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## Main Question or Discussion Point

Is it possible for an electron in the 1s orbital of an hydrogen atom to be indefinitely far from the nucleus in a given instant?

From the Schrodinger equation we can see that the radial probability is NEVER zero, so it would be possible to see an electron in the moon, for example.

But if I understood correctly, all orbitals have an specific energy associated to it. In the cas of the 1s Hydrogen orbital is -13,6eV. The average potential energy of an electron in that orbital is -2 *13,6 eV and the average kinetic energy is +13,6eV.

But consider an electron in the moon. The potential electric energy of that electron would be practically zero. So, for the total energy to be -13,6 eV, the kinetic energy would have to be -13,6eV, which is impossible.

What is wrong with this reasoning?

From the Schrodinger equation we can see that the radial probability is NEVER zero, so it would be possible to see an electron in the moon, for example.

But if I understood correctly, all orbitals have an specific energy associated to it. In the cas of the 1s Hydrogen orbital is -13,6eV. The average potential energy of an electron in that orbital is -2 *13,6 eV and the average kinetic energy is +13,6eV.

But consider an electron in the moon. The potential electric energy of that electron would be practically zero. So, for the total energy to be -13,6 eV, the kinetic energy would have to be -13,6eV, which is impossible.

What is wrong with this reasoning?