Question

In the periodic table we come across diagonal relationship where by the top member of each group resembles the second member of next group. For example Boron resembles silicon. Can it be explained on the basis of I.E. and charge density data? Explain your answer.

Answer 1

Boron belongs to P–block element and and is the first element in the group 13 and present in third period.

Its density is $2.46g/cm^3$ and has atomic number 5.

Silicon also belongs to P- block element and is the first element in the group 14 and present in the third period.

Its density is $2.3290 g/cm^3$ and has atomic number 14.

The electron configuration of  Boron is $1s^{2}2s^{2} 2p^{1}$ and Silicon $1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{2}$.

Since both have two electrons in 1s orbital, have high melting point and are non metals. So, Boron resembles silicon.