MadSci Network: Chemistry |
Rich, In regards to displacement reactions with water to produce hydrogen gas and the activity series, I believe the answer lies in the periodic table and electrochemistry. Historically, the IA metals are most reactive. Compared to IA metal ions, IIA metal ions have higher ionic charge-to-size ratios. Because of this, their energy of hydration is about 5 times higher than the cooresponding IA ion in the same row or period. So Mg, for instance, will have a lot of covalent character and will tend to complex with water instead of ionically bonding with it. The trend of ionization potential as well as standard electrode potentials mimic the energy of hydration trends, especially down a family or group... Electrochemically, any metal with a negative standard reduction electrode potential (more negative than -.8 volts which is where water reduces) will have a tendency to reduce water to hydrogen gas. Note that Li, Na, K, and Mg all fall into this catagory. Magnesium should not, but recognize that it DOES react with water with energy (THE WATER MUST BE BOILING). The above data helps explain the trend of how the IIA metals interact with water: Beryllium does not react (weakest reducing agent), whereas magnesium will react in boiling water, and the rest will react with ease (in cold water), especially barium which is the strongest reducing agent of the group.
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