Reducing power of alkaline earth metals

In summary, the standard reduction potential of beryllium and magnesium is lower compared to heavier members of the group, while the opposite is true for the alkali group. This is due to the more negative hydration enthalpies of these metals. However, this should theoretically make oxidation of these metals more favorable, but it is not the case for beryllium and magnesium. This is because lithium is an anomaly with a high hydration enthalpy, while potassium, rubidium, and cesium have a lower SRP than sodium. It is also believed that the low reduction power of beryllium and magnesium can also be attributed to their high hydration enthalpies.
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Why is standard reduction potential of beryllium and magnesium lower as compared to heavier members of the group while the reverse is true for alkali group? I read somewhere that this is due to more negative hydration enthalpies of these metals but shouldn't it make oxidation of these metals more favoured?
 
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  • #3
Yes but my question was something else. I read in a book that reducing power of Li is due to its high hydration enthalpy. But somewhere else the authors also attributed the low reduction power of beryllium and magnesium to the same cause - high hydration enthalpy. Any ideas?
 

1. What is the reducing power of alkaline earth metals?

The reducing power of alkaline earth metals refers to their ability to donate electrons during a chemical reaction, resulting in the reduction of another element or compound. This is due to their low ionization energies and large atomic radii, which make it easier for them to lose electrons and form positive ions.

2. How does the reducing power of alkaline earth metals compare to other groups?

Alkaline earth metals have a higher reducing power compared to most other groups in the periodic table, with the exception of alkali metals. This is because they have a higher number of valence electrons, making it easier for them to lose electrons and form positive ions.

3. How does the reducing power of alkaline earth metals change down the group?

The reducing power of alkaline earth metals decreases down the group. This is because as we move down the group, the atomic size and ionization energy increase, making it more difficult for the elements to lose electrons and form positive ions.

4. What factors affect the reducing power of alkaline earth metals?

The reducing power of alkaline earth metals is affected by their atomic size, ionization energy, and electronegativity. Larger atomic size and lower ionization energy increase reducing power, while higher electronegativity decreases reducing power.

5. How is the reducing power of alkaline earth metals used in industries?

The reducing power of alkaline earth metals is used in various industries, such as metallurgy and pharmaceuticals. They are commonly used as reducing agents in the extraction of metals from their ores and in the production of certain drugs. They are also used in the production of alloys and as catalysts in chemical reactions.

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