In its ground-state, a H atom absorbs a photon of wavelength 97.20 nm. To what energy level does its electron move?
The answer is 4.
How is this value reached?
Here's what I did:
c=(freq)(wavelength), (3x10^8)/(97.20x10^-9), so freq. = 3.09x10^15 Hz.
Then I used E=hv, (6.626x10^-34)(3.09x10^15), so E = 2.05x10^-18 J(?).
Finally, I plugged it into the energy level equation: 2.05x10^-18 = -B(1/x^2 - 1/1^2), with B = 2.179x10^-18...
The answer I got was 1 - which is incorrect!
I know I made a mistake on the last part, so could anyone please clarify?
2006-12-06
06:49:00
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2 answers
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asked by
other_user
2
in
Chemistry