The physical basis of the Heisenburg uncertainty principle is that?
I don't agree with any of these answers: 1. We can never determine the physical properties precisely. The more we know about the position, the less we know about the momentum or velocity, and vice versa. 2. Again, these two values can NEVER be both determined due to the eingenstates never being simultaneous or relatable at the same time. 3. This is somewhat true, but this is NOT what the uncertainty principle states. It has nothing to do with equipment. Even with the most perfect, non-distrubing, high-tech equipment and measure, we will still have errors in the data due to the particle-wave duality. 4. We can study the behaviors of electrons with dependable forms of certainty. For example, we know how electrons generally behave in orbitals, the probability of us finding them essentially defines the orbital shape, we know how they help atoms bond together and how the interact in certain metals to create charge - this has nothing to do with how numerous the electrons are. These properties can be isolated (take for example, a particle accelerated), and studied for spin states. Electrons are leptons, still a quantum state that can be observed with a degree of accuracy. 5. This is again, completely not the point of the principal. We could have equipment (again, the particle accelerator), that measures everything perfectly, but still at the quantum level, everything tends to become more wave-like meaning even perfect conditions and machinery cannot measure it to such accuracy that we could determine the position and velocity. --- I am sorry, but I do not think any of these corruptly represent the principle and your professor/teacher may have a slight misunderstanding. I would lean towards "3" as the best answer, but it is still wrong. Anything that has to deal with current experimenting methods or equipment disrupting measurements is completely wrong in terms of the principle represents. Anything stating that we can get the exact position of a particle is incorrect, and there is not even mass to a photon that could give an eigenstate. All wrong.
What is heisenberg`s uncertainity principle?
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).
Please describe the Quantum Theory?
in accordance to Bohr's concept orbit is a around path wherein electron revolces, orbital is the three dimentional area around the nucleus the place there is maximum hazard of looking the electron.
Niels Bohr’s principle of complementarity is a general principle that he viewed as applying to many areas of thought including psychology and biology. Heisenberg’s uncertainty principle, on the other hand, could be viewed as a specific quantitative instantiation of the principle of complementarity in the subatomic world.Macroscopic objects that we normally interact with in everyday life do not exhibit observable effects of wave-particle duality or the uncertainty principle (which is not to say that it isn't at work on the atomic scale). This is why quantum theory was not discovered until experimental physics was able to precisely measure subtle atomic phenomena outside of our range of normal experience.However, some people have suggested that there are analogies to the uncertainty principle in our everyday experience. For example, David Bohm in his classic text Quantum Theory writes,If a person tries to observe what he is thinking about at the very moment that he is reflecting on a particular subject, it is generally agreed that he introduces unpredictable and uncontrollable changes in the way his thoughts proceed thereafter. Why this happens is not definitely known at present, but some plausible explanations will be suggested later. If we compare (1) the instantaneous state of a thought with the position of a particle and (2) the general direction of change of that thought with the particle’s momentum, we have a strong analogy.Saying that our experience with observing thought is analogous to the uncertainty principle, however, is not the same as saying the uncertainty principle or quantum theory can be properly applied to thoughts.However, Niels Bohr viewed his principle of complementarity as applicable to much more than just physics. He wrote quite a bit about this: Complementarity Beyond Physics (1928-1962), Volume 10The Heisenberg uncertainty principle could be viewed as the specific quantitative way that complementarity manifests for conjugate pairs of physical properties. It doesn’t apply beyond this physical domain, but one could argue, with Bohr, that the principle of complementarity does.
orbit;Orbit is a well defined circular path around the nucleus in which an electron revolvesit represents the planar motion of an electronorbits gives a definite path of an electron and this concept is not in accordance with the uncertainty principleall orbits are circularorbits do not have directional characteristicsan orbit can accommodate electrons equal to 2n^2 where n represents the principle quantum number.ORBITALit represents the region in space around the nucleus in which the probability of finding the electron is maximum.It represents the three dimensional motion of an electron around the nucleusorbital does not specify definite path and according to this concept,electron may be any where in this region .this concept is in uncertainty principleorbitals have different shapes .For example,s-orbital is spherical, p-orbital is dumb bell shapedexcept s=orbitals , all other orbital have directional characteristisan orbital cannot accommodate more than two electrons.Orbital is the probability picture of of an electron.This concept put forward as:The wave character of an electron and uncertainty in its position gave a serious blow to Bohr’s model .According to Bohr,the electron revolve in well -defined circular orbits.but the idea of uncertainty in position and velocity over ruled the Bohr’s picture of fixed circular orbits Scientist start looking for a theory which may explain1.stability of atom2.dual character of matter3.uncertainty principleThis resulted in a new approach known as wave mechanics .In 1927,Schrodinger described the behaviour of electron by a mathematical equation known as Schrodinger Wave equation.The solution of wave equation led to the concept of most probable regions in place of well defined circular paths proposed by Bohr.According to this approach , we cannot say simply that the electron exists at a particular point ,but talk about certain regions in space around the nucleus where the probability(chances )of finding the electron is maximum(90–95%). These most probable regions in space are called orbitals
Wave functions and atomic orbital?
Hi! You have the basics, just a bit confused. Lets try to clear some up then. First, a wave function is a SOLUTION OF an equation. That equation is the Schrodinger equation when we speak of quantum mechanics. The location of a particle is given by the wave function squared. This is the probability of it being found in space. Unfortunately, their are only a handful of exactly solvable systems; that is, by analytical methods i.e. pencil and paper (dont forget coffee!). For atomic systems, we solve the hydrogen atom and build off of that with better approximations for the rest of the atoms since hydrogen is the base atom from which to construct all others. Please understand that I am making tremendous simplifications and omissions in the interest of brevity. So, with the electron, we look at the orbitals given by the complete solution of the hydrogen atom; that is, there are radial and angular components not to mention intrinsic "spin." So you see, the location, or orbital, is part of the wave function since it gives a complete description of the system. Technically speaking we are usually only concerned with what are called eigenvalues, which are the energy levels. Things we can measure are the key! The conceptual framework or theoretical foundation is only a model! We dont actually measure wave functions. This is the area of "math meets science" that leaves room for all the metaphysical and philosophical mumbo jumbo out there. Not that that is a bad thing, just not totally necessary either if you just want to build a laser and make it work. Know what I mean? Now, for Heisenberg all that you really need to make clear is that you cannot have perfect precision in one value or another i.e. position and momentum. There are different "types" of uncertainty relations you can have e.g. energy and time. Another way of thinking about it is this: in order to tune a guitar perfectly to some note (or frequency) you would need an infinite amount of time. So with regards to getting the exact position of an electron, you would have infinite uncertainty with the momentum. More or less you have the basics there, so good analogy with the car except remember that you are always concerned with the car and not the road. I hope that helps.
Orbit vs OrbitalIn atomic theory, these two similar-sounding terms “orbit” and “orbital” often confuse people. You must have seen in pictures that an atom is a simple, solar-system-like structure in which electrons are like our planets revolving around a nucleus which may be considered as our sun. Actually, the truth is much more complex. Orbits and orbital are different paths of atoms.Orbit In our solar system, the paths on which the planets revolve are called orbits. These are strange elliptical paths which are fixed for every single planet, and these planets move on this path with their angular velocities and central acceleration. The same is the case with atoms. Orbits are the fixed paths around which electrons revolve around the nucleus of the atom following the same principle as that of the planets.An orbit is a planar or two-dimensional circular pathway. The maximum number of electrons in a particular orbit is 2n2 . An orbit follows Newton’s laws of motion. In atomic theory, an orbit is created because of the pull of the negatively charged electron to the positively charged nucleus while having the same angular velocity. But as Heisenberg’s Uncertainty Principle proves it as uncertain, we cannot easily determine the exact orbit of an electron.Orbital If you think that one can tell the exact position of electrons at a certain time, you are actually wrong. According to Heisenberg’s Uncertainty Principle:“One can never know with perfect accuracy both of those two important factors which determine the movement of one of the smallest particles (electrons)—its position and its velocity. It is impossible to determine accurately both the position and the direction and speed of a particle or electron at the same instant.”So an orbital is an uncertain area inside an atom within which the probability to find an electron(s) is highest. It represents the three-dimensional space around the nucleus. Orbitals occur in various shapes and capacities in accordance with the element and its atomic number. They are categorized as s, p, d and f type orbital. The maximum capacities of these orbital are: s orbital – 2 electrons p orbital – 6 electrons d orbital – 10 electrons f orbital – 16 electrons