Why Iron Produces Green Light in Visible Spectrum

[Idyllic]

Homework Statement

Iron produces many lines in the visible spectrum when given energy. Suggest why a sample of iron sulphate only produces lines in the green section of the spectrum.

Sorry if it doesn't sound very scientific, I am recalling the question from memory since I've already handed up the assignment. Assume that the answer has nothing to do with the sulfate or water present.

Homework Equations

The Attempt at a Solution

Im doing yr12 physics in South Australia, so far in 'the structure of the atom' we have learned about the absorption and emission spectrum.
This is one question from our homework assignment, and i refused to answer it because i believe the answer involves a great deal more than just what we've learned so far. iron in iron sulphate has 2 less electrons, and i don't believe that its as simple as saying that its 'combinations' or 'possibilities' of different energies of photons released has changed because of the different ratio of protons/electrons attracting each other.

I think this is a question that the teacher made up, no its not a very good one, and i reckon a question like this will definately not be in the exam.

 

[jbsteele]

My teacher is not very good at physics, so i don't think the answer to this question is actually something that is even taught in yr12.I believe the reason why iron sulphate only produces lines in the green section of the spectrum is because the energy levels of the electrons in the iron are different than in pure iron. When an electron in the iron sulphate is excited, it can only reach certain energy levels due to the way the electrons interact with each other, and therefore it can only emit photons of certain energies. Therefore, the photons emitted will only be in the green section of the spectrum.

 

[baba89]

I would suggest that the reason iron produces green light in the visible spectrum is due to its electronic structure and energy levels. Iron has multiple energy levels within its electrons, and when given energy, these electrons can jump to higher energy levels. When the electrons return to their original energy level, they release energy in the form of light. The specific wavelength of light that is released depends on the difference in energy between the two levels. In the case of iron, the energy difference between the levels that produce green light is the most common and easiest to achieve. This could explain why a sample of iron sulfate only produces lines in the green section of the spectrum. Additionally, it is possible that the other energy levels are not easily accessible or are not affected by the energy given to the sample, resulting in only green light being produced. However, further research and experimentation would be needed to fully understand the specific reasons for this phenomenon.