Assign oxidation numbers to each element in the following ions. (a) ClO3-

검증된 단계별 안내

Step 1: Understand the rules for assigning oxidation numbers. The sum of oxidation numbers in a polyatomic ion is equal to the charge of the ion.

Step 2: Assign the oxidation number for oxygen. Oxygen typically has an oxidation number of -2.

Step 3: Calculate the total oxidation number for all oxygen atoms. Since there are three oxygen atoms, the total is 3 * (-2) = -6.

Step 4: Let the oxidation number of chlorine be x. Set up the equation based on the sum of oxidation numbers: x + (-6) = -1 (the charge of the ion).

Step 5: Solve the equation for x to find the oxidation number of chlorine.

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Oxidation Numbers

Oxidation numbers are a way to keep track of electrons in chemical compounds. They indicate the degree of oxidation of an atom in a molecule, helping to determine how electrons are transferred in redox reactions. The oxidation number of an element can be positive, negative, or zero, depending on its electron gain or loss relative to its elemental state.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as: the oxidation number of an atom in its elemental form is zero; for monoatomic ions, it equals the charge of the ion; oxygen typically has an oxidation number of -2, and hydrogen is usually +1. These rules help in systematically determining the oxidation states of elements in compounds and ions.

Polyatomic Ions

Polyatomic ions are charged species composed of two or more atoms covalently bonded, which collectively carry a charge. In the case of ClO3-, known as the chlorate ion, the overall charge must be considered when assigning oxidation numbers to each constituent atom. Understanding the structure and charge of polyatomic ions is essential for correctly determining the oxidation states of their elements.