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Why are atomic absorption lines very narrow?
Atomic absorption lines are very narrow because they result from the absorption of light by individual atoms at specific energy levels. This absorption occurs at precise wavelengths corresponding to the energy differences between the atom's electron orbits. The narrowness of the lines is due to the limited number of possible energy transitions within an atom, resulting in distinct and well-defined absorption peaks.
Why in an absorption spectrum the back ground is bright and the lines are dark?
Because it is an absorption spectrum. An absorption spectrum begins with a source of pure white light. This hits a prism which spreads it out into a spectrum and the result shows on a screen as a bright band of colours. If you put this into a glass case and seal it to the outside world, nothing changes. Now if blow a gas into the tank, the atoms in the gas absorb different wavelengths (colours) of light. The result you see is a normal spectrum of colours, but with one or more dark lines across it. This is because the atoms in the gas through which the white light is shining are absorbing some or all of various colours in the spectrum. What those colours are is absolutely characteristic and definitive of that particular gas. This is a very powerful technique for identifying elements which are present only in trace amounts. An interesting light on this is that the element Helium was first discovered not on earth, but on the sun by some dark lines in the sun's spectrum which did not belong to any known element.
What causes the lines in an atomice spectrum?
The lines in an atomic spectrum are caused by the emission or absorption of photons as electrons move between different energy levels within the atom. Each line corresponds to a specific energy transition, and the distinct set of lines is unique to each element, making them a fingerprint for identifying elements.
How are fraunhofer lines observed?
Fraunhofer lines are observed in the solar spectrum by using a spectroscope to disperse sunlight into its component colors. These dark absorption lines are caused by the absorption of specific wavelengths of light by elements in the Sun's atmosphere. By studying the positions and intensities of these lines, scientists can learn about the composition and physical properties of the Sun.
An element is selective in the frequency of light it will absorb This selectivity is due to its?
Every element can only absorb certain wavelengths of light because of how the electrons are positioned around the nucleus. There is a fixed number of energy levels that each electron may move to, and each move will only occur if a specific amount of energy is absorbed. Thus each element, having differing electron orbital states can only absorb certain frequencies of light.
Fraunhofer lines in the solar spectrum are actually?
Fraunhofer lines are dark absorption lines in the solar spectrum caused by specific elements absorbing certain wavelengths of light. These lines help astronomers identify the chemical composition of the Sun and other stars because each element absorbs light at characteristic wavelengths, leaving dark lines in the spectrum.
Are there as many absorption lines in the solar spectrum as there are elements present in the Sun?
There are a lot more. Each element has several possible absorption lines. In fact the element iron has several hundred lines.
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.
Can the pattern of dark lines recorded by a spectrograph be used to identify the elements that are in the stars atmosphere?
Yes. Dark lines are absorption lines, they are due to relatively cool matter (such as that which might be found in a star's atmosphere as opposed to being in the body of the star itself), and each element has a characteristic pattern.
What evidence do you have the sun contains the element iron?
The spectral lines. Each element has a characteristic "fingerprint" in a spectrum.
How does the number of lines in the emission spectrum for an element compare with the number of lines in the absorption spectrum?
The number of lines in the emission spectrum is the same as in the absorption spectrum for a given element. The difference lies in the intensity of these lines; in emission, they represent light being emitted, while in absorption, they represent light being absorbed.
Why would the absorption of each element have lines in the same places as its emission spectrum?
The absorption spectrum of an element features lines at the same wavelengths as its emission spectrum because both processes involve the same energy transitions between electron energy levels. When an electron absorbs energy, it moves to a higher energy level, resulting in the absorption of specific wavelengths of light. Conversely, when an electron falls back to a lower energy level, it releases energy in the form of light at those same wavelengths. This correspondence between absorbed and emitted wavelengths is a fundamental characteristic of atomic structure.
What evidence do you have that the sun contains the element iron?
One piece of evidence that the sun contains iron is the absorption lines in its spectrum that match the wavelengths associated with iron atoms. Additionally, studies of the sun's composition through spectroscopy and helioseismology have identified iron as one of the elements present in the sun's core and atmosphere.
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.
What is band spectrum?
A band spectrum is an absorption or emission spectrum consisting of bands of closely-spaced lines, characteristic of polyatomic molecules.
Do lines of a particular element appear at the same wavelength in both emission and absorption line spectra?
No, lines of a particular element do not appear at the same wavelength in both emission and absorption line spectra. In absorption spectra, dark lines are seen where specific wavelengths are absorbed by elements in a cooler outer layer of a star or a cooler interstellar cloud. In contrast, emission spectra display bright lines when elements emit specific wavelengths of light at higher energy levels.
What are examples of atomic absorption spectroscopy?
When white light from mercury vapour lamp is passed through sodium vapour then we have as outcome a continuous spectrum of colours with two black lines in the yellow-orange region. These two lines stand for the absorption of 5890 A and 5896 A lines of sodium atom Another example is Fraunhofer lines seen in the continuous spectrum got from sun. These lines are due to absorption of characteristic frequencies of metals present in the chromosphere of the sun
