1. Number of Protons
Atomic Number

2. Number of Protons + Neutrons
Mass Number

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

4. Left Superscript = mass number6

5. Left Subscript = atomic number6

6. 35
80Br 35
Atomic Number = ?

7. 20
20Ne 10
Mass Number = ?

8. 238
238U 92
Mass Number = ?

9. 27
27Al 13
Mass Number = ?

10. 20
40Ca 20
Atomic Number = ?

11. 9
19F 9
Atomic Number = ?

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

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

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

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

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

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

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

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

20. Protons & Neutrons
Nucleons

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

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

23. # protons - # electrons
Charge

24. Mass number – atomic number
# of neutrons

25. 8
14C 6
# of neutrons = ?

26. 5
9Be 4
# of neutrons = ?

27. 22
40Ar 18
# of neutrons = ?

28. 8
15N 7
# of neutrons = ?

29. Right superscript = charge
24Mg 2+ 12

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

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

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

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

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

35. Positive ion: atom lost electrons
Cation

36. Negative ion: atom gained electrons
Anion

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

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

39. Billiard Ball Model
Dalton’s Model

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

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

42. Rutherford’s Experiment
Source:

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

44. Planetary Model
Bohr’s Model

45. Modern or Quantum Mechanical Model
Schrodinger’s Model
Source:

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

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

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
Bohr Configuration of Na = 2-8-1

49. +11
Bohr Diagram of Na

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

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

52. 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.
Bohr Model

53. Maximum Capacity of Bohr Levels
Shell #
Max # of electrons 1 2 3 4 n 2 8 18 32
2n2

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

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

56. Ground state configuration of O
2-6

57. Ground state configuration of Kr?
Ground state configuration of Kr?

58. Principle Energy Level?
Shell #
Principle Energy Level?

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.
Excited State

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

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

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

63. 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.
Bright Line Spectrum
Source:

64. Excited state E3 E2
Ground state h E1
Absorbtion of Energy

65. Excited state h E3 E2
Ground state E1
Emission of Energy

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

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