Explanation
Correct option: $$D$$
Explanation:
Step: 1 calculate the oxidation state of central atom$$ Mn$$ In $$MnO_4^{-}$$
Let us assume the $$oxidation$$ $$state$$ of $$Mn$$ be x.
Overall charge on the complex: $$−1$$
Thus, $$Mn + 4 \times O = - 1$$
$$x+4(−2) = −1$$ ($$O$$ has $$-2$$ charge )
So, $$x=+7$$
Hence, the $$oxidation$$ $$state$$ is $$+7$$.
Step: 2 calculate the oxidation state of central atom $$Cr$$ In $$\left [ Cr\left ( CN \right )_6 \right ]^{3-}$$
Let us assume the $$oxidation$$ $$state$$ of $$Cr$$ be x.
Overall charge on the complex: $$−3$$
Thus, $$Cr + 6 \times CN = -1 $$
$$x+6(−1) = −3$$ (Where $$CN$$ has $$-1$$ overall charge )
So, $$x=+3$$
Hence, the $$oxidation$$ $$state$$ is $$+3$$.
Step: 3 calculate the oxidation state of central atom $$Cr$$ In $$Cr_2O_3$$
Overall charge on the complex: $$0$$
Thus, $$2 \times Cr + 3 \times O = 0$$
$$2x+3(−2) = 0$$ ($$O$$ has $$-2$$ charge )
Step: 4 calculate the oxidation state of central atom $$Cr$$ In $$CrO_2Cl_2$$
Thus, $$1 \times Cr + 2 \times O + 2 \times Cl$$
$$x+2(−2)-2 = 0$$ ($$O$$ has $$-2$$ charge while $$Cl$$ has $$-1$$ charge)
So,$$x=+6$$
Hence, the $$oxidation$$ $$state$$ is $$+6$$.
Hence, the species having oxidation state of $$+6$$ is $$CrO_2Cl_2$$.
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