Explain the following observations:
(i) Transition elements are known to form many interstitial compounds..
(ii) With the same `d^4` configuration `Cr^(2+)` ion is reducing while `Mn^(3+)` ion is oxidising.
(iii) The enthalpies of atomization of the transition elements are quite high.

Explain the following observation : (i) Transition elements generally form coloured compounds. (ii) Zinc is not regaded as a transition element.

Explain the following observations : (i) Many of the transition elements are known to form interstitial compounds . (ii) There is a general increase in density from titanium (Z =22) to copper (Z = 29). (iii) The members of the actinoid series exhibit a larger number of oxidation states than the corresponding members of the lanthanoid series.

Assertion : Cr^(2+) is reducing and Mn^(3+) is oxidising. Reason : Cr^(2+) and Mn^(3+) have d^4 configuration.

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^(4) configuration ?

Why is Cr^(2+) reducing and Mn^(3+) oxidising when both have d^4 configuration?

Explain the following : (i) Why do transition metal ions possess a greater elements increases upto Mn and then decrease.

Explain the following : The paramagnetic character in 3d-transition series elements increases upto Mn and then decreases.

How would you account for the following ? (i) Many of the transition elements are known to form interstitial compounds. (ii) The metallic radii of the third (5d) series of transition metals are virtually the same as those of the correponding group members of the second (4d) series.

Explain why: (i) Transition elements form coloured compounds. (ii) Cu^(+) is diamagnetic but Cu^(2+) is paramagnetic (Z=29)

Among the following series of transition metal ions the one where all metal ions have 3d^2 electronic configuration is