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To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy

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Objectives To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy To learn about Bohr s model of the hydrogen atom – PowerPoint PPT presentation

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Title: To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy


1
Objectives
  1. To understand how the emission spectrum of
    hydrogen demonstrates the quantized nature of
    energy
  2. To learn about Bohrs model of the hydrogen atom
  3. To understand how the electrons position is
    represented in the wave mechanical model

2
A. The Energy Levels of Hydrogen
  • Only certain types of photons are produced when
    excited Hydrogen atoms release energy. Why?

3
A. The Energy Levels of Hydrogen
  • Atomic states
  • Excited state atom with excess energy
  • Ground state atom in the lowest possible state
  • When an H atom absorbs energy from an outside
    source it enters an excited state.

4
A. The Energy Levels of Hydrogen
  • Energy level diagram
  • Energy in the photon corresponds to the energy
    used by the atom to get to the excited state.

5
A. The Energy Levels of Hydrogen
  • Only certain types of photons are produced when H
    atoms release energy. Why?

6
A. The Energy Levels of Hydrogen
  • Quantized Energy Levels
  • Since only certain energy changes occur the H
    atom must contain discrete energy levels.

7
B. The Niels Bohr Model of the Atom (1913-1915)
  • Bohrs model of the atom
  • Quantized energy levels
  • Electron moves in a circular orbit
  • Electrons jump between levels by absorbing or
    emitting photons of a particular wavelength

Able to mathematically explain the emission
spectrum of Hydrogen (compare with Rutherford)
8
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9
B. The Bohr Model of the Atom
  • Bohrs model of the atom was not totally correct.
  • Had difficulties with spectra of larger atoms
  • Electrons do not move in a circular orbit and
    dont seem to behave like discrete particles all
    the time

Maybe small particles, such as electrons, can
also behave like waves having a dual nature (just
like photons)?
10
C. The Wave Mechanical Model of the Atom (de
Broglie and Schroedinger mid-1920s)
  • Orbitals
  • Nothing like orbits
  • Probability of finding the electron within a
    certain space
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