The d-And-f-Block Elements

Short Answer Type

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How is the variability in the oxidation states of transition metals different from that of the nontransition metals? Illustrate with examples.

The various oxidation states of transition metals have the unique property, that the different oxidation states differ by a difference of one unit for example Fe (Fe2+, Fe3+), Cu(Cu2+, Cu+), Ti(Ti3+, Ti4+), Co(Co2+, Co3+), Mn(Mn+2, Mn+3, Mn+4, Mn+7) etc.
But in the non-transition metals, oxidation states differs by the difference of two, e.g., Pb(Pb2+, Pb4+), Sn(Sn4+, Sn2+), Ti(Ti3+, Ti+).
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    Assign reasons for the following:
    The enthalpies of atomisation of transition metals are high.

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    What is the reason for the decreasing tendency to form divalent cation across the series as indicated by the decreasing E°M2+ /M values?
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    What are inner transition elements? Write their general electronic configuration.
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    Why the transition element series show fewer oxidation states at their extreme ends e.g., Sc, Ti, Ni and Cu.
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    Long Answer Type

    What are paramagnetic and ferromagnetic substances? Account for the paramagnetic character of transition metal compounds. How does the paramagnetic character of the bivalent ions of first transition metal series vary from titanium (Z = 22) to copper (Z = 29)?
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    Short Answer Type

    In what way are the observed oxidation states of the lanthanides related to their electronic configurations?

     
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    Why are the absorption bonds of lanthanoids narrow
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    Long Answer Type

    Describe the general characteristics of the transition elements with special reference to their tendency to:
    (i)    Exhibit paramagnetism.
    (ii)    Form complex compounds.
    (iii)    Their catalytic behaviour.

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    Short Answer Type

    Why are transition metals able to form alloys?

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