2. BOHR’S LIFE AND HIS WORKS WHEN AND WHERE WAS OUR SCIENTIST BORN? WHAT EXPERIMENTS DID OUR SCIENTIST DO? HOW DID SUCH EXPERIMENTS HELP IMPROVEMENT OF ATOMC MODEL? HOW DID OUR SCINETIST’S FINDINGS HELP ADVANCEMENT OF OUR UNDERSTANDING OF ATOMIC STRUCTURE?

3.  In Copenhagen on october 7,1885.  As the son of Christian Bohr, professor of physiology at Copenhagen University.  His mother came from a family distinguished in the field of education.  In 1903, he entered Copenhagen University  His Master's degree in Physics in 1909 and his Doctor's degree in 1911.  The award of the Nobel Prize for 1922. WHEN AND WHERE WAS OUR SCIENTIST BORN?

4.  Determination of the surface-tension of water by the method of jet vibration  The spectra of helium and hydrogen  Atomic models and X-ray spectra.  X-ray spectrums and the periodic system of elements  The polarisation of fluorescent light  The quantum theory of radiation  Planck ' s constant and the atomic nucleus  Atomic structure

5.  Surface tension with Sir J.J. Thomson at Cambridge.  Manchester in March 1912 and joined Ernest Rutherford's group studying the structure of the atom.  Bohr was among the first to see the importance of the atomic number.  Rutherford's nuclear atom was both mechanically and electromagnetically unstable, but Bohr imposed stability on it by introducing the new and not yet clarified ideas of the quantum theory being developed by Max Planck, Albert Einstein, and other physicists. Departing radically from classical physics

6. 1) Electrons assume only certain orbits around the nucleus. These orbits are stable and called "stationary" orbits. 2) Each orbit has an energy associated with it. For example the orbit closest to the nucleus has an energy E1, the next closest E2 and so on. 3) Light is emitted when an electron jumps from a higher orbit to a lower orbit and absorbed when it jumps from a lower to higher orbit. 4) The energy and frequency of light emitted or absorbed is given by the difference between the two orbit energies, e.g.,  E(light) = Ef - Ei  n = E(light)/h  h= Planck's constant = 6.627x10-34 Js  where "f" and "i" represent final and initial orbits

10.  Bohr postulated that Electrons move around the nucleus in “circular orbits” with an angular momentum, mvr,given by mvr=nh/2∏  m = mass of e-  v = velocity of e-  r = radius of orbit  h = Planck’s constant  n = principle quantum number.  This description of atomic structure is known as the Bohr atomic model.

12.  http://tr.wikipedia.org/wiki/Bohr_modeli http://tr.wikipedia.org/wiki/Bohr_modeli  http://nobelprize.org/nobel_prizes/physics/laureates/1922/bohr- bio.html http://nobelprize.org/nobel_prizes/physics/laureates/1922/bohr- bio.html  http://abyss.uoregon.edu/~js/glossary/bohr_atom.html http://abyss.uoregon.edu/~js/glossary/bohr_atom.html  http://www.colorado.edu/physics/2000/quantumzone/bohr.html http://www.colorado.edu/physics/2000/quantumzone/bohr.html  http://www.youtube.com/watch?v=t005KSfs03g&feature=related http://www.youtube.com/watch?v=t005KSfs03g&feature=related

13. THANK YOU FOR YOUR ATTENTION