Questions: For the perchlorate ion ClO4-, what are the oxidation states of the Cl and O, respectively?

Transcript text: 7. For the perchlorate ion $\mathrm{ClO}_{4}{ }^{-}$, what are the oxidation states of the Cl and O , respectively? $+2,-1$ $+6,-2$ $-1,-2$ $+8,-2$ $+7,-2$

Solution

Solution Steps

Step 1: Determine the overall charge of the ion

The perchlorate ion, $\mathrm{ClO}_{4}^{-}$, has an overall charge of $-1$.

Step 2: Assign the oxidation state of oxygen

Oxygen typically has an oxidation state of $-2$.

Step 3: Calculate the total oxidation state contributed by oxygen

There are 4 oxygen atoms in $\mathrm{ClO}_{4}^{-}$. Therefore, the total oxidation state contributed by oxygen is: \[ 4 \times (-2) = -8 \]

Step 4: Determine the oxidation state of chlorine

Let the oxidation state of chlorine be $x$. The sum of the oxidation states in the ion must equal the overall charge of the ion, which is $-1$: \[ x + (-8) = -1 \] Solving for $x$: \[ x - 8 = -1 \implies x = +7 \]

Final Answer

\[ \boxed{+7, -2} \]

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