalized among metal atoms Bond Formation Type of Structure “electron sea” Physical State solid Melting Point very high Solubility in Water no yes (any form) Electrical Conductivity malleable, ductile, lustrous Other Properties

20. Ionic, Covalent, Metallic?: • Electrons are transferred • Great Conductor of Electricity • Lustrous (shiny) • Crystal Lattice • True Molecules • Soluble in Water • Electrons are Shared • Electrons are in a “sea” (delocalized) • Low Melting Point

21. Pause for a Cause: • What are the different types of bonds? (3) • If a compound with a high melting point, fails to dissolve in water it must consist of ______________ bonds… • What if if does dissolve in water?

22. B. Types of Bonds RETURN

23. B. Types of Bonds RETURN

24. B. Types of Bonds Ionic Bonding - Crystal Lattice RETURN

25. B. Types of Bonds Covalent Bonding - True Molecules Diatomic Molecule RETURN

26. B. Types of Bonds Metallic Bonding - “Electron Sea” RETURN

27. C. Bond Polarity • Most bonds are a blend of ionic and covalent characteristics. • Difference in electronegativity determines bond type.

28. C. Bond Polarity • Electronegativity • Attraction an atom has for a shared pair of electrons. • higher e-neg atom  - • lower e-neg atom +

29. C. Bond Polarity • Electronegativity Trend (p. 151) • Increases up and to the right.

30. C. Bond Polarity • Nonpolar Covalent Bond • e- are shared equally • symmetrical e- density • usually identical atoms

31. - + C. Bond Polarity • Polar Covalent Bond • e- are shared unequally • asymmetrical e- density • results in partial charges (dipole)

32. C. Bond Polarity • Nonpolar • Polar • Ionic View Bonding Animations.

33. C. Bond Polarity Examples: • Cl2 • HCl • NaCl 3.0-3.0=0.0 Nonpolar 3.0-2.1=0.9 Polar 3.0-0.9=2.1 Ionic

34. Ne B. Lewis Structures • Octet Rule • Most atoms form bonds in order to obtain 8 valence e- • Full energy level stability ~ Noble Gases

35. Exit Card: • Examine the following compounds and determine their bond type: • ____________________ • ____________________ • ____________________ • Choose one compound above and draw the Lewis Dot structure of its atoms • Choose another compound and describe its properties

36. Do Now: • Look at the following Lewis Dot Structures: • Define a process you could use to create them!

37. X 2s 2p B. Lewis Structures • Electron Dot Diagrams • show valence e- as dots • distribute dots like arrows in an orbital diagram • 4 sides = 1 s-orbital, 3 p-orbitals • EX: oxygen O

38. Ne B. Lewis Structures • Octet Rule • Most atoms form bonds in order to obtain 8 valence e- • Full energy level stability ~ Noble Gases

39. Quick Write: • Draw the Lewis Dot Structure for Lithium Chloride (LiCl) • Draw the Lewis Dot Structure for Sulfur Dioxide (SO2)

40. Today… • A lab! • Groups of 4 • NO EATING THE MATERIALS • Grade comes from correct explanation of what is happening in your bond (this will be modeled momentarily)! • Each group member must initial beside the models they designed! (So at least two/member.) • Let’s start!

41. Sample: Ammonia • I would first model the compound using my gum drops and toothpicks. • Then draw the Lewis Dot Structure: • Covalent = “share e-”

42. Don’t Lose your handout! • Give the lab handout to the most trusted (and most often present) member of your group!

43. Do Now: • What is a polar covalent compound? • Can you give an example of one? • What is a non-polar covalent compound? • Can you give an example? • What is the Lewis dot structure for water?

44. Quick Write: • Draw the Lewis Dot Structure for Lithium Chloride (LiCl) • Draw the Lewis Dot Structure for Sulfur Dioxide (SO2)

45. Today…(for 20 minutes) • Finish your lab! • Draw all Lewis Dot Structures and each member must explain the two types of bonds that can be established between atoms in a paragraph—inc. characteristics and Lewis Dot Structures. • Each group member must initial beside the models they designed on your handout! (So at least two/member.) • Let’s start!

46. Look Back: • Briefly read through your notes and write 3-4 questions in the margin of your paper beside those notes to help you better understand them now and better study them later! • Remember you have a note-check tomorrow and an on-line quiz during which you may use your notes! • Please bring an electronic device tomorrow if possible! 

47. Do Now: 11/04/2016 • https://www.quia.com/quiz/6069530.html • Get out your notes and get ready to take the quiz on-line! • Any unauthorized web page viewing during the quiz—an automatic ‘0’ that cannot be made up!

48. On-Line Quiz: • All normal testing guidelines apply. • Do your best, use your notes. I will be walking around to check them as you work! • Finish early? Feel free to browse the web, but not videos/music/games (i.e., nothing that makes noise (even if you have headphones))!

49. 10 minutes—Science Fair/ Lab Work • If your lab is not done, please complete it now and turn it in—all groups require their lab handout and one paragraph per person! • If you lab is done, spend this time working on other slides in your Science Fair project. Complete the Hypothesis slide, materials slide, etc.

50. Have a great weekend!