## Ch.1 #13

H-Atom ($E_{n}=-\frac{hR}{n^{2}}$)

Michael Lonsway 3O
Posts: 43
Joined: Wed Sep 21, 2016 2:57 pm

### Ch.1 #13

In the question section of chapter 1 #13 asks: Use the Rydberg formula for atomic hydrogen to calculate the wavelength for the transition from n = 4 to n = 2. b) What is the name given to the spectroscopic series to which this transition belongs? c) Use Table 1.1 to determine the region of the spectrum in which the transition takes place. If the change takes place in the visible region of the spectrum, what is the color of the radiation emitted?

I was able to use the Rydberg formula to get 486 nm and could tell that the series was a Balmer series since it ends in the second energy level. I was wondering how to tell what color the radiation is. I looked at the table but I'm not sure how to tell the color radiation is based on frequency/wavelength.

Ethan Frankel 2C
Posts: 20
Joined: Wed Sep 21, 2016 2:56 pm

### Re: Ch.1 #13

486 is the wavelength in nm. When you compare that to Table 1.1 (on page 4), it is closest to 470 nm, which is blue visible light.