(D) The element that can exhibit oxidation states ranging from $+4$ to $+6$ is chromium $(Cr)$.Chromium has an electronic configuration of $[Ar] 3d^5

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(D) The element that can exhibit oxidation states ranging from $+4$ to $+6$ is chromium $(Cr)$.Chromium has an electronic configuration of $[Ar] 3d^5 4s^1$.It can show various oxidation states from $+1$ to $+6$ in its compounds,such as in $CrO_2$ $(+4)$ and $CrO_3$ $(+6)$.

Class 12 Chemistry d-and f-Block Elements Chemical properties

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Which element can have oxidation state from $4$ to $6$?

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A
$Fe$
B
$Mg$
C
$Co$
D
$Cr$

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d-and f-Block Elements

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Chemical properties

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The compound $AgF_2$ is an unstable compound. However,if formed,the compound acts as a very strong oxidizing agent. Why?

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What is the correct order of basic character for the following transition metal monoxides?

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Assertion : $PbI_4, BiCl_5, FeI_3, CuI_2$ do not exist. Reason : Higher oxidation states of metal ions are strong oxidising agents which give redox reactions with the iodide ion.

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Assertion $(A):$ $VF_5$ is stable while $VCl_5$ is not.
Reason $(R):$ Fluorine stabilizes the higher oxidation state due to its higher bond enthalpy.
The correct option among the following is

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Ferrous sulphate on heating gives

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Which element can have oxidation state from $4$ to $6$?

Similar Questions

The compound $AgF_2$ is an unstable compound. However,if formed,the compound acts as a very strong oxidizing agent. Why?

What is the correct order of basic character for the following transition metal monoxides?

Assertion : $PbI_4, BiCl_5, FeI_3, CuI_2$ do not exist. Reason : Higher oxidation states of metal ions are strong oxidising agents which give redox reactions with the iodide ion.

Assertion $(A):$ $VF_5$ is stable while $VCl_5$ is not.Reason $(R):$ Fluorine stabilizes the higher oxidation state due to its higher bond enthalpy.The correct option among the following is

Ferrous sulphate on heating gives

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Assertion $(A):$ $VF_5$ is stable while $VCl_5$ is not.
Reason $(R):$ Fluorine stabilizes the higher oxidation state due to its higher bond enthalpy.
The correct option among the following is