#Does reactivity increase down a group for metals full#
The outer shell will more easily attract another electron, which needs an electron to complete its full outer shell, when there is more attractive force.Ī useful mnemonic picture to help you recall that:Īs you go up group 7 (the halogens), again the elements get more reactive. The reactivity of metals increase as we go down in a group,for example-In group 1, Cesium is more reactive than sodium.
The fewer electron shells (rings) between the nucleus and the outer shell (ring) also has less shielding effect and again this increases the electron attraction. The distance "a" is less than "c" and the force of attraction between the nucleus and the outer shell increases with shorter distances. Halogens from bromide to fluorine get more reactive because the force of attraction between the nucleus (core) and the outer electron get stronger as you go up group 7 elements. Why do halogens get more reactive going upwards in group 7? The outer electron is more easily transferred to say an oxygen atom, which needs electrons to complete its full outer shell. The more electron shells (rings) between the nucleus and outer electron also creates shielding and again this weakens the nuclear attraction.
The distance "c" is greater than "a" and the force of attraction between the nucleus and the outer shell (rings) diminishes with distance. Why do alkali metals get more reactive going down group 1?Īlkali metals from lithium to potassium get more reactive because the force of attraction between the nucleus (core) and the outer electron gets weaker as you go down group 1 elements. As you go down group 1 (the alkali metals) in the periodic table, the elements get more reactive.Īs you go up group 7 (the halogens), again, the elements become more reactive.
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