Why is N(3-) larger than O(2-)?
*or the ionic radius
Both are within the same period and, due to the electrons they have gained, essentially have the same electron configuration. Why is the radius of triple-negative nitrogen still larger?
I have to be able to justify this whole thing in an exam, and my only argument is that the atomic radius generally decreases periodically from left to right, and if N has one more electron, it's clear that nitrogen is larger. But then I can't explain why both have the same electron configuration.
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Electronegativity increases from left to right within the period. With a constant number of electron shells, the number of positive protons in the core increases and this attracts the negative electrons more strongly (small radius).
The different electronegativity of the various elements also plays a role in polar molecules such as water (imbalance distribution of the binding electrons).
I hope I could help you and wish you a nice Sunday.
have definitely helped, thank you!
Thanks for the star!
N3 – and O2 – have the same electron configuration as F-, Ne, Na+, Mg2+ and Al3+. However, the positive charge of the core that attracts the electrons increases. It’s trivial.
The decrease of the atomic radius within a period and the jump at the beginning of a new period are more complicated to explain, because the shielding effect of closed electron shells comes into play, which exists only outwards.
This is because the core has a proton more and thus attracts the negative charge more strongly on the outside. This reduces the ion radius