Finding the electron increases if we go towards the nucleus?

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SUMMARY

The probability of finding an s-electron increases as one approaches the nucleus, but only up to the Bohr radius. Beyond this radius, the probability density decreases towards zero. The confusion arises from interpreting the square modulus of the wave function without considering the radial probability density, which incorporates the factor of 4πr². This radial probability density reaches its maximum at the Bohr radius, illustrating the stability of the electron's orbit without collapsing into the nucleus.

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photon79
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Is it true that the probability of finding the electron (s-electron) increases if we go towards the nucleus? then what accounts for its stability from not being attracted by the nucleus n collapsing into it..its a basic question but i don't have an idea now! Is it just the concept of constant orbits in which electron doesn't lose or gain energy??more info pls!
 
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photon79 said:
Is it true that the probability of finding the electron (s-electron) increases if we go towards the nucleus?

Only up to the Bohr radius.

After that the probability decreases towards zero. I suspect that you are confused because you are looking at the square modulus of the wave function and you see that it increases monotonically as [itex]r \rightarrow 0[/itex]. But you have to remember that that probability density function must be weighted by the factor [itex]4\pi r^2[/itex]. This weighted probability density is the so-called radial probability density, and it attains its maximum value at the Bohr radius.
 

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