Assign oxidation numbers to each element in the following ions. (d) MnO4 2-

Verified step by step guidance

1. Step 1: Recall the rules for assigning oxidation numbers. Oxygen typically has an oxidation number of -2.
2. Step 2: Let the oxidation number of manganese (Mn) be x.
3. Step 3: Write the equation for the sum of oxidation numbers in the ion: x + 4(-2) = -2.
4. Step 4: Simplify the equation: x - 8 = -2.
5. Step 5: Solve for x to find the oxidation number of Mn.

Key Concepts

Oxidation Numbers

Oxidation numbers are a way to keep track of electron transfer in chemical reactions. They represent the hypothetical charge an atom would have if all bonds were ionic. Assigning oxidation numbers helps in identifying the oxidation state of elements in compounds and ions, which is crucial for understanding redox reactions.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as: the oxidation number of an element in its standard state is zero, the oxidation number of a monoatomic ion is equal to its charge, and in compounds, the sum of oxidation numbers must equal the overall charge of the compound or ion. These rules provide a systematic approach to determine oxidation states.

Polyatomic Ions

Polyatomic ions are charged species composed of two or more atoms covalently bonded together, which collectively carry a charge. In the case of MnO4 2-, the ion consists of manganese and oxygen atoms, and understanding the oxidation states of each element within the ion is essential for determining the overall charge and behavior of the ion in chemical reactions.