![]() Thus the orbit with n = 1 is the lowest in energy. The latter condition is arbitrarily assigned an energy of zero. The negative sign in Equation 6.9 is a convention indicating that the electron-nucleus pair has a lower energy when they are near each other than when they are infinitely far apart, corresponding to n = ∞. ![]() Where ℛ is the Rydberg constant, h is Planck’s constant, c is the speed of light, and n is a positive integer corresponding to the number assigned to the orbit, with n = 1 corresponding to the orbit closest to the nucleus. ![]() In 1885, a Swiss mathematics teacher, Johann Balmer (1825–1898), showed that the frequencies of the lines observed in the visible region of the spectrum of hydrogen fit a simple equation that can be expressed as follows: If a hydrogen atom could have any value of energy, then a continuous spectrum would have been observed, similar to blackbody radiation. Thus the energy levels of a hydrogen atom had to be quantized in other words, only states that had certain values of energy were possible, or allowed. Part of the explanation is provided by Planck’s equation ( Equation 6.5): the observation of only a few values of λ (or ν) in the line spectrum meant that only a few values of E were possible. Such emission spectra were observed for many other elements in the late 19th century, which presented a major challenge because classical physics was unable to explain them. (b) When the light emitted by a sample of excited hydrogen atoms is split into its component wavelengths by a prism, four characteristic violet, blue, green, and red emission lines can be observed, the most intense of which is at 656 nm. (a) A sample of excited hydrogen atoms emits a characteristic red light. With sodium, however, we observe a yellow color because the most intense lines in its spectrum are in the yellow portion of the spectrum, at about 589 nm.įigure 6.9 The Emission of Light by Hydrogen Atoms The light emitted by hydrogen atoms is red because, of its four characteristic lines, the most intense line in its spectrum is in the red portion of the visible spectrum, at 656 nm. When the emitted light is passed through a prism, only a few narrow lines, called a line spectrum A spectrum in which light of only a certain wavelength is emitted or absorbed, rather than a continuous range of wavelengths., are seen ( Figure 6.9 "The Emission of Light by Hydrogen Atoms"), rather than a continuous range of colors. Unlike blackbody radiation, the color of the light emitted by the hydrogen atoms does not depend greatly on the temperature of the gas in the tube. For example, when a high-voltage electrical discharge is passed through a sample of hydrogen gas at low pressure, the resulting individual isolated hydrogen atoms caused by the dissociation of H 2 emit a red light. Note how they are complete inverses of each other.Although objects at high temperature emit a continuous spectrum of electromagnetic radiation ( Figure 6.6 "Relationship between the Temperature of an Object and the Spectrum of Blackbody Radiation It Emits"), a different kind of spectrum is observed when pure samples of individual elements are heated. I am attaching the images of the emission and absorption spectra of hydrogen atom. For absorption spectroscopy, varying wavelengths of photons are incident on the atom and the corresponding photon is absorbed by the atom resulting in no photon of that particular wavelength being detected. When atoms releases photons (light), the detector catches the production of the photon and gives out emission spectra. What kind of spectrum you have at hand depends on which instrument and detector you are using. When a photon is absorbed, the electron uses this energy to excite to a higher energy state. However, the processes by which these two spectra are generated are completely the opposite of each other.Īn atom emits a photon when an electron goes from a higher energy state to a lower energy state, thereby releasing energy in the form of light. So, naturally, if an atom exhibits some emission spectrum, it will also give an absorption spectrum. Emission and absorption are inverse processes.
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