How Do The Various Filters Change The Spectrum Produced By The Hydrogen Lamp?

Let's go back to unproblematic assimilation and emission spectra. Nosotros can apply a star's assimilation spectrum to figure out what elements it is made of based on the colors of light it absorbs. We can utilize a glowing nebula's emission spectrum to figure out what gases it is made of based on the colors it emits. We can practise both of these because each chemical element has its own unique spectrum.

Why is this? Let'south have a look at hydrogen, the nigh arable element in the universe.

Absorption of Light by Hydrogen

A hydrogen cantlet is very unproblematic. It consists of a single proton in the nucleus, and one electron orbiting the nucleus. When a hydrogen cantlet is just sitting around without much energy, its electron is at the everyman energy level. When the atom absorbs light, the electron jumps to a college energy level (an "excited state"). Information technology can jump i level or a few levels depending on how much energy it absorbs.

The interesting thing is that the electron can move merely from ane energy level to another. Information technology tin't go partway between levels. In addition, it takes a very detached amount of free energy—no more, no less—to move the electron from one particular level to some other.

The energy that an electron needs in club to jump up to a certain level corresponds to the wavelength of low-cal that information technology absorbs. Said in some other mode, electrons blot only the photons that requite them exactly the right free energy they need to jump levels. (Call back when nosotros said that photons only carry very specific amounts of energy, and that their energy corresponds to their wavelength?)

The assimilation spectrum of hydrogen shows the results of this interaction. In the visible role of the spectrum, hydrogen absorbs light with wavelengths of 410 nm (violet), 434 nm (blue), 486 nm (blueish-light-green), and 656 nm (red). Each of the assimilation lines corresponds to a specific electron jump. The shortest wavelength/highest free energy light (violet 410 nm) causes the electron to leap up four levels, while the longest wavelength/lowest energy light (red 656 nm) causes a jump of just 1 level.

The relationship betwixt a hydrogen atom and its assimilation spectrum. (Left) A unproblematic model of a hydrogen cantlet showing 4 of the many possible "jumps" the electron could make when it absorbs low-cal. (Right) The relationship betwixt the electron jumps and the specific wavelengths of low-cal that the atom absorbs. An electron jumps from one energy level to another only when it absorbs a very specific wavelength of low-cal (i.e., when it absorbs a photon with a specific energy). The shorter the wavelength, the higher the energy, and the college the bound. This analogy shows a set of jumps that stand for to absorption of visible wavelengths (the Balmer Series). CREDIT: NASA, ESA, and 50. Hustak (STScI). Become THE FULL Prototype IN Resource GALLERY >

Emission of Low-cal past Hydrogen

Electrons can also lose energy and drop down to lower energy levels. When an electron drops downward between levels, it emits photons with the same amount of energy—the same wavelength—that it would need to absorb in order to move up between those same levels. This is why hydrogen'southward emission spectrum is the inverse of its absorption spectrum, with emission lines at 410 nm (violet), 434 nm (bluish), 486 nm (blue-green), and 656 nm (red). The highest energy and shortest wavelength light is given off past the electrons that fall the farthest.

The relationship betwixt a hydrogen atom and its emission spectrum. (Left) A unproblematic model of a hydrogen atom showing four of the many possible "drops" the electron could brand when information technology emits calorie-free. (Right) The human relationship between the electron drop and the specific wavelengths of light that the atom emits. When an electron drops downwardly from one energy level to another, it emits a very specific wavelength of lite (i.e., it emits a photon with a specific energy). The farther the drop, the shorter the wavelength and the college the energy of the photon. This analogy shows a set of drops that correspond to emission of visible wavelengths (the Balmer Serial). CREDIT: NASA, ESA, and L. Hustak (STScI). Get THE FULL IMAGE IN RESOURCE GALLERY >

Other Atoms and Molecules

Different elements take dissimilar spectra because they accept different numbers of protons, and different numbers and arrangements of electrons. The differences in spectra reverberate the differences in the amount of energy that the atoms blot or give off when their electrons motility between energy levels.

Molecules, similar water, carbon dioxide, and methane, also accept distinct spectra. Although it gets a fleck more complicated, the basic idea is the aforementioned. Molecules can blot specific bands of light, corresponding to detached changes in energy. In the example of molecules, these changes in energy can be related to electron jumps, but can also exist related to rotations and vibrations of the molecules.

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Source: https://webbtelescope.org/resource-gallery/articles/pagecontent/filter-articles/spectroscopy-101--how-absorption-and-emission-spectra-work?filterUUID=a776e097-0c60-421c-baec-1d8ad049bfb0

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