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The emission spectrum of a molecule displays the specific wavelengths of light emitted when electrons transition from higher energy levels to lower ones. Each wavelength corresponds to a unique energy difference between these levels, allowing for the identification of the molecule. The resulting spectrum appears as a series of lines or bands, which can be used to determine the molecular structure and composition. Overall, it serves as a fingerprint for the molecule, revealing information about its electronic states.
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What is the difference between absorption and emission spectrum?
Emission spectrum: lines emitted from an atom.Absorption spectrum: absorbed wavelengths of a molecule.
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 is the name of the spectrum when elements produce different colors when heated?
The spectrum produced when elements emit different colors when heated is called an emission spectrum. Each element has a unique emission spectrum based on the specific wavelengths of light it emits.
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 the difference between absorption and emission spectrum?
Emission spectrum: lines emitted from an atom.Absorption spectrum: absorbed wavelengths of a molecule.
Explain why the fluorescence emission spectrum of a polyaromatic molecule in solution mirrors the shape of the absorption spectrum regardless of the excitation frequency?
Generally fluorescence emission spectrum is independent of the excitation wavelength because of the rapid internal conversion from higher energy initial excited states to the lowest vibrational energy level of the excited state
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.
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?
Niels Bohr studied the emission lines 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 of sodium lies in the yellow region
What is the emission spectrum of elements list?
The emission spectrum of elements is a unique pattern of colored lines produced when an element is heated or excited. Each element has its own distinct emission spectrum, which can be used to identify the element.
How can you Distinguish absorption spectrum from emission spectrum?
Emission spectra are bright-line spectra, absorption spectra are dark-line spectra. That is: an emission spectrum is a series of bright lines on a dark background. An absorption spectrum is a series of dark lines on a normal spectrum (rainbow) background.
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?
The difference between continuous spectrum and the atomic emission espectrum of an element is that in emission spectrum, only certain specific frequencies of light are emitted while in a continuous spectrum, a continuous range of colors are seen in the visible light.
