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The d-And-f-Block Elements

Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?

Both oxide and fluoride ions are highly electronegative and have a very small size. Due to these properties, they are able to oxidize the metal to its highest oxidation state.

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Silver atom has a completely filled d orbitals (4d¹⁰) in its ground state. How can you say that it is a transition element?

The E° (M²⁺/M) value for copper is positive (+ 0.34 V). What is possibility the reason for this?

How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of the transition elements?

In the series Sc (Z = 21) to Zn(Z = 30), the enthalpy of atomisation of zinc is the lowest i.e., 26, kJ mol. Why?

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