Discussion_2_Solution - EXPLORING d (I). Convert the energy...

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EXPLORING d (I). Convert the energy from J/atom to kJ/mol. 1 mole = 6.02 10 23 atoms ( or molecules or any things) 2.179 x 10 -18 atom J x mole atoms 1 10 02 . 6 23 = 1312000 J/mol = 1312 kJ/mol This is the exact amount of energy on the spectrum which ejects electrons( look at the diagram). If you shine light of that energy on one H atom, the light is absorbed and the electron is removed and AT REST. The electron doesn’t have excess energy to run further more. e(I). It requires 2.179 x 10 -18 J to eject an electron from one H atom and this value is clearly less than 4.36 x 10 -18 J (look at the table, page 13). The reason is that the kinetic energy of the electron has a positive value and the total energy is less negative than the potential energy alone. As long as you shine light of energy ! 2.179 x 10 -18 J, the electron is ejected. d(II). e(II). 2.179 x 10 -18 J corresponds to the exact energy to remove an electron. This generates a separated electron AT REST. 3.179 x 10
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This note was uploaded on 09/28/2009 for the course CHEM 1A taught by Professor Nitsche during the Spring '08 term at University of California, Berkeley.

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Discussion_2_Solution - EXPLORING d (I). Convert the energy...

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