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What is a degenerate orbital - Chemistry Stack Exchange This energy order for multielectronic species, by the way, is exactly what you derive from the Aufbau principle Notice that in the orbital energy level diagram for monoelectronic species (each box corresponds to one orbital), all the orbitals in the $2s$ and $2p$ subshells, for example, have the same energy, and are thus degenerate
Are electron orbitals in a helium atom degenerate? In a hydrogen atom, the presence of only one electron allows various orbitals' energy states to be dependent only on the principal quantum number and not on angular momentum Orbital degeneracy and
Which orbitals of the hydrogen atom are degenerate for n=3? First of all isn't there only 1 electron in hydrogen? yes And how could the s orbital 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
physical chemistry - Why are degenerate orbitals called degenerate . . . The way i would explain to a high schooler is that degenerate orbitals mean orbitals with the same energy level Simple as that People got bored of always having to say "orbitals in the same subshell" or "orbitals at the same energy level" hence, someone came up with the phrase "degenerate orbitals" There's no need to take naming so seriously, focus on actual concepts
Degeneracy of Orbitals - Chemistry Stack Exchange Important note: it's a common misconception to separate orbitals and electrons The orbitals ARE the electrons If the energy of two orbitals (electron) are the same, they are defined as degenerate This can be related to the symmetry of the system (which is fully defined within the full Hamiltonian), system with high symmetry (such as atoms) have "a lot of" degeneracy whereas system with low
Octahedral Crystal Field Splitting Orbital Degeneracy How are the $\mathrm {e_g}$ orbitals degenerate with each other? Note: This isn't a homework question After the semester ended (I don't go to MIT), I ended up on MIT open course-ware to watch some
Are the 2s and 2p subshells degenerate in the He+ ion? 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