1. Chemistry SM-1131 Week 4 Lesson 2 Dr. Jesse Reich Assistant Professor of Chemistry Massachusetts Maritime Academy Fall 2008

2. Class Today Test in 1 Week Atomic Theory Protons, Neutrons, and Electrons Elements by the protons Periodic Table Gaining and losing electrons Isotopes Atomic Mass

3. Democritus The material cause of all things that exist is the coming together of atoms and void. Atoms are too small to be perceived by the senses. They are eternal and have many different shapes, and they can cluster together to create things that are perceivable. Differences in shape, arrangement, and position of atoms produce different things. By aggregation they provide bulky objects that we can perceive with our sight and other senses. We see changes in things because of the rearrangement of atoms, but atoms themselves are eternal. Words such as ‘nothing’, ‘the void’, and ‘the infinite’ describe space. Individual atoms are describable as ‘not nothing’, ‘being’, and ‘the compact’. There is no void in atoms, so they cannot be divided. I hold the same view as Leucippus regarding atoms and space: atoms are always in motion in space. (www.humanistictexts.org) ~460, Greece-371 BCE

4. His Buddy Aristotle Aristotle emphasized that nature consisted of four elements: air, earth, fire, and water. Aristotle

5. The Greek Gods Empedocles associates the Elements with four Gods: Hera (Earth), Persephone (Water), Zeus (Air) and Hades (Fire),

6. Fast Forward to Dalton Sept. 6, 1766, England-July 27, 1844 Dalton's Atomic Theory 1) All matter is made of atoms. Atoms are indivisible and indestructible. 2) All atoms of a given element are identical in mass and properties 3) Compounds are formed by a combination of two or more different kinds of atoms. 4) A chemical reaction is a rearrangement of atoms.

7. Dalton’s Creek, err, element set

8. So what changed? abyss.uoregon.edu

9. Crooks Tube Current moved from the cathode to the anode through a vacuum It moved in lines similar to light But magnets could deflect the current The new path could be used to calculate a mass to charge ratio but couldn’t calculate mass or charge

10. J. J. Thompson Dec. 18, 1856, England - Aug. 30, 1940

11. Wilhelm Conrad Röntgen March 27, 1845, Germany - Feb. 10, 1923 “On the evening of November 8, 1895, he found that, if the discharge tube is enclosed in a sealed, thick black carton to exclude all light, and if he worked in a dark room, a paper plate covered on one side with barium platinocyanide placed in the path of the rays became fluorescent even when it was as far as two metres from the discharge tube. During subsequent experiments he found that objects of different thicknesses interposed in the path of the rays showed variable transparency to them when recorded on a photographic plate. When he immobilised for some moments the hand of his wife in the path of the rays over a photographic plate, he observed after development of the plate an image of his wife's hand which showed the shadows thrown by the bones of her hand and that of a ring she was wearing, surrounded by the penumbra of the flesh, which was more permeable to the rays and therefore threw a fainter shadow. This was the first "röntgenogram" ever taken. In further experiments, Röntgen showed that the new rays are produced by the impact of cathode rays on a material object. Because their nature was then unknown, he gave them the name X-rays. Later, Max von Laue and his pupils showed that they are of the same electromagnetic nature as light, but differ from it only in the higher frequency of their vibration.” (nobelprize.org)

13. Henri Becquerel Dec. 15, 1952, France – Aug. 25, 1908 Following a discussion with Henri Poincaré on the radiation which had recently been discovered by Röntgen (X-rays) and which was accompanied by a type of phosphorescence in the vacuum tube, Becquerel decided to investigate whether there was any connection between X-rays and naturally occurring phosphorescence. He had inherited from his father a supply of uranium salts, which phosphoresce on exposure to light. When the salts were placed near to a photographic plate covered with opaque paper, the plate was discovered to be fogged. The phenomenon was found to be common to all the uranium salts studied and was concluded to be a property of the uranium atom. Later, Becquerel showed that the rays emitted by uranium, which for a long time were named after their discoverer, caused gases to ionize and that they differed from X-rays in that they could be deflected by electric or magnetic fields. For his discovery of spontaneous radioactivity Becquerel was awarded half of the Nobel Prize for Physics in 1903, the other half being given to Pierre and Marie Curie for their study of the Becquerel radiation. (nobelprize.org)

14. A Nobel Next to Socks

15. Pause for Dramatic Effect What We Know Up to Now! There are different elements Elements are made up of atoms Atoms have positive and negative components Some elements are radioactive

16. Anyone for a Curie November 7, 1867, France – July 4, 1934 She helped to discover Polonium and Radium. To do this she and her husband took Pitchblend, which contained the radioactive element Uranium by the ton and carefully isolated the radioactive components over several years. What they found was that there were more than one radioactive element in it because they found an element that was far more radioactive than the element uranium. She got a Nobel in Physics for radioactivity. She got a Nobel in chemistry for discovering two new elements.

17. Raw Materials PitchblendeRadium There is 1 gram of radium in 7 tons of pitchblende “It therefore appeared probable that if pitchblende, chalcolite, and autunite possess so great a degree of activity, these substances contain a small quantity of a strongly radioactive body, differing from uranium and thorium and the simple bodies actually known. I thought that if this were indeed the case, I might hope to extract this substance from the ore by the ordinary methods of chemical analysis.” [Curie 1961 (1903), p. 16].

18. In her own words If we assume that radium contains a supply of energy which it gives out little by little, we are led to believe that this body does not remain unchanged, as it appears to, but that it undergoes an extremely slow change. Several reasons speak in favor of this view. First, the emission of heat, which makes it seem probable that a chemical reaction is taking place in the radium. But this is no ordinary chemical reaction, affecting the combination of atoms in the molecule. No chemical reaction can explain the emission of heat due to radium. Furthermore, radioactivity is a property of the atom of radium; if, then, it is due to a transformation, this transformation must take place in the atom itself. Consequently, from this point of view, the atom of radium would be in a process of evolution, and we should be forced to abandon the theory of the invariability of atoms, which is the foundation of modern chemistry [M. Curie 1904].

19. Ernest Rutherford Aug. 30, 1871 New Zealand – Oct. 19, 1937

20. In Simpler terms…

21. So what just happened? It was almost as incredible as if you fired a 15-inch shell at a piece of tissue paper, and it came back to hit you "On consideration, I realized that this scattering backwards must be the result of a single collision, and when I made calculations I saw that it was impossible to get anything of that order of magnitude unless you took a system in which the greater part of the mass of the atom was concentrated in a minute nucleus. It was then that I had the idea of an atom with a minute massive center carrying a charge."

22. WTH?

23. So what’s an atom look like? The Planetary Model

24. Robert A. Millikan March 22, 1868, U.S.A. – Dec. 19 1953 Established the charge of an electron and Determined the atomic structure of electricity

25. So What’d He Do?

26. Well, what’s that thingy? www.physchem.co.za

27. So, what’d it look like inside? www.nikhef.nl

28. So, what changed?

29. A Nagging Concern Rutherford’s Model Positive Protons and Oppositely Charged Electrons What should happen? Collapse!

30. Skipping Ahead I’m skipping a lot of scientists and a lot of story We have a nucleus and it contains Protons and Neutrons Electrons are on the outside in set patterns

31. Nucleus Masses Protons have masses of 1.67262e-27kg Neutrons have masses of 1.67493e-27kg OK, talking about that mass is obnoxious. So chemists came up with another scheme. They took an atom of Carbon, which has 6 neutrons and 6 protons, and they said 1/12 of that mass is now 1 amu. Protons by themselves have a mass of 1.0073 amu. Neutrons have a mass of 1.0087 amu.

32. Electrons Protons are over 1800 times larger than electrons. So, chemists say electrons have no mass. This is not exactly true, it’s more like they have negligible mass.

33. Charge Protons have a charge of +1 Electrons have a charge of -1 Neutrons have no charge at all. Oppositely charged particles attract. Similarly charged particles repel. If an atom has an equal number of protons and electrons the atom has no charge. For every extra proton it has +1 charge. For every extra electron it has -1 charge.

34. Periodic Table Hydrogen is the element 1 is the atomic number 1.0079 is the atomic mass

35. Elements The number of protons is called the atomic number. If two elements have the same atomic number they are the same element. If two elements have different atomic numbers they are different.

36. The Table Groups/families are up and down Rows/periods are left to right

37. The Table Group 1. Alkali Metals Group 2. Alkaline Earth Metals Group 3-12 Transition Metals Group 17. Halogens Group 18. Noble Gases H, C, N, O, P, S, Se are organic elements 57-71 lanthanides 89-103 actinides B, Si, Ge, As, Sb, Te, Po are metaloids

38. Metals Shiny Reflect Malleable (bendable) Ductile (can be drawn into strips) Conduct electricity LOSE ELECTRONS

39. Non-Metals Dull Brittle Don’t conduct GAIN ELECTRONS (think graphite)

40. Metalloids Mixed Properties Semiconductors Some dull, some shiny Etc.

41. Get Ready Monday – 1/3 review, 1/3 New Material, 1/3 test review TEST WEDNESDAY!!!