Group 1: Reactivity & Electronic Configurations (Edexcel GCSE Chemistry)

Group 1: Reactivity & Electronic Configurations

• The reactivity of the group 1 metals increases as you go down the group

• When a group 1 element reacts its atoms only need to lose electron, as there is only 1 electron in the outer shell

  • When this happens, 1+ ions are formed

• The next shell down automatically becomes the outermost shell and since it is already full, a group 1 ion obtains noble gas configuration

• As you go down group 1, the number of shells of electrons increases by 1

  • This means that the outermost electron gets further away from the nucleus, so there are weaker forces of attraction between the outermost electron and the nucleus

  • Less energy is required to overcome the force of attraction as it gets weaker, so the outer electron is lost more easily

  • So, the alkali metals get more reactive as you descend the group

These electron shell diagrams of the first 3 alkali metals show that the group 1 metals have 1 electron in their outer shell