![]() ![]() People will respond when they have time, not because you repeat it. Side note, you don’t need to post the same question multiple times to get a response. And like aluminum, its +5 cation has the same electron configuration as neon and wants to remain as such. ![]() To confirm this here are the first seven ionization energies of phosphorus in kJ/mol: 1011.8, 1907, 2914.1,Ĕ963.6, 6273.9,Ē1267, 25431 and we can see that abnormally large difference between the fifth and sixth ionization energies as expected. The main culprit for huge energy difference between ionization energies is the cation achieving a noble gas electron configuration and not wanting to lose that stability.įor phosphorus we would expect a large difference between the fifth and sixth ionization energies, not between the third and fourth. There is an energy difference between the 3s and 3p subshells, but it’s slight and this wouldn’t correspond to such a large energy difference as the one between the third and fourth ionization energies here. So we’re looking for a third period element which has a cation of +3 charge with the same electron configuration as the previous noble gas, neon. Such a large difference between the third and fourth ionization energy corresponds to the stability associated with a noble gas electron configuration. The reason for this resistance is because the atom reaches a relatively stable electron configuration by losing the first three electrons and does not want to disturb that stability by losing a fourth electron. This tells us the atom resisted losing that fourth electron more so than the first three. Since ionization energy is the amount of energy required to remove an electron, a high ionization indicates a difficult to remove electron. Much higher than the transition from any of the other ionization energies. When we look at the changes between different ionization energies, we see an abnormally large increase from the third to the fourth ionization energies.
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