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In an atom of any element there are electrons in the valence shell . Each shell has a fixed no of sub shells that are characterized by specific quantum nos. So this holds true for the valence shell also . Depending on the distance of the valence electrons from the nucleus and its electro static effect on the valence electrons these valence electrons absorb energy from any high energy source that comes in its proximity. Now the entire atom has become a high energy species but by the law of thermodynamics
(and nature )
every body in the universe tends to have minimum energy and achieve stability. So these high energy electrons tend to emit the absorbed energy and come back to a lower energy state for maximum stability .In the process the emitted energy is observed as spectral lines in a spectrometer .These spetral lines together form what we call as emission spectrum
What else can I help you with?
Would the atomic emission spectra for sodium be the same on Earth as on the moon?
The atomic emission spectra for sodium would be the same on Earth and the Moon, as these spectra are determined by the electronic transitions of sodium atoms, which do not change based on location. However, the observed intensity and clarity of the spectra might differ due to atmospheric effects on Earth, such as air pressure and composition, which do not exist on the Moon. In a vacuum, like that on the Moon, the emission spectra would be more easily observed without interference.
What is the band of light obtained on the screen called?
Not sure exactly what this question refers to, but it may be asking about the atomic emission spectra where each element of the periodic table emits certain colors of light when excited.
Is solar spectra a continuous spectra?
The Sun spectra is considered continuous.
Why does the sides of the sun have different frequncys?
I'm not sure what the question is referring to . . . the "sides of the sun" don't have frequencies.So, as we always do in the case of a garbled or almost meaningless question, I'll search thethings I know about to find a question that might match this one, and then answer a questionthat I can find.Maybe it's talking about the emission spectrum of the hot gases on the surface of the sun.We do know that the characteristic 'benchmarks' in an emission spectrum are shiftedtoward higher frequencies if the source is approaching us, and toward lower frequenciesif the source is receding from us. So the emission spectra from the sun's left and right'edges' (limbs) would be shifted in opposite directions, because the sun is rotating . . .one edge is moving toward us and the other edge is moving away from us.How do you feel about that question and answer ?
How can absorption and emission spectra be used by the Hubble space telescope to study the structured of stars or other objects found in deep space?
The light generated by stars is mostly generated by hydrogen fusion. The light emitted from hydrogen has a distinctive emission spectrum. The emission spectrum undergoes shifting when the source and the receiver (Hubble) are moving in relation to each other. The spectrum will shift to the higher frequencies and shorter wavelengths ("blue shift") when the source and receiver are moving towards each other. Due to the "fact" that the universe is expanding, the source and receiver are moving away from each other. This causes the emission spectrum to shift to lower frequencies and longer wavelengths ("red shift"). The amount of red shift is an indication of the rate at which the cource and the receiver are moving away from each other. The expanding of the universe implies that the farther a source is from the receiver, the farther away the source and receiver are from each other. The red shifts of current objects have estimated that the farthest objects that we see are ~10-15 (not sure of exact number) billion light years distant from earth. As for absorption, the light emitted from a star that passes through gases of interspace and of planets will be absorbed at different wavelengths depending on the elements contained within the gas. This allows the determination of planetary atmospheres and intergalactic clouds.
Which part of the electromagnetic spectrum do the atomic emission spectra show?
Atomic emission spectra show specific wavelengths of light emitted by atoms when electrons transition from higher energy levels to lower ones. These spectra typically lie in the visible and ultraviolet regions of the electromagnetic spectrum.
Who discovered the atomic emission spectra?
The atomic emission spectra were discovered by Gustav Kirchhoff and Robert Bunsen in the mid-19th century. They observed that elements emit light at specific wavelengths when heated, leading to the development of spectroscopy.
Would the atomic emission spectra for sodium be the same on Earth as on the moon?
The atomic emission spectra for sodium would be the same on Earth and the Moon, as these spectra are determined by the electronic transitions of sodium atoms, which do not change based on location. However, the observed intensity and clarity of the spectra might differ due to atmospheric effects on Earth, such as air pressure and composition, which do not exist on the Moon. In a vacuum, like that on the Moon, the emission spectra would be more easily observed without interference.
What is atomic spectra explain its types?
Atomic spectra refer to the distinct lines of light emitted or absorbed by atoms when electrons transition between energy levels. There are two main types of atomic spectra: emission spectra, which are produced when electrons fall to lower energy levels and release energy as photons, resulting in bright lines on a dark background; and absorption spectra, which occur when electrons absorb energy and move to higher energy levels, showing dark lines on a continuous spectrum. Each element has a unique atomic spectrum, acting like a fingerprint for identification.
How Many types of Infrared Spectra?
There are three main types of infrared spectra: absorption spectra, emission spectra, and reflection spectra. Absorption spectra are produced when a material absorbs infrared energy, emission spectra are produced when a material emits infrared radiation, and reflection spectra result from the reflection of infrared radiation off a material.
Why is the atomic emission spectra like fingerprints?
Atomic emission spectra are like fingerprints because they are unique to each element. Each element has its own specific set of energy levels and electron configurations, resulting in a distinct pattern of spectral lines when the element emits light. This characteristic pattern can be used to identify and distinguish different elements, similar to how fingerprints are unique to each individual.
Does atomic emission come from the sun?
there is no atomic emission from the sun.
The atomic emission spectra of a sodium atom on earth and of a sodium atom in the sun would be?
The atomic emission spectra of a sodium atom on Earth and in the Sun would be similar, as they both involve the same transitions between energy levels in the sodium atom. However, the intensity and specific wavelengths of the spectral lines may differ due to the different conditions and temperatures present on Earth compared to in the Sun.
Advantages and disadvantages of atomic emission spectrometry?
advantages of atomic emission
What is the atomic emission spectra?
The colors of light given off when an element loses energy
What has the author R K Winge written?
R. K Winge has written: 'Inductively coupled plasma-atomic emission spectroscopy' -- subject(s): Chemical elements, Spectra
What statement of emission spectra is correct?
Emission spectra consist of discrete, colored lines at specific wavelengths, corresponding to the emission of photons as electrons transition from higher to lower energy levels. Each element has a unique emission spectrum due to its specific electron configuration and energy levels. Emission spectra are useful for identifying elements present in a sample and are commonly used in analytical chemistry and astronomy.
