Chemistry Test Chapters 10/11

description of matter as particles in motion

average kinetic energy of particles

particle size - small, mostly empty space, particles are far apart, only a few atoms (O2)

particle motion - constantly moving in a straight line until a collision with a solid or another gas particle

particle energy - particles can move at different velocities, smaller mass takes less energy to move and vice versa

behavior - low density, can compress and expand

one gas mixes with another gas

gas released through a small opening

force per unit area (air pressure, barometer)

-strongest

-ionic bonds (+/-)

-covalent bonds (shared electrons)

-metallic bonds (electron sea model)

-weaker

-dispersion forces

-dipole-dipole forces

-hydrogen bonds

-temporary shifts in electron clouds in nonpolar molecules

-attraction between temporary dipoles

-stronger based on number of electrons

-attraction between permanent dipoles in polar molecules

-can be strong in small molecules with large dipoles (electronegativity difference)

-generally weaker than dispersion forces

-special dipole-dipole bonds formed when H is bonded to F, O, or N

-generally strongest intermolecular forces

-density and compression (more dense than gases, almost never compress)

-fluid (flow - fill a space, diffuse - movement of one liquid through another)

-cohesion (liquid + liquid) and adhesion (liquid + other) (force of attraction between molecules)

-meniscus (water molecules attract each other - cohesion, dip - and glass molecules - adhesion, raised)

-resistance to flowing that a fluid has

-intermolecular forces (stronger = molecules closer together = harder to flow)

-size and shape of particles (larger particles = harder to flow, long particles drag/catch)

-temperature (higher temp = atoms move faster = flow faster)

layer of intermolecular forces are stronger, creating tension

-follow kinetic molecular theory (still move)

-density and compression (more dense than liquids)

atomic (dispersion forces holding together elements that otherwise would not bond)

molecular (all 3 forces allow molecules to be pulled together)

covalent network (molecules form solids from repeated covalent bonds)

ionic (positive-negative repeated bonds)

metallic (formed from metallic bonds)

single solid forms different structures

no order or pattern in molecules, rapidly cooled into solids

melting (solid to liquid) require energy

vaporization (liquid to gas) require energy

deposition (gas to solid) release energy

freezing (liquid to solid) release energy

condensation (gas to liquid) release energy

sublimation (solid to gas) require energy

specific temp and pressure where a substance can exist as all 3 types of matter simultaneously