Why is Li a stronger reducing agent than Na?
A strong reducing agent is one that gives up an electron freely. If you look at the periodic table, LI and Na both have one electron they can give up. So in that sense they are the same. Li lets that one electron loose a little easier because it has less protons holding the electrons in place. Li has 3 protons, NA has 11. So there is less mass in the nucleus holding the outer electron in place. Both are good reducing agents, but Li reacts very violently (it tends to explode) so most people choose Na when possible. By the way… I’m sure it was just a mistake, but the “economics” section may not be the best place to ask this question.
