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So I was going through the Schrödinger wave equation to determine the shapes of orbitals. We know that an orbital is nothing more than a region where probability of finding an electron is maximum.

Further, we know that the probability of finding a 2s electron in 1s orbital is just too low! Why do 1s orbital and 2s orbital intersect? I mean both the orbitals have the same shape and the radial function of 2s orbital is more than that of 1s which clearly means that 1s orbital lies inside 2s orbital!

But as it's impossible to find a 2s orbital electron in 1s orbital, shouldn't the shape of 2s orbital be something like a hollow sphere with thick walls instead of a complete sphere?

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    $\begingroup$ I suspect you are trying to visualize the orbitals stacked as a matryoshka doll. The thing is, this "atomic doll" isn't made of wood, it's more like a 3D model made in Blender consisting of a of bunch of intersecting meshes that are not baked together yet. $\endgroup$ – andselisk Aug 21 '20 at 12:24
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    $\begingroup$ You have it all backwards. Any orbital intersects any other. $\endgroup$ – Ivan Neretin Aug 21 '20 at 12:26
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    $\begingroup$ Electrons aren't running in circles. $\endgroup$ – Mithoron Aug 21 '20 at 13:45
  • $\begingroup$ Does this answer your question? How are subshells and shells arranged in an atom? $\endgroup$ – M.A.R. Aug 31 '20 at 21:27
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I read your question a few times, and I think you're confusing occupancy with spatial probability distribution.

Orbitals have a lot of spatial overlap. But if the orbital has two electrons “in it,” then it cannot describe the probability behavior of any other electrons in that atom, as other electrons must be in another orbital.

A 2s electron absolutely can go into a 1s orbital provided there is space. This is exactly what happens with atomic emission spectra when an electron in energy level $n=2$ transitions to $n=1$ and releases energy.

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I would even dare to say that, generally, orbitals largely overlap each other. By other words, if there is nonzero probability of occurence of an electron in the particular quantum state, it does NOT mean the probability of occurence of electrons in other quantum states is in the same point zero.

The probability of occurance near kernel for 2s electron has a local maximum, as ns orbitals have (n-1) radial nodes. So no, 1s and 2s orbitals do not have the same shape, neither 2s and 3s. They just share the spherical symmetry.

Here is the ( local PNG copy of not pastable SVG) picture for 1s,2s,3s orbital from the page radial probability distribution function.

Local PNG copy of the SVG picture on the referred page

Note the quantity on the y-axis of the chart: $4 \pi r^2 \Psi^2$ what is probability an electron occurs in the infinitesimal spherical shell $r,r+\mathrm{d}r$

One can also check the radial term R(r) of wave function on chem.libretexts.org on Figure 8.2.2, describing orbitals 1s, 2s, 2p.

There is a close analogy with the Maxwell-Boltzmann distribution for the speed of ideal gas molecules. Even if the maximum probability of 1-axis velocity component is at zero axis velocity, following the Boltzmann energy distribution, for the speed is the maximum at nonzero speed.

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  • $\begingroup$ The curves reported by Putnik show the probabilité of finding the electron in a given sphere around the nucleus. If the probability $\psi^2$ of finding an electron at position ($x,y,z$) were reported, the obtained curves would always show a maximum at $r$ = $0$. $\endgroup$ – Maurice Aug 21 '20 at 12:32
  • $\begingroup$ Sure, that is why I have explicitly written the radial probability distribution functions. See also the A update. $\endgroup$ – Poutnik Aug 21 '20 at 12:39

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