3. I. History of the P.T. A.) Dmitri Mendeleev –Russian Chemist who 1st arranged elements in usable manner (1869). –Arranged elements in order of increasing atomic mass (“weight”).

4. History - Mendeleev (cont’d) Noticed chemical and physical properties appearing at periodic intervals. Paved the way for current P.T. “Father of the Periodic Table” Mendeleev link (pictures 1)Mendeleev linkpictures 1

5. History – Henry Moseley B.) Henry Moseley (1915) “Reorganized” the P.T. Arranged according to increasing atomic #. Current (present) P.T.

6. History – Periodic Law Periodic Law - Relationship b/t properties of elements and their atomic #. Physical and Chemical properties show a periodic pattern when arranged according to atomic #. P.T. is arranged according to this law.

8. II. Division of the P.T. Q.: How is the electron configuration affected??? –P.T. showing IonizationP.T. showing Ionization

9. A.) General Info. P.T. often includes phase at room temperature (temp.) “ STP ” ( S tandard T emperature and P ressure) Table A on Chemistry Ref. Tables. 3 Phases of matter... –Solid (s), liquid (l), gas (g)

10. Phases @ STP Solid(s) – Vast majority of elements Liquid(l) – Hg (mercury – metal), Br (bromine – nonmetal). Gas(g)– H, O, F, N, Cl, + Group 18 Group 18 = He, Ne, Ar, Kr, Xe, Rn

11. B.) Periods Horizontal (  ) rows (1-7) Period # = # of E.L. (a.k.a. “principal energy levels” or “shells”) –Eg.1: Elements in Period 3 have _____E.L.

12. Periods (cont’d) Na  Mg  Al  Si  P  S  Cl  Ar Q.1.: List how many E.L. each element has? Q.2.: List how many valence electrons each element has?

13. Periods (cont’d) # of valence electrons increases from left  right

14. Periods (cont’d) Q.3.: How can we describe the location of solids and gases within a period? Solid (left side)  Gas (right side) Q.4.: How can we describe the location of Metals and Nonmetals within a period? Metals (left side)  Nonmetals (right side)

15. C.) Groups Vertical (up and down) columns (1-18). 1.) Elements in same group = same # valence electrons –Except Helium.

16. Quick Review Q.1: What are valence electrons? Q.2: What is the maximum # of valence electrons allowed in an atom? Q.3: How many electrons do all elements want to have?

17. Groups (cont’d) Elements in the same group have more in common than elements in the same period. The closer the elements in the same group, the more similar their properties.

18. Important Group Names Group(s)Group Name 1Alkali Metals (Very Reactive) 2Alkaline Earth Metals (Very Reactive) 3-11Transition Metals (Transition Elements) 17Halogens (Very Reactive) 18Noble Gases (Not Reactive) *Stable

19. Properties of the Elements Q. What are the 3 types (not phases) of elements? –Draw the Periodic Table and divide it according to these 3 types of elements.

20. METALS 75% of the Periodic Table

21. METALLOIDS (Semi-Metals) Stair line on P.T. (label it!) Share both Metal / Nonmetal properties Metalloids = B, Si, As, Ge, Sb, Te, At –Al and Po are NOT metalloids. What are they???

22. NONMETALS Contain the only elements on the P.T. in the gas (g) phase.

23. Properties of the Elements METALSNONMETALS

24. Draw the Bohr models of Sodium and Chlorine (side-by-side) –Q. How do the structures of these elements differ? –Q. Describe what each will do to achieve the Octet Rule.

25. –P.T. showing IonizationP.T. showing Ionization

26. Properties of Metals Solid (except Hg) Silver-colored (except Cu and Au) Soft Malleable – “hammered into shape” Ductile – form into wire Excellent conductors of heat and electricity High melting point (M.P.) Luster – shiny Transitional Metals form colored compounds Few valence electrons Lose electrons to form “+” ions

27. ** Which of the following metal ions forms a colored compound when bonded to a nonmetal? 1.K +1 2.Ba +2 3.Cu +2 4.Sr +2

28. Properties of Nonmetals All Phases (solid, liquid (Br), and gas) Dull surface (no luster) Hard solids Brittle (not malleable or ductile) Poor conductors of heat and electricity. 4 or more valence electrons Gain electrons to become “–” ions Low Melting Point (in general)

29. Properties of Metalloids All solid (s) @ STP Contain properties of both Metals and Nonmetals.

30. (First) Ionization Energy – amount of energy needed to remove the most loosely held electrons.

31. Draw the Bohr models of Sodium and Fluorine (side-by-side) –Q.1. Which element has a greater ionization energy? –Q.2. What can we conclude about the ionization energy of metals compared to nonmetals?

32. The “Shielding” Effect The “Shielding” Effect refers to the weakening of attraction (“magnetic pull”) between the nucleus and the valence electrons, caused by the energy levels (shells) in between them. ** Shielding LOWERS the Ionization Energy! ** –Q.1. When does “Shielding” increase? –Q.2. Which element would have more shielding, Chlorine or Bromine?

33. (First) Ionization Energy Draw Lithium and Sodium side-by-side –Q.1. Which element has a greater ionization energy? ** Think in terms of MAGNETS! **... (and the Shielding Effect)

34. Q.4: Draw Na, Mg, and K side by side. Which of these 3 examples will take the least amount of energy (“ionization energy”) to lose 1 e ??? Why?

35. Q. Which Metals do you think contain the MOST metal properties??? Explain.

36. Q. Which Nonmetals do you think contain the MOST nonmetal properties??? Explain.

37. Electronegativity – the attraction for electrons by an element “Electronegativity is the attraction for an e”

38. Draw the Bohr models of Lithium and Fluorine (side-by-side) –Q.1. Which element has a greater electronegativity? –Q.2. What can we conclude about the electronegativity of metals compared to nonmetals?

39. Electronegativity Draw Fluorine and Chlorine side-by-side –Q.1. Which element has a greater electronegativity? ** Think in terms of MAGNETS! **

40. Electronegativity Draw Neon –Q.1. How would you describe the electronegativity? ** Think in terms of MAGNETS! **

41. Atomic Radius Atomic Radius: ½ the distance between two adjacent nuclei.

42. Trends in the P.T. 1.) Reactive Groups: –Metals: Group 1 (Alkali) and Group 2 (Alkaline Earth) are VERY REACTIVE! Group 1 are the MOST REACTIVE Metals. Reactivity of Group 1 –Nonmetals: Group 17 (Halogens) are VERY REACTIVE! –Group 18 is STABLE (NOT Reactive)

43. Trends in the P.T. Atomic Radius –Within a Period –Within a Group (Atomic Radii) (Atomic Radii.2) (Atomic Radii.3)Atomic RadiiAtomic Radii.2Atomic Radii.3

44. Trends in the P.T. Ionization energy –Within a Period: –Within a Group:

45. Trends in the P.T. Electronegativity –Within a Period: –Within a Group:

46. Graphing Trends Rule #1: Always set up graph as you do in all science/math classes. A.) Title: Independent (X) vs. Dependent (Y) Variable B.) Set up X (independent) and Y (dependent) axes. C.) Always have Equal INCREMENTS!!! D.) Use as much of the graphing space as possible. E.) Always write a CONCLUSION!!!

47. Rule #2: Make a Table! –Refer to this table when making the graph. Rule #3: Always circle your dots!

48. Graphing (Cont’d) 1.) Graph Group 1 (atomic #) vs. Electronegativity (Electron Affinity)Group 1 (atomic #) vs. Electronegativity (Electron Affinity) 2.) Graph the trend of Ionization Energy in Period 2. (Period 2 vs. Ionization Energy) 3.) Graph the trend of Atomic Radius in Group 1. (Group 1 vs. Atomic Radius) Graphing Classwork/Homework.Graphing Classwork/Homework

49. Ionic Radius Ionic radius – The new radius of an element, after it becomes an ion. –Eg. Draw Na and Cl. Show their radius as ions. What is the general rule for the ionic radius of Metals? Nonmetals?

50. Allotropes Allotrope : An element that exists as 2 or more forms in the same phase. Oxygen Ozone Form O2O2 O3O3 Phase (g)

51. The Element Song