Answer:
Explanation:
<em><u>1. Identify the oxidation state of Cl in Cl₂O₇ . </u></em>
Cl₂O₇ is a neutral compound.
In a neutral compound the oxidation states add up 0.
The oxidation state of oxygen in all the binary compounds, except the peroxides (where two oxygen atoms are bonded together and with other elements) is -2.
Since there are 7 atoms of O, the total oxidation number from it is (-2) × 7 = -14.
Then, the oxidation number from the Cl atoms must add up +14 (because the compound is neutral).
Since there are two atoms of Cl each one must contribute with +14/2 = +7 to the oxidation number.
That is the oxidation state of Cl in the compound. The answer is +7.
<u><em>2 Identify the oxidation state of Cl in AlCl ₄⁻ (the formula was corrected)</em></u>
The most common oxidation state of Al is +3.
Since the net charge of the ion is -1, the oxidation number of the other atom (call it x) must be such that four times it and +3 add up -1:
In conclusion, the oxidation state of Cl in the ion is -1
<u><em>3. Identify the oxidation state of Cl in Ba (ClO₂)₂ . </em></u>
This is a neutral compound. Thus the overall oxidation number is 0.
The oxidation state of Barium, Ba, such as of the other members of the group 2, alkaline earth metals, is +2.
The oxydation state of oxygen, O, in ternary compounds is -2
Thus, calling x the oxidation state of Cl and taking in account the number of atoms in the compound:
Therefore, the oxidation state of Cl in this compound is +3
<u><em>4. Identify the oxidation state of Cl in ClF₄⁺</em></u>
Fluor has oxidation state -1. Since there are four atoms, it contributes with 4 × (-1) = - 4
The overall charge of the ion is +1.
Thus, the oxidation state of Cl, x, is:
Hence, the oxidation state of Cl in this ion is +5.
