If the 2 electrons of a hydrogen molecule are more likely to be found between the 2 hydrogen atoms, why does this diagram says otherwise?

[![enter image description here](https://i.stack.imgur.com/wxEZb.png)](https://i.stack.imgur.com/wxEZb.png)


So I am reading about bonding and antibonding molecular orbitals and i can't understand how does the probability diagram show that the electron density in the sigma 1s molecular orbital is greatest between the two positively charged nuclei.


As i read this diagram [(b) in the picture],the probability of finding the 2 electrons in a hydrogen molecule is higher around each hydrogen atom nucleus. But molecular theory says that the electron density is the highest between the 2 nuclei.
The diagram shows that the highest ψ^2 values are on the hydrogens nuclei and not between them.
So what am i getting wrong?




The shape of the orange blob is highly affected by the chosen contour level. In the image below, if you choose a contour level of 0.04, you get a oval much like the one shown. If you choose a contour level of 0.2, you get a dumbbell shape. If you choose a contour level of 0.4, you get two spheres around the atoms, which does not look connected at all.


[![enter image description here](https://i.stack.imgur.com/o7pt8.png)](https://i.stack.imgur.com/o7pt8.png)


It turns out that the electron density of two bonded atoms is very similar to the electron density of the two individual atoms, especially for atoms with inner electrons. The difference, called the deformation density, gives you an idea how the electron density "shifted" with respect to that of the unbound atoms. Unfortunately, I did not find a deformation density for dihydrogen in a quick internet search. Maybe someone can calculate it, though.


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