For a hydrogen atom, all orbitals with the same n-value are degenerate. In atomic units, the energies go as E = - 1 2n2 For multielectron atoms, the average energies go as (Ens) < (Enp) < (End) . (a) What is the primary reason for this effect? (b) The energies of a multielectron atom go as E = Z² 2n2 (1) (2) Give a brief description of how you would use the variational method to account for the effect that you stated in part (a).
For a hydrogen atom, all orbitals with the same n-value are degenerate. In atomic units, the energies go as E = - 1 2n2 For multielectron atoms, the average energies go as (Ens) < (Enp) < (End) . (a) What is the primary reason for this effect? (b) The energies of a multielectron atom go as E = Z² 2n2 (1) (2) Give a brief description of how you would use the variational method to account for the effect that you stated in part (a).
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Transcribed Image Text:For a hydrogen atom, all orbitals with the same n-value are degenerate. In atomic units, the energies
go as
E
=
-
1
2n2
For multielectron atoms, the average energies go as (Ens) < (Enp) < (End) .
(a) What is the primary reason for this effect?
(b) The energies of a multielectron atom go as
E
=
Z²
2n2
(1)
(2)
Give a brief description of how you would use the variational method to account for the effect
that you stated in part (a).
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