* Rules for Assigning Oxidation Numbers:
* The oxidation number of an element in its elemental form is 0.
* The oxidation number of a monatomic ion is equal to its charge.
* The sum of the oxidation numbers in a neutral compound is 0.
* The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.
* Fluorine has an oxidation number of -1 in its compounds.
* Oxygen has an oxidation number of -2 in its compounds, except in peroxides (where it is -1) and in compounds with fluorine (where it is positive).
* Hydrogen has an oxidation number of +1 in its compounds, except in metal hydrides (where it is -1).
* Group 1 elements have an oxidation number of +1.
* Group 2 elements have an oxidation number of +2.
* Group 17 elements (halogens) have an oxidation number of -1, except when combined with oxygen or another halogen higher in the group.
* Applying the Rules to AlBr3:
* Aluminum (Al) is in Group 3, so it usually has an oxidation number of +3.
* Bromine (Br) is in Group 17, and its oxidation number is typically -1.
* Calculating the Oxidation Numbers:
* Since AlBr3 is a neutral compound, the sum of the oxidation numbers must be 0.
* Let the oxidation number of Al be x and the oxidation number of Br be y.
* We have the equation: x + 3y = 0
* Substituting the known values: x + 3(-1) = 0
* Solving for x: x = +3
Therefore, the oxidation numbers in AlBr3 are:
* Al: +3
* Br: -1
