Reactivity of alkaline earth metals towards water In general, it seems to be a trend regarding the reactivity of alkaline metals with water which says that as you go down the group, they become more reactive towards water. But I'm curious about which factors explain this trend.

When Group 2 metals react to form oxides or hydroxides, metal ions are formed.So this must be explained by the atomization energy of the metal and also the first and second ionization energies?(Ionization energies fall down the group, it gets easier to form the ions, the reactions will happen more quickly.)

But apart from these two factors, should we also take into consideration the atomic radius, the hydration energy, the ionic radius or something else in order to fully understand why the reactivity towards water increases as we go down the group?  Also,  do the standard potential value has to do with it?
Do not forget solubility effects involving the hydroxide product.  Magnesium is plenty electropositive enough to decompose water, only to passivate with a hydroxide that has limited solubility (you can detect the presence of some reaction by decanting the liquid and then adding phenolphthalein, or by carefully looking for a few hydrogen bubbles during the reaction).  Put magnesium in methanol, which is less protic than water; the methoxide is less passivating and you can actually bring the alcohol to a boil!  See https://www.google.com/url?sa=t&amp;source=web&amp;rct=j&amp;url=https://m.youtube.com/watch%3Fv%3DNMfs3e9OdZQ&amp;ved=0ahUKEwjlnLOxpPDWAhVDKiYKHVFwB5wQwqsBCCgwAA&amp;usg=AOvVaw2TaAZjVq0m8EHL-JluhxGn.