What is heisenberg`s uncertainity principle?

Answer 1

It states that estimation of both position and velocity is impossible...

Answer 2

Heisenberg's Uncertainity Principle says that it is impossible to predict the exact position and energy of any particle which is in the state of random motion.

Answer 3

Heisenberg uncertainty principle states that it is impossible to determine both the position and momentum of a microscopic moving particle with absolute accuracy.

Answer 4

In quantum physics, the Heisenberg uncertainty principle or the Heisenberg indeterminacy principle — the latter name given to it by Niels Bohr — states that one cannot measure values (with arbitrary precision) of certain conjugate quantities, which are pairs of observables of a single elementary particle. The most familiar of these pairs is the position and momentum.

A fundamental consequence of the Heisenberg Uncertainty Principle is that no physical phenomena can be (to arbitrary accuracy) described as a "classic point particle" or as a wave but rather the microphysical situation is best described in terms of wave-particle duality. The uncertainty principle, as initially considered by Heisenberg, is concerned with cases in which neither the wave nor the point particle descriptions are fully and exclusively appropriate, such as a particle in a box with a particular energy value. Such systems are characterized neither by one unique "position" nor by one unique value of momentum (including its direction).

Answer 5

In quantum mechanics there are various pairs of quantities that cannot be determined individually to an infinite degree of precision. Two such pairs are position/momentum and energy/time. The mathematics only allows a determination of the product of these quantities to be determined precisely, not the individual components. Two effects of this are:

1. The position of a particle cannot be determined precisely when its momentum (velocity * mass) is high (or vice versa). This means that quantum particles have to be thought of as "smeared out", like a wave, rather than occupying a specific point in space.

2. Energy is not conserved over very short intervals of time. Thus, "virtual particles" can appear out of nothing as long as they disappear again within a particular period of time (the higher the mass of the virtual particle, the less time it can exist).

Physicists can measure both of these effects.

Answer 6

It s a postulate by Heisenberg which states that it is impossible to simultaneously determine the velocity and mass of an electron within the specified orbital regions of electrons in an atom.

Answer 7

The position and momentum of a particle cannot be simultaneously measured with arbitrarily high precision. There is a minimum for the product of the uncertainties of these two measurements. There is likewise a minimum for the product of the uncertainties of the energy and time.

Answer 8

You dont know.

For a more wordy version of "You don't know" look below.


Uncertainty principle

Main article: Uncertainty principle

In 1927, Heisenberg made a new discovery on the basis of his quantum theory that had further practical consequences of this new way of looking at matter and energy on the atomic scale. In Heisenberg's matrix mechanics formula, Heisenberg had encountered an error or difference of h/2π between position and momentum. This represented a deviation of one radian of a cycle when the particle-like aspects of the wave were examined. Heisenberg analyzed this difference of one radian of a cycle and divided the difference or deviation of one radian equally between the measurement of position and momentum. This had the consequence of being able to describe the electron as a point particle in the center of one cycle of a wave so that its position would have a standard deviation of plus or minus one-half of one radian of the cycle (1/2 of h-bar). A standard deviation can be either plus or minus the measurement i.e. it can add to the measurement or subtract from it. In three-dimensions a standard deviation is a displacement in any direction. What this means is that when a moving particle is viewed as a wave it is less certain where the particle is. In fact, the more certain the position of a particle is known, the less certain the momentum is known. This conclusion came to be called "Heisenberg's Indeterminacy Principle," or Heisenberg's Uncertainty Principle. To understand the real idea behind the uncertainty principle imagine a wave with its undulations, its crests and troughs, moving along. A wave is also a moving stream of particles, so you have to superimpose a stream of particles moving in a straight line along the middle of the wave. An oscillating ball of charge creates a wave larger than its size depending upon the length of its oscillation. Therefore, the energy of a moving particle is as large as the cycle of the wave, but the particle itself has a location. Because the particle and the wave are the same thing, then the particle is really located somewhere in the width of the wave. Its position could be anywhere from the crest to the trough. The math for the uncertainty principle says that the measurement of uncertainty as to the position of a moving particle is one-half the width from the crest to the trough or one-half of one radian of a cycle in a wave.

For moving particles in quantum mechanics, there is simply a certain degree of exactness and precision that is missing. You can be precise when you take a measurement of position and you can be precise when you take a measurement of momentum, but there is an inverse imprecision when you try to measure both at the same time as in the case of a moving particle like the electron. In the most extreme case, absolute precision of one variable would entail absolute imprecision regarding the other.
Heisenberg voice recording in an early lecture on the uncertainty principle pointing to a Bohr model of the atom: "You can say, well, this orbit is really not a complete orbit. Actually at every moment the electron has only an inactual position and an inactual velocity and between these two inaccuracies there is an inverse correlation."

The consequences of the uncertainty principle were that the electron could no longer be considered as in an exact location in its orbital. Rather the electron had to be described by every point where the electron could possibly inhabit. By creating points of probable location for the electron in its known orbital, this created a cloud of points in a spherical shape for the orbital of a hydrogen atom which points gradually faded out nearer to the nucleus and farther from the nucleus. This is called a probability distribution. Therefore, the Bohr atom number n for each orbital became known as an n-sphere in the three dimensional atom and was pictured as a probability cloud where the electron surrounded the atom all at once.

This led to the further description by Heisenberg that if you were not making measurements of the electron that it could not be described in one particular location but was everywhere in the electron cloud at once. In other words, quantum mechanics cannot give exact results, but only the probabilities for the occurrence of a variety of possible results. Heisenberg went further and said that the path of a moving particle only comes into existence once we observe it. However strange and counter-intuitive this assertion may seem, quantum mechanics does still tell us the location of the electron's orbital, its probability cloud. Heisenberg was speaking of the particle itself, not its orbital which is in a known probability distribution.

It is important to note that although Heisenberg used infinite sets of positions for the electron in his matrices, this does not mean that the electron could be anywhere in the universe. Rather there are several laws that show the electron must be in one localized probability distribution. An electron is described by its energy in Bohr's atom which was carried over to matrix mechanics. Therefore, an electron in a certain n-sphere had to be within a certain range from the nucleus depending upon its energy. This restricts its location. Also, the number of places an electron can be is also called "the number of cells in its phase space". The uncertainty principle set a lower limit to how finely one can chop up classical phase space. Therefore, the number of places that an electron can be in its orbital becomes finite due to the Uncertainty Principle. Therefore, an electron's location in an atom is defined to be in its orbital and its orbital although being a probability distribution does not extend out into the entire universe, but stops at the nucleus and before the next n-sphere orbital begins and the points of the distribution are finite due to the Uncertainty Principle creating a lower limit.

Classical physics had shown since Newton that if you know the position of stars and planets and details about their motions that you can predict where they will be in the future. For subatomic particles, Heisenberg denied this notion showing that due to the uncertainty principle one cannot know the precise position and momentum of a particle at a given instant, so its future motion cannot be determined, but only a range of possibilities for the future motion of the particle can be described.

These notions arising from the uncertainty principle only arise at the subatomic level and were a consequence of wave-particle duality. As counter-intuitive as they may seem, quantum mechanical theory with its uncertainty principle has been responsible for major improvements in the world's technology from computer components to fluorescent lights to brain scanning techniques.

Answer 9

"the uncertainty relation between position and momentum of a particle in space:

(delta x)(delta p) >= h/4pi", where
x = position
p = momentum,
h = Plank's constant

Answer 10

definite, she will do this. you're in college to study, no longer make out with your lady friend. even as the hand-holding prohibition seems a touch harsh, it remains considered a public demonstrate of love and that is almost continually antagonistic to the regulations in college.