Determine the oxidation number for the indicated element in each of the following compounds:(a) Co in LiCoO \(_{2}\), (b) Al in NaAlH\(_{4}\) (c) \(\mathrm{C}\) in \(\mathrm{CH}_{3} \mathrm{OH}\) (methanol), (d) \(\mathrm{N}\) in GaN, (e) Cl in \(\mathrm{HClO}_{2},\) (f) \(\mathrm{Cr}\) in \(\mathrm{BaCrO}_{4}\).

Redox chemistry, also known as oxidation-reduction chemistry, is a fundamental concept of chemistry involving the transfer of electrons between substances. It's a two-part process: oxidation, where an atom or molecule loses electrons, and reduction, where it gains electrons. The substance that loses electrons is said to be oxidized, while the substance that gains electrons is reduced. These reactions are essential to many natural and technological processes, such as cellular respiration, photosynthesis, and battery operations.

In a redox reaction, the total number of electrons lost is always equal to the number of electrons gained, maintaining the charge balance. This balance is crucial in determining the oxidation state of elements in chemical compounds, as seen in the provided textbook exercises.

The oxidation state, or oxidation number, is a concept in chemistry used to describe the degree of oxidation of an atom within a chemical compound. Determining the oxidation state of an element is a step-by-step process that depends on a set of rules. These rules include knowing the typical oxidation states of different elements - for example, hydrogen usually has an oxidation state of +1, oxygen typically has an oxidation state of -2, and alkali metals in compounds are often +1.

When determining oxidation states, it is important to know that the total oxidation state of a neutral compound is zero, and for polyatomic ions, it's equal to the charge of the ion. By using these rules, as in the provided steps for each compound in the exercise, students can correctly assign oxidation states. This process is essential for understanding redox reactions and many other chemical processes.

Chemical compounds are substances composed of two or more different types of atoms that are chemically bonded together. The properties of a compound are distinct from those of its constituent elements. In chemistry, understanding the composition and structure of compounds helps predict their behavior and interaction with other substances.

A key aspect of compounds is how atoms are oxidized or reduced within them. Each element in a compound has its own oxidation number, which helps in assessing the result of redox reactions. As seen in the workbook solutions, complex compounds like NaAlH₄ or BaCrO₄ have distinct oxidation states that contribute to their chemical properties and reactions they undergo. Understanding the distribution of oxidation states among the atoms of a compound is crucial for a comprehensive grasp of chemical reactions and bonding.