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A linear emission spectrum is the collection of frequencies that a substance can emit when the atoms in it are excited (say, by heating) or can absorb. Where visible light frequencies are involved the emitted frequencies may be made to appear as a series of coloured lines on an axis representing frequency. Such a spectrum may also be represented as a series of dark lines presented against a straightened rainbow of colours where the axis along the edge of the rainbow represents light frequency.
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A linear emission spectrum displays a series of distinct colored lines at specific wavelengths, resulting from the emission of light by excited atoms or molecules returning to lower energy states. Each line corresponds to a specific electron transition within the atom or molecule, allowing for identification of the elements or compounds present in a sample based on their unique line patterns.
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Is an atomic emission spectrum a continuous range of colors?
No, an atomic emission spectrum is not a continuous range of colors. It consists of discrete lines of specific wavelengths corresponding to the emission of light from excited atoms when they return to lower energy levels. Each element has a unique atomic emission spectrum due to its unique arrangement of electrons.
What is a star's emission spectrum?
A star's emission spectrum is a unique pattern of light emitted by the star, showing distinct wavelengths or colors of light. It provides information about the star's composition, temperature, and other properties. By analyzing the emission spectrum, astronomers can learn about the chemical elements present in the star and its physical characteristics.
What is the sun's wavelength of maximum energy emission in what range?
The Sun's wavelength of maximum energy emission falls within the visible light spectrum, specifically in the range of around 500 to 600 nanometers. This corresponds to the green to yellow part of the spectrum.
Which type of spectrum is associated with the radiation of most stars?
Most stars exhibit a continuous spectrum, which contains all wavelengths of light in a continuous distribution. This is often referred to as a blackbody spectrum due to its smooth curve.
The lines at the ultraviolet end of the hydrogen spectrum are known as the lyman series wich electron transitions within an atom are responsible for these lines?
The Lyman series in the hydrogen spectrum corresponds to electron transitions from higher energy levels to the n=1 energy level. These transitions result in the emission of photons in the ultraviolet region of the electromagnetic spectrum.
What is a flame tested used for?
To identify an unknown sample by its emission spectrum
Which element did Bohr study the line emission spectrum of?
Bohr studied the line emission spectrum of hydrogen.
Is an atomic emission spectrum a continuous range of colors?
No, an atomic emission spectrum is not a continuous range of colors. It consists of discrete lines of specific wavelengths corresponding to the emission of light from excited atoms when they return to lower energy levels. Each element has a unique atomic emission spectrum due to its unique arrangement of electrons.
In what region of visible range does the emission spectrum of sodium lie?
The emission spectrum of sodium lies in the yellow region of the visible spectrum, specifically around 589 nanometers.
Is it possible for two metals to have the same emission spectrum?
No. It is not possible for two metals to have the same emission spectrum. For metals to have the same emission spectrum, they would need for their electrons to have duplicate orbitals. That would be impossible due to the exclusion principle.
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.
Explain the difference between the continuous spectrum of white light and the atomic emission spectrum of an element?
White light has a continuous spectrum with all wavelengths of light present, while the atomic emission spectrum of an element consists of specific wavelengths corresponding to the energy levels of the element's electrons. The emission spectrum is unique to each element and can be used to identify the element present.
An emission spectrum can be used to?
Identify elements
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.
Could you use an emission spectrum of an element to identify it?
No.
What element can produce an atomic emission spectrum in its natural state neon chlorine silicon or Krypton?
Every element can produce an emission spectrum, if it is sufficiently heated. Of the 4 elements that you mention, neon is the most useful, in terms of its emission spectrum, and it is used in a certain type of lighting.
Which region gives rise to an emission spectrum?
The photosphere.
