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The correct answer in Laymen's terms: In quantum mechanics, the Heisenberg uncertainty principle states by precise inequalities that certain pairs of physical properties, like position and momentum, cannot simultaneously be known to an arbitrary precision. That is, the more precisely one property is measured, the less precisely the other can be measured. In other words, the more you know the position of a particle, the less you can know about its velocity, and the more you know about the velocity of a particle, the less you can know about its instantaneous position.
Although the following answer is related to the topic it is not directly answering the question.
This is because what the answerer is speaking of is the standard deviation of the expectation value for the position operator. Although that is part of the Uncertainty Principle story it is not a good explanation of what is being asked.
**In the quantum mechanical realm -- at the sub-atomic level -- this is not true. We can not determine a particle's location with absolute certainty. We can only state the probability of a particle in a particular location at a given time. We might say, for example, there is a 99% chance of a particle being in a particular place and a 1% chance it will be somewhere else. If the particle is not located in the 99% given location, it may be ANYWHERE else. It could be in your backyard, on mars, on the other side of the galaxy, or even on the other side of the universe, assuming is has "sides". The reason why reducing the space that is being dealt with is not just reduced to find the answer is because the velocity of the particle increases, and vice versa, rendering it impossible.
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The formula is given by this:
Δx*Δp>= ħ/2.
In other words, the change in x (position) multiplied by the change in p (momentum) is greater than or equal to ħ ((Planck's Constant) 6.58211899(16)×10^-16 eV·s) divided by two.
Or simply put, the momentum and the position of the particle (electron, proton, etc.) cannot be measure accurately and simultaneously.
Flavio Mitchell
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What is the significance of uncertainty principle in your daily life?
The Heisenberg uncertainty principle, which is very important at the subatomic level, has no affect on my daily life.
Heisenberg is famous for what principle?
the Heisenberg uncertainty principle
What is the relation between orbital concept and heisenberg's uncertainty principle?
Heisenberg's uncertainty principle affects the behaviour of orbitals.
Who develped a principle that says it is impossible to know both location and mass of an electron at the same time?
Werner Heisenberg developed this principle, known as the Heisenberg Uncertainty Principle.
Who invented the heisenberg's uncertainty principle?
Werner Heisenberg. Born in Munich, Germany in 1901 and died in 1976. Heisenberg examined features of qauntum mechanics that was absent in classical mechanics. Thus created the "Heisenberg Uncertainty Principle".
Proof of Heisenberg's uncertainty principle?
Electron diffraction.
Who came up with the uncertainty principle?
Werner Heisenberg
Who was best known for his uncertainty principle?
Werner Heisenberg published this principle in 1927.
States that is imposible to know both the velocity and the position of a particle at the same time?
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).
Why Heisenberg principle introduce?
The German scientist Werner Heisenberg developed his uncertainty principle, a major concept in quantum mechanics, in 1927.
Is the Uncertainty Principle a scientific law or theory?
Since it is called "the Heisenberg Uncertainty Principle" it is neither a scientific law nor a theory. It is a principle.
What are the two parts of the Heisenberg uncertainty principle?
Heisenberg uncertainty principle states that , the momentum and the position of a particle cannot be measured accurately and simultaneously. If you get the position absolutely correct then the momentum can not be exact and vice versa.
