CHEM 18.1 Discussion 1: Formulas and Nomenclature of Ionic and Covalent Compounds

Introduction to Symbols and Covalent CompoundsPage 1

Elements are represented by specific symbols based on their names, often derived from Greek, Latin, or German. Binary covalent compounds, formed by two non-metals, are named by identifying elements, using Greek prefixes (mono, di, tri, etc.) to indicate the number of atoms, and replacing the second element's suffix with -ide.

Ionic CompoundsPage 3

Ionic compounds form through electrostatic attraction between metal cations and nonmetal anions. Main group metals form cations based on group number, while nonmetals form anions by gaining electrons to fill valence shells, resulting in names ending in -ide. Transition metals often have multiple charges, denoted by the Stock system (Roman numerals) or common -ic/-ous endings.

Polyatomic Ions and HydratesPage 5

Polyatomic ions are covalently bonded groups with an overall charge. Hydrates are ionic compounds that incorporate specific ratios of water molecules, denoted in the name by a Greek prefix followed by 'hydrate' and represented in the formula with a centered dot.

Rules for Formulas and AcidsPage 8

Formulas for ionic compounds must be electrically neutral with the simplest whole-number ratios. Acids are named based on their composition: binary acids are named 'hydro-ic acid', while oxyacids are named based on their oxyanions, where '-ate' anions become '-ic acids' and '-ite' anions become '-ous acids'.