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As changes in energy levels of electrons increase the frequencies of atomic line spectra they emit .?
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Will the number of lines in an atoms spectra increase or decrease as the number of electrons in an atom increase?
increase
Why amonia solution of alkali metals are blue in clour?
Solvated electrons. The electrons "dissolve" from the metal. It's blue because electrons have a different absorption spectra.
Why is it that different light sources have different types of spectra?
Different atoms have a different number of electrons. This is why they show different spectra.
Under what circumstances does the Bohr model fail to make accurate predictions of an atoms spectra?
The Bohr model fails to accurately predict an atom's spectra when dealing with more complex atoms that have multiple electrons. This is because the model assumes that electrons move in circular orbits around the nucleus, whereas in reality, electrons occupy regions of space called orbitals. Additionally, the model only accounts for the behavior of electrons in the ground state and does not consider excited states where electrons can transition between different energy levels.
What was Niels Bohr's key hypothesis about the behavior of electrons in atoms that he formulated to explain the discrete pattern of atomic spectra?
That electrons can orbit their nucleus in only certain discrete orbits at certain specific levels of energy
Will the number of lines in an atoms spectra increase or decrease as the number of electrons in an atom increase?
increase
Characteristic series of frequencies of electromagnetic radiation substances emit?
Spectra
What are the similarities between emission and absorption spectra?
The lines are at the same frequencies
The line spectra of atoms provides experimental evidence for?
the arrangment of electrons
What has the author Michael Edward O'Byrne written?
Michael Edward O'Byrne has written: 'Combination frequencies and infra-red absorption spectra of certain alkaloids' -- subject(s): Absorption spectra, Alkaloids, Infrared spectra, Spectrum analysis, Tables
Why are the spectra of different light sources different?
A single, extremely tiny unit of light known as a photon is produced when one electron in an atom undergoes a quantum drop in energy level. There are many such energy changes that electrons in the atoms of a single element can undergo, and they are all different. Furthermore, the energy changes for one element differ from the energy changes for all other elements. Now for why this is important: The amount of energy in a photon is directly proportional to the frequency of the light or other electromagnetic radiation of that photon. Therefore, each atom produces a set of electromagnetic frequencies that represents the possible downward changes in energy levels of its electrons.
What effect does the nucleus have on atomic spectra of different elements?
Aside from determining how many electrons the atom has, the nucleus does not affect the spectra of that atom in any way.
Why amonia solution of alkali metals are blue in clour?
Solvated electrons. The electrons "dissolve" from the metal. It's blue because electrons have a different absorption spectra.
What is the frequency of a hydrogen atom?
An atom doesn't have a frequency. It can vibrate with many different frequencies. It can absorb radiation of different frequencies under different circumstances. For instance, electrons moving between various energy levels absorb and release characteristic frequencies of visible and ultra-violet light, and in a magnetic field radio frequency energy can be absorbed as the nucleus moves from one spin state to another. Bonds between hydrogen and other atoms absorb energies in the infra red. All these things give spectra of various frequencies, not an individual frequency.
Why is it that different light sources have different types of spectra?
Different atoms have a different number of electrons. This is why they show different spectra.
How do scientists use different spectra to figure out the composition of the stars outer layer?
Different chemical elements emit (or absorb) certain specific frequencies of light. When the light from a star is split in to it's rainbow spectrum of light, certain parts of the spectrum will be black (in absorption spectra) or brighter (in emission spectra). By comparing these lines to the known emission and absorption spectra of elements, the composition of a stars atmosphere can be determined.
Under what circumstances does the Bohr model fail to make accurate predictions of an atoms spectra?
The Bohr model fails to accurately predict an atom's spectra when dealing with more complex atoms that have multiple electrons. This is because the model assumes that electrons move in circular orbits around the nucleus, whereas in reality, electrons occupy regions of space called orbitals. Additionally, the model only accounts for the behavior of electrons in the ground state and does not consider excited states where electrons can transition between different energy levels.
