History and Structure of the Atom. From Democritus to...
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1 1 History and Structure of the Atom From Democritus to...
2 History of Atomic Theory 2 Democritus (from about 440 BC) coined the term atom which means uncuttable He felt that if you kept cutting matter smaller and smaller eventually you will no longer be able to cut any further.
3 John Dalton ( ) 3 Felt that an atom was indivisible spherical in shape Model: Sphere Analogy: Billiard ball
4 JJ Thomson ( ) 4 Discovered electrons Felt that an atom was negatively charged particles floating in a positive soup Model: Charges floating around Analogy: Raisin bun or Plum Pudding
5 The Atom Thompson proved in 1897 that cathode rays were particles from inside the a-tomos or un-cuttable atom Nagaoka pictured a planetary model for the atom, with electrons around a central mass
6 Hantaro Nagaoka ( ) 5 Analogy Developed the planetary model of atom Model: Positive sphere with electrons orbiting in a ring Analogy: Saturn
7 Ernest Rutherford ( ) 6 Discovered the nucleus, the proton and first split an atom Model: An atom was a small positively charged nucleus surrounded by electrons orbiting around it. Analogy: A beehive
8 Rutherfords Famous Experiment 7 Called the Gold Foil Experiment Alpha particles were fired at thin gold foil A detector encircled the foil and lit up when hit with alpha particles. If the plum pudding model were true it was expected most particles would go straight through the foil with only slight deflection. However, in the experiment, some particles were deflected back at a sharp angle proving the existence of a small, dense, and positively charged nucleus.
9 8 Rutherford's results Plum pudding expected results. Particles all go through. Text Actual results. Some are deflected back due to a nucleus
10 Data table for 50 shots Straight Slight Bounce # times Through Deflection Back IIII II
11 Another view of the experiment 9
12 Niels Bohr 10 Worked out details of atomic structure. Notably orbital layers. Solved problems related to Rutherfords model. Model: Electrons orbit in rings at different distances from the nucleus. Analogy: Planets orbiting the sun
13 Erwin Schroedinger ( ) 11 Major discoveries in quantum mechanics. Nature of electrons in atoms. Model: Electrons exist in a probability distribution around the atom. Kind of like a cloud. Analogy: A spinning fan blade.
14 Radioactivity Marie and Pierre Curie discovered that some isotopes are unstable: they spontaneously decay and give off radiation
15 What are the effects of radiation?
16 Up and Atom!
17 You wouldn t like me when I m angry...
18 Check your understanding P. 279 even Steven
19
20 Quick Quiz: Historical Atom What did Dalton say an atom was like? 1. A billiard ball, or a pool table ball 2. What did JJ Thomson say an atom was like? 2. Raisin bun 3. What did Rutherford say an atom was like? 3. A beehive 4. What are the 3 parts of an atom? 4. Proton, Neutron, Electron
21 Parts of the Atom 13 The Nucleus Electrons
22 Parts of the Atom 14 Electrons Mass=0 Charge=-1 Protons Mass=1 Charge=+1 The Nucleus Neutrons Mass=1 Charge=0
23 Atoms on the Periodic Table 15 3 Be 7.0 Atomic # = Number of protons neutrons + protons Atomic mass
24 Try This 16 Atomic # Element Symbol Atomic Mass Be Na Fe I
25 To Determine Other Numbers 17 To find Do this Proton # Electron # same as atomic number same as atomic number for neutral atoms Neutron # =atomic mass-atomic number Mass =Prot # + Neut#
26 Fill in the blanks 18 Element Atomic # e- # Mass # Neut # 12 P
27 Summary 19 The model of the atom has progressed over time from a simple ball to the mysterious quantum structure. An atom contains protons, neutrons and electrons. You can calculate the number of each using the atomic number and atomic mass Electrons are negative, protons are positive, and neutrons are neutral
28 Check your understanding P. 283 Odd Todd
29 Isotopes Elements have a characteristic number of protons, e.g. Hydrogen always has one proton They may have different numbers of neutrons Neutrons help to glue together the nucleus of mutually repulsive protons
30 Radiation Radiation from the nucleus comes in three flavors: α (Alpha): massive, slow, low penetration. He 2+ β (Beta): fast, low mass, medium penetration. e - γ (Gamma): high energy E-M radiation. Gamma ray photon.
31 Check your understanding P. 289 even Stephen
32
33 100 y f(x)=100(0.5)^x % Remaining vs. Half-lives elapsed x
34 Activity level: 1 bequerel = Decays per second Ex: what is the activity level for decays per minute? 12000decays/60s =200 Bq
35 100 y f(x)=100(0.5)^x 80 % activity vs. Half-lives elapsed x
36
37 Half Life λ When a radioactive isotope decays, the amount remaining can be described by a half life relation: A = A t λ Ex 1: find the amount remaining of 55g of Ne-18 in 26s, if it has a half life of 13 s
38 Ex 1: find the amount remaining of 55g of Ne-18 in 26s, if it has a half life of 13 s How many half lives? 26/13=2 A = A t λ Amount remaining=55x1/2x1/2=12g
39 Check your understanding P. 295 q's 4-9
40 Chapter Review P. 295 q's 4-9 Choose 10 vocab p. 302 P. 304 q's 1-10, choose 5 of 11-18
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