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Intermolecular Forces (Simplified) definitions

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  • Intermolecular Forces
    Electrostatic attractions between molecules that influence physical properties like boiling and melting points.
  • Intramolecular Forces
    Strong attractions within a molecule that hold atoms together, determining chemical properties and bond types.
  • Ion-Dipole
    Strongest attraction between an ion and a polar molecule, crucial in dissolving ionic compounds in water.
  • Hydrogen Bonding
    Special attraction between hydrogen and fluorine, oxygen, or nitrogen, significantly affecting water's properties.
  • Dipole-Dipole
    Attraction between polar molecules due to partial positive and negative charges aligning with each other.
  • London Dispersion Forces
    Weak, temporary attractions from momentary dipoles in all molecules, especially significant in nonpolar substances.
  • Polarity
    Uneven distribution of electron density in a molecule, leading to partial positive and negative regions.
  • Electronegativity
    Tendency of an atom to attract electrons in a bond, creating partial charges and influencing molecular interactions.
  • Aqueous Solution
    Mixture where a substance is dissolved in water, allowing ions to interact with water molecules.
  • Solvation
    Process where solvent molecules surround and interact with solute particles, stabilizing them in solution.
  • Partial Charge
    Slight positive or negative character on atoms within a molecule due to unequal electron sharing.
  • Van der Waals Forces
    General term for weak attractions, including London dispersion, present in all molecular interactions.
  • Covalent Bond
    Strong connection formed by sharing electrons between atoms within a molecule, influencing chemical structure.
  • Ionic Compound
    Substance composed of positive and negative ions held together by strong electrostatic attractions.
  • Physical Properties
    Characteristics like boiling point and melting point, determined by the strength of attractions between molecules.