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Electrons can have only specific energy (corresponding to specific levels), but nothing in between. By changing levels they absorb or emitt energy equal to the difference beteen levels. This particular amount of energy can be observed as monochromatic light, that is light of a particular wavelength (color) that looks like a line on a spectrum. Transition between different levels give several lines on a spectrum.
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Can atomic spectra be explained on the basis of quantum mechanics?
Yes, atomic spectra can be explained and understood through quantum mechanics. Quantum mechanics provides a framework to describe the discrete energy levels of electrons in atoms, leading to the observation of specific wavelengths in atomic spectra. The theory helps explain phenomena such as line spectra and transitions between energy levels within an atom.
What particle is responsible for spectra?
Spectra are produced by interaction of electromagnetic radiation with matter, typically atoms or molecules. The particle responsible for spectra is the photon, which carries energy and interacts with electrons in the atoms or molecules to produce the spectral lines observed in both emission and absorption spectra.
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?
Niels Bohr's key hypothesis was that electrons orbit the nucleus in specific energy levels or orbits, and they can only transition between these levels by absorbing or emitting specific amounts of energy. This hypothesis explained the discrete pattern of atomic spectra by linking the spectral lines to the energy differences between electron orbits.
Sharing of electrons in the outer energy levels of two atoms?
The sharing of electrons in the outer energy levels of two atoms is called bonding.
What experiments led to bohrs model?
Experiments like the photoelectric effect and atomic emission spectra provided evidence that electrons exist in discrete energy levels. These findings challenged the classical model of the atom, leading to Niels Bohr proposing his model in 1913 to explain the quantization of electron energy levels in atoms.
The line spectra of atoms provides experimental evidence for?
The line spectra of atoms provide experimental evidence for the quantization of energy levels in atoms. This supports the idea that electrons can only exist in specific energy levels within an atom's electron shells. The specific wavelengths of light emitted or absorbed by atoms in their line spectra confirm the discrete nature of energy levels and the transitions between them.
How does quantum theory explain the emission spectra of atoms?
Quantum theory explains the emission spectra of atoms by proposing that electrons in atoms can only exist in specific energy levels. When an electron moves from a higher energy level to a lower one, it emits a photon of light with a specific energy corresponding to the difference in energy levels. This results in the unique emission spectra observed for each element.
How do Spectra from neutral atoms compared with spectra from ionized atoms of the same element?
Spectra from neutral atoms show a series of discrete lines corresponding to transitions between different energy levels within the atom. These lines are unique to each element and can be used to identify the element. When an atom is ionized, electrons are removed, leading to changes in the energy levels and resulting in a different set of spectral lines. The spectra from ionized atoms will have different line patterns and energy levels compared to those of neutral atoms of the same element.
What experimental evidence led to bohr to believe that electrons can posses only specific amounts of energy?
The observation of discrete emission spectra from elements provided the experimental evidence for Bohr's model. The only way to explain these spectra was through quantization of electron energy levels in atoms. This led Bohr to propose that electrons could only exist in specific orbits with quantized energy levels.
Can atomic spectra be explained on the basis of quantum mechanics?
Yes, atomic spectra can be explained and understood through quantum mechanics. Quantum mechanics provides a framework to describe the discrete energy levels of electrons in atoms, leading to the observation of specific wavelengths in atomic spectra. The theory helps explain phenomena such as line spectra and transitions between energy levels within an atom.
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.
How is atomic Spectra helpful to scientist?
Atomic spectra are helpful to scientists because they provide valuable information about the energy levels of atoms, which can be used to identify elements and study their properties. By analyzing the spectra produced when atoms absorb or emit light, scientists can determine the composition of substances, study chemical reactions, and investigate the structure of atoms. This information is crucial for various fields such as chemistry, physics, astronomy, and material science.
What particle is responsible for spectra?
Spectra are produced by interaction of electromagnetic radiation with matter, typically atoms or molecules. The particle responsible for spectra is the photon, which carries energy and interacts with electrons in the atoms or molecules to produce the spectral lines observed in both emission and absorption spectra.
Why are atomic spectrum discontinuous?
Atomic spectra are discontinuous because they result from the quantized energy levels of electrons within an atom. Electrons can only exist at specific energy levels, leading to distinct spectral lines corresponding to transitions between these levels. This quantization of energy in atoms gives rise to the phenomenon of discrete spectral lines.
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?
Niels Bohr's key hypothesis was that electrons orbit the nucleus in specific energy levels or orbits, and they can only transition between these levels by absorbing or emitting specific amounts of energy. This hypothesis explained the discrete pattern of atomic spectra by linking the spectral lines to the energy differences between electron orbits.
Who discovered that electrons move in specific levels or shells?
Neil Bohr discovered that each electron shell has specified energy levels and limited place for electrons.
What is found in the energy levels of atoms?
electrons
