Problem: One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (b) Determine the initial and final values of n associated with this emission.

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The emitted light has a wavelength of 93.8 nm. When you look at the electromagnetic spectrum, this wavelength lies in the UV region. When the emission is within the UV region we call this the Lyman Series.

Lyman series is referred to when an electron goes from higher numbered shell to the 1st shell.

Based on the Lyman Series, we know now that the final energy level is the first shell where:

nf = 1

We can determine ninitial using the Bohr Equation shown below:

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Problem Details

One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (b) Determine the initial and final values of n associated with this emission.

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Our data indicates that this problem or a close variation was asked in Chemistry: The Central Science - Brown 11th Edition. You can also practice Chemistry: The Central Science - Brown 11th Edition practice problems.