Silicon (atomic no-14) and phosphorus (atomic no-15) belong to the same period of the periodic table. Write down the electronic configuration of silicon and phosphorus and find the period in which these elements occur.
Silicon (atomic no-14) and phosphorus (atomic no-15) belong to the same period of the periodic table. Write down the electronic configuration of silicon and phosphorus and find the period in which these elements occur.
The electronic configuration of silicon and phosphorus is as follows:
Atomic no of silicon(Si) is 14
Electronic configuration of silicon(Si): 2, 8, 4
As we can see a total of three shells are there in silicon so its period no will be 3 and as the 4 electrons are there in the last shell so the group no will be 14.
Atomic no of phosphorus(P) is 15
Electronic configuration of Phosphorus(P): 2, 8, 5
As we can see a total of three shells are there in phosphorus so its period no will be 3 and as the 5 electrons are there in the last shell so the group no will be 15.
Hence, both elements have three shells (K, L, and M) and should be accommodated in the same 3rd period in the periodic table.
The electronic configuration of silicon and phosphorus is as follows:
Atomic no of silicon(Si) is 14
Electronic configuration of silicon(Si): 2, 8, 4
As we can see a total of three shells are there in silicon so its period no will be 3 and as the 4 electrons are there in the last shell so the group no will be 14.
Atomic no of phosphorus(P) is 15
Electronic configuration of Phosphorus(P): 2, 8, 5
As we can see a total of three shells are there in phosphorus so its period no will be 3 and as the 5 electrons are there in the last shell so the group no will be 15.
Hence, both elements have three shells (K, L, and M) and should be accommodated in the same 3rd period in the periodic table.
