Electrons and Quantum Mechanics - Oakland Schools
Electrons and Quantum Mechanics - Oakland Schools
Electrons and Quantum Mechanics - Oakland Schools
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Summary<br />
• An electron absorbs heat or electrical energy <strong>and</strong> is promoted to a higher level<br />
• The electron returns to the original level <strong>and</strong> emits the difference as a specific<br />
electromagnetic radiation.<br />
• The wavelength seen is related to the energy of the emission by Planck’s<br />
equation E=hv<br />
E = energy of the emission<br />
h = Planck’s constant (6.02 x 10 -34 )<br />
ν = frequency of the radiation (the frequency is related to the wavelength by c = λν,<br />
c is the speed of light <strong>and</strong> λ is the wavelength)<br />
Example:-<br />
giving series of lines in<br />
the visible range<br />
Hydrogen spectrum transitions<br />
due to transitions --><br />
n=2:(Balmer series)<br />
http://ibchem.com/IB/ibnotes/full/ato_htm/12.2.htm - Periodic table showing<br />
absorption <strong>and</strong> emission spectrum.<br />
http://www.wwnorton.com/college/chemistry/gilbert/overview/ch3.htm#spectrum -<br />
Light emission <strong>and</strong> absorption Tutorial for Na.<br />
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