Skip to main content
Chemistry LibreTexts

11: Intermolecular Forces and Liquids

  • Page ID
    41989
  • \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\)

    ualrimage_burned.png

     UALR 1403: General Chemistry II
    Belford: LibreText

    image.png
    Unit I: Matter           Unit II: Kinetics & Equilibria         Unit III: Acid/Base          Unit IV: Thermo & Electrochemistry

    • 11.0: Prelude
      Review of Van Arkel-Ketelaar diagram, Coulomb's Law and potential wells.
    • 11.1: States of Matter and Intermolecular Forces
      We have learned how chemistry is the study of matter and how matter transforms from one type of "stuff" into another. We have been introduced to 4 states of matter and the next two chapters will look at the condensed phases of matter, the solid and liquid states. We are going to start with a quick review, and then move into the cohesive forces that hold matter together.
    • 11.2: Ion-Dipole Forces
      Ion-Dipole Forces are involved in solutions where an ionic compound is dissolved into a polar solvent, like that of the solution of table salt (NaCl) into water. So these must be for solutions (and not pure substances).
    • 11.3: Dipole-Dipole Forces
      Dipole-Dipole interactions occur between polar molecules. Polar covalent bonds occur between atoms of different electronegativity, where the more electronegative atom attracts the electrons more than the electropositive atom. This results in a molecule where the center of positive charge (defined by the nuclei) does not coincide with the center of negative charge (defined by the electron orbitals).
    • 11.4: NonPolar Molecules and IMF
      Van der Waals interactions are very weak short range interactions involving non-polar molecules and are inversely proportional to the 6th power of the distance of separation. There are two types of IMF involving non-polar molecules.
    • 11.5: Hydrogen Bonds
      Hydrogen bonds are a strong type of dipole-dipole interaction. As a Rule of Thumb, they are weaker than covalent and ionic ("intramolecular") bonds", but stronger than most dipole-dipole interactions.
    • 11.6: Properties of Liquids
      Now that we have covered the basic Intermolecular Forces, we will cover some of the properties of liquids. These will include: Vaporization and Condensation Vapor Pressure Enthalpy of Vaporization, Clausius-Claperyron Equation Boiling Point Critical Temperature and Pressure Surface Tension, Capillary Action, and Viscosity


     

    The following box will aggregate annotations with the public hypothes.is tag of f21c1403c11: 


    This page titled 11: Intermolecular Forces and Liquids is shared under a not declared license and was authored, remixed, and/or curated by Robert Belford.

    • Was this article helpful?