So if we look at the periodic table, we see that for electron affinity, we're going to say that it becomes more exothermic. So we can say that it increases as we move to the top right corner of the periodic table. So notice here we have -72.8 for hydrogen and we have -328 for fluorine. Remember, the more negative your electron affinity, the more exothermic the reaction. That means it wants the electron even more. So we can see that fluorine wants an electron even more than hydrogen.
If we go down, we can see here that cesium is -45.5, so it doesn't as readily want an electron. Also notice here that the bottom row does not have any values. Those elements are so large, so unstable, that we tend not to talk about their electron affinity. You'll also notice that certain elements are have electronic affinities that are equal to or greater than 0. So we have beryllium here, we have nitrogen. We have the noble gas, which makes sense because they're perfect. So they don't require accepting an electron, they don't need it.
Some others are not, as commonly seen. Here we have manganese, we have zinc, cadmium, and mercury, and we'll see why those are less than 0 or not less than 0, equal to or greater than 0. Then we have HF over here in yellow. That's because it's a weird element. There's no real solid like justification for why it's greater than or equal to 0 is just one of those auto elements out there. But for all the ones that are in Aqua, we'll see the justification of why they have electron affinities that are greater than or equal to 0.