Chapter 6: Intermolecular Forces- Attractions between Particles

Chapter 6: Intermolecular Forces- Attractions between Particles

1. 6.3 Trends in Solubility

   • Solvent
     • defined as: the component of a solution for which the largest number of moles is present
   • Hydrophillic
     • defined as: describes a "water-loving" or attractive solute & water that increases water solubility
   • Solute
     • defined as: any component in a solution other than the solvent. A solution may contain one or more solutes
   • Solubility
     • defined as: the maximum quantity of a substance that can dissolve in a given volume of solution
   • Miscible
     • defined as: liquids that are mutually soluble in any proportion
   • Dipole-Induced Dipole Interaction
     • defined as: an attraction between a polar and the oppositely charged pole it causes in another molecule
   • Hydrophobic
     • defined as: describes a "water-fearing" or repulsive interaction between a solute & water that decreases water solubility

2. 6.1 London Dispersion Forces: They're Everywhere

   • Viscosity
     • defined as: a measure of the resistance to flow of a fluid
   • Polarizability
     • defined as: the relative ease with which the electron cloud in a molecule, ion, or atom can be distorted, inducing a temporary dipole
   • Temporary Dipole
     • London Dispersion Force
       • defined as: an intermolecular force between atoms or molecules caused by the presence of temporary dipoles in the molecules
       • Interaction based on the presence of temporary dipoles (in honor of Fritz London's work)
     • defined as: the separation of charge produced in atom or molecule by a momentary uneven distribution of electrons; also called induced dipole.
   • Hydrocarbon
     • Alkane
       • defined as: a hydrocarbon in which each carbon atom is bonded to four other carbbon or hydrogen atoms
       • Is a particular hydrocarbon
     • defined as: an organic compound whose molecules contains only carbon & hydrogen atoms
   • Constitutional Isomer
     • defined as: one of a set of compounds with the same molecular formula but different connections between the atoms in their molecules; also called structural isomer

3. 6.5 Some Remarkable Properties of Water

   • Surface Tension
     • defined as: the ability of the suface of a liquid to resist an external force
   • Meniscus
     • defined as: the concave or convex surface of a liquid
   • Capillary Action
     • defined as: the rise of a liquid in a narrow tude as a result of adhesive forces between the liquid & the tube & cohesive forces within the liquid

4. 6.2 Interactions Involving Polar Molecules

   • Sphere of Hydration
     • defined as: the cluster of water molecules surrounding an ion in an aqueous solution
   • Hydroxyl Group
     • defined as: a functional group that consists of an oxygen atom with a single bond to a hydrogen atom
   • Ion-Dipole Interaction
     • defined as: an attractive force between an ion & a molecule that has a permanent dipole
   • Ketone
     • defined as: an organic compound that contains a carbonyl group boned to 2 other carbon atoms
   • Carbonyl Group
     • defined as: a functional group that consists of carbon atom with a double bond to an oxygen
   • Organic Compounds
     • defined as: compounds that contain carbon, hydrogen, & sometimes other elements, including oxygen, nitrogen, sulfur, & a halogen
   • Dipole-Dipole Interaction
     • defined as: an attraction between regions of polar regions of polar molecules that have partial charges of opposite sign
   • Functional Group
     • defined as: a group of atoms in a molecule that is largely responsible for the physical and chemical properties of a molecular compound
   • Ether
     • defined as: an organic compound that contains an oxygen atom with single bonds to 2 carbon atoms
   • Alcohol
     • defined as: an organic compound whose molecular structure includes hydroxyl group bonded is not bonded to any other functional group(s)
   • Hydrogen Bond
     • defined as: a strong dipole-dipole interaction, which occurs between a hydrogen atom bonded to an N,O, or F atom and another N, O, or F atom

5. 6.4 Phase Diagrams: Intermolecular Forces at work

   • Triple Point
     • defined as: the temperature & pressure where all 3 phases of a substance coexist. Freezing & melting, boiling & liquefaction, & sublimation & deposition all proceed at the same rate, so no net change takes place in the system
   • Supercritical Fluid
     • defined as: a subtance in a state that is above the temperature & pressure at the critical point, where the liquid & vapor phases are indistinguishable
   • Phase Diagram
     • defined as: a graphical representation of the dependence of stabilities of the physical states of a substance on temperature & pressure
   • Standard Atmosphere (atm)
     • defined as: the average pressure at sea level on Earth
   • Critical Point
     • defined as: a specific temperature & pressure at which the liquid & gas phases of a substance have the same density & are indistingulishable from each other
   • Green Chemistry
     • defined as: laboratory practices that reduce or eliminate the use or generation of hazardous substances
   • Pressure (P)
     • defined as: the ratio of a force to the surface area over which the force is applied