Why are metals in aqueous solution basic, and non-metals acidic?

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The discussion centers on the concepts of proton acceptors and lone pair donors within acid-base theory, particularly in relation to metals and non-metals in water. It is noted that metals, being less electronegative than non-metals, tend to donate electrons to hydrogen in water, leading to the release of hydrogen ions (protons) as hydrogen separates from oxygen. In contrast, non-metals, which are more electronegative, form larger acid molecules by attracting electrons from water without releasing them, resulting in a structure where hydrogen is the least electronegative atom, potentially leading to the formation of protons. The conversation emphasizes the need for clearer explanations and specific references to support these claims, as vague assertions are not deemed acceptable in the forum.
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Why are metals in aqueous solution basic, and non-metals in water acidic?
I heard an explanation about something being a better proton acceptor or lone pair donor but that doesn't make sense. I couldn't explain in in terms of acid-base theory.

The hand-waving way I saw it was that metals are less electronegative than non-metals, so in water, they'll donate their electron to the hydrogen, the hydrogen will break away from the oxygen because hydrogen hates oxygen hogging its electrons, and because hydrogen electronegative enough.

With non-metals, my hand-waving is that metals are more electronegative, when they bond with water, they'll just form one bigger molecule because they suck on other's electrons without letting go and form one big acid molecule where the least electronegative thing in there is a hydrogen, which falls of into a proton, and it may or may not be polyprotic.
 
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adf89812 said:
I heard

adf89812 said:
The hand-waving way I saw it
These vague "citations" are not acceptable here on PF. Please post exactly what you heard/saw.
 
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