Atomic Structure Timeline. History of Atomic Theory
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1 Atomic Structure Timeline History of Atomic Theory
2 Essential Questions What does it mean when my science teacher says stuff cannot be created or destroyed? What is matter made up of? And who figured it out?
3 Evolution of Modern Atomic Theory
4 Democritus (400 B.C.) Proposed that matter was composed of tiny indivisible particles Not based on experimental data Greek: atomos
5 The Early Atom Aristotle succeeded Democritus and did not believe in atoms. Instead, he thought that all matter was continuous. It was his theory that was accepted for the next 2000 years.
6 Alchemy (next 2000 years) Mixture of science and mysticism. Lab procedures were developed, but alchemists did not perform controlled experiments like true scientists.
7 Lavoisier 1777 French chemist, who is considered the founder of modern chemistry. Lavoisier clarified the concept of an element as a simple substance that could not be broken down by any known method of chemical analysis He devised the Law of Conservation of Mass
8 Basic Laws of Matter Law of Conservation of Mass- mass is neither created nor destroyed during ordinary chemical reactions or physical changes. CH 4 + 2O 2 2H 2 O + CO 2 16g + 64g 36g + 44g Antoine Lavoisier stated this about 1785
9 Alka Seltzer in Water Ziploc bag Alka seltzer tablet Water Using the reaction between the tablet and the water, prove that the Law of Conservation of matter is true.
10 Proust (1794) Proust stated the Law of Definite Proportions. The law states that the ratio of elements in a compound is always the same.
11 Basic Laws of Matter Law of Definite Proportions no matter how much salt you have, it is always 39.34% Na and 60.66% Cl by mass. Example: Sodium chloride always contains 39.34% Na and 60.66% Cl by mass. 2NaCl 2Na + Cl 2 100g 39.34g g g? +? Joseph Louis Proust stated this in 1794.
12 John Dalton (1808) Dalton add his own - the Law of multiple proportions He proposed a theory to summarize and explain these three laws I was a school teacher at the age of 12!
13 Basic Laws of Matter Law of Multiple Proportions- Two or more elements can combine to form different compounds in whole-number ratios. Example John Dalton proposed this in 1803.
14 John Dalton Dalton s Four Postulates 1. Elements are composed of small indivisible particles called atoms. 2. Atoms of the same element are identical. Atoms of different elements are different. 3. Atoms of different elements combine together in simple whole number ratios to create compounds. 4. In a chemical reaction, atoms are rearranged, but not changed.
15 John Dalton s Elements
16 Was Dalton right? Elements are composed of small indivisible particles called atoms. Subatomic particles electrons, protons, neutrons, and more Atoms of the same element are identical. Atoms of different elements are different. No, isotopes are atoms that have the same number of protons but a different number of neutrons
17 Was Dalton right? Atoms of different elements combine together in simple whole number ratios to create a compound. Yes! He was right! In a chemical reaction, atoms are rearranged, but not changed. Yes! He was right!
18 Essential Questions So, Dalton figured out the atom, how did we figure out what the inside of an atom looks like?
19 How Big (Small) Is the Nucleus of an Atom? If the total atom was the size of a football field, then the nucleus would be the size of an apple in the middle of the field.
20 How Small is an Atom? The width of a human hair = 1,000,000 carbon atoms across One bucket full of water contains more atoms than there are bucketfuls of water in the Atlantic ocean
21 Discovery of the Electron In the late 1870 s many experiments were performed in which electric current was passed through gases at low pressures due to the fact that gases at atmospheric pressure don t conduct electricity well. These experiments were carried out in glass tubes called cathode-ray tubes or Crookes tubes for the man that developed them.
22 Crookes Tube CRT
23 J. J. Thomson (1903) Cathode Ray Tube Experiments beam of negative particles Discovered particles smaller than the atom!
24 J.J. Thomson (1903) Proved that the atom was divisible and that all atoms contain electrons. This contradicted Dalton s Atomic Theory. This allowed a new model of the atom.
25 J. J. Thomson (1903) Plum-pudding Model positive sphere (pudding) with negative electrons (plums) dispersed throughout v=gzmh4q-2hjm
26 Robert Millikan (1910 s) American physicist Determined the mass and charge of an electron Oil drop experiment Hag7Liw
27 Oil Drop Experiment Millikan dropped negatively charged microscopic oil particles into a chamber containing metallic plates and viewed them with a microscope. By applying voltage to the metallic plates, Millikan created an electric field. He was able to suspend the oil droplets by adjusting the electric field to the appropriate strength and direction to overcome gravity.
28 Oil Drop Experiment Knowing the mass of the droplets and the strength of the electric field necessary to suspend them, he was able to calculate the charge of the electron. He noticed that the charge was always a whole-number multiple of X10-19 Coulombs.
29 Ernest Rutherford (1911) Gold Foil Experiment Discovered the nucleus dense, positive charge in the center of the atom Nuclear Model
30 Gold Foil Experiment
31 Gold Foil Experiment As expected, most of the alpha particles passed straight through with little or no deflection. However, 1/8000 of the positively charged alpha particles were deflected, some back at the source.
32 Gold Foil Experiment
33 Gold Foil Experiment From this experiment, Rutherford discovered that there must be a very densely packed positively charged bundle of matter within the atom which caused the deflections. He called this positive bundle the nucleus. He tried this experiment with other metals and found the same results.
34 Gold Foil Experiment The volume of the nucleus was very small compared to the volume of the atom. Therefore, most of the atom was composed of empty space.
35 It was about as believable as if you had fired a 15-inch shell at a piece of tissue paper, and it came back and hit you. -Ernest Rutherford
36 Hkraf8iE Ernest Rutherford (1911) Nuclear Model
37 Let s take a break Work with a partner to complete the Rutherford s Gold Foil Experiment
38 Evolution of Modern Atomic Theory Almost there!
39 Niels Bohr (1913) Met with J.J. Thomson but didn t impress him Worked with Rutherford and liked his model of the atom Incorporated idea of quantum mechanics into the Rutherford model
40 Niels Bohr (1913) Introduced the idea of electrons traveling around the nucleus in orbits or energy levels. Like the planets, there are multiple orbits like concentric circles around the nucleus Planetary Model
41 Niels Bohr (1913) He used Bright-Line Spectrum tried to explain presence of specific colors in hydrogen s spectrum Built upon Max Planck s concepts of quantized energy
42 Erwin Schrödinger (1926) Treats electrons as waves Tells us the probability of finding an electron at any given location at any given moment Electron cloud model Atomic orbital: region around the nucleus where electrons are likely to be found
43 Erwin Schrödinger (1926) Electron Cloud Model (orbital) dots represent probability of finding an e - not actual electrons
44 James Chadwick (1932) Studied under Rutherford and built upon his model Discovered neutrons neutral particles in the nucleus of an atom
45 He projected alpha particles (from a decaying polonium) towards beryllium target. The particles released are uncharged and have the same mass as protons. He called them neutrons.
46 James Chadwick (1932) Neutron Model revision of Rutherford s Nuclear Model
47 Models of the Atom Timeline Let s recap with a video (10:52) vkoplq
48 Dogs teaching Atoms hs87xq8&list=fltwkpm0rnahux5d RoXcf7qw&index=2
49 Atomic Timeline Poster Project Divide into 7 groups and make a poster that includes: Year of discovery Name of model Name of scientist (s) Picture of the model Picture of equipment used in discovery Key information about model
50 Poster project Group 1 Dalton (pg ) Group 2 Thompson (pg ) Group 3 Millikan (pg. 109) Group 4 Rutherford (pg ) Group 5 Niels Bohr (handout) Group 6 - Schrödinger (pg ) Group 7 Chadwick (pg )
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