atoms truc lect 1
TRANSCRIPT
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Structure of the Atom
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Atoms ?~400 BC:
Greek Philosopher Democritus believed that each kind of
matter could be subdivided into smaller and smaller bits untilone reached the very limit beyond which no further divisionwas possible.
atomos = that cannot be cut
As of 1900, about 70 different atoms are knownelements different chemical properties
it is argued that this number is too large to really be an elementary
constituant of matter
Hints:- Atoms and electromagnetic radiations (not understood but)- Chemistry: the problem of valence. How molecules are formed ?
Why some combinations of atoms just dont bind as molecules ?- New phenomena: X-rays, Radioactivity (1896),
Henri Becquerel 1852-1908, Nobel Prize in Physics 1903
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Inside the atom ? Scientists are struggling to understand the atom and
reproduce experimental results, such as the spectral lines.[Physics of the electrons inside the atom] Atomic Physics
Also puzzled with a new observed phenomenon:radioactivity. [Physics of the nucleus] Nuclear Physics
But, around 1900, nobody knows the structure of the atom:a puzzle of evidences that needs to be put together.
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Discovery of Radioactivity (1896)1895: X-rays are interpreted as a chemical process similar to phosphorescence
and fluorescence An external source is required to trigger the emission of X-rays
Henri Becquerels idea:look for X-ray emission in known phosphorescent/fluorescent substances.
Experimental procedure:wrap a photographic plate with thick black paper, place the substance to be
tested on the paper and then expose to sunlight for several hours
Sunlight = external source
If X-rays were emitted, they would pass through the paper and fog the plate.
Tests are all negative, except for a Uranium Salt.
Sunlight
Substance
Photographic Plate
Black paper
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Becquerel ExperimentReproducibility: an experimental result should be reproducible
End of February, Henri Becquerel is ready to repeat the experiment.
But it is cloudy over Paris !!!
Put his experimental setup in a drawer till March 1st.
When Becquerel develops the plate (not exposed to sunlight), he finds thatthe fogging is just as intense as when the uranium salt had been exposed to sunlight.
No need for external energy source !!!
The energy is already available/stored in the material.
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Search for elementsof similar properties
Pierre 1859-1906 and Marie Curie: Isolation of Radium and Polonium (1898)Nobel Prize in Physics in 1903
Marie Curie 1867-1934: Got her PhD in 1903Also: Nobel Prize in Chemistry (1911)
Radium is so active that it shines brightly in its pure form
Marie Curie about Radium:its active and it radiates RADIOACTIVITY
She died of Leukemia at 67 (Exposure to radiations)
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The atomic models ofThomson and Rutherford
J.J.Thomson
1856-1940
Nobel Prize in Physics 1906
Ernerst Rutherford
1871-1937
Nobel Prize in Physics 1908
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Known facts (~1900) Atoms are neutral
Electrons are much less massive than the atom
Number of electrons Ne- corresponds to about half the
atomic mass number. Example: Carbon: Atomic Mass Number = 12; Ne-=6
Oxygen: Atomic Mass Number = 16; Ne-=8
Size of the atom ~ 10-10m
The atoms can emit and absorb electromagnetic radiations
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Thomsons atomic model Thomsons plum-pudding model of the atom had the positive
charges spread uniformly throughout a sphere the size of the atom,
with electrons embedded in the uniform background.
In Thomsons view, when the atom is heated, the electrons couldvibrate about their equilibrium positions, thus producingelectromagnetic radiation.
The model fails: cannot reproduce the spectral lines of the Hydrogen
atom
Positively charged, so thatthe whole atom is neutral
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Radioactivity ?
1898: Pierre and Marie discover theRadium Emission of -particle
1900: Rutherford and Roydsdetermine the nature of the -particles, they are charged Heliumatoms
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Ernest Rutherford 1871-1937Nobel Prize in Physics 1908
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Geiger and Marsden Experiments
1909: Rutherford, Geiger andMarsden conceive a new technique toprobe the structure of matter by
scattering -particles from atoms
Geiger shows that many -particlesare scattered from thin gold-leaftargets at backward angles greater
than 90
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Analysis / Conclusions
In contradiction with J.J.Thomsons model:
At best, -particles should only be slightlydeflected
Large deflections ? (see example 4.1, p129-130)
99.95% of the MASS of the atom lies in ahard, dense nucleus occupying only ~10-15mof the atomic volume.
Rutherford (1911): Considering the evidence as a whole, it seems simplest
to suppose that the atom contains a central charge distributed through asmall volume, and that a large single deflections are due to the central
charge as a whole, and not to its constituents.
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Rutherford Scattering
Impact parameter b:
Note: the nucleus is 105 times smaller than the atom, large
deflections do not occur often !!!
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Failure of the classical(planetary) atomic model
Assuming the Hydrogen atom:
The electron is attracted by thenucleus
Even in circular motion around thenucleus, the electron loses energy:
Radial acceleration: ar = v2/R
Classical e.m. theory: an accelerating
charge continuously radiates energy, rdecreases
Atom (neutral) = nucleus (+q) + q electrons
The electron would eventually crash into the nucleus