wave functions and the heisenburg uncertainty  [ENDORSED]

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Ryan Cerny 3I
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wave functions and the heisenburg uncertainty

Postby Ryan Cerny 3I » Thu Oct 06, 2016 4:33 pm

If (Psi)^2 that represents the probability of finding an electron, how does the Heisenburg equation relate to that?

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Re: wave functions and the heisenburg uncertainty  [ENDORSED]

Postby Eunnie_Lee_3H » Thu Oct 06, 2016 8:00 pm

The Heisenberg indeterminancy equation shows us that there is no way for us to know both the exact position and momentum of an electron at a certain point in time, and that we can only know the "range" of the possible positions and momentum the electron could be at.

2 shows the probability of finding an electron.
Since we don't know the exact position of the electron, we can only look at an atom's diameter (and/or also its orbitals) and assume that the electron must be zipping around within this "area/volume."
This "area/volume" = probability of finding an electron = 2

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