AICE Marine - Chapter 1 Review

• Kinetic Particle Theory

  All particles are in constant motion
• Solid to Liquid: Melting


  Ice is heated and energy is added to the water molecules and they break apart from each other
• Liquid to Gas (water vapor): Evaporation


  Particles move faster and further from each other, when they collide they evaporate
• Gas to Liquid: Condensation


  Water vapor is cooled, losing energy and brought together
• Liquid to Solid: Freezing


  Liquid is brought below freezing point, bringing particles together and forming lattice/crystaline structure
• Subatomic particles

  • Protons
  • Neutrons
  • Electrons
  • Nucleus
  • Shells
• Atoms are most stable when the outermost shell is full
• Seawater is a complex mix of chemicals, with nearly every element can be found, usually combined with others elements to form a compound
• Covalent Bonding


  Sharing of electrons usually between non-metals, makes water polar, emergent properties
• Ionic Bonding


  Giving and receiving of electrons between atoms, ions gain a respective charge causing them to attract to each other, all salts are made from ionic bonds
• Formation of hydrogen bonds in water

  Unequal sharing of electrons giving different sides of an element having different charges, more electrons are pulled closer to oxygen, gives ice its hexagonal crystal lattice structure
• Affect on properties of water

  Highly soluble, universal solvent, can break bonds of ionic and covalent substances and form new ones, high density, high specific heat capacity
• Dissolution

  The process of being dissolved
• How solutes dissolve in water

  Water's polarity allows it to interact with ions, +H is attracted to Cl- and -O is attracted to Na-, as temperature increases, dissolution rate increases
• Salinity

  Concentration of dissolved salts in water, unit is measured in ppt (parts per thousand), average salinity is 35 ppt, hypersaline is when water is more than 40 ppt
• Salt lowers the freezing point of water

  Salt molecules block water molecules from coming together and forming hydrogen bonds
• Precipitation

  Lowers salinity by adding more water molecules to dissolve salts
• Evaporation


  Increases salinity by removing water molecules that dissolve salts
• Fresh water run-off

  Lowers salinity by adding more water molecules to dissolve salts
• Salt water run-off

  Increases salinity by adding more salts
• pH scale


  Logarithmic scale measuring the concentration of hydrogen ions, acidic - higher concentration of hydrogen ions (<7), neutral - point of comparison; pure water (=7), alkaline - lower concentration of hydrogen ions (>7), ocean has average pH of 8.1
• Litmus Indicator, Universal Indicator, and pH Probes

  Litmus indicator determines if acidic or alkaline, but not the strength, universal indicator gives a color that shows the strength of range and then needs to be compared to a color pH scale to estimate a whole number, pH probes give a precise numerical value
• Oxygen has a low solubility in water, it cannot combine with water molecules, as temperature and salinity increase, oxygen concentration decreases
• Carbon dioxide is very soluble because it is a weak/carbonic acid
• Increased water temperature


  Lower solubility
• Increased atmospheric pressure


  Increased solubility
• Increased water pressure due to depth


  Increased solubility
• Increased salinity


  Lower solubility
• Higher temperature


  Lower density
• Higher pressure


  Higher density
• Higher salinity


  Higher density
• Pycnocline

  Area of rapid pressure change
• Halocline

  Area of drastic salinity change