intermolecular forces

London dispersion forces (LDF)

-Present in ALL molecules

-Only IMF in non polar molecules

-Caused by temporary/ instantaneous dipoles

-Larger molecules usually have stronger LDF

-More Electrons → stronger LDF

ALL MOLECULES

Dipole-dipole

• Occurs between polar molecules

Positive end of one molecule attracts negative end of another

Polar +Polar

Hydrogen Bonding

• A strong type of dipole- dipole force (polar molecules- slightly more + or more -)

• Positive end of one molecule attracts negative end of another

• Hydrogen directly attracts to nitrogen, oxygen or fluoride FON directly with hiydrogen

Ion dipole

• An ion with an actual change full charge integrating with a molecule that had a partical change

• - ion + polar molecule

Viscosity

.resistance of flowing (the resistance of a liquid to flow is called)

Honey=high viscosity

Water= low viscosity

Stronger IMF's → higher viscosity

High temp→ lower viscosity

Surface tension

Resistance of a liquids surface to being broken

-Strong IMFs→ higher surface tension (hard to pull molecules apart)

because of hydrogen bonding

Cohesion

Attraction between the same substance

How well the groups stay together

Water. → water

Adhesion

Attraction between the different substance

Between surface and molecules water → glass

Capillary Action

:liquid moving thought a narrow space

depends on 3 things…..

Adhesion- liquid sticks tot he surface

Cohesion- liquid sticks to itself

Surface tension- molecules at the surface hold together

Solid → Liquid

Melting/Fusion

Liquid → Gas

Vaporization

Solid → Gas

Sublimation

Gas → liquid

Condensation

Liquid → Solid

Freezing

Gas → Solid

Deposition

Endothermic

absorbs heat

melting+ vaporization + sublimation

Exothermic

releases heat

Freezing + Condensation+ Deposition

Supercritical Fluids

A substance becomes a supercritical fluid when it is above its

-critical temp

-critical pressure

it has properties of both liquid and gas

Solute

is what is doing or being dissolved (getting dissolved)

Solvent

is what doing the dissolving (dose the dissolving)

Unsaturated

can dissolved ore

Saturated

at a max amount

Supersaturated

more dissolved then normally possible unstable max capacity

Pressure increases

Gas solubility increases

Temperature increases

gass solubility decreases

colligative properties

are characteristics of a solution that depend on the radio of the number of solute particles to solvent particles

Vapor pressure

pressure caused by vapor above liquid

Castled

helps reaction and is regenerated

intermediate

made during one step and used up in another

activated complex

high energy arrangement at the top o the reaction barrier