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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.
What experimental evidence supports that atoms are destructible?
The experimental evidence that atoms are destructible comes from nuclear reactions such as fission and fusion. These processes involve splitting or combining atomic nuclei, leading to the release of energy and the transformation of atoms into different elements. Additionally, particle accelerators have been used to smash atoms into smaller particles, demonstrating that atoms can indeed be broken apart.
Which scientist offered proof that atoms exist?
The existence of atoms was proposed by the ancient Greek philosopher Democritus in the 5th century BCE. However, John Dalton provided experimental evidence for the existence of atoms in the early 19th century through his atomic theory, which explained chemical reactions in terms of the combination of atoms.
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 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 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.
Who didn't have experimental evidence to support his theory of atoms?
The Greek philosopher Democritus first put forward the idea of atoms as an intellectual theory.
What experimental evidence did Thomson have atoms of all elements contain electrons?
The deflection of cathodic rays was the source of inspiration for Thomson.
What experimental evidence did Thomson have for the atoms of all elements contain electrons?
The deflection of cathodic rays was the source of inspiration for Thomson.
What experimental evidence supports that atoms are destructible?
The experimental evidence that atoms are destructible comes from nuclear reactions such as fission and fusion. These processes involve splitting or combining atomic nuclei, leading to the release of energy and the transformation of atoms into different elements. Additionally, particle accelerators have been used to smash atoms into smaller particles, demonstrating that atoms can indeed be broken apart.
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.
How can the existence of spectra help to prove that energy levels in atoms exist?
The existence of spectra — such as emission or absorption lines — indicates that atoms emit or absorb specific energies in quantized amounts. These spectral lines correspond to transitions between distinct energy levels in atoms. Therefore, the observation of spectra provides empirical evidence that energy levels in atoms do indeed exist.
Proposed that matter was made of tiny indivisible particles He called these units atoms He did not have evidence to support his theory?
The proposed individual indivisible particles were atoms, and this idea laid the foundation for modern atomic theory. Although he lacked experimental evidence at the time, subsequent scientific discoveries have validated the existence of atoms as building blocks of matter.
How did niels bohr make his discovery?
Niels Bohr made his discovery by proposing a new model of the atom, known as the Bohr model, which incorporated the concept of quantized energy levels. He based his model on experimental evidence, particularly the analysis of the emission spectra of hydrogen gas, and it successfully explained the stability of atoms and the quantization of energy levels within them.
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.
Which scientist offered proof that atoms exist?
The existence of atoms was proposed by the ancient Greek philosopher Democritus in the 5th century BCE. However, John Dalton provided experimental evidence for the existence of atoms in the early 19th century through his atomic theory, which explained chemical reactions in terms of the combination of atoms.
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.
