1. Test Review – U2SB Metals and Reactivity

2. Atmosphere

3. Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide

4. Hydrosphere

5. Liquid portion composed of water and dissolved minerals and salts.

6. Lithosphere

7. Solid part of earth. Greatest variety of chemical resources. Includes petroleum and metal-bearing ores.

8. Ore

9. Naturally occurring rock or mineral that can be mined

10. Minerals

11. Naturally occurring solid compounds containing elements or groups of elements

12. How are metals generally found?

13. Metals are not generally found in their pure state. They react and combine with other elements to form ionic and covalent compounds.

14. What does their reactivity depend on?

15. Their reactivity depends on their chemical families and properties

16. Electrons

17. Negatively charged particles orbiting the nucleus

18. Where are Electrons found?

19. Electrons are found in orbitals or shells outside the nucleus

20. Where are electrons with the highest energy?

21. The electrons with the highest energy are on the outside shell.

22. Where are electrons with the lowest energy?

23. The electrons with the lowest energy are on the inside

24. Periods

25. Show the number of electron shells or orbitals. Horizontal columns.

26. Families

27. Vertical columns. Show the number of outside electrons.

28. Valence Electrons

29. The electrons found in the outside energy level

30. The number of valence electrons determines?

31. The number of valence electrons determines many properties of that element

32. The number of valence electrons make up?

33. The number of valence electrons make up the groups or families

34. Octet rule –

35. The maximum number of electrons in the outside shell is 8. The exception is shell # 1 with 2.

36. The first electron shell has __, the second shell has __, the third shell has ___

37. The first electron shell has 2, the second shell has 8, the third shell has 18(8)

38. Electron dot diagram

39. Shows each element with its valence electrons only Outside electrons are placed in pairs Dots show outside electrons

40. Explain the valence electron structures for the following groups: Noble Gases: Nonmetals: Metals:

41. Explain the valence electron structures for the following groups: Noble Gases:have 8 valence electrons (2 for He) and are stable Nonmetals: Metals:

42. Explain the valence electron structures for the following groups: Noble Gases:have 8 valence electrons (2 for He) and are stable Nonmetals:Groups 5a to 7a will gain electrons to become stable Metals:

43. Explain the valence electron structures for the following groups: Noble Gases:have 8 valence electrons (2 for He) and are stable Nonmetals:Groups 5a to 7a will gain electrons to become stable Metals:Groups 1a to 3a will lose electrons to become stable

44. Chemical Bonds

45. Chemical forces which hold atoms together and form complete electrons shells

46. Ionic Bond

47. Positive (+) and negative (-) ions attract – formed by the transfer of valence electrons.

48. Ion

49. is an atom or group of atoms that have an electric charge.

50. Atoms which lose electrons become: Atoms which gain electrons become: Lose 1 = Gain 1 = Lose 2 = Gain 2 = Lose 3 = Gain 3 =

51. Atoms which lose electrons become: positive ions Atoms which gain electrons become: Lose 1 = Gain 1 = Lose 2 = Gain 2 = Lose 3 = Gain 3 =

52. Atoms which lose electrons become: positive ions Atoms which gain electrons become: negative ions Lose 1 = Gain 1 = Lose 2 = Gain 2 = Lose 3 = Gain 3 =

54. Atoms which lose electrons become: positive ions Atoms which gain electrons become: negative ions Lose 1 = +1Gain 1 = Lose 2 = +2Gain 2 = Lose 3 = +3Gain 3 =

55. Atoms which lose electrons become: positive ions Atoms which gain electrons become: negative ions Lose 1 = +1Gain 1 = -1 Lose 2 = +2Gain 2 = -2 Lose 3 = +3Gain 3 = -3

56. Oxidation – Reduction Reactions Reduction:

57. Oxidation – Reduction Reactions Reduction: Any reaction in which a reactant can be considered to gain one or more electrons.

58. Elements or ions which lose electrons are said to be reduced.

59. Oxidation – Reduction Reactions Oxidation:

60. Oxidation – Reduction Reactions Oxidation: Any reaction in which a reactant can be considered to lose one or more electrons.

61. Elements or ions which gain electrons are said to be oxidized.

62. Name the type of reaction: Cu 2 + + 2e- = Cu : = Reduction Cu: = Cu 2 + + 2e- = Oxidation Cu + O 2 = 2CuO Copper is ____________ Oxygen is ____________ Copper ____________electrons Oxygen ____________electrons

63. Name the type of reaction: Cu 2 + + 2e- = Cu : = Reduction Cu: = Cu 2 + + 2e- = Oxidation Cu + O 2 = 2CuO Copper is Oxidized Oxygen is Reduced Copper ____________electrons Oxygen ____________electrons

64. Name the type of reaction: Cu 2 + + 2e- = Cu : = Reduction Cu: = Cu 2 + + 2e- = Oxidation Cu + O 2 = 2CuO Copper is Oxidized Oxygen is Reduced Copper loses electrons Oxygen gains electrons

65. Metallic bond

66. Metal atoms combine in regular patterns in which valence electrons are free to move from atom to atom.

67. Most metals have _____electrons and are __ions

68. Most metals have 1-3 electrons and are positive ions

69. Explain the relationship between these properties of metals and valence electrons: Malleable and ductile: Luster: Electrical and Thermal conductivity:

70. Explain the relationship between these properties of metals and valence electrons: Malleable and ductile Luster Electrical and Thermal conductivity metal’s positive ions are attracted to electrons and can slide into different positions When light strikes the valence electrons they absorb it than give it off again valence electrons move freely and cause electric current to flow or heat to flow easily from hot to cold