General Chemistry

Cards (183)

  • What does the Kinetic Molecular Theory (KMT) explain about the properties of matter?
    It explains the properties of matter in the three phases: gas, liquid, and solid.
  • What is the first assumption of the Kinetic Molecular Theory?
    All matter is made of tiny particles.
  • What is the second assumption of the Kinetic Molecular Theory?
    These particles are in constant motion.
  • How does temperature affect the speed of particles according to KMT?
    The speed of particles is proportional to temperature; increased temperature means greater speed.
  • What are the differences among solids, liquids, and gases in terms of particle distances and interactions?
    Solids, liquids, and gases differ in distances between particles, freedom of motion, and extent of interactions.
  • What are condensed phases?
    • Liquids and solids
    • Characterized by closely packed particles
  • How would you rank the phases of matter in increasing distance between particles?
    Solid, liquid, gas.
  • How do the particles of gas, liquid, and solid move?
    Gas particles move rapidly in all directions, liquid particles slip and slide over one another, and solid particles vibrate in fixed positions.
  • What property of matter corresponds to molecular behavior?
    The property of matter that corresponds to molecular behavior is the state of matter (solid, liquid, gas).
  • What shape and volume does matter in the gas state have?
    Indefinite shape and volume.
  • What shape and volume does matter in the liquid state have?
    Indefinite shape and definite volume.
  • What shape and volume does matter in the solid state have?
    Definite shape and volume.
  • What are the basic assumptions of the KMT common to the three states of matter?
    They are composed of molecules and these molecules possess kinetic energy.
  • What is the role of intermolecular forces in the properties of gases?
    Intermolecular forces account for the motion, kinetic energy, distance, and attraction between molecules.
  • How do the shape and volume of gases differ from those of liquids and solids?
    Gases have no definite shape or volume, while liquids have a definite volume but no definite shape, and solids have both definite shape and volume.
  • What is the definition of intermolecular forces?
    Intermolecular forces are attractive forces between molecules.
  • What are intramolecular forces?
    Intramolecular forces hold atoms together in a molecule.
  • What is a polar molecule?
    A polar molecule is a molecule with a negative end and a positive end, due to unequally distributed electrons.
  • What are the different types of intermolecular forces?
    • London Dispersion Force (LDF)
    • Dipole-dipole forces
    • Ion-dipole forces
    • Hydrogen bond
  • What are London Dispersion Forces (LDF)?
    They are forces of attraction resulting from temporary dipole moments induced in ordinarily nonpolar molecules.
  • What is polarizability?
    Polarizability refers to the ease with which the electron distribution can be distorted.
  • How does the size of an atom or molecule affect its polarizability?
    The larger the number of electrons and the more diffused the electron cloud, the greater its polarizability.
  • What is the relationship between dispersion forces and the size of atoms?
    Dispersion forces may be the weakest of intermolecular forces, but they become stronger with larger atoms.
  • How do London Dispersion Forces manifest in helium atoms?
    Helium atoms can have a transient dipole moment due to uneven electron distribution at a given instant.
  • What are dipole-dipole forces?
    Dipole-dipole forces are attractive forces between polar molecules that possess dipole moments.
  • How do dipole-dipole forces compare to dispersion forces?
    Dipole-dipole forces are stronger than dispersion forces due to the permanent uneven distribution of electrons in polar molecules.
  • What are ion-dipole forces?
    Ion-dipole forces exist when polar molecules are attracted to ions.
  • How do hydrogen bonds differ from regular dipole-dipole interactions?
    Hydrogen bonds are a special type of dipole-dipole interaction involving hydrogen and electronegative atoms like O, N, or F.
  • What is the significance of hydrogen bonding in water?
    Hydrogen bonds between water molecules are particularly strong.
  • What are the important terms related to liquids and intermolecular forces?

    • Fluid: a gas or a liquid; a substance that can flow.
    • Surface tension: measure of elastic force in the surface of a liquid.
    • Capillary action: tendency of a liquid to rise in narrow tubes.
    • Viscosity: measure of a fluid’s resistance to flow.
    • Vapor: gaseous substance that exists naturally as a liquid or solid.
    • Vaporization: change of phase from liquid to vapor.
    • Vapor pressure: equilibrium pressure of a vapor above its liquid.
    • Boiling point: temperature at which a liquid boils.
    • Molar heat of vaporization (ΔHvap): energy required to vaporize 1 mole of a liquid.
  • What is surface tension?
    Surface tension is the measure of the elastic force in the surface of a liquid.
  • How does surface tension relate to intermolecular forces?
    Liquids with strong intermolecular forces have high surface tension due to the strength of attractive forces between molecules.
  • What is capillary action?
    Capillary action is the tendency of a liquid to rise in narrow tubes or be drawn into small openings.
  • What forces are involved in capillary action?
    Cohesion (attraction between like molecules) and adhesion (attraction between unlike molecules) are involved in capillary action.
  • How does surface tension change with temperature?
    Surface tension decreases as temperature increases.
  • What is the boiling point of a liquid?
    The boiling point is the temperature at which a liquid boils.
  • What is the molar heat of vaporization (ΔHvap)?
    It is the energy required to vaporize 1 mole of a liquid at a given temperature.
  • How does temperature affect the surface tension of water?
    The surface tension of lukewarm water is greater than that of hot water.
  • What is capillary action and what causes it?
    • Capillary action is the tendency of a liquid to rise in narrow tubes or small openings.
    • It is caused by intermolecular attraction between the liquid and solid materials.
  • What is another name for capillary action?
    Capillarity