'O' level chemistry: Reactivity Series.
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"A more reactive metal is able to reduce the ions of a less reactive metal"
Given so, a more reactive metal would be a reducing agent, and thus get oxidised (loss of electrons)
Would this rule apply in the same manner as it would in a solid state? Be it solid-solid, aqueous-aqueous, or solid-aqueous, the same rule would apply? That a more reactive metal will ALWAYS lose its electrons in the presence of a less reactive metal?
Also, would reactive metals prefer to stay as a solid or as an ion? I know it sounds wierd..but in electrolysis, we learn that the more reactive metals generally prefer to lose electrons and exist as an ion, and are preferentially reduced as compared to the less reactive metals..
Sorry for the long question, and thanks for any clarifications!
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solid = reduced state = atom
aqueous = oxidized state = cation
Reactive metals love to be in the oxidized state.
When we say a metal is "more reactive" than another, it means the more reactive metal has a higher oxidation potential, ie. potential/tendency to be oxidized, compared to a "less reactive" metal.
Hence a more reactive metal (in the solid, reduced, atomic form) oxidizes itself (into the aqueous, oxidized, cationic form), and the electrons lost in the process are accepted by a less reactive metal (in the aqueous, oxidized, cationic form), which is reduced as a result (into the solid, reduced, atomic form).
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my 2 cents...
your rule would only most probably apply to aqueous-solid. during a redox there must be transfer of electrons resulting in change of oxidation state, but if u put 2 solid metals side by side there is no way their oxidation state will change(from 0). aqueous aqueous state both metal species already exist in ions, neither has electrons to donate so there is no oxidising species present.
den...reactive metals...prefer to stay alone with a metal oxide on it LOL. thats all i know haha. very reactive metals such as Na will be oxidised by air quickly to form their oxides(in this way i guess it has lost electrons to form ionic bons alr -> existing as ions). so normally metals have a dull surface, thats because its their oxide layer on top. peel off the top surface and u will reveal e shiny metal underneath. the more reactive the metal is, the faster the oxide will form back once you've peeled off the top oxide layer. reactive metals are simply strong reducing agents(eager to donate off their valence electrons).
"[more reactive metals] are preferentially reduced as compared to the less reactive metals."
^i think you mean preferentially oxidised?
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