Orbital Nodes (Diagrams of Psi/Psi^2)

In summary, the graphs of Ψ for atomic orbitals show that there are two radial nodes and two angular nodes, but the angular nodes are not represented by x-intercepts.
  • #1
mistertaylor9
2
0
I am having a hard time understanding the nodes on the graphs of Ψ for atomic orbitals. Take for example, the graph of Ψ for a 2s orbital as seen on the left here:

http://winter.group.shef.ac.uk/orbitron/AOs/2s/wave-fn.html

The graph intersects at two points, but these two intercepts represent the same spherical node.

Now consider the graph of Ψ for a 5d orbital.

http://winter.group.shef.ac.uk/orbitron/AOs/5d/wave-fn.htmlThe number of of radial nodes is 2 (from equation n-l-1) and the number of angular nodes is l=2. If one radial node causes the graph to cause the x-axis twice (on each side of nucleus, as in the case of the 2s orbital) then shouldn't there be 2 nodes * 2 intercepts/node = 4 intercepts just for the angular nodes? And then 2 more intercepts for the angular nodes? But the graph hits the x-axis at 5 (instead of 6) separate points which would imply 5 nodes but this isn't the case.

My only clue for the answer to my question is that maybe angular nodes are not represented by x-intercepts. Help meh!
 
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  • #2
What they're plotting on the (2D) graph in those figures is a cross section of the wavefunction. The cross section is taken along a radial line, i.e. a line that passes through the origin. So what you're seeing in the 2D graph is just the radial part of the wavefunction. The angular part is just a scaling factor.

In other words, you know that the wavefunction can be decomposed as
[tex]\psi(r,\theta,\phi) = R(r)Y(\theta,\phi)[/tex]
where R and Y are the radial and angular parts, respectively. For a radial line, [itex]\theta[/itex] and [itex]\phi[/itex] are fixed, so [itex]Y(\theta,\phi)[/itex] is just a constant for any given radial cross section. If you switch to a different radial cross section, though, it would have a different value. For example, in the 5d orbital you showed, the cross section was taken along the line [itex]x = y[/itex]. If they had used [itex]x = 3y[/itex] instead, the 2D graph would be smaller, but it would still have the same shape.

There are some particular angles at which the scaling factor [itex]Y(\theta,\phi)[/itex] is zero; in this case, [itex]\phi = \{0,1,2,3\}\pi/2[/itex]. If they had plotted a cross-section corresponding to one of those angles, the entire graph would be zero. Those angles are the angular nodes. You're correct that the angular nodes are not represented by x-intercepts.

By the way, since the cross sections they show in those graphs are taken along a full line, not a ray emanating from the origin, they actually show the radial wavefunction twice. So I'd actually suggest that you look only at the right half of the graph; the left half is just the mirror image. The center of the graph, of course, corresponds to the center of the atom, which is why a node at the center isn't part of a pair.
 
  • #3
You have cleared a lot up for me. Thank you!
 

Related to Orbital Nodes (Diagrams of Psi/Psi^2)

1. What are orbital nodes in diagrams of Psi/Psi^2?

Orbital nodes refer to the regions in an orbital diagram where the probability of finding an electron is zero. These nodes are represented by the areas of the diagram where there is no shading or where the wave function is equal to zero.

2. How do orbital nodes affect the shape of an orbital?

The number and placement of orbital nodes determine the shape and orientation of an orbital. For example, in a s orbital, which has no nodes, the probability of finding an electron is highest at the nucleus and decreases as you move away from it. In contrast, a p orbital has one node and its shape resembles a dumbbell with a node at the center.

3. What is the significance of orbital nodes in quantum mechanics?

Orbital nodes play a crucial role in understanding the electronic structure of atoms. The number and placement of nodes determine the energy and stability of an orbital, which in turn affects the reactivity and chemical properties of an element.

4. How are orbital nodes related to the quantum numbers n and l?

The principal quantum number (n) determines the number of radial nodes, while the azimuthal quantum number (l) determines the number of angular nodes. The total number of nodes in an orbital is equal to n-1.

5. Can an orbital have multiple nodes?

Yes, an orbital can have multiple nodes, depending on the values of n and l. For example, a d orbital has two radial nodes and two angular nodes, while an f orbital has three of each type of node. The maximum number of nodes in an orbital is equal to n-1.

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