6. What is the oxidation number of Cl in \( \mathrm{ClO}_{2}{ }^{1} \) ? You number.

In the chlorite ion, \( \mathrm{ClO}_{2}^{1} \), you can determine the oxidation number of chlorine (Cl) by applying the rule that the sum of oxidation states in the ion must equal the overall charge. Oxygen typically has an oxidation state of -2, and since there are two oxygen atoms, that contributes -4 to the overall charge. Based on the charge of the ion being -1, the oxidation number of chlorine can be calculated as follows: Let \( x \) be the oxidation number of Cl. Thus, the equation looks like this: \( x + 2(-2) = -1 \) This simplifies to \( x - 4 = -1 \), leading to \( x = +3 \). Hence, the oxidation number of Cl in \( \mathrm{ClO}_{2}^{1} \) is +3. For a fun twist, think of Cl as the middle manager trying to keep the team (the oxygen atoms) in check. It jumps into action with a +3 mindset to balance everything out and ensure the whole ion stays positive despite the odds!