Basicity Trend and Ionization Energy

[JogoBonito]

Kind of got two topics confused


So I know Basicity tends to increase as you move from Right to left on the periodic table and as you go up the period table. Meaning Li is more basic than Na? (Does this apply to LiOH vs NaOH? Im pretty sure NaOH is a stronger base?)

But according to first ionization energy (Na's being lower than Li). Na would lose the electron (electron donating) more readily than Li.


Are these two trends unrelated? I feel like I remember basicity wasn't about electron donating or reactivity but something else and I can't seem to find it in my notes


Thanks

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[erythrocyte666]

that's an interesting question, never thought about it
but now that i do, this is what comes to mind: electronegative but basic elements like N (in amines), P (in phosphines), and O are willing to share their lone pairs but will still keep most of it to themselves, but when you go far to the left the group 1 and 2 metals are willing to share their electrons so much that they are extreme enough to give them up. in a sense, these epitomize the idea of bases since that's the most any atom could do to act like a base. unfortunately, terminology comes in the way: nonmetals are the only ones that are traditionally called bases since by sharing their lone pair they form a covalent bond with a Lewis acid; but all metals display the "extreme" behavior of completely losing electrons and so they are called reducing agents (Li would be a stronger reducing agent than Na)

 

[JogoBonito]

Wouldn't Na be a stronger reducing agent than Li due to a smaller ionization energy?

Does the whole basicity trend only apply to the right side of the periodic table maybe? Although the acidity and size trends, electronegativity and electron affinty trend seems to apply to the entire table