Nitrogen from only Ncl3 but phosphorus forms pcl3 and pcl5 both. Explain
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Nitrogen has no d- orbitals so it exhibits only sp3 hybridisation. Phosphorous has d-orbitals so it can undergo even sp3d2 hybridisation to form PCl5.
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Phosphorus has 15 electrons. So its electronic configuration is:
Phosphorus is a period 3 element. Hence it has an empty d-orbital which the period 2 elements do not have.
When phosphorus forms a compound, if there is enough energy available then one electron from one of the orbitals jumps to the vacant d-orbital. This gives phosphorus extra 2 valencies. This is called expanded octet.
As phosphorus initially has valency as 3 it forms PCl3, and due to this expanded octet, PCl5 can also be formed.
*Note that the expanded octet phenomenon can occur only in period 3 elements.
As Nitrogen lies in period 2, it does not have the empty d-orbital and so does not form NCl5
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Phosphorus is a period 3 element. Hence it has an empty d-orbital which the period 2 elements do not have.
When phosphorus forms a compound, if there is enough energy available then one electron from one of the orbitals jumps to the vacant d-orbital. This gives phosphorus extra 2 valencies. This is called expanded octet.
As phosphorus initially has valency as 3 it forms PCl3, and due to this expanded octet, PCl5 can also be formed.
*Note that the expanded octet phenomenon can occur only in period 3 elements.
As Nitrogen lies in period 2, it does not have the empty d-orbital and so does not form NCl5
Hope it helps u friend... if possible then please mark it as brainlest answer
thankuuu
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