Black lines in elements' emission spectra

[Intimidat0r]

My understanding of analyzing emission spectra is that when the quantum number of an electron decreases (i.e. when it falls closer to the nucleus) it emits energy. I understand that this is a very basic understanding but I have not yet made it to college, so please bear with me. :) Now, what I can't figure out is why different elements' emission spectra have black parts in different places, or why the black parts are even there. Does it have something to do with electrons not being able to exist between two energy levels?

Unfortunately, my chemistry teacher and my textbook do not explain things too well, so I can't turn to them for help, especially when we aren't really expected/required to know any more about this than what I already know for the course.

Thank you for your time.

 

[mgb_phys]

Dark absorbtion linesare formed in exactly the same way - if you have a continuous spectrum illuminated some colder molecules theelectrosn absorb energy and are promoted to higher orbitals - since this only occurs if they absorb a photon of exactly the right energy you get sharp absorbtion features in the spectrum.

 

[sir-pinski]

First of all, it's great that you are interested in learning more about emission spectra even before starting college. It shows a strong curiosity and passion for science. Now, let's dive into your question about the black lines in elements' emission spectra.

The black lines that you see in an emission spectrum are called absorption lines. These are specific wavelengths of light that are absorbed by the atoms in the element, resulting in a "gap" or a black line in the spectrum. This happens because the electrons in the atoms can only exist in specific energy levels, and when they absorb a photon of light, they jump up to a higher energy level. This causes a gap in the spectrum because the energy of the absorbed photon is not emitted back out.

The specific placement of these absorption lines is determined by the energy levels of the electrons in the atom. Each element has a unique arrangement of electrons, and therefore, the energy levels are also unique. This results in a unique emission spectrum for each element, with different black lines in different places.

To understand this concept better, think of the electrons in an atom as being in different "shells." The first shell is closest to the nucleus, and the subsequent shells are further away. The electrons in the first shell have the lowest energy, and as you move outwards, the energy of the electrons increases. When an electron jumps from a lower energy level to a higher one, it absorbs a photon of light, resulting in a black line in the emission spectrum.

I hope this explanation helps you understand the concept of absorption lines in emission spectra a bit better. Keep exploring and asking questions, and you will surely learn more about this fascinating topic as you progress in your studies. Best of luck!