Alkaline earth group ionic hydroxides

The purely hydrogen-bonded structures range from the acids to the polyhydroxyl compounds such as carbohydrates. In contrast the alkali h3rdroxides are not hydrogen bonded to any extent, but resemble more closely ionic compounds with polarizable ions. Even in alkaline earth hydroxides, except those of beryllium, no true hydrogen bonds are formed, and it is only in the hydr oxides of the third group, which are of amphoteric character, that the hydrogen bonds reassert themselves [I]. 

Reactive electrodes refer mostly to metals from the alkaline (e.g., lithium, sodium) and the alkaline earth (e.g., calcium, magnesium) groups. These metals may react spontaneously with most of the nonaqueous polar solvents, salt anions containing elements in a high oxidation state (e.g., C104 , AsF6 , PF6 , SO CF ) and atmospheric components (02, C02, H20, N2). Note that ah the polar solvents have groups that may contain C—O, C—S, C—N, C—Cl, C—F, S—O, S—Cl, etc. These bonds can be attacked by active metals to form ionic species, and thus the electrode-solution reactions may produce reduction products that are more stable thermodynamically than the mother solution components. Consequently, active metals in nonaqueous systems are always covered by surface films [46], When introduced to the solutions, active metals are usually already covered by native films (formed by reactions with atmospheric species), and then these initial layers are substituted by surface species formed by the reduction of solution components [47], In most of these cases, the open circuit potentials of these metals reflect the potential of the M/MX/MZ+ half-cell, where MX refers to the metal salts/oxide/hydroxide/carbonates which comprise the surface films. The potential of this half-cell may be close to that of the M/Mz+ couple [48],... 

There are relahvely few common strong bases. The most common soluble strong bases are the ionic hydroxides of the alkali metals (group lA) and the heavier alkaline earth metals (group 2A), such as NaOH, KOH, and C a(OH)2. These compounds completely dissociate into ions in aqueous solution. Thus, a solution labeled 030 M NaOH consists of 0.30 M Na iaq) and 0.30 M OH aq) there is essentially no undisstKiated NaOH. 

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