Chemistry Ch 13
Terms
undefined, object
copy deck
- The Kinetic Molecular Theory
- behavior of gases in terms of particles in motion
- Particles size of Gases
- small particles are separated by empty space
- Particle motion
- gas is in constant random motion
- Elastic Collisions
- particles bounce off each other and no kinetic energy is lost
- Particle Energy
- KE = 1/2mv2
- Temperature
- measurement of average kinetic energy
- low density
- small and light
- Compression and Expansion
- large empty space -> release -> expand
- Diffusion
- movement of 1 material through another concentration (HI -> LO)
- effusion
- gas escaping from a tiny opening
- Graham's Law of Effusion
- rate A over rate B equals the square root of the molar mass of B over the molar mass of A
- Pressure
- Force per unit of area (P =F/A)
- Barometer
- device used to measure pressure
- Manometer
- closed ended and open ended
- Units of Pressure
- mmHg= Torr
- Dalton's Law of Partial Pressures
- indv. gases exert own pressure: totall pressure is sum of partial pressure
- Partial Pressure
- depends on mols present, size of container, and temperature
- Strong Forces
- have low vapor pressures
- Dispersion Forces
- Found in all covalent bonds but significant in non-polar
- dipole-dipole forces
- only found in polar molecules
- Hydrogen Bonds
- special type of dipole-dipole; has hydrogen (H) bonds
- Liquids
- indefinite shape and volume; has greater density than gas because of greater volume
- Density and Compression of Liquids
- have greater density than gas because of greater volume
- Fluidity
- the ability to flow
- viscosity
- the resistance to flow
- Viscosity and Temperature of liquids
- when the temperature is increased, the viscosity decreases
- Surface Tension
- measure of inward pull by interior particles (Skin of Substance)
- Surfactants
- the greater the forces, the greater the surface tension
- Capillary action
- liquid rising on the walls of a container
- Volatile
- the ability to evaporate easily/readily
- Density of Solids
- not compressible
- Crystalline solids
- atoms, ions, or molecule arranged in an organized repetitive pattern; all ionic compounds
- unit cell
- smallest arrangement of connected points that can be repeated in 3 directions to form the lattice
- Amorphous solids
- lacks organization or pattern WAX, PLASTIC, GLASS, RUBBER.
- 4 types of Solids
- molecular, covalent network, ionic, and metallic
- Molecular Solids
- nonconductors when pure, insoluble in water (generally), volatile, lo melt/boil points.
- Covalent Network Solids
- always solids, extremely high MP, insoluble in all solvents, poor conductors (except GRAPHITE), all network solids: C, Si, Ge, P, SiC, BN, SiO2
- Ionic Solids
- nonvolatile, and high MP, don't conduct as solids, many soluble in water
- Metallic Solids
- Composed of ions surrounded by valence electrons, can be soft or hard,
- Melting
- from solid to liquid
- Vaporization
- from liquid to gas
- Vapor Pressure for Gases
- pressure exerted by a gas above its liquid
- Boiling point
- time at which vapor pressure equals the atmosphere pressure
- Sublimation
- From solid to gas
- condensation
- from gas to liquid
- deposition
- from gas to liquid
- freezing
- from liquid to solid
- triple point
- where all effects happen at the same time
- critical point
- where water can no longer be a liquid
- equilibrium
- point where both sides are equal to each other
- LeChatelier's Principle
- if stress is put on the system it will move to relieve stress