Determine the oxidation number for the indicated element in each of the following substances: (f) Cl in NaClO4.

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Identify the oxidation number of each element in the compound NaClO₄. Sodium (Na) is in Group 1 of the periodic table, so it has an oxidation number of +1.

Oxygen (O) typically has an oxidation number of -2. Since there are four oxygen atoms, the total contribution from oxygen is 4(-2) = -8.

Let the oxidation number of chlorine (Cl) be x. Write the equation for the sum of oxidation numbers in the compound: +1 (for Na) + x (for Cl) + 4(-2) (for O) = 0.

Simplify the equation: 1 + x - 8 = 0.

Solve for x to find the oxidation number of Cl.

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Oxidation Number

The oxidation number, or oxidation state, is a value assigned to an element in a compound that reflects its degree of oxidation or reduction. It indicates the number of electrons an atom gains, loses, or shares when forming chemical bonds. Oxidation numbers are crucial for understanding redox reactions and determining the electron flow in chemical processes.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as the fact that the oxidation number of an element in its elemental form is zero, and for monoatomic ions, it equals the charge of the ion. In compounds, the sum of the oxidation numbers must equal the overall charge of the compound. These rules help in systematically determining the oxidation states of elements in various compounds.

Chlorine Compounds and Oxidation States

Chlorine can exhibit multiple oxidation states, commonly ranging from -1 to +7. In compounds like NaClO4, chlorine typically has a positive oxidation state due to its bonding with more electronegative elements like oxygen. Understanding the common oxidation states of chlorine is essential for accurately determining its oxidation number in different chemical contexts.