Energy Levels of atomic orbit | Hydrogen like (single electron) vs multi electrons atom |

hey, visitors so here is a problem or i can say difference between single electron atom like hydrogen (H) He+ ,Li++ and other multi atoms like sulphur carbon.. take any of d-block

the energy levels differ in both cases and we will find out why !


the basic difference stand here is why bohr's model fails for multi-atoms ?

 because of the heisenberg uncertainty principle & the splitting orbital (the factor of today's case)

the splitting happen due to the repulsion of electrons and the difference between hydrogen and other multi-atom i also.

 

lets first start with hydrogen. 

 the energy chart of hydrogen like atom orbitals

2s energy level is similar to 2p and 3d < 4s but if this is true then why d-block elements or any heavy atom violate this kind of filling?

the answer is because they follow afbau principle  'building up' as we all know the electron filling happen from lower to higher energy levels

the energy chart of filling in multi- electron atoms.

CONCLUSION:

confused don't  be in hydrogen or hydrogen like atoms there is only one force acting the positive charge of nucleus  that's why the difference between orbit and orbital is insignificant for hydrogen like atoms and 3d < 4s while in multi-atoms the repulsion of electrons are also present that makes big orbitals like d-orbital higly unstable. therefore the energy of 3d orbital is higher then 4s for multi atoms.  alright i hope you all got it :) :) !

keep visiting !