Question

The oxidation states of iodine in $HI{O}_4,H_{3}I{O}_5$ and $H_{5}I{O}_6$ are respectively

• A. $+1,+3,+7$
• B. $+7,+7,+3$
• C. $+7,+7,+7$
• D. $+7,+5,+3$

Answer 1

The correct option is C $+7,+7,+7$

An oxidation state is a number that is assigned to an element in a chemical combination. This number represents the number of electrons that an atom can gain, lose, or share when chemically bonding with an atom of another element.

The total sum of the oxidation state of all atoms in any given species is equal to the net charge on that species. In neutral species, the total sum of the oxidation state of all atoms is $0$. The oxidation state of $H$ is $+1$ in a compound.The oxidation state of $O$ is $-2$ in a compound. Calculating the oxidation states of $I$, we get

$H_{5}I{O}_6;5+x-12=0$ or $x=+7$
$H_{3}I{O}_5;3+x-10=0$ or $x=+7$
$HI{O}_4;1+x-8=0$ or $x=+7$
Thus, the correct answer is $+7,+7,+7$