Chemical Bonding Notes

Chapter 8: Basic Concepts of Chemical Bonding

General Overview of Chemical Bonds

  • Definition: Chemical bonds are forces that hold groups of atoms together, allowing them to function as a unit.

  • Formation: Bonds form when the energy of the aggregate is lower than that of separate atoms.

  • Bond Energy: Energy required to break a chemical bond.

  • Bonding involves

  • Valence electrons

  • Lowering energy levels of atoms

Types of Chemical Bonds

  • Ionic Bonds:

  • Involves the transfer of electrons from a metal (M) to a nonmetal (NM).

  • Resulting electrostatic attraction between cations and anions.

  • Covalent Bonds:

  • Formed by the sharing of electrons between atoms.

  • Nonpolar Covalent Bonds: Equal sharing of electrons (e.g., H2, Br2).

  • Polar Covalent Bonds: Unequal sharing of electrons, resulting in partial charges (e.g., HCl).

  • Metallic Bonds:

  • Formed by a "sea of electrons" that are shared among many atoms, which allows for conductivity and malleability.

  • Involves metal atoms that release some of their electrons, providing a collective pool that enhances attraction between positively charged metal ions and negatively charged electrons.

  • Examples include metals like copper (Cu), aluminum (Al), and iron (Fe).