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Who came up with the concept of energy levels?
The concept of energy levels in atoms was developed by Niels Bohr in 1913 as part of his atomic model. Bohr proposed that electrons orbit the nucleus in specific energy levels, and that they need a specific amount of energy to jump between these levels.
What was Niels Bohr contribution to the atom?
The Bohr model of the atom, the theory that electrons travel in discrete orbits around the atom's nucleus.The shell model of the atom, where the chemical properties of an element are determined by the electrons in the outermost orbit.The liquid drop model of the atomic nucleus.Identified the isotope of uranium that was responsible for slow-neutron fissionThis answers came from wikipedia
What areas did Niels Bohr make contributions in?
He made a model of the atom, with electrons circling the nucleus.
Who was neils bohr and what did he do?
Niels Bohr was a Danish physicist who made significant contributions to our understanding of atomic structure and quantum theory. He is best known for proposing the Bohr model of the atom, which introduced the idea of electrons orbiting the nucleus in specific energy levels. This model laid the foundation for modern quantum mechanics and earned him the Nobel Prize in Physics in 1922.
What element did neil bohr invent?
He didn't. He came up with the Bohr equation explaining the probability of finding a single electron around a hydrogen atom, and Bohrium is named after him, but he himself did not discover an element.
Who came up with the concept of energy levels?
The concept of energy levels in atoms was developed by Niels Bohr in 1913 as part of his atomic model. Bohr proposed that electrons orbit the nucleus in specific energy levels, and that they need a specific amount of energy to jump between these levels.
Where does energy came from?
energy came from many different way. like electrical
Why energy levels named k l m n o p?
It is all because of a man named Charles Barkla. He was measuring the energy levels of X-rays, and noticed that they came in two main categories, one of which had a higher energy level than the other. He first called them A and B, then realized that there might be levels higher than the one he had called "A". Wanting to leave some room, he decided that K would be a good starting point, and if he later discovered an even higher energy levels he could call them J, I, H and so on down. It turns out there aren't... the K-series was the highest possible energy level for a given atom. But the name had stuck by that point.
How does the energy of a photon compare in difference in energy levels of the atom from which it is emitted?
The energy of a photon emitted from an atom is determined by the energy difference between the initial and final energy levels of the atom. The energy of the photon is directly proportional to this difference in energy levels. If the energy levels are farther apart, the emitted photon will have higher energy, whereas if the levels are closer together, the photon will have lower energy.
Why does atomic radii increase down a periodic table?
From what I understand, the guy who came up with the periodic table just used trial and error to find a way to chart the elements, the way he arranged them is as close as it gets to fitting a pattern.
Why is the emission spectrum different for every element?
When light hits an atom the atom absorbs certain wavelengths of light and reflects others. Upon gaining energy from light the electrons in the atom are elevated to a higher energy state. Upon returning from this state to the ground state the electrons lose energy in the form of a photon (which may be within the visible spectrum). As different elements have different gaps between each energy level, different elements will have different wavelengths of photon given out and thus different emission spectrums.
Explain how the wavelengths of light emitted by an atom provide information about electron energy levels?
We know what a wavelength is, and when we apply the term to the phenomenon of electron energy levels, something amazing happens. Let's review by looking at atomic structure for a moment and take off from there. We know that electrons form up in orbitals and shells around an atomic nucleus. These orbitals are defined as energy levels, and an electron is said to be in a given energy level. When electrons get just the right amount of energy, they can "jump" to a higher energy level. There are places that they cannot go, but there are other places that are "just right" for an electron from that particular starting energy level. A specific quantity of energy (a quantum, perhaps) is the key to electrons changing energy levels. If an electron is "bumped" to a higher energy level because it has "accepted" a packet of energy that is just right, it moves up to that energy level. But it cannot stay there, so it "falls back" to where it came from. In returning to its original energy level, it must "give up" the exact amount of energy that it took to move up. This specific amount of energy translates into radiated electromagnetic energy of a given wavelength or frequency. And each wavelength corresponds to a given amount of energy. Let's apply this and see what happens. Should we consider a bunch of atoms of a given kind, they will have a specific electron structure. The electrons of these atoms "live" in given energy levels. If we excite these atoms with the right amounts or quanta of energy, the electrons that will only respond to that amount of energy will move to a higher energy level. Then the electrons will return to their original levels, giving up that wavelength of energy when they drop down. If the wavelength of electromagnetic energy is in the optical band, visible light will appear. The atoms will "glow" at a specific color associated with the wavelength of the energy that is released when those electrons return to their original energy levels. If those atoms in our experiment are a gas and we apply sufficient voltage, the gas atoms will ionize and the gas will glow. Electrons are accepting energy quanta, are moving to higher energy levels, and are then returning to their original energy levels by releasing visible light of a given color. Electron energy levels are directly related to wavelengths of electromagnetic radiation.
How did Bohr improve Planck's theoory?
Bohr improved Planck's theory by incorporating the concept of quantized energy levels for electrons in atoms. He proposed that electrons could only exist in certain distinct energy levels, which helped explain the stability of atoms and the emission/absorption of light in atomic spectra. This led to the development of the Bohr model of the atom.
How would the variety of organic compounds be different if carbon had seven electrons in its outmost energy level instead of four?
i dont now i just ask you if you now this is came to my test and i want to make sure
What was Niels Bohr contribution to the atom?
The Bohr model of the atom, the theory that electrons travel in discrete orbits around the atom's nucleus.The shell model of the atom, where the chemical properties of an element are determined by the electrons in the outermost orbit.The liquid drop model of the atomic nucleus.Identified the isotope of uranium that was responsible for slow-neutron fissionThis answers came from wikipedia
Is the mass of an ion different from the mass of the atom it came from?
A small difference of mass exist because the gain or loss of electrons.
What is runescapes new skill?
the new skill that came out is called dungonerring its where you can go through different levels of dungeons and fight mosters of different levels but make sure you unequip everything before you enter otherwise it will not let you in .
