Improvements

1. Improvements • Students write subscripts in names! • Students don’t know when to chris cross…especially with transition metals • Students sometimes want to reduce covalent molecules • Need to make notes that follow powerpoint…adapt notes of hardens • Also change the accompanying worksheets • Include equations for reacting sodium n stuff with alkali metals (and burning equation)…maybe other metals as well • Also cut them on aluminum foil, wash the aluminum foil as well & talk about safety with chemicals • Have students determine properties of each family by observing demo, video, or reading, or thinking aloud • Last chapter should have had students make bohr models & electron dot diagrams on the periodic table, like an enlarged one, which would help to see trends • Find website that students can practice naming & getting formulas for compounds on • Worksheets don’t correlate with order of teaching in notes. Fix this! Must change one of the two… • Also must explain more in depth again what his happening with bonding the first time you do it, what the subscripts mean, what the charges mean, why they have the charges, ask questions on those topics • Talk more about how where first element in chemical is on periodic table determines how to name it…include in notes • Ask tom harden for his advice and info • Need some demos to go with this! And group work (like the cool one where I write equations around the room) • Get instructional videos online

2. Bell Work 1/2/14 – 3 min • Start a new bell work sheet titled “Periodic Table & Bonding” • Draw the Lewis Dot Diagram for: • Na • Mg • Al • Si • P • S • Cl • Ar • W5SAYBoS

3. Midterm/Final Schedule • Friday January 10 • Pd 1,4, & 6 • Monday January 13 • Pd 3 & 7 • Tuesday – Regular classes • Wednesday January 15 • Pd 2 & 5 • Thursday – makeup day • Friday – no school! • Monday – no school! • Tuesday – semester 2 begins

4. Today you are going to…take notes on the periodic table. So you can…predict the charges & properties of elements, which will later enable you to see how they bond. You’ll know you’ve got it when you can • Identify the groups & periods of elements • Determine the charges of elements using periodic table

5. The Periodic Table

7. Dmitri Mendeleev – organized elements according to atomic mass and noticed a repeating pattern of properties • Idea came to him in a dream! • Lead to discovery of periodic law • Repeating pattern = periodic

8. Mendeleev put the elements with similar properties into columns, (now called families or groups) creating the periodic table! • Sometimes he had to move an element over a column so it would be in a column with similar elements. Then they weren’t exactly in order of increasing atomic mass (but close). • Left 3 blank spaces • Said elements would be discovered and predicted their properties (1871) • By 1886, Sc, Ga, & Ge were discovered, so people began to like Mendeleev’s periodic table.

11. Bell Work • Draw the Lewis Dot Diagram for: • Na • Mg • Al • Si • P • S • Cl • Ar

12. Important Info! • Valence electrons • electrons in an atom’s outer energy level • Largely determine the chemical properties of an atom • Octet rule • All atoms want 8 valence electrons* • They will gain, lose, or share electrons to make this happen. • When they gain, lose, or share electrons , they form • compounds

13. Organization of Periodic Table • Elements arranged in order of increasing atomic number (number of _____ in atom). • Families/groups • Columns (vertical; up & down) • Have similar properties because they have the same number of valence electrons! • Periods • Rows (horizontal; left & right)

14. Hydrogen • Hydrogen has many unique properties, so it is not part of any family.

15. Group 1 – Alkali Metals • Soft & shiny • Lose their ___ valence e- to form compounds • most reactive metals because they easily give away 1 e- • Charge of +1 • Demo? • Run water on aluminum foil • Extremely reactive! • Not found alone in nature • Rubidium & Cesium • Francium - most reactive metal!

16. Group 2 Alkaline-Earth Metals • Denser, stronger, & higher melting pts than alkali metals • Lose their ____ valence e- to form compounds • Charge of ____ • Reactive, but less reactive than alkali metals • (still too reactive to be found as pure elements in nature)

17. Groups 3 –12 Transition Metals • Shiny, good conductors • Most have 2 valence electrons • Less reactive…some are very unreactive & are found in nature as pure elements • Lose different number of e-, so charges vary

18. Group 13 Boron Group • Lose their ___ valence e- to form compounds +3 charge

19. Group 14 Carbon Group • Gain or lose their ___ valence e- to form compounds +4 or -4

20. Group 15 Nitrogen Group • Gain ___ valence e- to form compounds • Charge of -3

21. Group 16 Chalcogens(or Oxygen Group) • Gain ___ valence e- to form compounds • Charge of -2

22. Group 17 Halogens • Most reactive nonmetals • React with most reacting metals • Gain ____ valence e- to form compounds • Charge of ____

23. Group 18 Noble Gases • Nonreactive because they have _____ valence e- • Gases at room temperature

24. Lanthanide Series • Shiny metals, similar reactivity to alkali earth metals • Filling f orbital

25. Actinide Series • All radioactive • Only first 4 found at all in nature…rest were made in lab • Filling f orbitals

26. Other stuff

27. Metalloids/semiconductors – B, Si, Ge, As, Sb, Te • Stair-step between metals and non metals • Some properties of metals, some of nonmetals

28. Other Metals! • Al, Ga, In, Sn, Ti, Pb, Bi, Po

29. Identify the number of valence electrons in each column of the periodic table.

30. SOLIDS, LIQUIDS, & GASES

31. Mr. Shuster’s Famous Uncle! THE Dr. Brinclhof

32. Diatomic Elements • Dr. BrINClHOF • Memorize these!

33. Meet the Elements - TMBG • http://www.youtube.com/watch?v=Uy0m7jnyv6U

34. Bell Work 1/7/13 – 3 min • List the 7 diatomic elements. • What does diatomic mean? • What halogen is in the 3rd period? • W5SAYWoS

35. Bell Work – 3 min • According to the ___________ rule, all atoms “want” _____ valence electrons. They will form chemical bonds to get them. • What is the lightest Alkaline Earth metal? • What element is located in the 4th period and has three valence electrons? • What element is the heaviest Noble Gas? • What group of elements has the oxidation state (oxidation number; “charge”) of -1? • What group of elements has the oxidation state (oxidation number; “charge”) of +2?

36. Bell Work 12/20 – 5 minutes • How can you tell if two elements are going to form an ionic compound or a covalent compound? • Name the following ionic compounds. (If they’re covalent molecules, do nothing.) 2. NaCl 3. CO2 4. K3P 5. CaO 6. Sr3N2 7. CH4 8. Fr2O 9. CsCl 10. NO2  11. What’s that little # 2 called?

37. Bell Work 1/8/13 – 3 min • What member of the nitrogen group is in the third period? • What group is aluminum in? • What group is potassium in? • What is the charge of lithium? How many valence electrons does it have? • What is the charge of oxygen? How many valence electrons does it have? • What noble gas is in the 3rd period?

38. Colored Periodic Table!! • Highlight zigzag line to separate metals & nonmetals • Identify ones that are a gas at room temperature • Identify ones that are liquid at room temperature • Identify diatomic elements • Color & Make a key (each group must be a different color) • Hydrogen • Alkali Metals • Alkali Earth Metals • Transition Metals • Other Metals (Al, Ga, In, Sn, Tl, Pb, Bi, Po) • Metalloids (semiconductors) (B, Si, Ge, As, Sb, Te) • Other nonmetals (C, N, O, P, S, Se) • Halogens • Noble Gases • Lanthanide series • Actinide series

39. Quiz Wednesday! • Diatomics • Periodic table • Charges • Properties of types of bonds • Identify types of bonds

40. Today you are going to…take notes on ionic & covalent bonds. So you can…explain how & why bonds form and describe the characteristics of ionic & covalent bonds. You’ll know you’ve got it when you can • Explain how & why bonds form • Complete the VENN diagram on ionic & covalent bonds

41. IONIC & COVALENT BONDS

42. Bonding - According to the octet rule, atoms want 8 electrons in their outer energy level. • To achieve this, elements chemically combine to form compounds (ionic bonds) or molecules (covalent bonds). • All bonds are a result of chemical reactions which result in new substances (products) being formed.

43. Ionic Bonds • Ion – atom (or atoms) that have gained or lost e-, and therefore have a + or - charge • Form compounds • Metal & nonmetal (or polyatomic ions) • Form when atoms gain or lose e- (e- transferred) • Atom gains e- , becomes Anion, negative charge • Metals usually form a cation • Atom looses e-. becomes cation, positive charge • Composed of negative & positive ions + charge = - charge, cancel out • Create a lattice of charged particles (look at magnets) • Look at charges on periodic table

45. Ionic Bond • Simulation of sodium reacting with chlorine Na + Cl2 NaCl • http://www.visionlearning.com/library/flash_viewer.php?oid=1349&mid=55

47. Covalent Bonds • Form covalent molecules • Names have prefixes: carbon dioxide, sulfur hexafluoride • 2 nonmetals • Form when atoms “share” e- • Coworkers share an office • Use prefixes when naming • Nonmetals can easily share because they’re close to each other on the periodic table. • Memory strategy…NOT REALLY TRUE AT ALL! • Why wouldn’t it make sense for metals to “share” electrons?

48. Covalent Bond • Simulation of hydrogen bonding • http://www.visionlearning.com/library/flash_viewer.php?oid=1348&mid=55

49. Covalent Bond