2. Chemistry 12/9/13 “Quality is never an accident. It is always the result of intelligent effort” John Ruskin DO NOW: 1.In your notes: When you look at the periodic table, how can you tell what energy level the outermost electrons are on? AGENDA: 1.Review periodic trends quiz 2.Students will be able to describe how ionic bonds form by taking notes ANNOUNCEMENT: 1. Science Club is meeting tomorrow! Be there or be square!

3. Chemistry 12/10/13 “Quality is not an act. It is a habit” -Aristotle DO NOW: 1.In your notes: How many valence electrons are in the following elements?: a. Ca b. I c. Ne AGENDA: 1.Students will be able to describe what valence electrons are by completing a worksheet ANNOUNCEMENT: 1. Science Club is meeting today! Be there or be square!

4. Chemistry 12/11/13 “Associate yourself with people of good quality, for it is better to be alone than in bad company” DO NOW: 1.In your notes: How many electrons does Sulfur need to follow the octet rule? What about Nitrogen? AGENDA: 1.Students will be able to describe what Lewis dot structures are by completing a worksheet ANNOUNCEMENT: 1. Extra credit due Friday, 12/20

5. Chemistry 12/12/13 “Quality means doing it right when no one is looking.” - Henry Ford DO NOW: 1.In your notes: only using the periodic table, determine the number of valence electrons in the following atoms: a. Li b. Pc. F AGENDA: 1.Students will be able to describe what Lewis dot structures are by completing a worksheet ANNOUNCEMENT: 1. Extra credit due Friday, 12/20

6. Why are electrons important? 1)Elements have different electron configurations  different electron configurations mean different types of bonding  Bonding determines what compounds will form to make up our environment, our body, etc.

7. electron shells a)Atomic number = number of Electrons b)Electrons vary in the amount of energy they possess, and they occur at certain energy levels or electron shells. c)Outermost electron shells determine how an atom behaves when it encounters other atoms

8. Electrons are placed in shells according to rules: 1)The 1st shell can hold up to two electrons, and each shell thereafter can hold up to 8 electrons.

9. Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to N would like to O would like to Gain 4 electrons Gain 3 electrons Gain 2 electrons

10. Octet Rule Atoms will always try to attain the electron configuration of the nearest noble gas on the period table Because noble gases have filled energy levels, they are unreactive Which noble gas electron configuration does potassium try to attain? Notice Helium is an exception to the “8” rule!

11. Valence electrons Electrons in the highest (outer) electron level Have most contact with other atoms Known as valence electrons Outer shells of noble gases contain 8 valence electrons (except He = 2) Example: Ne 2, 8 Ar2, 8, 8

12. The group number tells you how many valence electrons an element has!

14. Honors Chemistry 12/10/13 “Quality is not an act. It is a habit” -Aristotle DO NOW: 1.In your notes: How many valence electrons are in the following elements?: a. Ca b. I c. Ne AGENDA: 1.Students will be able to describe what Lewis dot structures are by completing a worksheet ANNOUNCEMENT: 1. Science Club is meeting today! Be there or be square!

15. Electron Dot Structures Symbols of atoms with dots to represent the valence-shell electrons 1 2 13 14 15 16 17 18 H  He:            Li  Be   B   C   N   O  : F  : Ne :                    Na  Mg   Al   Si   P   S  : Cl  : Ar :        

16. Learning Check A. X would be the electron dot formula for 1) Na2) K3) Al B. X would be the electron dot formula for 1) B2) N3) P

17. Chemical bonds: an attempt to fill electron shells to follow the octet rule and become stable 1.Ionic bonds 2.Covalent bonds 3.Metallic bonds

18. IONIC BOND bond formed between two ions by the transfer of electrons

19. Formation of Ions from Metals Ionic compounds result when metals react with nonmetals Metals lose electrons to match the number of valence electrons of their nearest noble gas Positive ions form when the number of electrons are less than the number of protons Group 1 metals  ion 1+ Group 2 metals  ion 2+ Group 13 metals  ion 3+

20. Formation of Sodium Ion Sodium atom Sodium ion Na  – e   Na + 2-8-1 2-8 ( = Ne) 11 p + 11 p + 11 e - 10 e - 0 1 +

21. Formation of Magnesium Ion Magnesium atom Magnesium ion  Mg  – 2e   Mg 2+ 2-8-2 2-8 (=Ne) 12 p + 12 p + 12 e- 10 e - 0 2 +

22. Some Typical Ions with Positive Charges (Cations) Group 1Group 2Group 13 H + Mg 2+ Al 3+ Li + Ca 2+ Na + Sr 2+ K + Ba 2+

23. Learning Check A. Number of valence electrons in aluminum 1) 1 e - 2) 2 e - 3) 3 e - B. Change in electrons for octet 1) lose 3e - 2) gain 3 e - 3) gain 5 e - C.Ionic charge of aluminum 1) 3- 2) 5- 3) 3 +

24. Solution A. Number of valence electrons in aluminum 3) 3 e - B. Change in electrons for octet 1) lose 3e - C.Ionic charge of aluminum 3) 3 +

25. Learning Check Give the ionic charge for each of the following: A. 12 p + and 10 e - 1) 02) 2+3) 2- B. 50p + and 46 e- 1) 2+2) 4+3) 4- C. 15 p + and 18e- 2) 3+ 2) 3-3) 5-

26. Ions from Nonmetal Ions In ionic compounds, nonmetals in 15, 16, and 17 gain electrons from metals Nonmetals add electrons to achieve the octet arrangement Nonmetal ionic charge: 3-, 2-, or 1-

27. Fluoride Ion unpaired electronoctet     1 - : F  + e  : F :     2-7 2-8 (= Ne) 9 p+ 9 p + 9 e- 10 e- 0 1 - ionic charge

28. Formation of sodium chloride (NaCl) http://www.youtube.com/watch?v=5IJqPU1 1ngYhttp://www.youtube.com/watch?v=5IJqPU1 1ngY

30. Ionic Bonds: One Big Greedy Thief Dog!

31. 1). Ionic bond – electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.

33. Chemistry 12/10/13 “Quality is not an act, it is a habit.” - Aristotle DO NOW: 1.In your notes: How many valence electrons do the following atoms have? A) barium B) iodine C) oxygen AGENDA: HOMEWORK: 1. Extra Credit due 12/20: Bring either a box of kleenex OR a hand sanitizer. 5 pts extra credit.

34. COVALENT BOND bond formed by the sharing of electrons

35. Covalent Bond Between nonmetallic elements of similar electronegativity. Formed by sharing electron pairs Stable non-ionizing particles, they are not conductors at any state Examples; O 2, CO 2, C 2 H 6, H 2 O, SiC

37. Bonds in all the polyatomic ions and diatomics are all covalent bonds

38. when electrons are shared equally NONPOLAR COVALENT BONDS H 2 or Cl 2

39. 2. Covalent bonds- Two atoms share one or more pairs of outer-shell electrons. Oxygen Atom Oxygen Molecule (O 2 ) Oxygen Molecule (O 2 )

40. when electrons are shared but shared unequally POLAR COVALENT BONDS H2OH2O

41. Polar Covalent Bonds: Unevenly matched, but willing to share.

42. - water is a polar molecule because oxygen is more electronegative than hydrogen, and therefore electrons are pulled closer to oxygen.

43. METALLIC BOND bond found in metals; holds metal atoms together very strongly

44. Metallic Bond Formed between atoms of metallic elements Electron cloud around atoms Good conductors at all states, lustrous, very high melting points Examples; Na, Fe, Al, Au, Co

45. Metallic Bonds: Mellow dogs with plenty of bones to go around.

46. Metallic Bond, A Sea of Electrons

47. Metals Form Alloys Metals do not combine with metals. They form Alloys which is a solution of a metal in a metal. Examples are steel, brass, bronze and pewter.

48. Formula Weights Formula weight is the sum of the atomic masses. Example- CO 2 Mass, C + O + O 12.011 + 15.994 + 15.994 43.999

49. Practice Compute the mass of the following compounds round to nearest tenth & state type of bond: NaCl; 23 + 35 = 58; Ionic Bond C 2 H 6 ; 24 + 6 = 30; Covalent Bond Na(CO 3 ) 2 ; 23 + 2(12 + 3x16) = 123; Ionic & Covalent