## Using the Rydberg Equation

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

K Stefanescu 2I
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### Using the Rydberg Equation

On question 1.15, I understood how to solve for n1 and n2 in every respect besides why we assume that n1=1. The way the textbook solves it requires that we assume n1=1 in order to find n2=3. Why is this the case? Does this apply in every scenario?

Chem_Mod
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### Re: Using the Rydberg Equation

Please type out the question from the text so that is it easier for students to see.

Chem_Mod
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### Re: Using the Rydberg Equation

The wavelength falls within the range of wavelengths (97-122 nm) that would constitute the Lyman Series. This has not yet been talked about, however all you need to know is that the final energy energy level of an electron that emitted this wavelength range of light will be n=1. Subsequently, the Balmer Series refers to a range of wavelengths (410-656 nm), which corresponds to the final energy level of an electron being n=2. Hope this helped.

Alissa Stanley 3G
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### Re: Using the Rydberg Equation

Is it essential to memorize which series corresponds to each n? And what wavelengths correspond to each series?

Guangyu Li 2J
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### Re: Using the Rydberg Equation

The given solution turns E/h to v first that we can set up an equation. Since we know the one of the n, we can figure the other one through the formula more easily.

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