So basically when it loses that electron that means that its oxidized and it forms a +1 ion so for instance, sodium will form sodium +ion usually that happens with an nonmetal. So they also have low ionization energies and that makes them very reactive so when something has a low ionization energy that just means that the ability of another of a nonmetal basically to come remove the electron from the outer most shell is it doesn't take very much energy it's low ionization energy so it can kind of just come pluck it out. So more specifically group 1a elements are the alkali metals and so these guys include Lithium, sodium, potassium, rubidium, cesium and francium, so they have one valence electron, so one electron in their outer most shell. Okay so remember that the s valence shell can have two electrons maximally and one of them is spin up and one of them is spin down right so they're spin paired. So again the electronic configurations, so how you kind of map where the electrons are in the atom is more specifically where they what their valence show electrons are like or their outer most shell electrons. So when I say s-Block elements, what exactly do I mean? So I'm referring to group 1a and group 2a and so when I'm saying s-Block I'm referring to the electronic configurations that the elements in these two groups or families actually have so let's kind of talk about what that means. So let's talk about the periodic table kind of in more depth and let's start talking about the s-Block elements.
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