1. Atomic Number Number of Protons

2. Mass Number Number of Protons + Neutrons

3. C-12 or carbon-12 12 is the mass number.

4. 12 C Left Superscript = mass number 6

5. 12 C Left Subscript = atomic number 6

6. 80 Br 35 Atomic Number = ?

7. 20 Ne 20 10 Mass Number = ?

8. 238 U 238 92 Mass Number = ?

9. 27 Al 27 13 Mass Number = ?

10. 40 Ca 20 Atomic Number = ?

11. 19 F 9 9 Atomic Number = ?

12. U-235 Mass Number = 235 Atomic Number = 92 (Look up!) Mass Number? Atomic Number?

13. C-14 Mass Number = 14 Atomic Number = 6 (Look up!) Number of neutrons = 14 - 6 = 8 How many neutrons?

14. Isotope Atoms of the same element with a different # of neutrons

15. Isotope Atoms with the same atomic # but different mass #

16. Characteristics of Proton Charge = +1, mass = 1 amu, location = inside nucleus

17. Characteristics of Neutron Charge = 0, mass = 1 amu, location = inside nucleus

18. Characteristics of Electron Charge = -1, mass = 1/1836 amu or 0.0005 amu, location = outside nucleus

19. Ion An atom that has gained or lost electrons & so carries charge

20. Nucleons Protons & Neutrons

21. atom Smallest bit of an element that retains the properties of the element.

22. atom Electrically neutral. # of protons = # of electrons.

23. Charge # protons - # electrons

24. # of neutrons Mass number – atomic number

25. 14 C 8 6 # of neutrons = ?

26. 9 Be 5 4 # of neutrons = ?

27. 40 Ar 22 18 # of neutrons = ?

28. 15 N 8 7 # of neutrons = ?

29. 24 Mg Right superscript = charge 12 2+

30. 24 Mg 10 electrons 12 2+ # of electrons?

31. 86 Rb 36 electrons 37 1+ # of electrons?

32. 127 Te 53 electrons 52 1- # of electrons?

33. 32 S 18 electrons 16 2- # of electrons?

34. 20 F 9 protons, 11 neutrons, 10 electrons 9 - # of protons, neutrons, electrons?

35. Cation Positive ion: atom lost electrons

36. Anion Negative ion: atom gained electrons

37. Avg. Atomic Mass Weighted avg. of masses of naturally occurring isotopes of an element.

38. 2 isotopes of Cl: 75% Cl-35 & 25% Cl-37. Calculate avg. atomic mass. Avg. atomic mass =.75(35) +.25(37) = 35.5 amu

39. Dalton’s Model Billiard Ball Model

40. Thomson’s Model Plum Pudding Model - - - - - + + + + +

41. Rutherford’s Model Nuclear Model + - - -

42. Rutherford’s Experiment Source: http://www.dlt.ncssm.edu/TIGER/chem1.htm#atomic

43. Rutherford’s Experiment: Results 1)Most of the alpha particles went straight through.  Most of the atom is empty space. 2)Some of the alpha particles were deflected back.  The nucleus was tiny, but contained most of the mass of the atom.

44. Bohr’s Model Planetary Model

45. Schrodinger’s Model Modern or Quantum Mechanical Model Source: http://www.dlt.ncssm.edu/TIGER/chem1.htm #atomic

46. Modern Model (Schrodinger or Quantum Mechanical Model) Electron treated as a wave. Never know exactly where it is.

47. Bohr Configuration Ground state configurations found in reference tables. Cannot be predicted.

48. Bohr Configuration of Na = 2-8-1 2 electrons in energy level 1 8 electrons in energy level 2 1 electron in energy level 3

49. Bohr Diagram of Na +11

50. Valence Electron(s) Electron(s) in outermost orbit or shell

51. Kernel Nucleus + all innershell electrons: Everything except the valence electrons

52. Bohr Model Electrons are restricted to specific orbits or shells or principle energy levels. Each shell holds a specific # of electrons. Each shell has a specific energy & radius. Energy of electron must match energy of shell.

53. Maximum Capacity of Bohr Levels Shell #Max # of electrons 1 2 3 4 n 2 8 18 32 2n 2

54. Ground State Bohr model Every electron is in the lowest available orbit.

55. 2-8-7 Ground state configuration of Cl

56. 2-6 Ground state configuration of O

57. Ground state configuration of Kr? 2-8-18-8

58. Principle Energy Level? Shell #

59. Excited State Bohr model An electron has absorbed heat, light, or electrical energy and moved to a higher energy level. Unstable. Returns to ground state quickly by emitting a photon.

60. 2-5-1 An excited state of O

61. 2-0-1 An excited state of Li

62. Continuous Spectrum Spectrum produced by holding a prism in sunlight. Contains light at every wavelength. Rainbow

63. Bright Line Spectrum Visible light produced by electrons in atom returning to ground state: light of only a few wavelengths is present. Each element has a unique bright line spectrum. Used to identify elements. Wavelengths of bright lines correspond to difference between energy levels. Source: http://www.dlt.ncssm.edu/TIGER/chem1.htm#atomic

64. Absorbtion of Energy h Ground state Excited state E1E1 E2E2 E3E3

65. Emission of Energy h Ground state Excited state E1E1 E2E2 E3E3

66. Orbital Modern Model Region of space that holds 2 electrons. Has a specific energy. Shapes vary.

67. E1E1 E2E2 Represents an electron dropping to a lower energy level, releasing energy in the process.