Explain chemical reactivity of transition metals. - Vidyadip

Question

Explain chemical reactivity of transition metals.

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Answer

→ Transition metals vary widely in their chemical reactivity.
→ Many of them are sufficiently electropositive to dissolve in mineral acids, although a few are 'noble' - that is, they are unaffected by simple acids.
→ The metals of the first series with the exception of copper are relatively more reactive and are oxidised by 1M H+, though the actual rate at which these metals react with oxidising agents like hydrogen ion (H+) is sometimes slow
. → The Eº values for M²⁺/M indicate a decreasing tendency to form divalent cations across the series
→ This general trend towards less negative Eº values is related to the increase in the sum of the first and second ionization enthalpies.
→ It is interesting to note that the $E ^{\ominus}$ values for $Mn , Ni$ and Zn are more negative than expected from the general trend.
→ An examination of the $E ^{\ominus}$ values for the redox couple $M ^{3+} / M ^{2+}$ shows that $Mn ^{3+}$ and $Co ^{3+}$ ions are the strongest oxidising agents in aqueous solutions. The ions $Ti ^{2+}, V ^{2+}$ and $Cr ^{2+}$ are strong reducing agents and will liberate hydrogen from a dilute acid, e.g.,
$2 Cr ^{2+}( aq )+2 H ^{+}( aq ) \rightarrow 2 Cr ^{3+}( aq )+ H _2(g)$

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