2nd October 2019

stackexchange
13

Is 2s or 2p closer to the nucleus?

Because it is less effectively shielded, a 2s electron experiences a higher effective nuclear charge and is held closer to the nucleus than a 2p electron which gives the 2s orbital a lower energy.

Also question is, what is the difference between 1s and 2s?

2s orbital has more energy than 1s orbital. Also 2s orbital has a nodal plane but 1s orbital doesn't have any nodes. They are in different shells. Both orbitals have the same spherical shape as indicated by the “s”.

Why is the energy of the 2s orbital lower than the energy of a 2p orbital Why is the energy of the 2s orbital lower than the energy of a 2p orbital?

The higher effective nuclear charge experienced by the 2s electrons in carbon (as a result of the closer penetration in to the nucleus) compared with the 2p electrons in carbon means that the 2s electrons experience a stronger attraction to the nucleus and therefore possess lower orbital energy than the 2p electrons.
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