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The ELECTRON: Wave – Particle Duality

The ELECTRON: Wave – Particle Duality. Graphic: www.lab-initio.com. The Dilemma of the Atom. Electrons outside the nucleus are attracted to the protons in the nucleus Charged particles moving in curved paths lose energy What keeps the atom from collapsing?. Wave-Particle Duality.

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The ELECTRON: Wave – Particle Duality

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  1. The ELECTRON: Wave – Particle Duality Graphic: www.lab-initio.com

  2. The Dilemma of the Atom • Electrons outside the nucleus are attracted to the protons in the nucleus • Charged particles moving in curved paths lose energy • What keeps the atom from collapsing?

  3. Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron. The electron is a particle! The electron is an energy wave!

  4. The Wave-like Electron The electron propagates through space as an energy wave. To understand the atom, one must understand the behavior of electromagnetic waves. Louis deBroglie

  5. Electromagnetic radiation propagates through space as a wave moving at the speed of light. c =  c = speed of light, a constant (3.00 x 108 m/s)  = frequency, in units of hertz (hz, sec-1)  = wavelength, in meters

  6. The energy (E ) of electromagnetic radiation is directly proportional to the frequency () of the radiation. E = h E= Energy, in units of Joules (kg·m2/s2) h= Planck’s constant (6.626 x 10-34 J·s) = frequency, in units of hertz (hz, sec-1)

  7. Long Wavelength = Low Frequency = Low ENERGY Wavelength Table Short Wavelength = High Frequency = High ENERGY

  8. Answering the Dilemma of the Atom • Treat electrons as waves • As the electron moves toward the nucleus, the wavelength shortens • Shorter wavelength = higher energy • Higher energy = greater distance from the nucleus

  9. The Electromagnetic Spectrum

  10. Electron transitionsinvolve jumps of definite amounts ofenergy. This produces bands of light with definite wavelengths.

  11. Spectroscopic analysis of the hydrogen spectrum… …produces a “bright line” spectrum

  12. Flame Tests Many elements give off characteristic light which can be used to help identify them. strontium sodium lithium potassium copper

  13. Exclusion Notice The contents of the next two slides reference equations that are no longer included on the AP Chemistry equations sheet, and can no longer be tested in a quantitative sense

  14. Electron Energy in Hydrogen Z= nuclear charge (atomic number) n= energy level ***Equation works only for atoms or ions with 1 electron (H, He+, Li2+, etc).

  15. Calculating Energy Change, E, for Electron Transitions Energy must be absorbed from a photon (+E) to move an electron away from the nucleus Energy (a photon) must be given off (-E) when an electron moves toward the nucleus

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