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Niels Bohr

His contribution to the atomic theory
by

Nisal Ekanayake

on 17 February 2013

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Transcript of Niels Bohr

Bohrium 107 Bh 264 his contrubution to the atomic theory & Niels Bohr Nisal, Alex, Gavin Introduction Bio file Theory Theory Theory Bibliography shells Energy levels Summary Energy levels movement Different colours represent the different wavelengths emitted by the atom. Bohr related the wavelengths to the differences between the energy levels of different electron orbits or shells. Therefore each line represents the amount of energy emitted as electrons move from higher shells to lower shells. When an electric current is passed through hydrogen gas a spectrum of different coloured lines is produced. What we'll be covering in this prezi The movement of electrons in energy levels. Bohr developed the Bohr's theory; related to the atomic theory Explained the hydrogen spectrum. He improved the model of planets orbiting the sun with his own shell model. Bohr based and developed his work on Max Planck and Ernest Rutherford. Later Bohr’s work was refined by Erwin Schrödinger. Niels Henrik David Bohr ( 7 October 1885 – 18 November 1962) was a Danish physicist who made contributions to understanding atomic structure , for which he received the Nobel Prize in Physics in 1922. In 1913 Bohr introduced his model of the atom which included shells.

He explained that electrons orbited the positively charged nucleus in separate shells.

Electrons in the outermost shell depict chemical properties. Electrons can only move up energy levels if they absorb a photon with exactly the right amount of energy.
Electrons release their acquired energy, in the form of a photon (heat light etc.) with the same amount of energy as the difference in energy levels of the shells. Each colour of light in the visible spectrum is produced by photons of a different energy (red light photons have less energy than blue light photons). Electrons orbited the positively charged nucleus in separate shells. Bohr theorized that electrons orbited at discreet energy levels. :Emission: The electron then falls back to its ground state releasing energy in the form a photon/light, equivalent to the difference in energy between the two shells. Absorption: He also theorized that when an electron absorbs energy it jumps to a higher shell. -Jacaranda, Study On Chemistry 1, Atomic Emission Spectrum, 10 February 2013
- MLA style: "niels Bohr - Biography". Nobelprize.org 10 Feb 2013 http://ww.nobelprize.org/nobel_prizes/physics/laureates/1922/bohr-bio.html
-Nels Bohr, The Science Classroom 10 Feb 2013 http://thescienceclassroom.wikispaces.com/Niels+Bohr Image1:http://en.wikipedia.org/wiki/File:Spectral_lines_continous.png
Image2: http://en.wikipedia.org/wiki/File:Bohr-atom-PAR.svg
Image3: http://en.wikipedia.org/wiki/File:Fraunhofer_lines.svg
Image4:http://mail.colonial.net/~hkaiter/astronomyimages1011/hydrogen_emis_spect.jpg
Image5:"Bohr Atomic Model." Bohr Atomic Model. N.p., n.d. Web. 17 Feb. 2013.
<http://abyss.uoregon.edu/~js/glossary/bohr_atom.html>. Bohr showed that the electrons could only orbit at discrete energy levels The difference in energy of the shells is equivalent to the amount of energy it received. "Atomic Hydrogen Emission Spectrum." Atomic Hydrogen Emission Spectrum. N.p., n.d. Web. 17 Feb. 2013.

"Niels Bohr." Wikipedia. Wikimedia Foundation, 17 Feb. 2013. Web. 17 Feb. 2013.

"Atomic Theory." Atomic Theory. N.p., n.d. Web. 17 Feb. 2013.

"Electron Configuration." Wikipedia. Wikimedia Foundation, 27 Jan. 2013. Web. 17 Feb. 2013.

"Atomic Theory." Atomic Theory. N.p., n.d. Web. 17 Feb. 2013.

"Dalton's Atomic Theory." Dalton's Atomic Theory. N.p., n.d. Web. 17 Feb. 2013. <http://www.iun.edu/~cpanhd/C101webnotes/composition/dalton.html>.

"Bohr Model." Wikipedia. Wikimedia Foundation, 02 Aug. 2013. Web. 17 Feb. 2013. <http://en.wikipedia.org/wiki/Bohr_model>.

"OChemPal." OChemPal RSS. N.p., n.d. Web. 17 Feb. 2013. <http://science.uvu.edu/ochem/index.php/alphabetical/e-f/excited-state-atom/>.

"Atomic Spectroscopy." - Atomic Absorption, Emission and Fluorescence Techniques. N.p., n.d. Web. 17 Feb. 2013. <http://www.andor.com/learning-academy/atomic- Historic Atomic theory Contribution Joseph von Fraunhofer (1814)
Kirchhoff and Bunsen (1869) Johannes Robert Rydberg (1888) Max Plank(1900) Niels Bohr (1913) Studied absorption lines Related the emission spectrum lines to each other using a formula.
Spectrum lines related with positive integers. discovered emission lines.
Related absorption lines and emission lines.
Theorised that these were the fingerprints of each element.
Discovered that matter can absorb radiation and releases it in a set band of wavelengths. Explained why the spectrum lines related in positive integers through shells.
Theorized the explanation for the spectrum lines through energy levels.
This amount of energy absorbed is called a quantum of energy.
Full transcript