[CHM 111] Chapter 6 question-CHM 111-Kristy Jones

[Andrew J. Pounds]

If you look back at the notes, the -2.18x10^-18 is the Rydberg constant 
in Joules.  It was the collection of a bunch of contants that we 
described just after the Bohr radius.

The 1.097x10^7   represents the Rydberg in units of Wavenumbers 
($\bar{\nu}$) -- which have units of reciprocal length.

$E = h \nu = \frac{h c}{\lambda} = hc\bar{\nu}$

so

$\bar{\nu}=\frac{1}{\lambda}$

The equation was derived for the hydrogen spectrum but was generalized 
to atom elements through the inclusion of the atomic number $Z$ in the 
equation.  As we discussed in class, the actual success of this 
formulation is limited -- mainly to the first and second row of the 
periodic table.


On 11/04/2017 05:22 PM,  wrote:
> Dr. Pounds,
> A question on sapling asks for the energy of an electron on certain levels of orbitals. I know that the equation we need to use is E(of n)= -2.18*10^-18 J * (1/n^2). Where does the -2.18 * 10^-18 come from? I know that Rydberg’s number is 1.097*10^7 and somehow these numbers are related, but I do not know how. And is this equation only good for hydrogen? Or should we know a similar formula for all elements?
>
> Thank you,


-- 
Andrew J. Pounds, Ph.D.  (pounds_aj at mercer.edu)
Professor of Chemistry and Computer Science
Mercer University,  Macon, GA 31207   (478) 301-5627
http://faculty.mercer.edu/pounds_aj

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