s-block vs p-block

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s-block vs p-block

Postby MichelleTran3I » Thu Nov 09, 2017 1:31 am

Why are s-block metals typically more reactive than p-block metals?

William Lan 2l
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Re: s-block vs p-block

Postby William Lan 2l » Thu Nov 09, 2017 2:45 am

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.

Pooja Nair 1C
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Re: s-block vs p-block

Postby Pooja Nair 1C » Tue Nov 14, 2017 12:54 pm

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.

Salman Azfar 1K
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Re: s-block vs p-block

Postby Salman Azfar 1K » Tue Nov 14, 2017 2:40 pm

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.

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Re: s-block vs p-block

Postby mayasinha1B » Tue Nov 14, 2017 3:18 pm

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.

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