Calculate Transition in Hydrogen for 600nm Wavelength

[unf0r5ak3n]

Homework Statement

use the RYDBERG formula to suggest a possible transition that would result in the observed wavelength

Homework Equations

Hydrogen - yellow wavelength about 600nm

The Attempt at a Solution

I used c= lambda x frequency(V) and found (V) to equal 5e14/second
I then used energy(E) = constant(h) x V and found E to equal 3.32e-19j
Last i used En = (-2.178e-18j)/n^2 to find the transition, I did 3.32e-19j = (-2.178e-18j)/n^2 and found n^2 to equal -6.57014 and I'm stuck there because it's a negative number...

 

[Borek]

Rydberg formula contains two integers, not one.

What is Rydberg constant value?

 

[chemisttree]

I believe negative results infer emission rather than absorption.

 

[unf0r5ak3n]

That formula finds the principle energy level, not the energy emission or absorption

 

[unf0r5ak3n]

We haven't learned rydbergs constant yet, so I was assuming we used the one I posted

 

[Borek]

http://en.wikipedia.org/wiki/Rydberg_formula

 

[unf0r5ak3n]

we haven'y learned that formula yet, he told us to use E(n) = (-2.178x10^-18)/n^2

 

[unf0r5ak3n]

ok well i did (change in energy) = E(f) - E(i)
delta(E) = 3.3e-19
E(f) = En when n=2
When n=2 E= -5.445e-19
so 3.3e-19 = -5.445e-19 - E(i)
E(i) = -8.745e-19
I then used E(i) = -2.178e-18/n2
i got n= 1.57815 which doesn't make sense, can anyone tell me what i did wrong?