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Who came up with the idea that electrons are in different energy levels?
Wiki User
∙ 7y ago
The very first to propose this was Neils-Bohr.
Wiki User
∙ 7y ago
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Who came up with the concept of energy levels?
it was by a scientist called Bohr
What areas did Niels Bohr make contributions in?
He made a model of the atom, with electrons circling the nucleus.
Is kinetic energy easily lost?
Kinetic Energy - this is the energy which came from the different radiation . the best example is MAGNET there is a popular energy that can attract to other materials and different metalic objects From: JayRica
Who was neils bohr and what did he do?
Nils Bohr designed an atomic model but eventually someone came up with an even more accurate model. He achieved the Nobel prize for physics.
Is light emitted when an electron makes a transition to a lower energy level?
No, as energy is absorbed. When the reverse happens, the higher state to lower state, the electron is returning to its lower energy level ground state and energy is released in the form of a photon.
Where does energy came from?
energy came from many different way. like electrical
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.
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 is equal to the difference in the energy level of the Atom that it came from.
Who came up with the concept of energy levels?
it was by a scientist called Bohr
What areas did Niels Bohr make contributions in?
He made a model of the atom, with electrons circling the nucleus.
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 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
Is kinetic energy easily lost?
Kinetic Energy - this is the energy which came from the different radiation . the best example is MAGNET there is a popular energy that can attract to other materials and different metalic objects From: JayRica
Who was neils bohr and what did he do?
Nils Bohr designed an atomic model but eventually someone came up with an even more accurate model. He achieved the Nobel prize for physics.
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.
Are simple cations always larger or smaller than the neutral atoms from which they were formed?
They have very similar sizes. An ion is an atom that is missing one or more electrons. The contribution of individual electrons to the size of an atom is very slight. Metal atoms. - A
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 .
