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This is kinda a simple way of thinking about it but atoms want to have a full electron shell and since s-block metals only need to lose 1-2 valence electrons in order to have a full shell they really want to lose them, which is why they react more easily.
I'm not too sure what you mean by p-block metals, since p orbitals normally refer to the gaseous elements, but the s-block metals normally are reactive (become cations) in the sense that they are willing to bond with p-block elements to form a complete octet. Hope this helps!
This is because s-block metals usually have lower ionization energies when compared to p-block metals. With this low ionization energy, s-block metals tend to form cations, because they are more willing to give their electrons away, are are thus more reactive.
Ionization energy (the energy required to remove an electron) is typically lower for s-block metals. Search up an image of ionization energy in relation to the period table for a more visual answer. But generally, ionization energy gets higher as you move from left to right of the periodic table and lower as you move down the table.
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