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1F.19

Posted: Sun Oct 20, 2019 10:07 pm
by 304976622
Why are s-block metals typically more reactive than p-block metals?

Re: 1F.19

Posted: Sun Oct 20, 2019 10:09 pm
by Philip
s-block metals have lower ionization energies compared so they tend to form cations since they are more willing to give electrons away, so they are more reactive.

Re: 1F.19

Posted: Sun Oct 20, 2019 10:10 pm
by Michelle Song 1I
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.

Re: 1F.19

Posted: Sun Oct 20, 2019 10:11 pm
by Kevin Liu 1J
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!

Re: 1F.19

Posted: Sun Oct 20, 2019 10:11 pm
by Akshay Chellappa 1H
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.

Re: 1F.19

Posted: Sun Oct 20, 2019 10:13 pm
by Indy Bui 1l
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.