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Ch 9 pages 444-445; 469-470

Lecture 19 – The Hydrogen atom. Ch 9 pages 444-445; 469-470. Summary of lecture 1 8. Planck’s theory of black body radiation proposed that energy is emitted by oscillators in discrete packets E=h n These packets, called photons, are treated as energy particles

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Ch 9 pages 444-445; 469-470

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  1. Lecture 19 – The Hydrogen atom Ch 9 pages 444-445; 469-470

  2. Summary of lecture 18 • Planck’s theory of black body radiation proposed that energy is emitted by oscillators in discrete packets E=hn • These packets, called photons, are treated as energy particles • As we shall see later, at least two additional experiments further support the particle nature of radiation.

  3. Photon Emission • Relaxation from one energy level to another by emitting a photon. • With DE = hc/l • If l = 440 nm, DE = 4.5 x 10-19 J Emission

  4. “Continuous” spectrum “Quantized” spectrum Emission spectrum of H DE DE Any DE is possible Only certain DE are allowed

  5. Emission spectrum of H Light Bulb Hydrogen Lamp Quantized, not continuous

  6. Emission spectrum of H We can use the emission spectrum to determine the energy levels for the hydrogen atom.

  7. Balmer Model • Joseph Balmer (1885) first noticed that the frequency of visible lines in the H atom spectrum could be reproduced by: n = 3, 4, 5, ….. • The above equation predicts that as n increases, the frequencies become more closely spaced.

  8. Rydberg Model • Johann Rydberg extends the Balmer model by finding more emission lines outside the visible region of the spectrum: n1 = 1, 2, 3, ….. n2 = n1+1, n1+2, … Ry = 3.29 x 1015 1/s • This suggests that the energy levels of the H atom are proportional to 1/n2

  9. Bohr’s Atom The stability of the nuclear atom cannot be explained by classical mechanics. Consider the hydrogen-like nuclear atom: an electron of mass m and charge –e is a distance R from the much-heavier nucleus of mass M and charge +Ze. Because the proton and electron are charged, they have a Coulombic interaction Where e0 is the vacuum permittivity (8.85x10-12 C2/Nt-m2) As a result of the Coulombic Force, the electron will be compelled to move toward the nucleus, eventually colliding with it

  10. Bohr’s Atom To mechanically stabilize the atom, the electron might be assumed to orbit the nucleus, just as a planet orbits the sun. In a planetary system, it is the motion of the planets and resulting centrifugal force that prevents them from colliding with the sun under the influence of gravitation We can by analogy propose that the electron orbits the nucleus such that the Coulomb Force, which is directed inward toward the nucleus, effects a centripedal acceleration of the electron Where V is the velocity of the electron in its orbit

  11. Bohr’s Atom Let us use F=ma where F is the Coulomb force and a is the acceleration to balance the two forces: (the reduced mass is used because we are discussing the motion of the electron relative to the center-of-mass of the atom, which is located at the nucleus to good approximation) One would think that the analogy would be sufficient to explain the stability of atoms

  12. Bohr’s Atom However, according to classical electrodynamics, an orbiting electron charge (any charge) must similarly emit radiation at the frequency of its orbital motion. As a consequence, atoms should be constantly radiating energy as a result of the motion of their electrons. As the electrons radiate, energy is lost, their orbits would decay and eventually they would collide with the nucleus, thus annihilating the atom. Such an atom should self-annihilate in about 10-12 sec

  13. Bohr’s Atom Furthermore, atoms do not spontaneously emit radiation, but only radiate when they absorb energy and then they give off radiation only at certain discrete frequencies Niels Bohr used a quantum hypothesis to explain the emission spectrum of hydrogen. He reasoned that the angular momentum mVR of an orbiting electron is quantized The orbit of an electron is assumed constant when the integral of the momentum along the circular orbit equals nh, where n=1,2,3. More explicitly:

  14. Bohr’s Atom When this condition holds, the electron does not radiate and the orbit is mechanically stable. Bohr’s momentum quantization equation: and the force equation requirement are combined to yield: This equation can be solved to yield the allowed orbital radii:

  15. Bohr’s Atom The Bohr orbit is: The force balance requirement gives the expression for the total quantized energy of Bohr’s atom:

  16. Bohr’s Atom The energy equation for the hydrogenic atom predicts that, as in the case of the black body radiator, energy can only be emitted in discrete quantities. If an atom absorbs energy, its electron will be promoted from the nth orbit to, say, the kth orbit. To return to the nth orbit, the atom must emit energy. The frequency of the energy particle or photon emitted by the atom is given by:

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