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But, (irrespective of whether the species in question is mono-electronic or multi-electronic) the three orbitals in the $2p$ subshell, namely $2p_x$, $2p_y$ and $2p_z$, do have the same energy, and thus we can say that they ARE degenerate, as Gaurav also pointed out. Hopefully, that alleviates your confusion.
Orbitals with the same energy. For example the p_x, p_y and p_z electron orbitals of an atom exist in the directions of the x, y and z coordinates but are all of equivalent energy, so are said to be degenerate.
Doesn't degenerate mean there are multiple places pairs of orbitals can be? "degenerate" means having the same energy. "Degenerate" refers to a set of orbitals. It doesn't make sense to say one orbital is degenerate. Solving the non-relativistic Schrodinger equation, all the orbitals for a given "n" are degenerate. Energy only depends upon n.
Degenerate orbitals in the Hydrogen atom. Ask Question Asked 8 years, 3 months ago. Modified 8 years, 3 ...
The $\mathrm{t}$ means triply degenerate while the $\mathrm{e}$ means doubly degenerate (degenerate means have the same energy). The $\mathrm{g}$ is not about how many energy levels are degenerate rather it is an indication of the answer to a certain operation we can perform on an orbital. It instead relates to how the orbitals behave if we ...
According to Hund's first rule, a set of degenerate orbitals are singly occupied first, before the second slot in any of the orbitals are populated. This is quite intuitive because electron-electron repulsions would make an atom more unstable if the electrons start filling two at a time in a single orbital.
The form of the p orbitals that we are familiar with are the $\\mathrm{p}_x$, $\\mathrm{p}_y$, and $\\mathrm{p}_z$ orbitals: (source: ChemTube 3D) I also know that the p subshells have the quantum n...
$\begingroup$ I'd point out that there is only one 2s orbital so it can't be degenerate. The various p, d, and f orbitals can be, and they are degenerate in the $\ce{He+}$ atom in the ground state. However if the electron is in a 2p orbital say, then the other two are degenerate, but the one with the electron has a different energy. $\endgroup$ –
In hydrogen, all orbitals with the same principal quantum number 'n' (1,2,3...) are degenerate, regardless of the orbital angular momentum quantum number'l' (0,1...n-1 or s,p,d..). However, in atoms with more than one electron, orbitals with different values of l for a given value for n are not degenerate.
I think it is the same reason why the orbitals 2s, 2px, 2py, and 2pz are all degenerate in the H atom. You can clearly see the symmetry between the 3 p orbitals but how can the spherical 2s be symmetric with the rest? The answer is that the Coulomb potential has a hidden symmetry that shows up in spaces of dimension higher than 3.