Electrons Jumping: What Does it Mean?

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In summary, an electron can change its energy level by emitting or absorbing a photon. This is sometimes referred to as a "quantum leap."
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What exactly do the mean when an electron "jumps" from an energy level to another energy level in an atom. Do they mean tunneling?
 
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  • #2
nuclear420 said:
What exactly do the mean when an electron "jumps" from an energy level to another energy level in an atom.

They change their energy by emitting or absorbing a photon to make up the difference.

Do they mean tunneling?

Tunneling through what?
 
  • #3
Well, i was under the assumption that the electron can exist in certain wave distributions according to the Schrodinger equation. Since it can't smoothly transition (or can it?), because its not a solution to the Schrodinger equation, it has to change its wave distribution instantly. So would this be a form of tunneling?
 
  • #4
I believe this is where the term "quantum leap" originated. The electron cannot smoothly transition, and so it goes from one energy state to another without passing through the space in between. This is not actual "tunneling" since, as JTBell points out, tunneling must pass through some obstacle or barrier. Also included within the definition of tunneling is the fact that a particle must overcome an obstruction that it does not have sufficient energy to surmount, if it were a classical particle.

However, the two phenomena are similar, and that the electron seems to go from one orbital to another without passing through the intervening space.
 
  • #5
nuclear420 said:
Well, i was under the assumption that the electron can exist in certain wave distributions according to the Schrodinger equation. Since it can't smoothly transition (or can it?), because its not a solution to the Schrodinger equation, it has to change its wave distribution instantly. So would this be a form of tunneling?

No, there's no tunneling here.

First of all, I'm not sure why you originally posted this in the classical physics forum. It has been moved into the Quantum Physics forum.

Secondly, in tunneling, the particle DOES go through the classical forbidden region. In an atomic transition, the atom (and electron in question) does not really make a "motion" across from one state to another. It is, as far as we know, an instant "jump".

Zz.
 

1. What is the definition of an "electron jump"?

An electron jump is a phenomenon in which an electron moves from one energy level to another within an atom or molecule. This movement can occur spontaneously or be induced by external factors such as heat or light.

2. How does an electron jump affect the physical properties of a substance?

An electron jump can lead to changes in the chemical and physical properties of a substance. This is because the movement of electrons can alter the way atoms and molecules interact with each other, ultimately affecting the substance's overall behavior and characteristics.

3. What causes an electron to jump?

Electrons can jump due to various factors, including changes in temperature, changes in the electric or magnetic field surrounding the atom or molecule, and the absorption or emission of photons (particles of light).

4. Can we control or manipulate electron jumps?

Yes, scientists have developed methods to control and manipulate electron jumps. This has led to advancements in technologies such as transistors, lasers, and solar cells.

5. Are electron jumps related to the concept of quantum mechanics?

Yes, electron jumps are a fundamental aspect of quantum mechanics, which is the branch of physics that studies the behavior of particles at a very small scale. The concept of electrons existing at specific energy levels and transitioning between them is a key principle of quantum mechanics.

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