The major difference between the emission spectrum and the absorption spectrum is that the absorption spectrum is continuous spectra whereas the emission spectrum is the discontinuous or line spectra. On the other hand, whenever electromagnetic radiation interacts with atoms, if their electrons in the ground level jump to an immediate higher energy level, absorbing energy will result in a continuous spectrum with dark lines, which is known as an absorption spectrum. Since the spectrum obtained is distinct and discontinuous it is also known as a line spectra. The radiation emitted by excited electrons will constitute a spectrum of distinct wavelengths known as emission spectra. In order to regain their stability, the electrons will emit energy in the form of radiation. Whenever white light or electromagnetic radiation have interacted with the atoms or molecules, their electrons absorb energy and transit from lower energy level to higher energy levels losing their stability. The atomic spectra are further classified into two types: When the white light interacts with atoms or molecules, it will absorb a certain amount of energy and emit radiation of different wavelengths resulting in atomic spectra. While studying the dual nature of light, we concluded that light behaves like both particles and waves. The spectra obtained will be a continuous spectrum, a spectrum is said to be continuous if the pattern obtained doesn’t have distinct spacing between the colors or the wavelengths. The splitting of white light into different wavelengths of colors is known as dispersion and the pattern of colors obtained is a spectrum. Now the visible spectrum is just an impression of particular wavelengths (ranging from 400nm-700nm) when white light is made incident on optical devices like Prism, diffraction grating. The electromagnetic spectrum is an arrangement of all wavelengths ranging from visible light to infrared lights. The spectrum is an important concept in order to understand the structure of atoms.
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