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Energy of orbitals

Whichis not true?

A. In the hydrogen atom, all subshells of a principle shell are at the same energy level.
B. Orbital energies are higher in multielectron atoms than in hydrogen atomes.
C. In a multielectron atom, the various subshells of a principle shell are at a different energy levels.
D. All orbitals within a subshell of a multielectron atom are at the same energy level.
E. In high numbered principal shells of a multielectron atom, some subshells of differetn princpal shells have nearly identical energies.

Solution This solution is FREE courtesy of BrainMass!

If we ignore the very small perturbations due to spin-spin and spin-orbit interactions (such as in the super-fine structure of hydrogen), then we can say that the energy level of hydrogen's electron is determined by the principal quantum number n - so A is true.

B is also true. When we have more than one electron, Pauli's exclusion principle prevents electrons to go to the lowest energy state if there is already an electron that occupies it.

C is true as well. In multi-electrons atoms, the spin-spin, spin-orbital and electrostatic interactions are much stronger than in the hydrogen atom. This leads to energy perturbations that depend on the angular momentum of the electron which is a function of the sub shell.

This contradicts D, so statement D is not true.

Even in hydrogen when n is approaching infinity (or at least a very large number) the difference between consecutive energy levels is very small, and practically we talk about "energy continuum". This is even more true for multi electron atoms, where an electron at a higher principal shell can have lower energy than an electron in a lower principal shell.....