Intramolecular Forces & Intermolecular Forces

Dipole-Dipole

-between polar molecules -more polar the higher strength of bond -perminant bonding -second weakest (in the middle of H-bonding and L.D -attractive force between perminite polar molecules positive attracts negitive -ploar molecules only -strength of the perminite dipole goes up. the strength of the dipole-dipole goes up

Metals are...

-ductile -malleable -lusterus -good conductors of heat and electricity

London Dispersion

-happens between any type of atom or molecule -random acusion between shift of electrons -domino effect -electrons will end up on one side -weakest strength -temporary bonding -only happnes when molecules get close enough -this will always be a posibility of the intermolecular forces -attractive force result of un even distribution of e- creating instentanious dipole -found in all types of molecules -forces affecting strength: strength of forces increases as the atomic or molecular weight increases. surface area increases the strength increases

Metallic

-metals bond to metals -hard (varries) -good conductor as a solid -doesnt desolve (varries) -conducts in solution -no odor -high boiling and melting points -have luster -solid at room temp. except Hg (murcury) -maliable -ductile -doesnt desolve *key word; delocalized (sea of e-) <most freely< is defined as a force of attraction between metal atoms due to pooling of their valence electrons to form a delocalized sea of electrons.

Ionic

-metals to non metals -high melting points -poor conductivity -good conductivity when delsoved -high boiling points -crystal structure -hard, brittle *key word; transfer electron

Alkenes

-molecular formula: CnH2 -formed with double bonds -unsaturated

Alkanes

-molecular formula: CnH2+2 -single carbon to carbon -saturated

Molecular (covalent)

-non metals -electrons are shared between two atoms -hard -doest conduct -doesnt conduct in solution (stays whole) -no odor -low melting and boiling points (varries) -insoliable mostly -nonpolar -soft if solid *key word; shared electron

Hydrogen Bonding

-special form of strong dipole dipole interaction. -the strongest form of intermolecular force -bond with F, O, or N * when a molecule contains a highly polar bond, such as an O-H bond, the positive end of which is hydrogen. hydrogen has a very low electronegitivity so it bonds with one with a high electronegitivity such as F, O or N. -weaker bond then covalent -molecule contains a highly polar bond, such as O-H nond. the positive end is H interacts easily with other unshared electrons. -hydrogen will always be slightly positive -only between polar molecules -has to be attraction between 1 proton with 2 electron pairs -covalently bonded to a more electronegitive atom -polar only -more O-H groups you have the greater the strength the hydrogen bond

Coulomb's Law

force of attraction between charged particles is directly porportional to the product of the charges and inversly porportional to the distance between them

Unsaturated

gaps are left

Alloy

homogeneous mixture of a base metal with other elements. the base metal is the metal which is present in the largest concentration. the elements are mised whe nthey are mlten and form metallic bonds because they solidify to form an alloy -often strong, more durable, lighter, visual appeal

Kinetic Energy

how fast the molecules move; when heat is added the K.E moves faster making the temp. go up. -the particles that move the fastes are the first ones to brake away

Volatility

how readily it becomes a vapor

Interstitial Alloy

if the added atoms are much smaller then the base metal atoms, they fit into the spaces between the base metal atoms

Substitutional Alloy

if the added metal atoms are about the same size as teh base metal atoms. then the added atoms just mix evenly through the alloy and the crystal strusture remaines similar

*Like Desolves Like*

if they have the same polarity they will desolve ex: polar desolves polar; nonpolar desolves nonpolar; polar and nonpolar substances do not desolve

Volatile

measure of how quickly somthing evaporates

Alloying

metals are alloyed to improve the qualities of the individual pure metals

Pure Metals

metals made up from a mixture of elements

Ferrous

metals taht contain iron and are affected by magnetism

Nonpolar

no shift (pull) in electrons; no net dipole, no semetry - 0.4 and lower

Sea of Delocalized Electrons

not loval; not sitting with home atoms

Mixture

physical combination of two or more substances

Viscosity

resistance to flow (syrup)

SATP

standard auomospheric temperature and preasure

Boiling

state from liquid to gas

Melting Point

temperature that you go from a solid to a liauid

Boiling Point

temperature to get from a liquid to a gas

Boiling Trend

the higher the boiling point the more intermolecualr forces

Relations of Carbons and Boiling Points

the more carbon the higher the boiling point

Isomers

two molecules have the same molecular formula but look diffrent.

Cohesion

two of the same molecules attracting eachother

Adhesion

two unlike substances attraction of gas

Homogeneous

uniform apperance throught. cant distenguish parts (food coloring and water)

Prefixes for Hydrocarbons

1- meth 2- eth 3- prop 4- but 5- pent 6- hex 7- hept 8- oct 9- non 10- dec

Vapor Pressure

After the substance is evaporated there becomes vapor; or a gas that builds up pressure and the substance keeps evaporating.

Polar

a shift in electrons; has a net dipole, are semetric - 0.5 to 1.7

Electronegitivity

ability of an atom to draw electrons twards it

Solubility

ability to desolve

Vapor Trend

as more of a substance evaporates the more vapor pressure occurs

Affinity

attractive forces between molecules

Ductile

being able to pull metal into wire (can not be done to ionic compounds)

Malleable

bendable, pounded out into sheets

Intermolecular

between two diffrent molecules; are what hold molecular materials together in a liquid of solid state. intermolecular bonds are broken when energy (heat) greater than the intermolecular bond strength is applies to the material. (this is wy materials have specific meltin and freezing points.

Intramolecular

bond within molecule; force that holds the atoms or ions together in a compound. 1. metallic 2. ionic 3. covalent stronger then intermolecular, and works deeper into the compound.

Heterogeneous

can observe diffrents parts. can distinguish diffrent parts (oil and water)

Corrosion

caused by oxygen in the air combining with the aton of metal, at the surface of the metal to create a new chemical called oxide; in non ferrous metals the oxide layer is dense and does not fall away, this creates a barrier to the oxygen in teh air and new corrosion occures very slowly. the layer is called tarnish.

Metalic Bonding

defined as teh force of attraction between metal atoms due to pulling of their valance electrons to form a delocalized sea of electrons

Saturated

filled to its maximum compasity