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What are the two types of spectrum?
The two types of spectrum are continuous spectrum, which shows a continuous range of colors with no gaps, and line spectrum, which consists of distinct lines of color separated by gaps.
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.
How did Sir Norman Lockyer discover helium?
Sir Norman Lockyer discovered helium in 1868 in the spectrum of the sun during a solar eclipse. He noticed a yellow line in the sun's spectrum that did not correspond to any known element at the time, leading to the discovery of the new element helium.
Is it true that each element has a unique set of lines on a spectrum?
Yes, each element has a unique set of spectral lines because the lines are determined by the energy levels of the electrons in that specific element. This uniqueness allows scientists to identify elements based on their spectral signature.
Why line spectrum is called finger print spectrum?
It is unique to a specific atom. The emission spectrum of sodium, for example, has two characteristic lines close together in the yellow part of the spectrum, which cannot be found in any other atom. Each line in a spectrum relates to a change in electron state or level.
Why is there a line spectrum over a continuous spectrum in a spectroscope?
The lines in a spectroscope tell what element(s) are being observed. The continuous color are background noise or put there for a reference.
Why can the bright-line spectrum of an element be used to identify an element?
The bright-line spectrum of an element is unique because it consists of specific wavelengths corresponding to the energy levels of electrons transitioning in that element's atoms. Since each element has a distinct arrangement of electrons, the pattern of lines in its spectrum is like a fingerprint, allowing scientists to identify the element based on the specific wavelengths present in the spectrum.
How does the color of the flame correspond to the distinct lines in its spectrum?
The color in the flame is the representation of a specific line in the spectrum.
What is the color of mercury spectrum line of wavelength 576.96 nanometet?
The color of a mercury spectrum line with a wavelength of 576.96 nanometers is green.
Element named after brilliant indigo line in its spectrum?
Indium
What does the term bright line spectrum mean?
A bright line spectrum refers to the pattern of distinct and bright lines of different colors that are produced when an element is excited and emits light. Each element has a unique bright line spectrum that can be used to identify the element through spectroscopy.
A line spectrum is to an element as a person is to a?
fingerprint. Each element has a unique line spectrum of light emissions associated with it, similarly to how each person has a unique set of fingerprints.
Which element did Bohr study the line emission spectrum of?
Niels Bohr studied the emission lines of Hydrogen.
What do you call a prism spreading out light into colors?
It is called Visible light Spectrum.
What are the two types of spectrum?
The two types of spectrum are continuous spectrum, which shows a continuous range of colors with no gaps, and line spectrum, which consists of distinct lines of color separated by gaps.
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.
The bright-line spectrum produced by the excited atoms of an element contains wavelengths that are?
specific to that element and correspond to the energy levels of the electrons transitioning between orbitals. The wavelengths in the bright-line spectrum are unique for each element, allowing scientists to identify elements based on their spectral lines.
