Sodium, one of the most abundant chemicals in the human body is usually found in it's freebase form
Na+ is not a freebase, it's a charged cation of a salt. The "free base" (conjugate base) of Na+ is Na(0), elemental sodium. As you might have guessed, elemental sodium is rather stronger a reducing agent than sodium cation. (likes to donate electrons, be oxidised). Na(0) has one electron in its outer shell it is dying to get rid of. Na+ is already as oxidised as it can comfortably be. Na2+ is unheard of due to the unprecedentedly large energy barrier of stripping an additional electron out of a full shell.
Sodium is also not all that terribly reactive as an alkali metal, either. It is more reactive with water than it is with oxygen, I think. (and we are full of water.) Either way, people can handle it (with gloves) and cut it in open air without too much issue. I think it would have to be molten or finely divided to be a real pyrophoric. (I've heard some shit about potassium and sodium-potassium alloy.)
Na+ is also not "addition of a proton", it's loss of an electron. If you add a proton to Na, you get NaH (sodium hydride, Na+H-) - actually an industrial chemical used as a very strong base & as a precursor to sodium borohydride.
This is a good first year chemistry gedankenexperiment to demonstrate oxidation states... Na(0) and Cl2 are rather nasty but NaCl (Na+ Cl-) is not, explain why in a paragraph... 10 marks..
