Skip to main content
Chemistry LibreTexts

3: Chemical Bonding. Solubility

  • Page ID
    • 3.1: Chemical Bonds
      Chemical bonds form when electrons can be simultaneously close to two or more nuclei, but beyond this, there is no simple, easily understood theory that would not only explain why atoms bind together to form molecules, but would also predict the three-dimensional structures of the resulting compounds as well as the energies and other properties of the bonds themselves.
    • 3.2: Ionic Compounds: Formulas and Names
      Chemists use nomenclature rules to clearly name compounds. Ionic and molecular compounds are named using somewhat-different methods. Binary ionic compounds typically consist of a metal and a nonmetal. The name of the metal is written first, followed by the name of the nonmetal with its ending changed to –ide. For example, K2O is called potassium oxide. If the metal can form ions with different charges, a Roman numeral in parentheses follows the name of the metal to specify its charge.
    • 3.3: Molecular Compounds: Formulas and Names
      Molecular compounds can form compounds with different ratios of their elements, so prefixes are used to specify the numbers of atoms of each element in a molecule of the compound. Examples include SF6, sulfur hexafluoride, and N2O4, dinitrogen tetroxide. Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix hydro-, changing the –ide suffix to –ic, and adding “acid;” HCl is hydrochloric acid.
    • 3.4: Summary of Inorganic Nomenclature
      Chemical nomenclature is the names we use for chemicals. For instance, H2O is called "water", and CH4 (the gas you burn in a stove) is called "methane." You should learn the chemical nomenclature here on this page now, so that you will be able to understand when it is used.
    • 3.5: Lewis Structures and Covalent Bonding
    • 3.6: Predicting the Geometry of Molecules
    • 3.7: Intermolecular forces
    • 3.8: Solubility and Structure
    • 3.9: Metallic Bonding