Confusion with problem 1.57 [ENDORSED]

[Anna De Schutter - 1A]

Hi!

Problem 1.57 says: "Lines in the Balmer series of the hydrogen spectrum are observed at 656.3, 486.1, 434.0, and 410.2 nm. What is the wavelength of the next line in the series?"

I thought because in the Balmer series we are starting at n=2, that the next line in the series would be n=6. However, the solutions manual says "For the Balmer series n1=2, so the fifth line in the spectrum should be n2=7." Isn't the fifth line n=6 in the Balmer series?

Thank you! :)
Anna De Schutter - section 1A

[AnnaYan_1l]

Hi, Anna! I had the same issue with this problem originally. It is important to remember that Balmer series means that the electron transitions from a higher energy level to n=2.

So, we can assume that:
656.3 nm is a transition from n=3 to n=2
486.1 nm is a transition from n=4 to n=2
434.0 nm is a transition from n=5 to n=2
410.2 nm is a transition from n=6 to n=2
So, the next line in the series would be a transition from n=7 to n=2.

(Then, you can use the equation to solve for the energy released. Finally, you would solve for wavelength.)

I hope that helps!

[Anna De Schutter - 1A]

That makes a lot of sense! Thank you so much! :)

[Joussie Camacho 4I]

Will we be tested on the Balmer series in Test 2?

[Joussie Camacho 4I]

Will we be tested on the Balmer series in Test 2?