2. THE P PP PERIODIC TABLE

3. THEPERIODIC TABLETHE PERIODIC TABLETHEPERIODIC TABLETHE PERIODIC TABLE

4. Not to be confused with this one…

5. Not to be confused with this one…

6. I. Introduction A. The Periodic Table is a table of the elements arranged according to repeated changes in chemical properties.

7. I. THE PERIODIC TABLE B.Historical Development 1.History records the isolation of the first element (phosphorous) in 1649. By 1869, a total of 63 elements had been isolated, but there was still no organized means to arrange them. Then along came a Russian named Mendeleev…

8. I. THE PERIODIC TABLE B.Historical Development 2. Originally developed by Dimitri Mendeleev Dimitri Mendeleev He arranged the elements in order of increasing atomic masses

9. B. Historical Development Mendeleev’s table had blank spaces. This caused Mendeleev to hypothesize that there other unknown elements. This bold hypothesis allowed Mendeleev to predict the properties and the mass numbers of these undiscovered elements.

11. B. Historical Development 2.Modern P.T. Henry MoseleyMade by Henry Moseley atomic numberElements are arranged by increasing atomic number and similarity of properties.

12. II. ORGANIZATION OF THE P. T. A.GROUPS OR FAMILIES 1.The vertical columns in the periodic table 2.Increase in atomic number as one goes down a family

13. II. ORGANIZATION OF THE P. T. A.GROUPS OR FAMILIES 2.Two main groups: Group A: Representative Elements Group B: Transition Elements Group A Group BGroup A

14. A. GROUPS OR FAMILIES 4. Elements in the same family have S imilar properties valenceThe same number of electrons in their outer (valence) energy level

15. II. ORGANIZATION OF THE P. T. B. Periods or Series 1.The horizontal rows 2.Increase in atomic number from left to right 3.Each represents a new valence energy level

16. 4.LanthanideSeries 4.Lanthanide Series Rare Earth Metals B. Periods

17. 5.Actinide Series All are radioactive Some are not found in nature Transuranium Elements: B. Periods Elements above atomic # 92. All are synthetic

18. Note: Together the Lanthanide Series and Actinide Series are referred to as the B. Periods Inner Transition Elements

19. C. Element location on the PT Use the period and group numbers as an “address” to help locate an element

20. III. Metals, Nonmetals, Metalloids

24. A. Stair Step Line 1.Separates Metals, Nonmetals and metalloids a.Left: metals b.Right: nonmetals c.Touching line: metalloids

25. Look at the stair step line on your P.T.

27. III. Metals, Nonmetals, Metalloids Look to the Left of the Line…

28. Look to the Left of the Line

29. III. Metals, Nonmetals, Metalloids B. Metals 1.Most elements are metals (88) 2.Examples: Zinc, iron, copper 3.Located to the left of the stair step line Exception ?

31. B. Metals 4.Physical Properties –Luster –Luster (shininess) –Good conductors –Good conductors of heat and electricity –High density –High density (heavy for their size) –High melting point –Ductile –Ductile (drawn out into thin wires) –Malleable –Malleable (hammered into thin sheets)

32. 5. Chemical Properties Easily lose electronsEasily lose electrons B. Metals Corrode easily. Corrode easily.

33. ELements to the Left of the Line Lose eLectrons

34. III. Metals, Nonmetals, Metalloids C. Nonmetals 1.Examples: P, C, S 2.Located to the right of the stair step line Exception: H is a nonmetal

35. C. Nonmetals 3. Physical Properties dull Poor conductor of heat and electricity Brittle (breaks easily) Not ductile Not malleable Low density Low melting point

36. C. Nonmetals 3. Chemical Properties Tend to gain electrons

37. Elements to the riGhtof the line Gain electrons

38. D. Metalloids 1.Examples: Si, B, As 2.On the stair step line Exception: Al is a metal B Si

39. III. Metals, Nonmetals, Metalloids D. Metalloids 3. Physical Properties SolidsSolids Can be shiny or dullCan be shiny or dull Can be ductile or notCan be ductile or not Can be malleable or brittleCan be malleable or brittle Semiconductors - Conduct heat and electricity better than nonmetals but not as well as metalsSemiconductors - Conduct heat and electricity better than nonmetals but not as well as metals

40. The Periodic Table Getting back to itGetting back to it

41. IV. The Families A. Alkali Metal Family 1.Group IA 2.Properties Lowest densities 1 valence electron Largest atomic radii Highly reactive –Stored under kerosene –Not found free in nature

42. IV. The Families B. Alkaline Earth Metal Family 1.Group IIA 2.Properties Two electrons in the outer shell 2 nd highest reactive metals Not found free in nature

43. IV. The Families C. Transition Metals 1.Group B Families 2.Properties Can have varying numbers of valence electrons Form brightly colored compounds

44. IV. The Families D. Boron Family 1.Group IIIA 2. Al is the most abundant metal in the Earth’s crust 3. Properties Have 3 valence e - Contains metals & metalloids

45. IV. The Families E. Carbon Family 1.Group IVA 2.Properties 1. Have 4 valence electrons 2. Family contains metals, metalloids, and nonmetals 3.Forms of carbon: diamond, coal, coke 4.Si second most abundant element in the Earth ’ s crust

46. IV. The Families F. Nitrogen Family 1.Group VA 2.Properties Have 5 valence electrons Contains metals, metalloids, and nonmetals 3.N makes up 80% of air

47. IV. The Families G. Oxygen Family 1. Group VIA 2. Properties Have 6 valence electrons 3. O most abundant element on earth

48. IV. The Families H. Halogen Family 1.Group VIIA 2.Properties Have 7 valence electrons Most reactive nonmetals 3.React with IA and IIA family members to form salts 4.F the most chemically reactive of all elements

49. IV. The Families Noble Gas Family I. Noble Gas Family 1.Group VIIIA 2.Properties Have 8 valence e - (full valence energy level) Inertstable, non-reactiveInert, stable, non-reactive All are gases Low boiling points

50. Periodic Trends

51. A. Periodic Law When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals. When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.

52. B. Chemical Reactivity Families Families o Similar valence e - within a group result in similar chemical properties

53. B. Chemical Reactivity Alkali Metals Alkali Metals Alkaline Earth Metals Alkaline Earth Metals Transition Metals Transition Metals Halogens Halogens Noble Gases Noble Gases

54. C. Other Properties Atomic Radius Atomic Radius o size of atom © 1998 LOGAL zFirst Ionization Energy Energy required to remove one e - from a neutral atom. © 1998 LOGAL zMelting/Boiling Point

55. D. Atomic Radius Atomic Radius Atomic Radius Li Ar Ne K Na

56. D. Atomic Radius Atomic Radius Atomic Radius Increases to the LEFT and DOWN

57. D. Atomic Radius Why larger going down? Why larger going down? o Higher energy levels have larger orbitals o Shielding - core e - block the attraction between the nucleus and the valence e - Why smaller to the right? Why smaller to the right? o Increased nuclear charge without additional shielding pulls e - in tighter

58. E. Ionization Energy First Ionization Energy First Ionization Energy K Na Li Ar Ne He

59. E. Ionization Energy First Ionization Energy First Ionization Energy Increases UP and to the RIGHT

60. E. Ionization Energy Why opposite of atomic radius? Why opposite of atomic radius? o In small atoms, e - are close to the nucleus where the attraction is stronger

61. F. Melting/Boiling Point Melting/Boiling Point Melting/Boiling Point Highest in the middle of a period.

62. G. Ionic Radius Ionic Radius Ionic Radius Cations (+) xlose e - xsmaller © 2002 Prentice-Hall, Inc. Anions (–) xgain e - xlarger

63. Examples Which atom has the larger radius? Which atom has the larger radius? Beor Ba Ca or Br BaCa

64. Examples Which atom has the higher 1st I.E.? Which atom has the higher 1st I.E.? N or Bi Baor Ne NNe

65. Examples Which atom has the higher melting/boiling point? LiorC CrorKr C Cr

66. Examples Which particle has the larger radius? Which particle has the larger radius? S or S 2- Alor Al 3+ S2- Al