Solids and Liquids

Intermolecular forces

attractive or repulsive interactions between beighboring molecules that determine physical properties

London Disperision

Exist between all moleucles

Dipole Dipole

Polar Molecules Interacting

Hydrogen Bonding

F-H, O-H, N-H

what is the weakest Intermoleuclar force

LDF

Increase in size of molecule means what for London Dispersion Force

Greater London Dispersion Force

Dpiole

The seperation of charges due to different electronegativites

Dipole Dipole only occurs in what

polar molecules, the ore polar the moelucle the stronger the dipole dipole

Increasing the number of polar molecules means what in terms of boilng point

increase in boiliing point

Hydrogen Bond

A strong type of dipole dipole interaction between H and N O F

Ranking Boiling points

Strongest to weakest

Hydrogen Bond

Dipole Dipole

London Dispersion

Non Branched Moleucles LDF

Intermoleucles

Between two moelculesI

Intramolecular FOrces

forces that are within a molecule

what is stronger intramolecular or internolecular

intramolecular

Types of intramoelcular forces

Polar Covalent- electrons shared between atoms of different electornegativity

Non POlar Covalent Bonds- electrons shared equally

ionic bonds- two ions

metallic - two metal ions

Polar Covalent

When atoms of different elecrronegativity share electrons

Non Polar Covalent bond

Atoms with similar electronegativity eqaully

Ionic Bond

The complete transfer of valence electron between a non metal and metal

Metallic Bpond

Form between metal cations moving freely through lattice

what is matter made up of

small particles of atoms or moleuclesth

three states of matter are what

solid liquid gas

All phase changes are what

physcla changes not chemcial

Solid to Liquid endo

fusion

Liquid to Gas endo

vaporization

Solid to Gas endo

sublimation

Gas to liquid exo

condensationl

liquid to solid exo

freezing

gas to solid exo

deposition

Solids are more organized in a solid form

that form a lattice and become more organized

When the substance tranfer when does it become less organized

solid is most organized and ordered

liquid is next most

gas is least ordered

Entropy or Delta S

Disorder or randomness

increase in disorder is positve SE

Enthalpy or Heat (H)

Heat or the heat that is gained or lost by the system

delta H > 0

endothermic

delta H < 0

exothermic

Endothermic

heat moves into the system

exothermic

heats move out of the systenm

Heat of Vaporization is greater than what

heat of fusionh

heat of sublimation is greater than

the heat of vaporization

Vaporization requires sufficent energy to break almost all forces of attraction between the moleucles

fusions requires only enogugh energy for molecules to escape from their sites in the crystal lattice

solids have stronger intermoleuclar forces than liquids

it takes more energy to excite a solid to gas than to exicte a liquid to gas

standard ethalpy of formation

ethalpy change when one mole of substance in the standrad state is formed from pure elements

Equation for standard ethalpy

(mols * heat ) of products - reactants

Phase Diagram

Graph the represent the effect of temperate and pressure on different states of matter

Phases on diagram and axis

solid then water then gas

pressure on Y and Temp on X

Triple point

A point where the sustance is present in solid liquid and gas phase

why is the slope of solid liquid kline negative

its solid state is less dense than its liquid state

Critical Point

the conditon of temperature and pressure at which liquid and gas becomes indistinguishble or you cant tell

supercritcal fluid

point where u cant even tell what it is past the gas and liquid form

Properties of Liquids

Volume but no fixed shape

Solubility

The degree to which a solute can be dissolved in a liquid (solvent )

Miscibility

The degere to which a liquid mixed with another liquid

for example alcohol and water

viscosity

thickness of liquid

as temp increases viscocity

decreases meaning more liquidy

surface tension

the ability of a lqiuid surfaces to resist external forces

increase temperature makes surface tension

decrease surface tension

vapor pressure

equilibroum pressure extrered by a vapor above its liquid in a closed system

increase in temperature what happens to vapor pressure

increase vapor pressure

Ice is less dense as a solid

ice floats in water because the solid are more tightly packed than liquid form creating lower density

liquid solid mixture Heterogenous

particles distributed non uniformly

liquid solid mixture Homogenous

Paritcles distributed uniformly

Liquid Liquid mixtures heterogenous

do not stick together

liquid liquid homegenous

stick togther

Ionic Solids

Hard Non Conductive Brittle and High Melting points

Metallic SOlids

Maellable ductile, conductive and variable melting point

covalent network solids

hard non conductive and high melting points m

molecular solids

soft non conductive and low melting point

amorphous solids

simple cubic cell

1 atom per unit cell one atom is at every corner of the cube

body centered cubic

2 atoms per unit cell one atom is at the cener of the cellf

face centered cube

4 atoms per unit cell one atom at the center