General Chemistry

• Cohesion - same molecules attract each other
• Adhesion - attraction between different molecules
• Surface Tension - phenomenon that occurs because of cohesive forces between liquid molecules
• Buoyancy - the ability of a material to float
• Viscosity - the quantity that describes "lapot" or "labnaw"
• Viscosity - the resistance of a fluid to flow smoothly
• High Viscosity means HIgh IMF
• Low viscosity means Low IMF
• Capillarity - rise or dispersion of a liquid in a small passage as a result of surface tension
• In Capillarity, the narrower the tube, the higher the liquid will rise
• Vapor Pressure - pressure exerted by a gas/vapor in a thermodynamics with its condensed phase
• In Vapor Pressure, number of evaporation equals the condensation
• Boiling Point is when vapor pressure = atmospheric pressure
• If the temperature increases, the vapor increases too
• Volatile materials - evaporate or sublimate at room temperature
• The higher the altitude, the lower the atmospheric pressure meaning lower temperature than normal
• The lower the altitude, the higher the atmospheric pressure
• Normal Boiling Point - temperature of liquid at which its vapor pressure is equal to 1 atm(atmospheric pressure)
• Bumping - When a liquid boils, forming bubbles; splashing of liquids due to high heat
• Molar Heat of Vaporization - high temperature = Gas ; low temperature = liquid
• Molar Heat of Vaporization - energy required to transform a given quantity of a substance from a liquid into gas at a given pressure
• Molar Heat of Vaporization;

  Evaporation = Change Liquid into Gas
• Molar Heat of Vaporization;

  Vaporization = Neither Liquid nor Gas
• "As long as it's not freezing point, the water will still boil slowly"
• Hydrogen Bonds:

  2 Hydrogen - The angle is 104.5 degrees
• Mercury is used in thermometer because it has the highest boiling point
• Solid - definite shape and volume
• Solid - rigid, can't compress easily
• Solid - can't diffuse to another solid
• Solid - does not flow and can be stored in container
• Solid - change by heat
• *Crystalline Solids

  • regarded as true solids
  • repeated order, symmetrical patterns
  • Unit cell - a small repeating structure of a solid; hexagonal
  • can't compress
• *Crystalline Solids

  Seven primitive crystal lattice:

  a.) triclinic

  b.) monoclinic

  c.) orthorhombic

  d.) tetragonal

  e.) trigonal

  f.) hexagonal

  g.) cubic
• *Solids

  Anisotrophy - refractive, conductivity, and tensile strength depends on the direction of force
• *Solids

  Cleavage - plane surface or straight edge when broken
• *Amorphous Solids

  • pseudo solids
  • Without form, no repeating lattice pattern
  • it melts gradually because do not break all at once
  • Edges may be curved when cut
• *Amorphous solids

  Isotrophe - properties like refraction, conductivity, and tensile strength is equal regardless of direction
• Types of Crystalline Solids:

  1.) Ionic Solids

  • Compose of opposite charged ions
  • have very high melting points
  • Crystal are hard, brittle, and non-conductive
  • most, dissolve in water
  • composed of metal and non-metal, also, polyatomic ions
• Types of Crystalline Solids

  2.) Covalent Solids

  • no individual molecules
  • covalently bonded in a continuous network
  • also called as "network solids" - emphasized by ma'am R Len
  • very hard, high melting points
  • do not dissolve in water and don't conduct electricity, like diamond
• Types of Crystalline Solids:

  3.) Molecular Solids

  • covalently bonded, attracted to each other by electronic forces (Van Der Walls)
  • shared electrons spend more time in electron clouds.
  • attraction is weaker, softer and low melting point.
  • non-polar can't dissolve in water, but benzene or octene
  • Polar solid molecule like sugar can dissolve in water but non-conductive