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There are several different cytochromes with diverse absorption spectra. Typically, c-type cytochromes have a prominent band peak at about 550 nm, b-type cytochromes at around 558-560 nm, and a type cytochromes out around 605 nm. There are other bands that every cytochrome has, but these regions (the so-called alpha absorption bands) are the best to distinguish the substance under study.
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FranCytochrome has a characteristic absorption spectrum with peaks around 520-550 nm, known as the Soret band, and additional peaks in the visible region around 600-700 nm, called the alpha and beta bands. These peaks correspond to different electronic transitions in the heme group of cytochrome.
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What does the absorption spectrum of an atom show?
The absorption spectrum of an atom shows that the atom emits that spectrum which it absorbs.
Dark lines in an absorption spectrum are called?
Dark lines in an absorption spectrum are called absorption lines. These lines correspond to wavelengths of light that have been absorbed by specific elements or molecules in the sample being analyzed. They appear as dips or gaps in the spectrum where less light is detected.
What does the absorption spectrum show us or tell us?
The absorption spectrum shows the specific wavelengths of light that are absorbed by a material, indicating the energy levels of electrons in the substance. By analyzing the absorption spectrum, scientists can identify the chemical composition of the material and understand its electronic structure.
What is a band spectrum?
A band spectrum is an absorption or emission spectrum consisting of bands of closely-spaced lines, characteristic of polyatomic molecules.
Why would the absorption spectrum of each element have lines in the same places as in its emission spectrum?
The absorption spectrum of an element have lines in the same places as in its emission spectrum because each line in the emission spectrum corresponds to a specific transition of electrons between energy levels. When light is absorbed by the element, electrons move from lower energy levels to higher ones, creating the same lines in the absorption spectrum as the emission spectrum. The frequencies of light absorbed and emitted are the same for a specific element, resulting in matching lines.
