Which of the following orders is correct?

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(D) $1$. $Cr^{+2}$ $(d^4)$ is a strong reducing agent because it changes to $Cr^{+3}$ ($d^3$,stable $t_{2g}^3$ configuration). $Fe^{+2}$ $(d^6)$ is a

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(D) $1$. $Cr^{+2}$ $(d^4)$ is a strong reducing agent because it changes to $Cr^{+3}$ ($d^3$,stable $t_{2g}^3$ configuration). $Fe^{+2}$ $(d^6)$ is a weaker reducing agent as it changes to $Fe^{+3}$ ($d^5$,stable half-filled configuration). Thus,$Cr^{+2} > Fe^{+2}$ is correct.$2$. $Mn^{+3}$ $(d^4)$ is a strong oxidising agent because it reduces to $Mn^{+2}$ ($d^5$,stable half-filled configuration). $Cr^{+3}$ $(d^3)$ is stable and does not easily reduce. Thus,$Mn^{+3} > Cr^{+3}$ is correct.$3$. In group $6$,stability of the highest oxidation state increases down the group. Therefore,$WO_3$ is more stable than $CrO_3$. Thus,$WO_3 > CrO_3$ is correct.

Column-$I$	Column-$II$
$(1)$ General electronic configuration of $d$-block elements	$(A)$ Transition elements
$(2)$ $d$-block elements	$(B)$ $(n-1)d^{1-10}ns^{1-2}$
$(3)$ Groups $3$ to $12$	$(C)$ $Z = 58$ to $71$
$(4)$ Lanthanoid elements	$(D)$ Last electron enters $d$-orbital

Similar Questions

The transition metals have a less tendency to form ions due to

Statement $(I)$ $Co^{2+}$ has a higher magnetic moment than $Cr^{3+}$.
Statement $(II)$ Ionisation enthalpies of $Ce$,$Pr$ and $Nd$ are higher than $Th$,$Pa$ and $U$.
Which of the following is correct?

Identify the $incorrect$ order of the given parameter.

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