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Anatomy & Physiology: Chemical Bonds and Water Properties Part 2

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Terms in this set (19)

  • Types of covalent bonds
    Polar and Nonpolar covalent bonds.
  • Polar covalent bond
    One atom has greater attraction (electronegativity) for electrons than the other, e.g. O-H, N-H, S-H, O-C.
  • Nonpolar covalent bond
    Atoms equally share electrons, e.g. H-H, C-H.
  • Hydrogen bond
    Between H in one polar covalent bond and another atom (e.g. O or N) in another molecule; directional and weakest bond, e.g. H\(_2\)O.
  • Types of compounds
    Inorganic compounds lack C and H; Organic compounds contain C and H.
  • Water as a universal solvent
    Water dissolves ions or polar solutes forming aqueous solutions due to its polarity.
  • Hydrophilic molecules
    Polar molecules that dissolve easily in water.
  • Hydrophobic molecules
    Non-polar molecules that do not dissolve in water.
  • Cohesion in water
    Attraction between water (H\(_2\)O) molecules.
  • Adhesion in water
    Attraction between water molecules and other types of molecules.
  • High heat capacity of water
    Water requires a lot of heat to raise its temperature, helping moderate local climate.
  • High heat of vaporization of water
    Water needs a lot of heat to evaporate, producing a cooling effect.
  • Water expands when it crystallizes
    Water expands upon freezing, making ice less dense than liquid water.
  • pH definition
    Measure of acidity based on H\(^+\) concentration; pH scale ranges from 0 to 14.
  • pH of pure water
    Ionization is rare; [H\(^+\)] = 10\(^{-7}\); pH = 7.
  • Acidic pH range
    pH less than 7 indicates high H\(^+\) concentration.
  • Basic pH range
    pH greater than 7 indicates low H\(^+\) concentration.
  • Neutral pH
    pH equal to 7, indicating balanced H\(^+\) concentration.
  • Buffers
    Compounds that resist pH change and minimize pH disturbance in living cells.