![]() So, large group I metal atoms are the most reactive and large halogens are the least reactive. Group I metals want to lose an electron while halogen atoms want to gain an electron. The small atoms are at the top of the groups. This is best when the atom is as small as possible and so fluorine is the most reactive of the halogens.īreak the idea down into clar statements:Īttraction between nucleus and electron is greatest for small atoms. This extra electron is held tightest when it is placed in a shell close to the nucleus. The halogens react by gaining an electron to form the halide ion (eg chlorine becomes chloride). The biggest atoms are at the bottom of the group so they are the most reactive. This can happen easiest if the electron is in a shell that is a long ay from the nucleus so that there is less attraction between the nucleus and the electron. Group I metals are aiming to lose an electron from their outside shell. The answer lies in understanding what the atoms are trying to do. I get why it does in group 1, but I don't get why it does in group 7? For instance, when we go from top to bottom in group 1, the size of the atoms gradually rises from lithium to francium.Why do the reactivity of the group 1 atoms increase as you go down the group, but the reactivity of group 7 decreases as you go down the group.
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