Explain the following :
(i) `Cu^(+)` is colourless and `Cu^(2+)` is coloured.
(ii) Zn shows only +2 oxidation state it its compounds.

Account for the following : Two S - O bond lengths in SO_(2) are equal. (ii) Fluorine shows only - 1 oxidation state in its compounds.

Why is Cu(II) ion coloured while Zn(II) ion is colourless in aqueous solution?

Explain the following : (i) Most of the transition elements show variable oxidation states. (ii) Many transition elements and their compounds are paramagnetic .

How many of the following show variable oxidation states in their compounds? Sc,Cr,Cu,Zn,Fe,Hg,La

Ions of Zn^(2+) and Ti^(4+) are colourless while Cu^(2+) and Ni^(2+) are coloured. Why?

Why Cu, Ni and Zn generally do not show oxidation state greater than 2?

(a) Account for the following : (i) Mn shows the highest oxidation state of +7 with oxygen but with fluorine it shows the highest oxidation state of +4. (ii) Cr^(2+) is a strong reducing agent. (iii) Cu^(2+) salts are coloured while Zn^(2+) salts are white. (b) Complete the following equations : (i) 2MnO_(2) + 4KOH + O_(2) overset(Delta)(to) (ii) Cr_(2)O_(7)^(2-) + 14H^(+)6I^(-) to