Energy levels

[Sarina Mak 1B]

Does using Rydberg's equation (v=-R[1/n^2 - 1/n^2)) and E=-hR/n^2 to find the energy level result in the same answer?

For example, in the module question: An excited H atom emits light with frequency of 1.14E14 Hz to reach the energy level n=4. In what level did the electron begin? When I used the first equation, I got about n=6, but when I used the second equation, I got about n=3.

Should there be situations for when I use one equation but not the other?

[Hailey Qasawadish 2J]

You should get the same answer either way! Maybe you made a calculation error somewhere? Or maybe you have the final and initial mixed up? If you want to include your work in this post, maybe we can find where it went wrong!

[CesarLec1]

As the person said above, it should lead to the same answer but one can be more useful to use than the other it all depends on the context and your organization but either one is good.

[Grace_Remphrey_2J]

Though context would suggest which is better to use, both formulas should produce the same result. There was probably an error in your calculation! Hope this helps.

[Eliana Witham 2H]

If this happened on the final and it was because you mixed up final and initial, you could also just reread the problem and look at whether the energy level needs to be above or below n=4. Because light was emitted, the answer should be n>4.

[Acharya Ranawat 3E]

I believe this is a calculation error. You should get the same answer. I believe the more intuitive way to do this problem however is to just use the E=(-hR)/(n^2) equation and use subtraction of the original energy state from the final energy state. Hope this helps!