The reactivity of Group 1A alkali metals inorganic compounds can be predicted based on their electronic configuration. Alkali metals have one electron in their outermost energy level s-orbital , which makes them highly reactive. This is because they have a strong tendency to lose this single electron to achieve a stable, full outer electron shell, forming a +1 cation.As we move down the group from lithium to francium , the reactivity increases. This is due to the increase in atomic size and the decrease in ionization energy. As the atomic size increases, the outermost electron is further away from the nucleus and less tightly held by the positive charge of the protons. This makes it easier for the electron to be lost in a chemical reaction, resulting in a more reactive alkali metal.In summary, the electronic configuration of Group 1A alkali metals leads to high reactivity, with reactivity increasing as we move down the group. These metals readily form inorganic compounds, such as ionic salts, by reacting with nonmetals like halogens, oxygen, and sulfur.