• Chemical bonding involves the forces that hold atoms together to form compounds.
• Ionic bonding occurs when electrons are transferred from one atom to another, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions are held together by electrostatic forces.
• Covalent bonding involves the sharing of electron pairs between atoms. It occurs between nonmetal atoms and results in the formation of molecules.
• Metallic bonding occurs in metals, where delocalized electrons are shared among a lattice of positive metal ions. This results in properties such as malleability, high thermal and electrical conductivity, and a metallic luster.
• Lewis dot structures are diagrams that represent the valence electrons of atoms in a molecule, allowing the prediction of molecular shapes and bond types.
• Valence Shell Electron Pair Repulsion (VSEPR) theory predicts the shapes of molecules based on the repulsion between electron pairs in the valence shell of an atom.
• Molecular shapes include linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral, among others.
• Intermolecular forces are attractive forces between molecules and affect properties such as boiling and melting points, solubility, and viscosity.
• Dipole-dipole forces occur between polar molecules and arise from the attraction between the positive end of one molecule and the negative end of another.
• Hydrogen bonding is a strong type of dipole-dipole interaction that occurs between hydrogen and highly electronegative atoms such as oxygen, nitrogen, or fluorine.
• London dispersion forces, also known as Van der Waals forces, are the weakest intermolecular forces and arise from temporary fluctuations in electron density, creating temporary dipoles.
• Crystalline solids have a regular, repeating arrangement of atoms or ions in a crystal lattice. They can be classified into ionic, covalent network, metallic, and molecular crystals.
• Ionic crystals consist of a three-dimensional array of cations and anions held together by electrostatic forces.
• Covalent network solids have an extended network of covalent bonds throughout the crystal structure, such as in diamond or quartz.
• Metallic crystals are formed by a lattice of positive metal ions surrounded by a sea of delocalized electrons.
• Molecular crystals are composed of individual molecules held together by intermolecular forces.
• Amorphous solids lack a long-range order and have a disordered arrangement of atoms or molecules.
• Polymers are large molecules made up of repeating subunits called monomers. They can have linear, branched, or cross-linked structures.