Unit 1: Atomic Structure AP Chemistry Evolution of Atomic Theory.
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Transcript of Unit 1: Atomic Structure AP Chemistry Evolution of Atomic Theory.
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Unit 1: Atomic StructureAP Chemistry
Evolution of Atomic Theory
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Democritus – 400 B.C.
Greek Philosopher Imagined particles
that were indivisible
Constituents of matter
Atom comes from “atomos”
Opposed Aristotle
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Aristotle – 350 B.C.
Widely accepted theory that all matter can be continually divided.
Set science back for thousands of years.
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Alchemy
A pseudoscience that superceded scientific discoveries.
Alchemists attempted to turn metals into gold and developing the “elixir” of life (able to cause immortality and create life).
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Pierre Gassendi - 1650
Reintroduced Particulate theory
No experimental evidence
Supported by Sir Isaac Newton
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Robert Boyle - 1661
Studied Gases 1st to use the term
element in its current context in his book The Skeptical Chemist
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George Stahl - 1717
Suggested “phlogiston” flowed from burning material
A necessary ingredient of combustible material
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Joseph Priestly - 1774
discovered oxygen supports combustion
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Antoine Lavoisier - 1778
Developed Law of Conservation of Mass
Explained combustion
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Joseph Proust - 1799
Developed “Proust’s Law” using copper oxide
Later renamed, the Law of Definite Proportions
Nearly discovered the Law of multiple proportions, but his data used percentages instead of weights.
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John Dalton - 1802
First to develop an atomic theory. It has 4 postulates. Each element is made
up of atoms Atoms of the same
element are identical in mass and properties. Atoms of different elements differ in some way.
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John Dalton - 1802
Compounds are made when atoms combine. If elements combine in more than one whole number ratio, the resulting compound has different properties
Chemical reactions involve the reorganization of atoms.
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Amedeo Avogadro - 1811
Developed Avogadro’s Law. Equal volumes of gases have equal number of molecules at constant temperature and pressure.
Expanded Dalton’s concept of atomic masses
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J.J. Berzelius - 1813
Established the 1st system of using letters to represent elements.
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William Prout - 1815
Proposed that Hydrogen was the fundamental material that all other elements were made from. All atomic masses were multiples of the mass of hydrogen.
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Michael Faraday - 1833
Found Faraday’s Constant. 1 mole of e- = 96500 coulombs.
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Alexandre Béguyer de Chancourtois - 1862
1st periodic arrangement of elements.
Divided surface of a cylindrical base into 16 segments because oxygen has a mass of 16.
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John Newland - 1863
Developed the law of octaves Properties of
elements repeat every eighth element.
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Dimitri Mendeleev - 1869
Classification based on chemical properties.
Considered the first periodic table.
Left gaps for missing elements and predicted their properties
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William Crookes - 1879
Showed that cathode rays stream from the negative pole
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Eugene Goldstein - 1886
Discovered the proton using a cathode ray tube.
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William Roentgen - 1895
Discovered x-rays. Rays were
penetrating and of short wavelength
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Henri Becquerel - 1896
Discovered radioactivity.
Used uranium salts
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Marie Curie - 1897
Student of Becquerel
Showed that radioactivity is atomic property
Isolated radium and polonium
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J.J. Thomson - 1897
Determined the mass/charge ratio of the electron.
5.69 x 10-9
Used the cathode ray tube
Proposed a model of the atom that was mockingly called the “plum pudding” model
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Robert Millikan - 1909
Determined the charge of the electron using the famous oil-drop experiment
1.60 x 10-19
From this and Thomson’s value, the mass was calculated to be 9.11 x 10-28g
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Ernest Rutherford - 1911
Performed the famous gold foil experiment
Determined 3 things The atom is mostly
empty space The nucleus is
positively charged The nucleus is a
small dense part of the atom
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Gold Foil Experiment
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Gold Foil Experiment
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Henry Moseley - 1913
Calculated atomic number by determining the nuclear charge of an atom.
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Niels Bohr - 1913
Observed spectral lines for hydrogen
Proposed an orbit theory of the electron around the atom.
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Bohr Model
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Hydrogen Spectrum
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Gilbert Lewis - 1916
Suggested that noble gases have 8 valence electrons
Atoms will gain or lose electrons to achieve 8 outer electrons.
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Louis De broglie - 1924
Suggested that matter could exhibit wave properties
Observed diffraction patterns in electrons
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Wolfgang Pauli - 1924
Pauli Exclusion Principle – 2 electrons cannot have the same 4 quantum numbers
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Erwin Schrödinger - 1926
Developed a wave equation.
Mathematical function that described the nature of the electron
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James Chadwick - 1932
Discovered the neutron
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Other Contributions
C.D. Anderson – 1932 Discovered the positron
Enrico Fermi – 1940 Prepared more than 40 radioactive
elements