Posted by **Amber** on Friday, April 6, 2012 at 1:24am.

for the transition of an electron in a hydrogen atom between the principal quantum number levels 4 and 3, calculate

a) the energy released

b) the wavelength of the line in the spectra.

- Please Chemistry Help -
**DrBob222**, Friday, April 6, 2012 at 1:35am
E = 2.180E-19 x (1/9 - 1/16)

Then E = hc/wavelength

- Please Chemistry Help -
**Amber**, Friday, April 6, 2012 at 2:03am
can you explain it a little more cuz i really didn't understand anything!!!!

thank you!

- Please Chemistry Help -
**DrBob222**, Friday, April 6, 2012 at 2:10am
Energy in joules = 2.180E-19(1/n1^2 - 1/n2^2)

n1 = 3 and 1/n^2 is 1/9

n2 = 4 and 1/n^2 is 1/16

The rest of it is algebra.

After you have the energy, then set that in the following equation.

E = hc/wavelength.

h is Planck's constant in J.s

c is speed of light in m/s

wavelength is in meters. Plug and chug.

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