Write the proper name for \(\mathrm{Ca}(\mathrm{ClO})_{2} .\)

Chemical nomenclature is the systematic process of assigning names to chemical compounds. It is a critical part of chemistry that ensures clarity and precision when identifying substances. In the example given, \(\mathrm{Ca}(\mathrm{ClO})_{2}\), we are working with an ionic compound, which is composed of a metal (calcium) and a non-metal (hypochlorite ion). The naming convention for such compounds involves first stating the name of the metal, followed by the name of the non-metal or polyatomic ion.

The key is to use the root name of the non-metal with an appropriate suffix (like '-ide', '-ate', or '-ite') that indicates a specific type of ion. Hypochlorite is a polyatomic ion with a specific charge and composition, so its name is used directly after 'calcium' to complete the nomenclature. Hence, in our case, the name 'Calcium Hypochlorite' correctly represents the compound. Understanding these conventions not only helps in naming compounds but also in deducing the composition of a compound based on its name.

Polyatomic ions are charged species made up of two or more atoms covalently bonded together that function as a single ion. When identifying or naming compounds like \(\mathrm{Ca}(\mathrm{ClO})_{2}\), recognizing the polyatomic ions involved is crucial.

For example, the hypochlorite ion (\(\mathrm{ClO}^-\)) is the component in question here. These ions have characteristic names and oxidation states that need to be known for correct nomenclature and chemical formulations. It's important to note that the oxidation state of oxygen is typically -2, but in polyatomic ions, the combined charges add up differently. In hypochlorite, with one chlorine and one oxygen atom, the overall charge of the ion is -1, which affects how it combines with other ions, such as calcium (\(\mathrm{Ca}^{2+}\)) to form a neutral compound.

Oxidation states, also known as oxidation numbers, represent the degree of oxidation of an atom in a chemical compound. This concept is pivotal when balancing chemical equations and understanding reaction mechanisms. In the Calcium Hypochlorite example, calcium exhibits an oxidation state of +2, indicating it has lost two electrons, which is typical for its group in the periodic table.

The polyatomic ion hypochlorite has an overall -1 charge, meaning each oxygen atom has an assumed oxidation state of -2 and the chlorine is adjusted to balance the charge. When two hypochlorite ions bond with one calcium ion, their charges balance out (+2 from calcium and a total of -2 from the two hypochlorite ions), resulting in a neutrally charged compound. Remember that the sum of oxidation states for all atoms in a neutral compound must equal zero, which is a good check for correctly identifying and naming chemical compounds.