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12 Cards in this Set

  • Front
  • Back
Describe the electromagnetic spectrum.
the range of all possible frequencies of electromagnetic radiation. It;s divided into emission spectrum
Explain how the lines in the emission spectrum of hydrogen are related to electron energy levels.
This line spectrum indicated that only certain energies are allowed for the electron in the hydrogen atom. Changes in energy between discrete energy levels in hydrogen will produce only certain wave-lengths of emitted light. This means, electrons can only be at certain energy levels around a nucleus.
Deduce the electron arrangement for atoms and ions up to Z = 20.
line spectrum
"a spectrum showing only certain colors or specific wavelengths of light.
Transitions Between Energy Levels
An electron in an atom can change energy only by going from one energy level to another energy level. By so doing, the electron undergoes a transition.
Gamma rays ( -12/-10); X rays (-10/-8); ultraviolet (-8/-7); visual (4x10-7/7x10-7); infrared (-6/-4); radio (-4/4) [meters]
electron transitions
movement of electrons between the shells
Describe and explain the difference between a continuous spectrum and a line spectrum
A continuous spectrum is created when white light is passed through a prism. This spectrum, like the rainbow produced when sunlight is dispersed by raindrops, contains all the wavelengths of visible light. In contrast, a line spectrum is when only a few lines are emitted rather then the entire spectrum
emission spectrum of hydrogen (5)
(1)When hydrogen gas is stimulated, it emits a characteristic set of spectral lines.(2)There are several series of lines, which become more closely packed at higher frequencies (lower wavelengths) until finally the series ends.(3)The lines are emitted by electrons in the hydrogen atoms. The electrons are ‘excited’ by the energy input to the hydrogen sample.(4)‘Excitation’ means that the electron leaves its usual low energy orbit (its ‘ground state’) and enters a higher-energy orbit. The orbits of electrons are often called ‘shells’.(5)Excited electrons eventually ‘relax’ to lower-energy orbits. They emit the excess energy in the form of photons.
Infrared - from M
Visible - from L
Ultraviolet - from K