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Why are Group 1 metals more reactive as you go down but Halogens are the opposite?

I'm confused:confused:. I meant down the periodic table.
(edited 9 years ago)
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Avatar for zak7399
zak7399
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Original post by Ben Johnson
I'm confused:confused:. I meant down the periodic table.


Hi its to do with the position of the electrons on the shells. As you go down group 1 the electrons become further away from the nucleus so there is less attraction , meaning electrons are lost more easily ; its the other way round for halogens.
Original post by zak7399
Hi its to do with the position of the electrons on the shells. As you go down group 1 the electrons become further away from the nucleus so there is less attraction , meaning electrons are lost more easily ; its the other way round for halogens.


Original post by Ben Johnson
I'm confused:confused:. I meant down the periodic table.


The decrease in reactivity of the halogens is more to do with the decrease in electronegativity down the group. Fluorine is the most electronegative element so it can rip electrons of almost anything making it very reactive
Reply 3
Avatar for Ben Johnson
Ben Johnson
OP
2
Original post by langlitz
The decrease in reactivity of the halogens is more to do with the decrease in electronegativity down the group. Fluorine is the most electronegative element so it can rip electrons of almost anything making it very reactive


Thanks. So will all non-metals (except for noble gases of course) be less reactive as you go down the table or just the halogens?
(edited 9 years ago)
Original post by Ben Johnson
Thanks. So will all non-metals (except for noble gases of course) be less reactive as you go down the table or just the halogens?


That's not necessarily true, there are other factors which will have an effect. But in general yes you could say that

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