+91-8076753736 support@wiredfaculty.com
logo
logo

Sponsor Area

The D-And-f-Block Elements

Question
CBSEENCH12007210
Wired Faculty App

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

Solution
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+).

Some More Questions From The d-And-f-Block Elements Chapter

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

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?

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?

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

Which is a stronger reducing agent Cr2+ or Fe2+ and why?

Explain why Cu+ ion is not stable in aqueous solutions?

Actinoid contraction is greater from element to element than lanthanoid contraction. Why?

On what ground can you say that scandium (Z = 21) is a transition element but zinc (Z = 30) is not?

Mock Test Series

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation