2. Atomic Theory and Structure Chapters 4-5

3. Atomic Theories Democritus ~ 400 BC believed that atoms were indivisible and indestructible Dalton ~ 1800’s Developed through experiments First Atomic Model

4. Dalton’s Atomic Model All elements are composed of tiny indivisible particles called atoms Atoms of the same element are identical. The atoms of any one element are different from those of any other element.

5. Dalton’s Atomic Model (cont) Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds. Chemical reactions occur when atoms are separated, joined, or rearranged. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction.

6. Discovery of Electron 1897 – JJ Thomson, using cathode ray tube, discovered negatively charged particles called electrons 1909 – Robert Millikan - Oil Drop Experiment Determined charge on an electron.

7. “Plum Pudding” Model Uniform positive sphere with negatively charged electrons embedded within.

8. Radiation Late 1800’s – discovery of radiation Three Types Alpha Beta Gamma

9. Rutherford Gold Foil Experiment - 1909 Shot alpha particles at gold foil Most went through foil with little or no deflection. Some were deflected at large angle and some straight back. A.K.A. Geiger Marsden Experiment

10. Rutherford Gold Foil Experiment - 1909

11. Rutherford Model Conclusions from Gold Foil Experiment Atom is Mostly Empty Space Dense positive nucleus Electrons moving randomly around nucleus

12. Subatomic Particles Electron Discovered in 1897 by JJ Thomson Negative charge (-1) Mass = 9.109389*10 -28 g Approx mass ~ 0 Found outside of nucleus

13. Subatomic Particles Proton Discovered in 1919 by Rutherford Positive charge (+1) Mass = 1.672623*10 -24 g Approx mass ~ 1 atomic mass unit (u) Found inside nucleus

14. Subatomic Particles Neutron Discovered in 1932 by James Chadwick No charge (0) Mass = 1.6749286*10 -24 g Approx mass ~ 1 atomic mass unit (u) Just slightly larger than a proton Found inside nucleus

15. Atomic Structure Atoms have no net charge # of electrons = # of protons # of electrons around nucleus = # of protons in nucleus

16. Atomic Structure Atomic Number Number of protons in an element All atoms of the same element have the same number of protons Mass Number Number of protons and neutrons in an atom

17. Atomic Structure # of Neutrons = Mass Number – Atomic Number Atoms of the same elements can have different numbers of neutrons Isotope – atoms of the same element with different number of neutrons

18. Chemical Symbols Cl-35 Chlorine-35 Mass Number Atomic Number

19. Ion Atom or group of atoms that have gained or lost one or more electrons Have a charge Example: H +, Ca 2+, Cl -, OH -

20. Ions H + 1 proton0 electrons Ca 2+ 20 protons18 electrons Cl - 17 protons18 electrons OH - 9 protons10 electrons

22. Atomic Theories Rutherford’s model could not explain the chemical properties of elements Niels Bohr believed Rutherford’s model needed to be improved Bohr proposed that electrons are found only in circular paths around the nucleus

23. Bohr Model Dense positive nucleus Electrons in specified circular paths, called energy levels These energy levels gave results in agreement with experiments for the hydrogen atom.

24. Bohr Model

25. Each energy level can only hold up to a certain number of electrons Level 1  2 electrons Level 2  8 electrons Level 3  18 electrons Level 4  32 electrons

26. Electron Configuration The way in which electrons are arranged in the atom Example: Na 2-8-1 Valence Electrons Electrons in the outermost energy level

27. Energy Level Transitions Electron energy is quantized Electrons can move between energy levels with gains or losses of specific amounts of energy.

28. Energy Level Transitions Gaining energy will move an electron outward to a higher energy level (Absorption) When an electron falls inward to a lower energy level, it releases a certain amount of energy as light (Emission)

29. Energy Level Transitions

30. Ground State vs. Excited State Ground State When the electrons are in the lowest available energy level Ex: Na 2-8-1 Excited State When one or more electrons are not in the lowest available energy level Ex: Na 2-7-2 or 2-8-0-1 or 2-6-1-1-1

31. Line Spectra Emission Spectra Shows only the light that is emitted from an electron transition Absorption Spectra Shows a continuous color with certain wavelengths of light missing (absorbed)

32. Energy Level Transitions

34. Wave Mechanical Model More detailed view of the Bohr Model Schrödinger Wave Equation and Heisenberg Uncertainty provides region of high probability where electron COULD be. Orbital Modern Model AKA Quantum Mechanical Model, Electron Cloud Model

35. Wave Mechanical Model Orbital Regions of space where there is a high probability of finding an electron

36. Wave Mechanical Model Each energy level is divided into sublevels 1 st Energy level has 1 sublevel, s 2 nd Energy level has 2 sublevels, s and p 3 rd Energy level has 3 sublevels, s, p, and d 4 th Energy level has 4 sublevels, s, p, d, and f These sublevels start to overlap as you move away from the nucleus

37. Wave Mechanical Model Sublevels are divided into orbitals s sublevel has 1 orbital p sublevel has 3 orbitals d sublevel has 5 orbitals f sublevel has 7 orbitals Each orbital can hold up to 2 electrons

38. Atomic Orbitals

39. Electron Orbital Configuration Sublevel order 1s 2s2p 3s3p3d 4s4p4d4f 5s5p5d5f5g 6s6p6d6f6g6h 7s7p7d7f7g7h

40. Electron Orbital Configuration One sublevel must be full before you can move to the next sublevel For sublevels with multiple orbitals Each orbital must have one electron before you can double up

41. Electron Orbital Configuration H____1s 1 He____ 1s 2 Li________ 1s 2 2s 1 1s 2s

42. Electron Orbital Configuration C____ ________ ____ ____ C1s 2 2s 2 2p 2 N____ ________ ____ ____ N1s 2 2s 2 2p 3 1s 2s2p 2s2p

43. Electron Orbital Configuration O____ ________ ____ ____ O 1s 2 2s 2 2p 4 F____ ________ ____ ____ F 1s 2 2s 2 2p 5 1s 2s2p 2s2p

45. M&M’s Demo What colors are found in a regular M&M’s bag? Green Yellow Orange Blue Red Brown

46. M&M’s Demo Do you get an equal amount of each color in each bag? If we opened up all the regular M&M bags in the world would we get an equal number of each color? Are you supposed to?

47. M&M’s Demo Color1 bagWorld Blue%24% Green%16% Yellow%14% Orange%20% Red%13% Brown%13%

48. M&M’s Demo M&M’s come in certain abundances (percentages) So do isotopes of each element Relative Abundance Percent of each naturally occurring isotope found in nature

49. Average Atomic Mass Atomic Mass Weighted average based on the relative abundance and mass number for all naturally occurring isotopes Example C-1298.9%12.011u C-131.1%

50. Atomic Mass C-1298.9% C-131.1% Carbon = 0.989*12 + 0.011*13 = 12.011u