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How do you account for the strong reduci...

How do you account for the strong reducing power of lithium in aqueous solution?

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Lithium has most negative electrode potential (-3.04V) among alkali metals and hence it is the strongest reducing agent. This is mainly due to very high enthalpy of hydration in its aqueous solution.
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Knowledge Check

  • The Strongest reducing agent in aqueous solution is:

    A
    Na
    B
    Li
    C
    K
    D
    Cs

  • Strongest reducing agent in the aqueous solution is

    A
    Na
    B
    Rb
    C
    Ca
    D
    Li

  • Which of the following is the strongest reducing agent in aqueous solution ?

    A
    Na
    B
    Li
    C
    K
    D
    Cs.

    • Similar Questions

    Explore conceptually related problems

    Li is very strong reducing agent in aqueous solution because of -

    (a) How would you account for the following : (i) Cobalt (II) is stable in aqueous solution but in the presence of strong ligands, it is easily oxidised. (ii) The transition metals form interstitial compounds. (iii) Silver halides find use in photography. (b) What is lanthanoid contraction ? Mention its main consequences.

    The reducing power of a metal depends on various factors . Suggest the factor which makes Li, the strongest reducing agent in aqueous solution .

    The reducing power of a metal depends on various factors. Suggest the factor which makes Li, the strongest reducing agent in aqueous solution.

    The reducing power of a metal depends on various factors. Suggest the factor which makes Li metal the strongest reducing agent in aqueous solution:

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