### Drawing orbitals

Posted:

**Sun Nov 04, 2018 10:40 am**Hi my TA mentioned that we might have to know how to draw the different orbitals like 3px, 3py, and 3pz. Can someone explain how to do this?

Created by Dr. Laurence Lavelle

https://lavelle.chem.ucla.edu/forum/

https://lavelle.chem.ucla.edu/forum/viewtopic.php?f=21&t=35696

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Posted: **Sun Nov 04, 2018 10:40 am**

Hi my TA mentioned that we might have to know how to draw the different orbitals like 3px, 3py, and 3pz. Can someone explain how to do this?

Posted: **Sun Nov 04, 2018 11:31 am**

I'm not 100% sure, but I think you would draw the shape of the p orbital, but would draw one on the x-axis, one on the y-axis, and one on the z-axis.

Posted: **Sun Nov 04, 2018 11:34 am**

The p orbitals have a shape with two lobes, and depending on whether it is px, py, or pz, you would draw the two lobes on the x axis for px, the y axis for py, and the z axis for pz.

Posted: **Sun Nov 04, 2018 11:37 am**

I believe that what your TA is trying to say by drawing 3px, 3py, and 3pz orbitals is by drawing a bell shaped on those axis. For instance, for 3px you will draw the bell shape on the x axis, 3py on the y axis, and 3pz on the z axis. These orbitals is where the electron will lie.

After you draw the bell shape on the attended axis, then you will draw the nodal planes, angular node, radial node, etc. We know that in the nodal planes and etc., there is 0 probability of electron density. You get the nodal plane by doing n-1, which in this case (3px,y,z) will be 3-1=2. This means you will have 2 nodes in your figure. You will have the angular node ( which is just a straight line through the dumbbell figure) and a radial node (which is the shape of a circle in the orbitals).

I'm sorry if this sounds confusing, it is hard for me to explain without a picture. But I found this video very helpful!

https://www.youtube.com/watch?v=wkrAtD1mp7k

After you draw the bell shape on the attended axis, then you will draw the nodal planes, angular node, radial node, etc. We know that in the nodal planes and etc., there is 0 probability of electron density. You get the nodal plane by doing n-1, which in this case (3px,y,z) will be 3-1=2. This means you will have 2 nodes in your figure. You will have the angular node ( which is just a straight line through the dumbbell figure) and a radial node (which is the shape of a circle in the orbitals).

I'm sorry if this sounds confusing, it is hard for me to explain without a picture. But I found this video very helpful!

https://www.youtube.com/watch?v=wkrAtD1mp7k

Posted: **Mon Dec 03, 2018 11:39 pm**

Draw the shape of the p orbital first and then draw it on the x axis and y axis and the z axis.