And because of our m sub l's, we have three of them, negative 1, 0, and

1, there are three orientations of the p orbital.

And here they are, so we have one along the x axis,

we have one along the y axis, and one along the z axis.

Now which one's which, I don't know, they usually call this one the z axis.

But we see that we have them in the, the three orientations.

Now these you need to imagine, in an atom, are actually all over top of each other so

they exist in the same, on the same axis, but there are three of them and

that's what a p orbital looks like.

So these are our five d orbitals, and we know that n sub l gives us five

different values for the d subshell, and this is how they're oriented.

So four of them look very similar.

They have these four lobes that we see here.

In the x-y plane, these two are different in that these are between the axes,

and this is on the axes, so we see that being different here.

This is along the x-z plane, and they're perpendicular to each other, so

that's four of them.

The fifth one is very unusual.

It doesn't look like any of the others.

Now remember, the mathematical equations,

the Schrödinger equations are what define these shapes.

And so with the right quantum numbers, you end up with this three-dimensional shape.

So the five d orbitals are four of them that look very similar with

the four lobes, and then the fifth one which is very different.