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Chapter 34: Problem 9

Why are the lines of the Lyman series in the ultraviolet while some Balmer lines are in the visible?

Short Answer

Expert verified
The lines of the Lyman series are in the ultraviolet because they correspond to transitions where the electron falls to the lowest energy level (n=1), releasing a large amount of energy that translates into the high frequency and short wavelength of UV light. On the other hand, some Balmer lines are visible because these transitions (n=2) involve less energy, which corresponds to longer wavelengths within the visible light spectrum.

Step by step solution

01

Understanding the Spectrum

The electromagnetic spectrum comprises of different ranges of wavelengths/frequencies. The visible light, which human eyes can detect, operates within a certain range of wavelengths (approx. 400-700 nm). The ultraviolet (UV) light, however, operates at both shorter wavelengths and higher frequencies than the visible light.
02

Understanding the Energy Transitions

In a hydrogen atom, when an electron moves from a higher energy state to a lower one, it emits energy in the form of light. This light may fall under different sections of the spectrum depending upon the energy of the transition.
03

Lyman Series

The Lyman series corresponds to the transition where the electron falls to the first energy level (n=1). As it descends from a higher energy level to the lowest one, it results in the release of a large amount of energy. This high energy release corresponds to a high frequency and short wavelength, which falls under the UV spectrum.
04

Balmer Series

The Balmer series refers to the transition where the electron falls to the second energy level (n=2). This means the energy release is less compared to the Lyman series. Hence, the frequency is lower and the wavelength is longer. Some of these transitions fall into the visible light spectrum, hence, we can see them.

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