states of matter

• pure substance: elements or compounds which are combinations of elements
• mixture: made up of 2 or more pure substances (separates using physical processes)
• matter: takes up space and has mass
• chemical properties can be observed or measured during or right after a chemical reaction

  • toxicity, flammability, heat of combustion
• chemical changes: atoms are rearranged to form new substances
• physical properties: properties that can be measured or observed without changing the chemical structure of a sample

  • extensive: change with amount of matter (mass, volume)
  • intensive: don't change with amount of matter (density, color, temperature, ect)
• homogenous mixtures: have visibly indistinguishable pats
• heterogenous mixtures: have visibly distinguishable parts
• separations are physical processes used to separate many mixtures
• filtration: depends on particle size differences
• distillation: a mixture is heated and substances are separated based on their boiling points
• chromatography: takes advantage of the physical property of affinity of individual substances to different lab tools, paper, or liquid solvent
• states of matter include solid, liquid, gas, plasma, glass, and liquid crystal
• gas: little to no intermolecular forces, not close together, can move anywhere, no shape or volume
• plasma: no shape or volume, electrically conductive
• liquid: particles close together, move around freely (intermolecular forces), definite volume, no definite shape, uncompressable
• solid: particles packed tightly together, vibrate but do not move past one another, definite shape and volume, compressible
• solute: substance that is dissolved
• solvent: the substance in which the solute dissolves
• precipitate: an insoluble substance formed during a chemical reaction
• most polar & ionic substances do not dissolve
• phase diagrams

  • solid state: high pressure, low temperature
  • liquid state: pressure increase/temperature decrease -> solid, pressure decrease/temperature increase -> gas
  • gas state: pressure increase/temperature decrease -> condense into liquid or deposit into solid
• triple point: set of conditions where gas, liquid, and solid can exist in the same sample
• critical point: end point of a phase equilibrium curve

  • conditions where a gas cannot be liquified using pressure and a liquid cannot be heated to form a gas
• time temperature graph
• specific heat: the energy that is involved in a temperature within a single state of a substance
• heat: energy transferred between substances at different temperatures
• latent heat of vaporization is the amount of energy needed to change the state of a substance from a liquid to a gas
• latent heat of evaporation is the energy needed to change the state of a liquid to a gas