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Why can't we evercome the uncertainty predicted by hesisenherg principle by building more precise devices to reduce the error in measurment below the `h//4pi` limit ?

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Heisenberg uncertainty principle is not due to any limitation of measuring instrument but is due to dual chracter of matter .Hence it is not possible to raduce the error in measurment below `h//4 pi` by buliding more photon devises
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The mass m of an electron is 9.1 xx 10^(31)kg and the velocity v of an electron in the first Bohr orbit of a hydrogen atom is 2.2 xx 10^(6)ms^(-1) . Assuming that the velocity is known within 10% (Deltav = 0.22 xx 10^(6)ms^(-1)) , calculate the uncertainty in the electron's position in a hydrogen atom. Strategy: According to Heisenberg's principle, the uncertainty in the postion (Deltax) of any moving particle multiplied by the uncertainity of momentum (Deltap_(x)) can never be less than h//4pi . In the given case, Delta v is known and we need to find Deltax .

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse also true. This is summed up in what we now call the Heisenberg uncertainty principle. The equation si deltax.delta (mv)ge(h)/(4pi) The uncertainty in the position or in the momentum of a marcroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electon is small enough for the uncertainty to be relatively large and significant. If the uncertainties in position and momentum are equal, the uncertainty in the velocity is :

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse also true. This is summed up in what we now call the Heisenberg uncertainty principle. The equation si deltax.delta (mv)ge(h)/(4pi) The uncertainty in the position or in the momentum of a marcroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electon is small enough for the uncertainty to be relatively large and significant. If the uncertainty in velocity and position is same, then the uncertainty in momentum will be :

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also true. this is summed up in what we now call the Heisenberg uncertainty principal. The equation is Deltax.Delta(mv) ge (h)/(4pi) The uncertainty is the position or in the momentum of a macroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electron is small enough for the uncertainty to be relatively large and significant. If the uncertainties in position and momentum are equal, the uncertainty in the velocity is:

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also true. this is summed up in what we now call the Heisenberg uncertainty principal. The equation is Deltax.Delta(mv) ge (h)/(4pi) The uncertainty is the position or in the momentum of a macroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electron is small enough for the uncertainty to be relatively large and significant. If the uncertainty in velocity and position is same, then the uncertainty in momentum will be

Werner Heisenberg considered the limits of how precisely we can measure the properties of an electron or other microscopic particle. He determined that there is a fundamental limit to how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse also true. This is summed up in what we now call the Heisenberg uncertainty principle. The equation si deltax.delta (mv)ge(h)/(4pi) The uncertainty in the position or in the momentum of a marcroscopic object like a baseball is too small to observe. However, the mass of microscopic object such as an electon is small enough for the uncertainty to be relatively large and significant. What would be the minimum uncetaintty in de-Broglie wavelength of a moving electron accelerated by potential difference of 6 volt and whose uncetainty in position is (7)/(22) nm?

We can pin point an aeroplane moving in the sky, whatever may be its speed i.e., we can locate both its exact position as wellas direction . However, it is not possible to doso in case of a moving microscopic particle such as electron. In fact, we cannot see any such particle without disturbing it. This has been stated by Heisenberg in the form of uncertainty principle. The mathematical form of this principle is : Deltax.DeltaP ge (h)/(4pi) (constant). Since the product of Deltax and Deltap(m Delta upsilon) is constant , if one is very small, the other is bound to be large. The principle as such has no significance in daily life since it applies to those particles which we can not see. If uncertainty in position and momentum are equal , then the uncertainty in velocity is :

CENGAGE CHEMISTRY-ATOMIC STRUCTURE-Concept Applicationexercise(4.2)
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  2. Using Bohr's model , calculate the wavelength of the radiation emitt...

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  3. What is the maximum number of emission lines when the excited electro...

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  4. Calculate the radius of bohr's third orbit in hydrogen atom.

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  5. The energy associatied with the first orbit in the hydrogen atom is -...

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  6. What transition in the hydrogen spectrum would have the same wavelen...

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  7. Calcultte the enrgy required for the process , He^+ (g) rarr He^(2+...

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  8. Explain why the uncertainty principle has significated when applied to...

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  9. What is the minimum product of the uncertainty in position and the ...

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  10. Why can't we evercome the uncertainty predicted by hesisenherg prin...

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  11. A single electron orbits around a stationary nucleus of charge + Ze wh...

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  12. Find the energy released (in erg) when 2.0 g atom of hydrogen undergoe...

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  13. Stationary He^(o+) ion emits a photon corresponding to the first line ...

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  14. The ratio of energy of photon of lambda = 2000 Å to that of lambda = 4...

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  15. Bohr's model can explain

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  16. The wavelength of the first Balmer line Li^(2+) ion is 136800 cm^(-1)...

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  17. If the uncertainty in the position of an electron is zero the nucerta...

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  18. If the following mater travel with equal velocity the longest wavele...

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  19. Which of the following postutales does not belong to Bohr's model o...

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  20. The Lyman series of hydrogen spectrom can be respectively by the eq...

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