The correct order of following 3d metal oxides, according to their oxidation numbers is :

(a) CrO₃, (b) Fe₂O₃, (c) MnO₂, (d) V₂O₅, (e) Cu₂O

(a) $\mathop C\limits^{ + 6} r{O_3}$ : Since there are three oxygen atoms each with an oxidation number of -2, the total oxidation number from the oxygen atoms is -6. To make the compound neutral, Chromium (Cr) must therefore have an oxidation number of +6. <br><br>(b) $\mathop {F{e_2}}\limits^{ + 3} {O_3}$ : Here, there are three oxygen atoms, contributing a total oxidation number of -6. To balance this, the total oxidation number for the two iron (Fe) atoms must be +6, meaning each Fe atom has an oxidation number of +3.<br><br>(c) $\mathop {Mn}\limits^{ + 4} {O_2}$ : With two oxygen atoms, the total oxidation number is -4. Thus, the manganese (Mn) atom must have an oxidation number of +4 to balance this.<br><br> (d) $\mathop {{V_2}}\limits^{ + 5} {O_5}$ : In this case, there are five oxygen atoms for a total oxidation number of -10. To balance this, the total oxidation number for the two vanadium (V) atoms must be +10, meaning each V atom has an oxidation number of +5.<br><br>(e) $\mathop {C{u_2}}\limits^{ + 1} O$ : Here, there's one oxygen atom with an oxidation number of -2. To balance this, the total oxidation number for the two copper (Cu) atoms must be +2, meaning each Cu atom has an oxidation number of +1. <br/><br/>So, the order of the oxidation numbers from highest to lowest is : <br/><br/>(a) CrO$_3$ > (d) V$_2$O$_5$ > (c) MnO$_2$ > (b) Fe$_2$O$_3$ > (e) Cu$_2$O. <br/><br/>Therefore, the answer is Option C : (a) > (d) > (c) > (b) > (e).