Examples Line emission spectrum of H violet n6-n2 blue ng-> nz green n4 n2 Yed ng n2 Calculate the energy of the light emitted when an e- from n=4 to n= 2 goe What is the wavelength of this light ? Line Spectrum. Please do not block ads on this website. Other articles where Line spectrum is discussed: spectroscopy: Basic atomic structure: The emission and absorption spectra of the elements depend on the electronic structure of the atom. An atom consists of a number of negatively charged electrons bound to a nucleus containing an equal number of positively charged protons. Line spectrum can therefore be found in both absorption and emission spectra which are exact opposites of each other. The line emission (atomic) spectrum of an element is unique. Hydrogen spectrum is an example of line emission spectrum or atomic emission spectrum. This hypothetical element shall have 4 energy levels. Spectroscopy is the study of emission and absorption spectra. Unlike visible light which shows a continuous spectrum of all wavelengths, the emission spectra of atoms in the gas phase emit light only at specific wavelengths with dark spaces between them. This means that the gas is receiving energy carried by the photons of light (as in E=hf). Every element has a unique atomic emission spectrum, as shown by the examples of helium $$\left( \ce{He} \right)$$ and iron $$\left( \ce{Fe} \right)$$. Classical theory was unable to explain the existence of atomic emission spectra, also known as line-emission spectra. In a very simplistic way you can consider a gas of atoms of a substance illuminated by light. No ads = no money for us = no free stuff for you! The first is also called a bright line spectrum and consists of a few brightly colored lines against a dark background. There are two types of line spectrum: an emission spectrum and an absorption spectrum. Explain why the line spectrum doÄs not contain a liné Corresponding to â¦ It is a sequence of lines of different color/frequency that represents a kind of "photograph" of the structure of an atom. The nucleus Each element has a specific set of energy levels, or allowed quantities of energy that electrons can absorb. Each line represents a unique wavelength, and the entire thing is unique to that particular element. This emission occurs when an atom, element or molecule in an excited state returns to a configuration of lower energy. (b) This light shows discontinuous line spectrum of several isolated sharp lines through prism. Line emission spectra (atomic spectra) can be used to identify the presence of an element in a sample because no two elements produce the same line emission (atomic) spectrum. When an absorption spectrum and emission spectrum are combined, you get a continuous spectrum with all the wavelengths. Take for example an element, which will be named X. Truly white light, like that emitted by some stars and moons is a perfect example of continuous spectrum. Emission-line spectra Low-density clouds of gas floating in space will emit emission lines if they are excited by energy from nearby stars. Planetary nebulae, for example, are the remnants of stars which have gently pushed their outer envelopes outwards into space. An emission line will appear in a spectrum if the source emits specific wavelengths of radiation. (a) When an electric discharge is passed through hydrogen gas at low pressure, a bluish light is emitted. The emission of photons through electronic relaxations in atoms produces a line emission spectrum. Structure of an atom by light discontinuous line spectrum and an absorption spectrum example. Atomic ) spectrum of several isolated sharp lines through prism hydrogen gas at low pressure, a light! For example, are the remnants of stars which have gently pushed their outer envelopes outwards into space colored against! 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