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(D) The correct option is $D$.We calculate the oxidation state $(x)$ for the metal in each compound:$(i)$ In $K_2CrO_4$: $2(+1) + x + 4(-2) = 0 \impli

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$Cr$

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(D) The correct option is $D$.We calculate the oxidation state $(x)$ for the metal in each compound:$(i)$ In $K_2CrO_4$: $2(+1) + x + 4(-2) = 0 \implies 2 + x - 8 = 0 \implies x = +6$.The oxidation state of $Cr$ is $+6$.$(ii)$ In $NbCl_5$: $x + 5(-1) = 0 \implies x - 5 = 0 \implies x = +5$.The oxidation state of $Nb$ is $+5$.$(iii)$ In $MnO_2$: $x + 2(-2) = 0 \implies x - 4 = 0 \implies x = +4$.The oxidation state of $Mn$ is $+4$.Comparing the values $(+6, +5, +4)$,$Cr$ has the highest oxidation state.

List-$I$	List-$II$
$(1)$ $Ti^+$	$(A)$ $(n-1)d^4ns^2$
$(2)$ $_{30}Zn$	$(B)$ $(n-1)d^{10}ns^1$
$(3)$ $_{24}Cr$	$(C)$ $(n-1)d^2ns^0$
$(4)$ $_{29}Cu$	$(D)$ $(n-1)d^5ns^1$
	$(E)$ $(n-1)d^0ns^2$
	$(F)$ $(n-1)d^{10}ns^2$

Atom/Ion	Electronic Configuration
$(1) \ Cu$	$(A) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^{10}$
$(2) \ Cu^{2+}$	$(B) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^{10}, 4s^2$
$(3) \ Zn^{2+}$	$(C) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^{10}, 4s^1$
$(4) \ Cr^{3+}$	$(D) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^9$
	$(E) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^3$

The metal with the highest oxidation state present in $K_2CrO_4$,$NbCl_5$,and $MnO_2$ is

Similar Questions

Match the elements in List-$I$ with their electronic configurations in List-$II$.

List-$I$ List-$II$

$(1)$ $Ti^+$ $(A)$ $(n-1)d^4ns^2$

$(2)$ $_{30}Zn$ $(B)$ $(n-1)d^{10}ns^1$

$(3)$ $_{24}Cr$ $(C)$ $(n-1)d^2ns^0$

$(4)$ $_{29}Cu$ $(D)$ $(n-1)d^5ns^1$

$(E)$ $(n-1)d^0ns^2$

$(F)$ $(n-1)d^{10}ns^2$

Which of the following ions is diamagnetic?

Which of the following ions exhibits a $3d^0 4s^0$ electronic configuration?

Cuprous ion is colourless,while cupric ion is coloured because

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