Since the user did not select any specific options (ExplainAnswer, TeachTopic, or GeneratePractice are all false), I will provide the final answer directly based on the standard rules for assigning oxidation numbers shown in the worksheet.
The worksheet asks to determine the oxidation number assigned to each element in various chemical formulas. Although the specific formulas in the grid are blurry, the "Rules for Assigning Oxidation Numbers" box at the bottom is legible and provides the standard rules used in chemistry. I will list these rules clearly as the solution to understanding how to solve the problems in the grid.
Final Answer:
Here are the
Rules for Assigning Oxidation Numbers as listed in the worksheet, which you use to solve for the elements in the grids:
1. The oxidation number of any uncombined element is
0.
2. The oxidation number of a monatomic ion equals the
charge on the ion.
3. The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion.
4. The oxidation number of Fluorine in a compound is always
-1.
5. Oxygen has an oxidation number of
-2, unless it is combined with F (where it is +2), or it is in a peroxide (such as H₂O₂ or Na₂O₂), where it is
-1.
6. The oxidation state of Hydrogen in most of its compounds is
+1, unless it is combined with a metal, in which case it is
-1.
7. In compounds, the elements of groups 1 and 2 as well as Aluminum have oxidation numbers of
+1, +2, and +3 respectively.
8. The sum of the oxidation numbers of all atoms in a neutral compound is
0.
9. The sum of the oxidation numbers of all atoms in a polyatomic ion equals the
charge of the ion.
Parent Tip: Review the logic above to help your child master the concept of oxidation number worksheet.
