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S-block metals are typically more reactive than p-block metals because they have a lower ionization energy, because of greater distance between the nucleus and the valence electrons. Furthermore, since s-block metals also typically have less electrons to lose than the p-block metals, they would be more reactive.
S-blocks are typically more reactive than p-block metals because as you move across a period in the periodic table, ionization energy increases. The s-block is more on the left of the periodic table compared to p-blocks so the ionization energy of the s-block is lower, which means that it is easier for them to lose electrons, so they are more reactive.
Does anyone else find the wording a little ambiguous? Because I think you can make the argument that fluorine is extremely reactive too, due to how close it is to a noble gas electron configuration, but fluorine is definitely not an s-block metal. In this case, fluorine readily takes electrons from other atoms around it, causing it to react. This leads me to find the wording of the problem troublesome.
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