I have two questions on chemistry involving the line spectrum?

Question

Explain the existence of a line spectrum instead of a continuous spectrum in emission as well as why is an emission spectrum of an element called a fingerprint...Please...I'm very grateful to those who help. Thank you. By the way...are there any like good chemistry websites that aren't too verbose?

Answer 1

Each atom type (element) is unique because of a difference in mass (number of protons and neutrons in the nucleus). Therefore, the number of electrons and the (diameter?) of the electron orbits differ for various elements. When an electron captures a photon (tiny mass-less packet of energy traveling at the speed of light) it is kicked up into a higher more energetic orbit. When the electron returns to its rest state (normal orbit) in one or more steps it gives up one or more photons. Different electrons from different orbits can give up photons of different energy levels distinguished by their different wavelengths of light. The spectra (fingerprint) of each element (photons of different wavelengths) are unique and help identify an unknown element when compared to spectra of know elements.

Answer 2

What type of emission spectrum are you asking about?

Generally speaking each element, due to it's electron configuation absorbs and emits energy of a specific frequency. If I were to apply energy to an element, it would be absorbed by an outter electron, exiting the electron to a higher energy state. As the electron returned to its normal state, it would emit this energy, and it could be detected. Because each element has a unique electron configuration, the frequency of this energy could be measured, and the unknown element determined from the information.

Just as an aside, the same technique is used to determine the concentration of elements. The more energy that is emitted, the more of the element there is present.

Answer 3

In a complex compound, or a solid crystal lattice, you get a more or less continuous spectrum; interactions between nearby atoms give emissions at millions of different frequencies. An atom in a gas, being isolated, emits distinct frequencies, so you get a series of lines in its spectrum corresponding to individual energy level transitions.

Answer 4

answer is a.a million. while the electron strikes from point 3 to a million means of the emitted ray is 12.087 eV. The wavelength of the spectrum is 1026 A ('A' for Angstroms) or 102.6 nM (nano-meters) The means emitted is in the Lyman spectrum. bear in mind the Bohr's variety ? means is emitted in quanta. each and every quanta has particular means stages based on the wavelength of the spectrum emitted. bear in mind the Planck’s equation : E = h v, the place v (suggested as new) is the frequency of the electro-magnetic radiation emitted. this is often rewritten as E = h * c / l the place 'E' is means, 'h' is Planck's consistent, 'c' is the speed of sunshine (electro-magnetic radiation) and 'l' is lambda wave length. Electron from means point E3 strikes to means point E1 then the means distinction is given as E3-E1 = dE = h c / l??? this suggests that the means given out is of one wave length of sunshine (electromagnetic radiation) particular to the quanta of means emitted.

Answer 5

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