Question

Nitrogen (atomic number 7) and phosphorus (atomic number 15) belong to group 15 of the Periodic Table. Write the electronic configuration of these two elements. Which of these will be more electronegative? Why?

Answer 1

Electronegativity:-

1. It is a chemical property which is basically defined as the tendency of an the atom which is participating in the covalent bond to attract the bonding electrons.
2. Electronic configuration is basically defined as the arrangement or the distribution of all the electrons of an atom or molecule in the atomic or molecular orbitals.
3. Atomic number of Nitrogen($\mathrm{N}$) = 7
4. Electronic configuration of Nitrogen= $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^3$.
5. Atomic number of Phosphorus ($\mathrm{P}$)= 15
6. Electronic configuration of Phosphorus= $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^3$
7. Nitrogen and Phosphorus are arranged in a group in a down manner respectively.
8. So, on moving down below as the number of shell increases due to which the valence electrons will move away and there would be the decrease in the effective nuclear charge.
9. This all will cause the decrease in the tendency for the attraction of the electron.
10. Hence, electronegativity will decrease.

Therefore, Nitrogen ($\mathrm{N}$) would be more electronegative than ($\mathrm{P}$).