Assertion: UF_6 is more covalent than UF_4.Re | vedclass

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(B) According to Fajan's rule,the covalent character of a compound increases with the increase in the oxidation state of the central metal atom. In $U

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Both Assertion & Reason are True but Reason is not a correct explanation of the Assertion.

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(B) According to Fajan's rule,the covalent character of a compound increases with the increase in the oxidation state of the central metal atom. In $UF_6$,the oxidation state of Uranium is $+6$,whereas in $UF_4$,it is $+4$. Since the oxidation state of $U$ in $UF_6$ is higher,it has higher polarizing power,making $UF_6$ more covalent than $UF_4$. The Reason states that Fluorine is smaller in size,which is a true statement,but it does not explain why $UF_6$ is more covalent than $UF_4$. The correct explanation relates to the oxidation state of the central metal atom.

Assertion: $UF_6$ is more covalent than $UF_4$.
Reason: Fluorine is smaller in size.

Similar Questions

Which of the following compounds is the most covalent?

The correct order of increasing ionic character is:

The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species,$K^{+}, Ca^{2+}, Mg^{2+}, Be^{2+}$?

$STATEMENT-1$: Boron always forms covalent bonds.
Because
$STATEMENT-2$: The small size of $B^{3+}$ favors the formation of covalent bonds.

Which of the following compounds exhibits covalent character?

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Assertion: $UF_6$ is more covalent than $UF_4$.Reason: Fluorine is smaller in size.