[20] Beryllium dissolves readily in non-oxidizing acids, such as HCl and diluted H2SO4, but not in nitric as this forms the oxide and this behavior is similar to that of aluminium metal.

Beryllium, again similarly to aluminium, dissolves in warm alkali to form the beryllate anion,

Be(OH)42−, and hydrogen gas.

Beryllium hydrolysis as a function of pH
Water molecules attached to Be are omitted
The beryllium atom has the electronic configuration [He] 2s2.

In beryllium compounds the two electrons are lost and beryllium is in the +2 oxidation state;

the only evidence of lower valence of beryllium is in the solubility of the metal in BeCl2.

[21] The small atomic radius ensures that the Be2+ ion is polarizing leading to significant covalent character in beryllium's bonding.

[20] Beryllium is 4 coordinate in virtually all of its derivatives, e.g. [Be(H2O)4]2+ and tetrahaloberyllates, BeX42−.

This characteristic is used in analytical techniques using EDTA as a ligand which preferentially forms octahedral complexes

– thus absorbing other cations such as Al3+ which might interfere, for example in the solvent extraction of a complex formed between Be2+ and acetylacetone.

[22]
Solutions of beryllium salts, e.g. beryllium sulfate and beryllium nitrate, are acidic because of hydrolysis of the [Be(H2O)4]2+ ion.

[Be(H2O)4]2+ + H2O [Be(H2O)3(OH)]+ + H3O+
Other products of hydrolysis include the trimeric ion [Be3(OH)3(H2O)6]3+.

Beryllium hydroxide, Be(OH)2, is insoluble even in acidic solutions with pH less than 6.

This means that it is insoluble at biological pH.

It is amphoteric and dissolves in strongly alkaline solutions.