Chapter 1, Question 1.13 [ENDORSED]

[Rosamari Orduna 1D]

Use the Rydberg formula for atomic hydrogen to calculate the wavelength of radiation generated by 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 light that will be emitted?

Hi, I'm not sure how to go about this problem. the equation we use is : 1/lambda= (1.097x10^7)*(1/n^2 - 1/n^2), right? Im still not getting an answer that seems right, perhaps I am doing it in the wrong order... help

[KateCaldwell 1A]

To solve part a you must use the equation v= R(1/n^2-1/n^2) and use the formula c=v times lambda. Then include both formulas, c= R(1/2^2-1/4^2)times lambda
To solve for part b you use the value you got for part a(486 nm) and classify which series that number falls under (Balmer).
To solve part c you take the same value from part a and use the 1.1 table to classify the radiation type (visible and blue).