Notes – Unit 2 Section B / Chapter 5 Earth’s Mineral Resources / Electron structure

1. Notes – Unit 2 Section B / Chapter 5Earth’s Mineral Resources / Electron structure

2. Earth’s composition • Atmosphere: Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide

3. Earth’s composition • Atmosphere: Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide • Hydrosphere: Liquid portion composed of water and dissolved minerals and salts.

4. Earth’s composition • Atmosphere: Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide • Hydrosphere: Liquid portion composed of water and dissolved minerals and salts.

5. Earth’s composition • Atmosphere: Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide • Hydrosphere: Liquid portion composed of water and dissolved minerals and salts. • Lithosphere: solid part of earth. Greatest variety of chemical resources. Includes petroleum and metal-bearing ores.

6. Earth’s composition 3) Lithosphere: solid part of earth. Greatest variety of chemical resources. Includes petroleum and metal-bearing ores.

7. Earth’s composition 3) Lithosphere: solid part of earth. Greatest variety of chemical resources. Includes petroleum and metal-bearing ores. Ore – Naturally occurring rock or mineral that can be mined

8. Earth’s composition 3) Lithosphere: Includes petroleum and metal-bearing ores. Ore – Naturally occurring rock or mineral that can be mined. Minerals -

9. Earth’s composition 3) Lithosphere: Includes petroleum and metal-bearing ores. Ore – Naturally occurring rock or mineral that can be mined. Minerals – Naturally occurring solid compounds containing elements or groups of elements

10. Earth’s composition Granite – Rock (Ore) 3) Lithosphere: Includes petroleum and metal-bearing ores. Ore – Naturally occurring rock or mineral that can be mined. Minerals – Naturally occurring solid compounds containing elements or groups of elements Quartz - mineral

12. Metals, Nonmetals and reactivity • Metals are not generally found in their pure state. • They react and combine with other elements to form ionic and covalent compounds. • Their reactivity depends on their chemical families and properties

13. Types of Atomic particles • Atoms - The building blocks of matter. • Particles – Electrons (-) e- Protons (+) p+ Neutrons (no charge) no • Nucleus Protons and neutrons

16. Atomic Particles • Sodium = Atomic Mass = Mass # = - # (rounded) mass = p+ = e- = no = • Chlorine = Atomic Mass = Mass # = - # (rounded) mass = p+ = e- = no =

17. Atomic Particles • Sodium = Na Atomic Mass = 22.99 Mass 23 # = 11- # 11 (rounded) mass = 23 p+ = 11 e- = 11 no = 12 • Chlorine = Atomic Mass = Mass # = - # (rounded) mass = p+ = e- = no =

19. Atomic Particles • Sodium = Na Atomic Mass = 22.99 Mass 23 # = 11- # 11 (rounded) mass = 23 p+ = 11+ e- = 11- no = 120 • Chlorine = Cl Atomic Mass = 35 .453 Mass 35 # = 17- # 17 (rounded) mass = 35 p+ = 17+ e- = 17- no = 180

20. Electrons Electrons – Negatively charged particles orbiting the nucleus Periods – Show the number of electron shells or orbitals. Horizontal columns. Families – Vertical columns. Show the number of outside electrons.

21. Electrons Electrons – Negatively charged particles orbiting the nucleus Periods – Show the number of electron shells or orbitals. Horizontal columns. Families – Vertical columns. Show the number of outside electrons.

23. Valence electrons 8 1 3 4 5 6 7 1 2 2 3 4 5 6 7 Periods

24. Electrons Valence electrons Valence Electrons – The electrons found in the outside energy level The number of valence electrons determines many properties of that element The number of valence electrons make up families

25. Electrons Valence electrons Valence Electrons – The electrons found in the outside energy level The number of valence electrons determines many properties of that element The number of valence electrons make up families

26. Honors ChemChapter 5Electrons in Atoms

27. Atomic models • Dalton – 1st Atom – no internal structures • Thomson – Plum pudding, electrons in sphere of positive • Rutherford - small dense positive nucleus with electrons around nucleus • Bohr – electrons in circular orbitals with fixed distances from nucleus. Lowest energy inside highest energy furthest from nucleus

28. Atomic models • Schrodinger – mathematical equation for location. Electron cloud model • Quantum Mechanical model – modern description from Schrodinger’s mathematical equations

29. Atomic models • Schrodinger – mathematical equation for location. Electron cloud model • Quantum Mechanical model – modern description from Schrodinger’s mathematical equations

30. Electron configuration • Quantum – the amount of energy required to move an electron from its present energy level to the next higher one • Energy levels – region in space around nucleus where an electron is likely moving

31. Electron configuration Electron configuration • Quantum – the amount of energy required to move an electron from its present energy level to the next higher one • Energy levels – region in space around nucleus where an electron is likely moving • Energy levels are labeled by principle quantum numbers (n). • n = 1,2,3,4, etc

32. Electron configuration • Quantum – the amount of energy required to move an electron from its present energy level to the next higher one • Energy levels – region in space around nucleus where an electron is likely moving • Energy levels are labeled by principle quantum numbers (n). • n = 1,2,3,4, etc • The higher the energy level occupied by an electron, the more energetic it is

33. Electron configuration • Energy levels are labeled by principle quantum numbers (n). • n = 1,2,3,4, etc • The quantum # equals the number of sublevels for each principle energy level • The formula 2n2 equals the maximum number of electrons allowed in a principle energy level • Shell n 2n2 • K 1 2(1)2= • L 2 2(2)2= • M 3 2(3)2= • N 4 2(4)2=

34. Energy levels • Energy levels are labeled by principle quantum numbers (n). • n = 1,2,3,4, etc • The quantum # equals the number of sublevels for each principle energy level • The formula 2n2 equals the maximum number of electrons allowed in a principle energy level • Shell n 2n2 • K 1 2(1)2= • L 2 2(2)2= • M 3 2(3)2= • N 4 2(4)2=

35. Electrons • Electrons are found in orbitals or shells • The electrons with the highest energy are on the outside shell. • The electrons with the lowest energy are on the inside

36. Electrons • Each shell can only hold a certain amount of electrons • The electrons with the highest energy are on the outside shell. • The electrons with the lowest energy are on the inside

38. # of electrons in orbitals Shell K L M N n2n2 1 2 3 4

39. # of electrons in orbitals Shell K L M N n2n2 1 2 2 3 4

40. # of electrons in orbitals Shell K L M N n2n2 1 2 2 8 3 4

41. # of electrons in orbitals Shell K L M N n2n2 1 2 2 8 3 18 4

42. # of electrons in orbitals Shell K L M N n2n2 1 2 2 8 3 18 432

43. # of electrons in orbitals Shell K L M N n2n2 1 2 2 8 3 18 (8) 432 (8)

44. Electron shells • Electrons fill from the inside out • The first shell has 2, the second shell has 8, the third shell has 18(8) • Octet rule – The maximum number of electrons in the outside shell is 8. The exception is shell # 1 with 2.

45. Electron shells • The atomic number of an element tells the number of protons and electrons • Electrons are drawn in shells in pairs from inside out. • The outside are valence electrons

47. Valence electrons

49. 8 1 3 4 5 6 7 2