1. A History of Atomic Theory Atomic Models

2. What is a model ? detailed, 3-D representation of an object - typically on smaller scale than original model car clothing model model airplane

3. Let’s Take a Trip Through Time!

4. It Started with the Greeks DEMOCRITUS Lived in Greece 2500 years ago (460-370 BC) “Father of modern science”

5. Demacritus said: “All matter is made of atoms that are tiny, indestructible and indivisible.”

6. Democritus Greek banknote with Democritus and drawing of atom Where did Democritus get his ideas for small, indestructible, indivisible atoms?

7. Atoms are small… new ringsold ring EVIDENCE: old gold rings wear away slowly, getting thinner and thinner, but you never see gold atoms on your finger, so gold atoms must be very small!

8. Atoms are indestructible… EVIDENCE: Earth has been around long time Mountains wash away but rocks continue to exist New plants grow where old plants die

9. Atoms are indivisible… EVIDENCE: EVIDENCE: None None This was HYPOTHESIS made by Democritus to explain nature as he saw it. This was HYPOTHESIS made by Democritus to explain nature as he saw it.

10. What did Democritus think atoms looked like? Appearance of atoms assumed based on behavior: Liquids pour Solids are hard and rigid

11. Liquids pour. Why? Liquids require a container If liquid atoms were like little balls they would roll out when you tip the container Greek idea of liquid atom

12. Solids are rigid. Why? cocklebur plant cockleburs stick on clothing and each other little hooks on cockleburs Velcro ® fastenerVelcro hooks and loopsGreek idea of solid atom

13. Aristotle had different ideas ARISTOTLE: famous Greek philosopher, born 384 BC student of Plato (another famous philosopher) teacher of Alexander the Great (who later conquered the world) Greek banknote and coin picturing Aristotle

14. Aristotle’s idea of matter Aristotle did not believe Democritus’s idea of atoms was correct Aristotle believed all matter made from four elements: Earth Air Fire Water

15. Aristotle’s idea of matter Aristotle was more famous than Democritus, so people believed him, even though he was wrong! Democritus’s idea of atomos (atoms) was lost for nearly 2000 years until John Dalton brought it back in 1803

16. Atom idea lost for ~2000 years

17. John Dalton, New Atom,1803 Born in England, 1766 Studied chemistry, physics, and color blindness Brought back Democritus’s idea of an indivisible atom

18. Color blindness Can you see a number in this box? If not, you may be color blind. (More males are color blind than females)

19. Start writing - Foldable information

20. Dalton’s Billard Ball Model

21. Dalton’s Theory of Atoms Five parts (postulates): # 1: Elements are made of extremely small particles called atoms

22. So according to Dalton’s theory: atoms are considered to be like billiard balls

23. # 2: Atoms of given element are identical in size, mass, & other properties; Atoms of different elements are different in size, mass, & other properties (later found not to be exactly correct)

24. #3: Atoms cannot be subdivided, created, or destroyed (later proved wrong)

25. #4: Atoms of different elements combine in simple whole-number ratios to form chemical compounds (H 2 O 2:1 ratio H:O)

26. #5: In chemical reactions, atoms are combined, separated and/or rearranged

27. Ex. of a chemical reaction: +  + 2H 2 O + 2Na  2NaOH + H 2 +

28. Dalton’s Chemical Symbols We use different symbols today

29. Thomson’s Plum Pudding Model

30. J.J. Thomson English physicist (1856-1940) won Nobel Prize in 1906 1897: discovered ELECTRON - studied cathode rays using Crooke’s tube - showed atoms were divisible

31. Crooke’s tube (stream of electrons) move from metal cathode (on left) to cross-shaped anode (on right) cathode ↓ cross-shaped anode ↑ cross-shaped shadow ↓ cathode rays: cross-shaped shadow is cast on glass (on right) shows … electrons are particles smaller than an atom and have negative charge

32. Cathode Ray Tube Experiment thought cathode rays were streams of particles smaller than atoms

33. magnetic fields deflect beam of charged particles magnetic fields deflect beam of charged particles

34. JJ Thomson’s discovery of (-) charged electrons proved that atoms were divisible!

35. Thomson’s “Plum pudding” atom  raisin ENGLISH PLUM PUDDING – electron

36. Thomson’s Plum Pudding Model: (+) charge evenly spread (+) charge evenly spread out while… out while… (-) charge found in (-) charge found in small bits – small bits – like raisins in plum pudding like raisins in plum pudding (or chocolate chips in cookies) (or chocolate chips in cookies)

37. More About Charge… opposite charges attract, like charges repel

38. RULE: Matter is NEUTRAL (no charge) so… for every one (-) charged electron there must be one something of (+) charge

39. What do we mean by charge? MATTER IS NEUTRAL (no charge): (+) charges equal (-) charges charges cancel out each other ELECTRONS are negatively charged (-1) PROTONS are positively charged (+1) ELECTRICAL CHARGE - property of matter: # electrons greater or less than # protons batteries have (+) and (-) ends

40. Rutherford’s Nuclear Model

41. Ernest Rutherford 1871-1937 1908: won Nobel Prize (Chemistry) 1920: discovered proton discovered that most of mass of atom is found in the center (nucleus)

42. Rutherford’s Experiment – 1911 Rutherford’s exp’t: animation Rutherford’s exp’t: animation

43. Rutherford’s Gold Foil Experiment Rutherford tested Thomson’s plum pudding model of atom: sent tiny radioactive alpha  (  ) particles, like bullets, towards thin sheet of gold foil

44. Rutherford gold foil experiment expected  particles to pass straight through, like this…

45. most  particles went straight through without hitting anything, BUT a few were deflected, this means  particles must have hit something: really heavy really heavy OR OR (+) charged (+) charged

46. gold foil experiment scattering results showed: Plum pudding model of atom was INCORRECT, so… Rutherford devised new model that fit his results…

47. proposed Nuclear Model Rutherford concluded: all atoms have dense, positive (+) center (center contains most of mass of atom) atom is mostly empty space (except very tiny (–) electrons; but didn’t say where are) nucleus / [protons (+)] electrons (–) /

48. Problems with Rutherford’s Model did not speculate how electrons arranged around (+) center did not speculate how electrons arranged around (+) center to prevent (-) electrons from being attracted to (+) nucleus, electrons must orbit nucleus like Earth orbits sun to prevent (-) electrons from being attracted to (+) nucleus, electrons must orbit nucleus like Earth orbits sun but… but… e - need energy to orbit nucleus & Rutherford didn’t address this e - need energy to orbit nucleus & Rutherford didn’t address this name nucleus came later

49. So how BIG is the nucleus compared to the entire atom?

50. If atom is as big as football stadium… the nucleus is smaller than a flea on 50-yard line! the nucleus is smaller than a flea on 50-yard line!

51. If atom is as big as a period at the end of a sentence in textbook, it would have the mass of 70 cars! it would have the mass of 70 cars!.

52. So how big is an atom? most atoms are 1-2 angstroms across most atoms are 1-2 angstroms across 1 Å = 1 X 10 -10 m 1 Å = 1 X 10 -10 m 6 Billion Cu atoms in a line = less than 1 meter! 6 Billion Cu atoms in a line = less than 1 meter! Can we “see” an atom? Can we “see” an atom? NO!

53. James Chadwick 1891-1974 worked with Rutherford worked with Rutherford 1932: discovered neutron 1932: discovered neutron 1935: Nobel Prize (Physics) 1935: Nobel Prize (Physics)

54. Bohr’s Planetary Model

55. Niels Bohr 1885 - 1962 created quantized atom model, 1915 worked on Manhattan Project won Nobel Prize in 1922 Bohr’s model: e - only move from one energy level to another in atom: e - absorb energy when jump from lower to higher levels e - emit energy when jump from higher to lower levels

56. Bohr’s new atomic model addressed issue of atom’s nucleus surrounded by electrons: e - have definite orbits e - have definite orbits e - orbiting at different energy levels e - orbiting at different energy levels e - energy levels are quantized e - energy levels are quantized e - only move by jumping levels (n = 1, n = 2, etc.) e - only move by jumping levels (n = 1, n = 2, etc.) :

57. electrons: absorb energy when they jump away from nucleus emit energy when they jump towards nucleus

59. Bohr’s Planetary Model electrons travel only in specific orbits electrons travel only in specific orbits each orbit has definite energy each orbit has definite energy inner most orbit (n=1): least energy inner most orbit (n=1): least energy outer most orbit (n=7): most energy outer most orbit (n=7): most energy atoms emit radiation when e - jumps from outer orbit to inner orbit (photons of light) atoms emit radiation when e - jumps from outer orbit to inner orbit (photons of light) e – in outermost orbits determine atom’s chemical properties e – in outermost orbits determine atom’s chemical properties

60. Modern Wave Mechanical Model

61. Erwin Schrödinger Austrian scientist (1887-1961) 1933: won Nobel Prize (Physics calculated wave model of hydrogen atom (1926) Today’s atomic model called: modern model quantum mechanical model wave model cloud model

62. Schrödinger’s wave model of atom: e - behaves as: energy wave AND as matter particle (light also behaves as particle and wave) Einstein had predicted that energy and matter were related in his equation E = mc 2 If we could see an electron’s path it might look like this “cloud”

63. Modern/Wave/Cloud Model electron’s energy is quantized (specific values) electron’s energy is quantized (specific values) electrons in probability zones called “orbitals”, not orbits electrons in probability zones called “orbitals”, not orbits - location cannot be pinpointed - location cannot be pinpointed e - considered as both particles & waves e - considered as both particles & waves electrons move around nucleus at speed of light (3 x 10 8 m/sec) electrons move around nucleus at speed of light (3 x 10 8 m/sec)

64. Orbitals

65. A Missing Particle – The Neutron 1932: James Chadwick discovered last major piece of atom: neutron (“neutral”, no charge) 1935: won Nobel Prize (Physics) neutron& proton weigh about same while electron weighs almost nothing (1891-1974)

66. The Modern Model an atom is: mostly empty space nucleus: most of atom’s mass nucleus contains protons & neutrons electrons in energy levels around nucleus electrons jump between levels, emitting & absorbing energy as jump

68. The development of atomic theory represents the work of many scientists over approximately 100 years

69. Next Atomic Theory ? Which one of you will discover something new to add to the atomic model of the atom and win a Nobel Prize in the future?