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easwar2641993
- 11
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Why Group 15 elements(except Nitrogen) have empty d orbitals while bonding?
Aufbau Principle states that electrons are added in orbitals only in the increasing order of energy of sub-shells.Also Bohr Bury rule adds to the above principle that increasing order of energy depends on the value of n+l where n is the principal quantum number and l is the azimuthal quantum no and according to these rules the increasing order of sub-shells is
1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f…
But my question is when higher p-block elements form compounds,it is said that they form bonds by
promoting the electron of the valence shell to the next available vacant orbital.
Consider the example.For PCl5.For this P in ground state is 1s2 2s2 2p6 3s2 3p3.In excited state ,it is 1s2 2s2 2p6 3s1 3p3 3d1. If the rules are followed correctly,it should be like this 1s2 2s2 2p6 3s1 3p3 4s1 right?I know hybridization but something is missing in my mind.
Aufbau Principle states that electrons are added in orbitals only in the increasing order of energy of sub-shells.Also Bohr Bury rule adds to the above principle that increasing order of energy depends on the value of n+l where n is the principal quantum number and l is the azimuthal quantum no and according to these rules the increasing order of sub-shells is
1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f…
But my question is when higher p-block elements form compounds,it is said that they form bonds by
promoting the electron of the valence shell to the next available vacant orbital.
Consider the example.For PCl5.For this P in ground state is 1s2 2s2 2p6 3s2 3p3.In excited state ,it is 1s2 2s2 2p6 3s1 3p3 3d1. If the rules are followed correctly,it should be like this 1s2 2s2 2p6 3s1 3p3 4s1 right?I know hybridization but something is missing in my mind.