Question

The transitions observed in the visible region correspond to the balmer series where n(intial) is more than 2 and n (final) = 2. Using the equation given for the hydrogen atom absorption or emission spectrum, determine which energy transition (n(intial) -> n(final)) each of the observed lines represents. Given that the energy levels, nfinal and ninitial are interegers and that nfinal = 2, trial and error will allow you to determine the transitions. Be sure to convert kJ/mol to kJ using Avogadro's number. Equation in comments. Can someone help please?

Answer 1

\[DeltaE = E _{final} - E _{intial} = -(2.18 x 10^-18)(1/n^2 _{final} - 1/n^2 _{initial}\] where n = 1,2,3,4... \[\infty \]

Answer 2

Do you know what the units of the constant are?

Answer 3

They didn't give me the units :/ Let me see if I can find it

Answer 4

Jules

Answer 5

Ok, cool. Are we supposed to have some lines given?

Answer 6

Oh oops. One second!

Answer 7

Oh, ok. It looks like we just need to guess and check using integers to try to get these wavelengths.

Answer 8

Won't all my answers come out as negative though? Don't I need positive wavelengths?

Answer 9

You will get negative energies, but that just means that energy is released.

Answer 10

You will need to convert to wavelength using E=hc/lambda

Answer 11

Will the wavelength come out as negative and then I just put a positive sign in front?

Answer 12

Yeah, pretty much.

Answer 13

Okay, I'll start on that, thank you!

Answer 14

Sure! :)

Answer 15

I think I did something wrong..I got 3.1 * 10^-33 s/J

Answer 16

oh J/s*

Answer 17

I'm not sure what do to next

Answer 18

Sorry, but I have to go for the evening. @abb0t Can you help? @dan815

Answer 19

Thank you for your help so far! I appreciate it.