Calculating the probability of finding an electron at a certain location

[ShravanPatel2B]

I am having trouble understanding the topic presented in Section 1D.4 having to do with the equation presented for finding the probability of an electron. If anyone could clarify this section for me it would be greatly appreciated.

Thanks!

[805097738]

for finding the probable location of an electron you multiple the uncertainty in momentum x uncertainty in position and set it equal to or greater than planck's constant / 4pi. to find uncertainty in momentum you multiply mass of electron which is given x uncertainty in velocity which you should be able to derive from the information given. Uncertainty in position is the diameter of the atom because its electron would be located somewhere within that region. Then it comes down to plugging in those variables and solving for whichever one is being asked for.

[christabellej 1F]

Hi,
1D4 talks about the probability of finding electrons depending on the shapes of the orbitals. In this class, we would be discussing the orbitals s, p, and d. As far as the probability of finding an electron goes, s orbitals are said to be spherically symmetrical, meaning that the probability is around the same. For p and d orbitals, these have nodes, where there is zero probability of finding an electron there.

[ShravanPatel2B]

Thank you this makes a little more sense now!

[Brian Tangsombatvisit 1C]

If you use Heisenberg's Indeterminacy Equation, you will find that the change in position and change in momentum variables are inversely related. Meaning, if you design your experiment so that you minimize the error found in its position, you will have a large error in momentum (velocity since mass of the electron is constant), and vice versa. The measurement process influences outcome.

[ShreyaKannan1B]

What's the difference between Heisenberg Uncertainty Principle and Shrodinger's? Is it cause Shrodinger deals with the wave function?