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 because, as explained previously, it is much easier to remove an outer shell. 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. The reactivity of the group 2 elements increase as you go down the group. 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). This makes it easier for the atom to give up the electron which increases its reactivity. Therefore, the attraction between the nucleus and the last electron gets weaker. The bigger the atom, the further away the last electron. The biggest atoms are at the bottom of the group so they are the most reactive. Why do metals become more reactive as you move down the periodic table As we go down the group, the atom gets bigger. 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?
Due to this, nuclear attraction to the valence electron. Group I metals are aiming to lose an electron from their outside shell. When we move from top to doon of periodic groups of metals, the atomic size increases gradually. 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. The answer lies in understanding what the atoms are trying to do.
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