1. Periodic Table Flashcards

2. Group or Family Column (up & down)

3. Period or Series Row (across)

4. # of valence electrons Elements in the same column have the same …

5. # of principle energy levels Elements in the same row have the same …

6. the number of valence electrons Chemical properties are determined by

7. one valence electron Elements in column 1 (IA) have

8. two valence electrons Elements in column 2 (IIA) have

9. Noble gases The name of the family in column 18 (VIIIA)

10. Halogens The name of the family in column 17 (VIIA)

11. H 2, N 2, O 2, F 2, Cl 2, He, Ne, Ar, Kr, Xe, & Rn Elements that are gases at room temperature

12. Hg (metal) & Br 2 (nonmetal) Elements that are liquids at room temperature

13. Diatomic Elements H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2

14. Chemical properties Elements in the same column have similar

15. 3 valence electrons Elements in column 13 (IIIA) have

16. 4 valence electrons Elements in column 14 (IVA) have

17. Half the diameter of an atom, a measure of size Atomic radius

18. Increases as you go down a column (more principle energy levels) & decreases across a row (greater effective nuclear charge) Trends for atomic radius

19. Alkali Metals Name of family for column 1

20. Alkaline Earth Metals Name of family for column 2

21. Amount of energy required to remove the most loosely held valence electron from a gas phase atom Ionization Energy

22. Decreases as you go down a column, increases across a row Trends for Ionization Energy

23. Format of Ionization Equation Na(g) + energy  Na +1 (g) + 1e -

24. Ionization Energy Always Endothermic!

25. LOSERS Metals are “_______”

26. Positive ions that are smaller than the parent atom. Metals lose electrons to form …

27. Most active metals Most “metallic” character Metals with the lowest ionization energy

28. Most Active Metal Cs

29. Ionization energy & Potential Well

30. What property do we use to assess the character of metals? Ionization Energy The best metals are the best losers! They have the lowest I.E.!

31. Properties of metals 1)Malleable 2)Ductile 3)Good conductors of heat & electricity 4)Lustrous 5)Low ionization energy 6)Low electronegativity

32. Properties of nonmetals 1)Brittle 2)Dull 3)Poor conductors of heat & electricity 4)High ionization energy 5)High electronegativity

33. Metals tend to have … Only a few valence electrons: 1, 2, or 3

34. winners Nonmetals are “_______”

35. Negative ions that are larger than the parent atom. Nonmetals gain electrons to form …

36. What property do we use to assess the reactivity of NONmetals? Nonmetals are winners, so it makes sense to use a property that has to do with GAINING electrons.

37. Electron Affinity Amount of energy required to add an extra electron to a neutral atom in the gas phase.

38. Format for Electron Affinity Equation Na(g) + 1e - + energy  Na -1 (g)

39. Electron Affinity Can be endothermic or exothermic Is really tough to measure

40. Compare Ionization & Electron Affinity Equations Na(g) + energy  Na +1 (g) + 1e - Na(g) + 1e - + energy  Na -1 (g) Electrons on different sides Ions on different sides Ions have opposite charges

41. What property do we use to assess the nonmetallic character? Electronegativity This is a “calculated” value

42. Electronegativity Ability of an atom to attract electrons in a bond.

43. Most Electronegative Element Fluorine

44. High ionization energies & high electronegativies Nonmetals have

45. low ionization energies & low electronegativies Metals have

46. Negative ions are Larger than the parent ion

47. Positive ions are smaller than the parent ion

48. Metalloids are located On the staircase

49. Metals are located To the left of the staircase (except for H!)

50. Nonmetals are located To the right of the staircase

51. Elements in column 15 (VA) have 5 valence electrons

52. Elements in column 16 (VIA) have 6 valence electrons

53. Trends for metallic character Decreases across. Increases down.

54. Metals are losers. Reactivity of metals is judged by how easily metals Lose electrons

55. Elements with strongest metallic properties are located In the lower left corner of the periodic table.

56. Periodic table is arranged by Atomic number

57. How do we judge the reactivity of Nonmetals? Nonmetals are winners so we judge the reactivity of nonmetals by how easily they gain electons.

58. Trends for nonmetallic character Increases across and decreases down.

59. Elements in column 17 (VIIA) have 7 valence electrons

60. Elements in column 18 (VIIIA) have 8 valence electrons

61. Form brightly colored salts and solutions (except Zn) Transition metal ions

62. Can have more than one positive oxidation state.

63. Allotropes Different forms of the same element in the same phase.

64. Allotropes Have different structures so they have different chemical & physical properties.

65. Allotropes of oxygen O 2 and O 3 Different formulas Different structures

66. Allotropes of carbon Graphite, diamond, & buckminsterfullerine (C 60 )

67. Lewis Diagrams of neutral atoms Use dots to represent valence electrons.

68. Lewis Structures of atoms Na Br Al Mg S

69. Lewis structures of ions Positive ions have no dots. Negative ions have 8 dots. All have [ ] and charge.

70. Lewis Diagrams of Cations [Na] +1, [Mg] +2, [Al] +3

71. Lewis Diagrams of Anions

72. Oxidation Number The charge on an atom when it has an octet in the valence level.

73. Oxidation #’s GroupOxidation # 1+1 2+2 13+1, +3 14+2, +4 15+3, +5, -3 16Mostly -2 17 180