Chemistry - Electron configuration and periodic classification: the group
Electron configuration and periodic classification: the group relationship
Although there is often wide variation in chemical properties across a
period, e.g. across period 3 from solid metallic sodium to gaseous
non-metallic chlorine, the contain elements with
The reactivity of the group I metals actually increases going down the
group from Li to Cs. In all of these elements, the outer-shell electron is
experiencing an effective attractive (core) charge of +1.
However, as you go down the group, the outer-shell electron of each
successive element moves further from the nucleus (because there are more
shells) and so is more easily removed. This makes the element more
Because these metals act as reductants, i.e. give up their valence
electron, or electrons and the valence electron is given up more easily
going down the group, the reducing strength of the metals also increases
going down the group.
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