The three ionisation enthalpies of boron atom are 800,2427and 3658kJmol-1 .Explain these values.
Answers
HELLO!
The values of ionisation enthalpies are just a mere representation of the concept. Ionisation energy is the energy required to remove an electron from the outermost shell of an isolated gaseous atom. If the atom is stabilised by half filled/full filled stability, it is very difficult to remove the electron and hence, ionisation enthalpy will be high.
Check out the attachment for the electronic configurations.
In Boron atom, the outermost electron is in the p orbital, which is not so difficult to be removed, so the energy required is just 800 kJ. However, once this electron is removed and a positively charged ion is formed, the atom now has a full filled stability, because of the fully filled s orbital, and removing this electron is gonna be tough. So, a huge energy is required this time, and so there's a huge difference between the first and second ionisation enthalpies (the second being 2427 kJ).
For the third electron, the atom now has a half filled stability because of half filled s orbital. So, again there is a large difference in the second enthalpy and the third enthalpy, the third being 3658 kJ.
Hope it's clear.
Thanks! :)
Answer:
This is your answer in attachment.........
