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I believe it is question 2.75 in the sixth edition where it is asking about whether the s-block or the p-block is more reactive. I know that elements in the s-block have lower ionization energies, but does this quality make it more reactive than p-block?
Yes, having a lower ionization energy means that these atoms can more easily lose or gain an electron, and thus more easily form bonds with other atoms. This lower ionization energy translates to increased reactivity, because the atoms can form compounds with other atoms with greater ease.
Elements in the s-block are more reactive. Yes, because they do have lower ionization energies, it is easier to remove electrons from the outer shell of these elements, making them more reactive. s-block elements usually have one or two electrons in the outer most shell, and it requires less energy to give away those two electro then to gain more electrons and fill up the outer shell to become stable.
The elements in the s-block are significantly more reactive than those in the p-block and this is because of their very low ionization energies whereas the p-block elements do have high electron affinities but still are not comparable to s-block's ionization energies. To see how reactive group 1 metals are watch this video: https://www.youtube.com/watch?v=m55kgyApYrY
I don't think ionization energy and reactivity are directly inverse. Low ionization energy only indicates the high reactivity with atoms with low electronic affinity. More specifically, the reactions between them are formed through ionic bonding. However, it does not indicate the reactivity of reactions formed through covalent bonding or metallic bonding. As a result, ionization energy and reactivity are not necessarily inverse.
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