Bright line spectra

An excited (heated) body gives off a bright-line spectrum. 

The electronic transitions that produce the bright-line spectrum of hydrogen. 

Every element produces a unique bright-line spectrum. No two elements have the same spectrum. The emission spectrum of an element is like a fingerprint of that element. That every element can produce a bright-line spectrum proves that electrons reside only in definite energy states in all elements, and that each element has its own set of allowed energy states that are unlike those of any other element. 

Explain how the bright-line spectrum of hydrogen is consistent with Bohr s model of quantized energy states for the electrons in the hydrogen atom. 

The equation AE hv is called the Bohr frequency condition and is the basic assumption that as the electron falls from one level to another, the energy evolved is given off as a photon of energy E hv. The energies and the energy differences are quantized, and so are the frequencies. The isolated atom emits hght of only certain definite frequencies, as observed in the bright line spectrum. ... 

Consider the bright line spectrum of hydrogen shown in Figure 11.11. Which line in the spectrum represents photons with the highest energy With the lowest energy ... 

The metal is characterized by a spectrum containing two bright lines in the blue along with several others in the red, yellow, and green. It is silvery white, soft, and ductile. It is the most electropositive and most alkaline element. 

If the atom or molecule loses all or part of this energy as radiation, photons of energy will be emitted which correspond to the difference between the energy levels involved. Since these levels are clearly defined for any given atom or molecule, the radiation emitted will be of specific frequencies and will show up as bright lines if the emitted light is dispersed as a spectrum. 

Caesium (Cs, [Xe]6.vl), name and symbol from the Latin caesius (sky blue, the colour of two bright lines in its spectrum). Discovered (1860) by Robert Bunsen and Gustav Kirchhoff. 

Sodium salts, when heated in a flame, give that flame a bright yellow color, and this color matches the two brightest lines in the emission spectrum of sodium. Sodium is found widely in nature, and lots of substances produce these lines. Fraunhofer had found that the spectrum of a candle flame contained two bright lines precisely corresponding to two dark lines, known as the D lines, in the emission spectrum of the sun. 

This figure shows the match between the bright lines in the spectrum of iron with some of the Fraunhofer lines, proving the presence of iron in the solar atmosphere. 

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