Heisenberg Uncertainty Principle electron simultaneously

The Bohr model is a determinant model of an atom. It implies that the position of the electron is exactly known at any time in the future, once that position is known at the present. The distance of the electron from the nucleus also is exactly known, as is its energy. And finally, the velocity of the electron in its orbit is exactly known. All of these exactly known quantities—position, distance from nucleus, energy, and velocity—can t, according to the Heisenberg uncertainty principle, be known with great precision simultaneously. 

Werner Heisenberg Heisenberg uncertainty principle It is not possible to simultaneously know information about the location and momentum of an electron. 

A photon that strikes an electron at rest alters the position and velocity of the electron. This collision illustrates the Heisenberg uncertainty principle It is impossible to simultaneously know both the position and velocity of a particle. Note that after the collision, the photon s wavelength is longer. How has the photon s energy changed ... 

Heisenberg uncertainty principle It states that it is not possible to determine accurately both the momentum and position of an electron simultaneously. 

Footnote The Wave Nature of the Electron. So far the electron has been considered as a particle, with clearly quantised energy levels, that can be precisely measured, as in the emission lines of the spectrum of hydrogen. Because the electron is so small and light, the accuracy with which it can be measured is very uncertain. This is associated with the Heisenberg Uncertainty Principle, which states that it is impossible to determine both the position and momentum of an electron simultaneously , i.e. Ax Ap = hl2it, where Ax is the uncertainty in measuring the position of the electron and Ap is the uncertainty in measuring the momentum (p = mass X velocity) of the electron. The two uncertainties bear an inverse relationship to each other. Consequently, if the position of the... 

We have seen that electrons are distributed into different atomic orbitals (Table 1.2). An orbital is a three-dimensional region around the nucleus where there is a high probability of finding an electron. But what does an orbital look like Mathematical calculations indicate that the 5 atomic orbital is a sphere with the nucleus at its center, and experimental evidence supports this theory. The Heisenberg uncertainty principle states that both the precise location and the momentum of an atomic particle cannot be simultaneously determined. This means that we can never say precisely where an electron is—we can only describe its probable location. Thus, when we say that an electron occupies a s atomic orbital, we mean that there is a greater than 90% probability that the electron is in the space defined by the sphere. 

The exact position of the electron is never known, which is consistent with the Heisenberg uncertainty principle it is impossible to know accurately both the position and the momentum of a particle simultaneously... 

Bohr s model was quite popular at the time because an electron circling the nucleus is conceptually similar to the earth circling the sun. The idea that orbiting electrons did not radiate was less easy to accept, Bohr simply insisted they did not and that was that Most importantly, the model explained a number of physical phenomena. Bohr s assumption that electrons are particles with well-defined orbits was not consistent with the concept of simultaneous interdeterminacy of position and momentum as propounded in the Heisenberg uncertainty principle. 

Heisenberg uncertainty principle The impossibility of making simultaneous measurements of both the position and the momentum of a subatomic particle (e.g. an electron) with unlimited accuracy. The uncertainty arises because, in order to detect the particle, radiation has to be bounced off it, and this process itself disrupts the particle s position. Heisenberg s uncertainty principle is not a consequence of experimental error . It represents a fundamental limit to objective scientific observation, and arises from the wave-particle duality of particles and radiation. In one direction, the uncertainty in position Ax and momentum Ap are related by AxAp h/4K, where h is the Planck constant. It is named for the German physicist... 

CONTEXT If we have two operators whose eigenvalues are experimentally measured quantities, such as energy and angular momentum, then we can determine both eigenvalues simultaneously only if the two operators commute. If the operators do not commute, then some form of the Heisenberg uncertainty principle (Eq. 1.19) applies no quantum state can be prepared in which both quantities can be known exactly at the same time. Our work on the atom is constrained by sets of non-commuting operators that determine which parameters we can measure simultaneously for any given state of the electron. 

The Heisenberg uncertainty principle states that it is impossible to determine simultaneously the position and velocity of an electron or any other particle. 

According to the Heisenberg uncertainty principle, the product of the uncertainty of the location and the uncertainty of the momentum of a very small particle must have a certain minimum value. It is thus impossible to know simultaneously both the location and momentum of an electron. 

Heisenberg uncertainty principle (Section 1.11) A fundamental principle that states that both the position and momentum of an electron (or of any object) cannot be exactly measured simultaneously. 

Uncertainty Principle n (1929) A principle in quantum mechanics which states it is impossible to discern simultaneously and with high accuracy both the position and the momentum of a particle (as an electron). Also known as Heisenberg Uncertainty Principle (Whitten KW, Davis RE, Davis E, Peck LM, Stanley GG (2003) General chemistry. Brookes/Cole, New York). 

Louis de Broglie postulated wave-particle duality in which particles of matter such as protons and electrons would at times display wave-like properties (equation 8.10). Because of an inherent uncertainty of the position and momentum of a wave-like particle, Heisenberg postulated that we cannot simultaneously know a subatomic particle s precise momentum and its position, a proposition referred to as the Heisenberg uncertainty principle (expression 8.11). 

UNCERTAINTY PRINCIPLE. Also sometimes referred to as the indelerminancy principle, this was first stated by Heisenberg, Werner P, in connection with the position and momentum of an electron. In essence, the postulate states that it is impossible to determine simultaneously both the exact position and the exact momentum of an electron and thus these... 

In Chapter 1 we learned that electrons are outside the atomic nucleus in probability areas that resemble clouds. We do not know exactly where these electrons are because they are in constant motion. In 1927 Werner Heisenberg (1901-1976), a German physicist and one of the founders of quantum mechanics, told us that it is impossible to know simultaneously the speed and position of an electron. He called this the uncertainty principle. Even though we cannot determine the exact position of an electron or how the electron moves in an atom, we can place an electron in an area outside the atomic nucleus where it is highly likely to be found, called a probability area. 

As far as Heisenberg s uncertainty principle is concerned, why is it impossible to determine the exact position and momentum of an electron simultaneously ... 

The extent to which statistical concepts enter the picture as we go from the micro- to the macroworld is not at all at our disposal. For example, quantum mechanics as we know it today teaches us that it is impossible in principle to obtain complete information about a microscopic entity (i.e., the precise and simultaneous knowledge of an electron s location and momentum, say) at any instant in time. On account of Heisenberg s Uncertainty Principle, conjugate quantities like, for instance, position and momentum can only be known with a certain maximum precision. Quantum mechanics therefore already deals with averages only (i.e., expectation values) when it comes to actual measurements. 

In the classical view of the world, a moving particle has a definite location at any instant, whereas a wave is spread out in space. If an electron has the properties of both a particle and a wave, what can we determine about its position in the atom In 1927, the German physicist Werner Heisenberg postulated the uncertainty principle, which states that it is impossible to know the exact position and momentum (mass times speed) of a particle simultaneously. For a particle with constant mass m, the principle is expressed mathematically as... 

One of the most important consequences of the dual nature of electrons is Heisenberg s uncertainty principle, which states that it is impossible to know simultaneously both the momentum and position of a particle with certainty. 

We recognize that matter also has wavelike properties. As a result, it is impossible to determine simultaneously the exact position and the exact motion of an electron in an atom (Heisenberg s uncertainty principle). 

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