Orbital shapes

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Nick Fiorentino 1E
Posts: 102
Joined: Wed Sep 18, 2019 12:16 am

Orbital shapes

Postby Nick Fiorentino 1E » Thu Oct 17, 2019 10:08 am

Is there a trick to remembering what all the orbital shapes look like? As in, is there a method to remembering what dxy, dy2, d2x,dx2y2, etc all look like?

Brooke Yasuda 2J
Posts: 102
Joined: Sat Jul 20, 2019 12:17 am

Re: Orbital shapes

Postby Brooke Yasuda 2J » Thu Oct 17, 2019 10:26 am

I think in class Dr. Lavelle said that we won't be asked to draw the orbitals on tests, but in general, you can guess the shapes based on the axes that they are on. So just remember which way is the x, y, and z axis.

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Re: Orbital shapes

Postby Veronica_Lubera_2A » Thu Oct 17, 2019 10:45 am

The p, d, and f orbitals also have a nodal plane where there is zero electron density (and therefore zero electron probability.)

There is a trend to how many 'petals' you draw on the axes as well:

S is just a circle because of its symmetric electron distribution.
P has 2 horizontal petals.
D has 4 petals on the x and y axes.

And if you are given d(xy), d(y^2), d (zx), there is a higher probability to find electrons on the xy/y^2/zx planes

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Re: Orbital shapes

Postby LReedy_3I » Thu Oct 17, 2019 6:33 pm

Also, the number of nodal planes is related to the value of l. As it increases, there are more conical nodes.

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