Whenever an alkali metal such as Lithium is hydrated/solvated, coordinate bonding occurs and it is the high hydration enthalpy of lithium which makes it the strongest reducing agent in aqueous solution. My question is, if lithium is hydrated and becomes surrounded by water molecules in coordinate bonding, then how does the overall reaction of adding lithium to water produce LiOH and H2(gas) ? Is the coordinated ion an intermediate product?
I also am wondering what happens to the "lost" electrons from the metal in coordinate bonding. Take Beryllium dissolving in water as an example. As it is hydrated it will lose the 2 valence electrons in its outer orbital and then it hybridizes its orbitals into 4 empty orbitals so that 4 molecules of water, supplying 1 lone pair each, can bond with the positive beryllium ion. Where did the original 2 electrons go? How do these electrons vanish in order to allow the hybridization of the 4 empty orbitals for water molecules to bond with?
And if Lithium is the strongest reducing agent in aqueous solution I assume it means it is reducing water itself, in order to create lithium hydroxide and hydrogen gas, but again, how does that come about from the coordinate bonding and the hydrated lithium? Coordinate bonds preserve the charge of the cation but I am not quite sure how this is so.
I have included an image below from a website that attempts to explain it, but I am confused about to where the original electrons go.
The website from which I took the image is: https://www.chemguide.co.uk/inorganic/group2/beryllium.html#top