5 posts • Page 1 of 1
s-block metals have lower ionization energies compared to p-block metals. Thus, due to their low ionization energies, s-block metals tend to form cations since they are more willing to give electrons away. Due to this, they are more reactive.
The p-block is actually mostly non-metals. Elements in the s-block have much lower ionization energies, so they give away electrons easily whereas the p-block elements have more filled shells, and are closer to having a full shell, so they are less likely to give away electrons as easily. Additionally, to achieve a noble gas electron configuration, elements in the s-block need only lose one or two electrons, so they are more reactive than the metals in the d-block. The comparison doesn't work for all the p-block elements - for example, flourine as the most electronegative is highly reactive.
It's also fairly important to consider that this isn't necessarily a trend. It's not like elements grow less reactive moving to the right towards the p-block or anything; in fact, the halogens are often very reactive as they very badly want to gain that one electron to fill an octet.
Since metals usually lose electrons in reactions, metals in the s-block have less electrons to lose and therefore are more likely to participate in a reaction. P-block metals have a few more electrons to lose to take part in a reaction and are less likely to form a compound or take part in a reaction.
Who is online
Users browsing this forum: No registered users and 1 guest