These are four questons and four answers:
Answers:
Explanation:
<u><em>Question 1) </em></u><u><em>Cl₂O₇:</em></u>
a) Net charge of the compound: 0
b) Rule: oxygen works with oxidation state +2, except with peroxides.
d) Rule: balance of charges: ∑ of the charges = net charge
Call X the oxidation number of Cl:
<em>Conclusion: the oxidation number of Cl in Cl₂O₇ is 7⁺.</em>
<u><em>Question 2) </em></u><u><em>AlCl₄⁻</em></u>
a) Net charge of the ion: - 1
b) Rule: common oxidation number of Al in compounds: +3
c) Rule: balance of charges: ∑ charges = net charge = - 1
<em>Conclusion: the oxidation number of Cl in AlCl₄⁻ is 1 ⁻.</em>
<em><u>Question 3)</u></em><em><u> Ba(ClO₂)₂</u></em>
a) Net charge of the compound: 0
b) Rule: common oxidation number of BA in compounds: +2
c) Rule: common oxidation number of O in compounds (except in peroxides): -2
d) Rule: balance of charges: ∑ charges = net charge = 0
<em>Conclusion: the oxidation number of Cl in Ba(ClO₂)₂ is 3⁺.</em>
<u><em>Question 4)</em></u><u><em> CIF₄⁺</em></u>
a) Net charge of the ion: + 1
b) Rule: common oxidation number of F : - 1 (it is the most electronegative)
c) Rule: balance of charges: ∑ charges = net charge = + 1
<em>Conclusion: the oxidation number of Cl in ClF₄⁺ is 5⁺.</em>
