Based on the Heisenberg uncertainty principle, the early developers of quantum theory determned that wave functions give only the probability of finding an electron at a given place around the nucleus. Thus, electrons do not travel around the nucleus in neat orbits, as Bohr had postulated. Instead, they exist in certain regions called orbtals. See pgs. 99-100 in Modern Chemistry Answer The Heisenberg uncertainty principle says that the position and momentum of a particle cannot be found simultaneously. In the case of electrons which have very high velocities (thus much momentum) they can only occupy spread-out regions if one knows their velocity. The spread-out region can be thought of as a cloud but is really a region of probability where the electron is likely to be found were one to determine its velocity. The fact that two electrons maximum can occupy a single orbital (be it an s, p, d or f orbital) at a time has much to do with the Pauli Exclusion Principle as well.
The heisenberg uncertainty principle is what you are thinking of. However, the relation you asked about does not exist. Most formalisms claim it as (uncertainty of position)(uncertainty of momentum) >= hbar/2. There is a somewhat more obscure and less useful relation (uncertainty of time)(uncertainty of energy) >= hbar/2. But in this relation the term of uncertainty of time is not so straightforward (but it does have an interesting meaning).
Since it is called "the Heisenberg Uncertainty Principle" it is neither a scientific law nor a theory. It is a principle.
Heisenberg's Uncertainty Principle is the principle that states that the momentum and the position of a quantum particle can not be simultaneously accurately known. This means that the more precisely you know the momentum, the less you know about the position and vice-versa.
Werner Heisenberg developed this principle, known as the Heisenberg Uncertainty Principle.
Heisenberg's uncertainty principle states that it is impossible to simultaneously know the exact position and momentum of a particle. This principle arises from the wave-particle duality in quantum mechanics, where the act of measuring one quantity disrupts the other. Mathematically, the principle is represented by the inequality Δx * Δp ≥ ħ/2, where Δx is the uncertainty in position, Δp is the uncertainty in momentum, and ħ is the reduced Planck constant.
noob valencia
motion... if they weren't they would violate Heisenburg's uncertainty principle.
Also referred to as the 'uncertainty' principle, it is a principle in quantum mechanics holding that increasing the accuracy of measurement of one observable quantity increases the uncertainty with which another conjugate quantity may be known.
The heisenberg uncertainty principle is what you are thinking of. However, the relation you asked about does not exist. Most formalisms claim it as (uncertainty of position)(uncertainty of momentum) >= hbar/2. There is a somewhat more obscure and less useful relation (uncertainty of time)(uncertainty of energy) >= hbar/2. But in this relation the term of uncertainty of time is not so straightforward (but it does have an interesting meaning).
The equation of uncertainty principle is ΔxΔp≥ℏ.
Uncertainty Principle - 2010 I was released on: USA: January 2010
Heisenberg's uncertainty principle affects the behaviour of orbitals.
Since it is called "the Heisenberg Uncertainty Principle" it is neither a scientific law nor a theory. It is a principle.
Germany
The cast of The Uncertainty Principle - 2011 includes: Olivia Chappell Dan Mersh
The Uncertainty Principle - The Spectacular Spider-Man - was created on 2008-05-10.
Einstein is. Check the uncertainty principle.