Atoms of hydrogen, formed on passing an electric discharge through hydrogen gas at a low emit, light which gives a spectrum of 4 bright lines: red, blue-green, blue and violet respectively in the visible region. These spectral lines were first studied by Ballmer and their wave lengths expressed by the Ballmer formula.
When the electron in the excited state comes back to the lower energy levels, it emits energy it had of absorbed earlier, in the form of photons of lights of specific frequency and hence of specific wavelength. Thus spectral lines of different series observed in the emission spectrum of hydrogen are due to the emission of energy of photons of different wavelength when the excited electrons in hydrogen atoms come back to lower energy levels. The wavelength of the spectral lines is dependent on the quantity of energy liberated. The greater the energy liberated, the shorter is the wavelength and hence greater is the frequency of the radiations emitted.
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