[cliverlong]

Hello is the following true?

Given: The oxidizing power of halogens decreases as the group is descended from Fluorine to Iodine. This is because a strong oxidizing agent attracts electrons strongly to itself and Fluorine is most able to do this because few electrons shielding the nucleus

Given: The reducing power of hydrogen halides increases as the group is descended from Fluorine to Iodine. This is because a strong reducing agent wants to lose electrons strongly

So is the following conclusion correct? The equlibrium

I^- <> I + e^- lies to the right
F^- <> F + e^- lies strongly to the left

Hence in the case of HI the I^- in molecule "wants" to form Iodine, hence it wants to lose its electrons by giving them to some other atom or ion or molecule. The recipient is more easily reduced than if HF was used as the reducing agent.

So is the following true ?

If X is a strong oxidizing agent then HX is a weak reducing agent?
If Y is a weak oxidizing agent then HY is a strong reducing agent?
(for any X or Y)


Thanks

Clive

[Joniaguis]

Apart from the fact that Fluorine has few electrons shielding the nucleus, the great oxidizing power of Fluorine is due to its low enthalpy of atomistaion and mainly because the small F- ion produces a large enthalpy of hydration in aqueous reactions and a large lattice enthalpy in case of the formation of an ionic compound.

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