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The uncertainty in position and momentu...

The uncertainty in position and momentum has a value ………..

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To solve the question regarding the uncertainty in position and momentum, we will follow these steps: ### Step-by-Step Solution: 1. **Understand the Concept**: The question refers to the Heisenberg Uncertainty Principle, which is a fundamental concept in quantum mechanics. It states that certain pairs of physical properties, like position and momentum, cannot be simultaneously measured with arbitrary precision. 2. **Identify the Mathematical Representation**: The Heisenberg Uncertainty Principle is mathematically represented as: \[ ...
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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 uncertainties in position and momentum are equal, the uncertainty in the velocity is :

It is not possible to determine precisely both the position and momentum (or velocity) of a small moving particle such as electron, proton etc. This is known as Heisenberg uncertainty principle. The mathematical form of this principle is : Delta x.Delta p ge (h)/(4pi) (constant) However this principle is irrelevant in case of bigger particles such as a cup, ball, car etc., that we come across in our daily life. If uncertainty in position and momentum are equal, the v uncertainty in velocity would be

If uncertainty in position and momentum are equal then uncertainty in velocity is.

What is the minimum product of the uncertainty in position and the uncertainty in momentum of a moving electron ?

The uncertainties in position and the velocity of a particle are 10^(-10) m and 10× 10^(−22).sec^(−1) respectively. The mass of the particle in kg is

The uncertainties in position and the velocity of a particle are 10^(10) m and 10× 10^(−24).sec^(−1) respectively. The mass of the particle in kg is

The uncertainties in position and the velocity of a particle are 10^(-10) m and 10× 10^(−24).sec^(−1) respectively. The mass of the particle in kg is

The uncertainties in position and the velocity of a particle are 10^(-10) m and 1× 10^(−24).sec^(−1) respectively. The mass of the particle in kg is

The uncertainties in position and the velocity of a particle are 10^(10) m and 1× 10^(−34).sec^(−1) respectively. The mass of the particle in kg is

CENGAGE CHEMISTRY ENGLISH-ATOMIC STRUCTURE-Exercises Fill In The Balnks
  1. In the third energy level , there are ….. Orbirtals

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  2. In the third energy level , the maximum number of electron can be acc...

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  3. The uncertainty in position and momentum has a value ………..

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  4. In the spectrum of visible light , the red light has maximum ……… and ...

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  5. The velocity of electromagnetic radiation in a medium of permittivity ...

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  6. The 2px and 2py, 2pz, orbitals of an atom have identical shapes but di...

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  7. According to pauli erxclasion principle , the maximum number of elect...

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  8. In hydrogen atom, the order of energies of sub-shell of third energy...

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  9. The electronic configuration of Ti^(2+) ion is ………….

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  10. What is the difference in the angular momentum associated with the e...

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  11. The orbital angular momentum of an electron in 2s orbital is ………

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  12. If the uncertainty in the position of an electron is zero the uncerta...

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  13. Hydrogen spectrum consists of ………..

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  14. The maximum number of electron inmn = 1,l = 0, m = 0,s= +- 1//2 is …...

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  15. Na^(Theta) and Ne are ……. To each other

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  16. Energy density in the region between 1s and 2s orbital is …………

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  17. When there are two electrons in the same orbitals , they have ……………s...

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  18. The values of n(1) and n(2) in the pfund spectral series of hydrogen ...

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  19. The angular momentum of an electron in Bohr is given as ……

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  20. The filling of degenrate orbital by electrons is govermed by ………. p...

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