Difference in energy between visible line spectrum and ultraviolet?

In summary: transitions) to the lowest energy level of orbit and thus releasing more energy and shorter wavelengths.
  • #1
cheekygeek
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Homework Statement


The emission spectrum of an unknown element contains two lines - one in the visible portion of the spectrum, and the other, ultraviolet. Based on the following figure and what you know about Niels Bohr's model of the atom, account for the difference in energy between these lines.

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Homework Equations


n/a

The Attempt at a Solution


Bohr suggests that colours in the line spectra are emitted by electrons. Electrons orbit the nucleus in very specific orbits, and each orbit has a distinct energy. When the electron absorbs energy from some external source, it jumps (transitions) to a higher orbit or energy level. The attraction of the nucleus eventually pulls the electron back to a lower energy level and when it does the energy that the electron absorbed is emitted. In this case the line which is in the visible portion of the spectrum is produced when the electron is transitioning from a high level of orbit to a lower level of orbit and in turn releases energy that features longer wavelengths, which means that the line is lower in energy compared to the line which is emitting on the ultraviolet portion of the spectrum. The line, which is on the ultraviolet region of the spectrum, indicates that the electron is jumping from the highest (higher than the previous one) energy level of orbit to the lowest energy level of orbit and thus releasing more energy and shorter wavelengths.How did I do? Would you give me full marks for my answer?

Thank you in advance!
 
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  • #2
In this case the line which is in the visible portion of the spectrum is produced when the electron is transitioning from a high level of orbit to a lower level of orbit and in turn releases energy that features longer wavelengths, which means that the line is lower in energy compared to the line which is emitting on the ultraviolet portion of the spectrum.
That part looks a bit strange. The first comparison ("longer") has nothing to compare with.
The main idea is right - the energy difference is larger for the transition which emits UV radiation.

The line, which is on the ultraviolet region of the spectrum, indicates that the electron is jumping from the highest(higher than the previous one)
Usually, that's not the dominant effect. The energy of the lower state (the "target" of the transition) is more important.
 

Related to Difference in energy between visible line spectrum and ultraviolet?

1. What is the difference between visible line spectrum and ultraviolet?

The main difference between visible line spectrum and ultraviolet is their wavelengths. Visible light has longer wavelengths, ranging from 400 to 700 nanometers, while ultraviolet light has shorter wavelengths, ranging from 10 to 400 nanometers.

2. Why is visible light visible to the human eye while ultraviolet light is not?

The human eye is only able to detect a small portion of the electromagnetic spectrum, known as visible light. Ultraviolet light has shorter wavelengths and higher energy levels, making it invisible to the human eye.

3. How is the energy of visible light different from the energy of ultraviolet light?

The energy of a photon of light is directly proportional to its frequency. Since ultraviolet light has shorter wavelengths, it has a higher frequency and therefore higher energy compared to visible light.

4. What causes the difference in energy between visible line spectrum and ultraviolet?

The difference in energy between visible line spectrum and ultraviolet is due to the different electronic configurations of atoms. When an atom absorbs energy, its electrons jump to higher energy levels. When these electrons fall back to their original energy levels, they emit light at specific wavelengths, resulting in a line spectrum. Different atoms have different energy levels and therefore emit different line spectra.

5. How is the difference in energy between visible line spectrum and ultraviolet used in scientific research?

The difference in energy between visible line spectrum and ultraviolet is used in various scientific fields, such as spectroscopy and astronomy. By analyzing the wavelengths of light emitted or absorbed by different substances, scientists can identify and study their chemical compositions and properties. In astronomy, the analysis of the line spectra of stars and galaxies can provide information about their composition, temperature, and motion.

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