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Kinetic Molecular Theory (Do not take notes). Composition & structure of molecules affect the chemical & physical properties of matter. Solids & liquids have a lot of variation between both physical & chemical properties. Gases, however, have very similar physical and chemical properties.

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kinetic molecular theory do not take notes
Kinetic Molecular Theory(Do not take notes)
  • Composition & structure of molecules affect the chemical & physical properties of matter.
  • Solids & liquids have a lot of variation between both physical & chemical properties.
  • Gases, however, have very similar physical and chemical properties.
kinetic molecular theory
Kinetic Molecular Theory
  • Explains the behavior of gases in terms of particles in motion
  • Assumptions:
    • Particles are very small with huge amounts of empty space between them (so no attractive or repulsive forces between them).
    • Gas particles are in constant, random motion. Move in straight lines until they collide with each other or container walls. Collisions are elastic – no energy is lost.
    • Mass & velocity affect the kinetic energy of individual gas particles (K.E. = ½ mv2)
using kmt to explain gases
Using KMT to explain gases
  • Low density: gases have extremely low densities because of the large spaces between gas molecules
  • Compression & expansion: gases can be compressed if you decrease the space between gas molecules; the random motion of gas particles will cause gases to expand to any space available
  • Diffusion & effusion: both of these properties occur because of the constant random motion of gas particles and the lack of attractive or repulsive forces among gas particles.
gas pressure
Gas Pressure
  • Pressure is the force exerted compared to the area so lying down on ice spreads out your weight.
  • Air pressure or atmospheric pressure is exerted in all directions since air is all around us moving randomly
  • Measured with a barometer – one end is a vacuum; the other is open to the air
  • Many units are used for pressure: pascal, torr, psi and atmospheres are all common
intermolecular forces of attraction
Intermolecular Forces of Attraction
  • Occur between identical particles & help explain how solids, liquids and gases exist at the same temperature
  • Three main types: dispersion, dipole-dipole and hydrogen bonds.
  • All intermolecular forces are weaker than intramolecular forces (they have to be)
dispersion forces
Dispersion Forces
  • The weakest intermolecular force
  • Significant in nonpolar substances because no other intermolecular forces exist
  • Explains why non-polar liquids are hard to pour and evaporate quickly (alcohols, gasoline, etc)
dipole dipole forces
Dipole-Dipole Forces
  • Occur in polar molecules because permanent dipoles exist
  • Molecules line up head to tail or positive region near a negative region
  • Stronger than dispersion forces but weaker than hydrogen bonds
hydrogen bonds
Hydrogen bonds
  • A special type of dipole-dipole bond
  • Occur only between H and fluorine, oxygen or nitrogen
  • Explains why water (18.00 g/mol) has such a huge surface tension and high boiling point while methane (16.05 g/mol) has very low surface tension and is a gas at room temperature
properties of liquids
Properties of liquids
  • Liquid particles have random motion but greater attractive forces than gases, so liquids have a volume but no shape
  • Density is also greater than gases while compression is much less since liquid particles are already close
  • Liquids are less fluid than gases because they diffuse much slower due to the intermolecular forces interfering
properties of liquids10
Properties of liquids
  • Viscosity is the measure of the resistance of a liquid to flowing
  • Viscosity is influenced by intermolecular forces, shape of the particle and temperature
  • Year round oils actually change shape from spheres in cold weather to long strands when hot to increase viscosity
properties of liquids surface tension
Properties of liquids – surface tension
  • Particles at the surface have a greater downward pull than particles in the middle
  • Greater intermolecular forces usually means greater surface tension
  • Water forms a drop because of its high surface tension
  • Surfactants are compounds that lower surface tension in a substance, like detergent in water
properties of liquids capillary action
Properties of liquids – capillary action
  • Occurs when water is placed in a container or substance that it’s highly attracted to
  • If the attraction (adhesion) is greater than water’s attraction to itself (cohesion), capillary action occurs.
  • Like the downward curve you see when a liquid is in a glass
  • When water is drawn up between the cellulose fibers of paper towels or the crystals in a diaper
properties of solids
Properties of Solids
  • According to KMT solids have as much kinetic energy at room temp as gases or liquids, but attractive forces are so great that particles in a solid move around a fixed point
  • Most solids are more dense than liquids or gases (water is the exception)
phase changes
Phase Changes
  • Most substances can exist in 1 of 3 states on Earth: solid, liquid or gas depending on the pressure and temperature
  • When energy is added or removed a substance may change from one phase to another
  • KMT predicts this because as temperature increases, motion increases and forces of attraction can be overcome.
phase changes that require nrg
Phase Changes that Require NRG
  • Includes melting, vaporizing (boiling), evaporating and sublimation
  • For melting, boiling and sublimation, the temperature plateaus where the phase change occurs because all incoming energy is being used to break bonds
  • Stronger bond = more energy = higher boiling point or lower freezing point
evaporation
Evaporation
  • When a liquid changes to a gas but only molecules at the surface escape to become vapor
  • Occurs at a lower temperature than boiling point and is also a slower process than vaporization
  • Explains why sweating cools us or other animals down
sublimation
Sublimation
  • Process in which a solid goes directly to a gas without a liquid phase
  • Iodine, dry ice, moth balls and air fresheners all tend to sublime
  • Water (ice) will sublime if pressure is decreased – like when ice cubes shrivel up in your freezer
  • Freeze dried food is when food is frozen in a vacuum so the water sublimes. Makes food lighter and unable to grow bacteria.
phase changes that release nrg
Phase Changes that release NRG
  • Includes condensation, freezing, & deposition
  • Occurs when a vapor or liquid comes into contact with a cooler substance. The gas or liquid loses heat and if enough heat is lost, the forces of attraction become great enough to form a liquid or solid.
  • This is why clouds form and why it warms up when it starts snowing
  • Deposition is when a gas goes right to a solid like when it snows or frost forms
phase diagrams
Phase Diagrams
  • Graphs pressure versus temperature
  • Lines on diagram indicate where more than one phase exists
  • Triple point is the temperature and pressure where all 3 states would exist or all 6 phase changes can occur
  • Critical point = pressure and temperature where water can not exist as a liquid; regardless of how much pressure you put on the vapor beyond this point it will be a gas