 Discovered by… that guy!   Describes the inverse relationship between the pressure and volume of a gas, if the temperature is kept constant in a vacuum.  How to Solve…  Label all values (Pressure= P, Volume=V)  Write base formula  Substitute variables with given information  Solve for unknown value Robert Boyle

 Discovered by that other guy   At constant pressure, the volume of a gas increases/decreases at the same rate as it’s temperature (the Kelvin scale, convert from Celsius).  Can be written in 3 different ways  How to solve…  Label all given values (V=Volume, T=Temperature in Kelvin)  Set up base equation (see formulas).  Substitute variables for values  and solve. Jacques Charles

 Discovered by another guy   The pressure of a gas is directly proportional to the gas's temperature.  How to Solve  Same as the other two!  Label given information (P=Pressure, T=Temperature)  Set up base formula  Substitute for given values  Solve for unknown Joseph Louis Gay-Lussac

 Combines the previous three Gas Laws into one.  The ratio between the product of pressure and volume of a gas and it’s temperature remains constant.  How to solve…  If you paid any attention to the last three slides, you should already know.  P=Pressure, V=Volume, T=Temperature

 Gasses are made up of tiny particles (atoms/molecules) with immense distances between them.  Gas particles are in constant, random motion and often collide with each other, with pressure being the result of this.  Molecular collisions are elastic, meaning that despite individual molecules gain or lose kinetic energy, the collisions don’t affect the whole gas sample’s kinetic energy.  At a given temperature, molecules in a gas sample have a range of kinetic energies, however the average remains constant and as the temperature increases, so does the average velocity and kinetic energy of the gas sample as a whole.

 Ideal Gases are those which adhere to all predictions made in the Kinetic Molecular Theory.  Usual atmospheric conditions produce Ideal Gases.  At very high pressures or very low temperatures, gases do not behave ideally, these resulting in physical changes to the gas.  At very high pressures, gases can condense into solids.  At very low temperatures, molecular attractions become weak and the gases become liquefied.  These state of matter changes do not affect the gas’s original chemical composition.

 Standard Temperature and Pressure  Used in Gas Laws as the ideal values for all gases  Standard Temperature = 0°Celsius, or 273 Kelvin  Standard Pressure:  1 atm  kPa  760 mmHg  760 torr

 Discovered by yet another dead guy!   Equal volumes of gases at the same temperatures and pressures contain the same number of molecules.  1 mol of any gas occupies 22.4 Liters at STP.  Coefficients in chemical equations can represent moles, molecules, and volumes of the reactants or products.  Equations can be…  Mole to Mole  Volume to Volume  Moles to Volume  All require factor-label method Amedeo Avogadro

Dan Jugo and Ryan Spoltore

 Organic Molecule- an organic molecule contains carbon and hydrogen ▪ Examples: carbohydrates, proteins, and lipids  Inorganic Molecules- inorganic molecules have either one or no carbon or hydrogens ▪ Examples: water, carbon dioxide (exception)

 Crude oil has components with different boiling points.  The components are heated and their vapors are passed into a column.  The vapors go from high to low  Components of higher boiling points condense and return to the solution  Components of lower boiling points pass through the column and are collected.

 Density is mass/volume  Density is affected by the number carbon atoms present in the solution  As we learned in the Viscosity Lab when there are more carbons the density of the solution is higher

 Hydrocarbons- molecular compounds that contain atoms of the elements hydrogens and carbons  Small hydrocarbon molecules (contain 1-4 carbons) have low boiling points because the are only slightly affiliated with each other or to other petroleum molecules

 Meth- 1 carbon  Eth- 2 carbons  Prop- 3 carbons  But- 4 carbons  Pent- 5 carbons  Hex- 6 carbons  Hept- 7 carbons  Oct- 8 carbons  Non- 9 carbons  Dec- 10 carbons

 Alkane- identify alkanes by ending: -ane  Saturated  Single bonds  Formula for linear alkanes: C n H 2n + 2  Formula for branched alkanes: C n H 2n + 2, n > 3  Fewer number of carbons, the lower the intermolecular forces; thus, the lower the boiling point  Greater number of carbons, the greater the surface area  The more carbon atoms, the higher the viscosity.  Example: Ethane

 Alkene identified by -ene ending  Unsaturated  Single bonds with at least one double carbon to carbon bond  Have a higher boiling point than alkanes because a double bond is stronger than a single bond.  Due to the double bonds, the substances are less viscous  Surface area is less than alkanes

 Alkynes- end in –yne  Unsaturated  At least one triple bond between carbons  Higher boiling points than alkanes or alkenes  Due to triple bonds alkynes are less viscous than alkenes  Surface area even less due to triple bonds

 Same number of carbons and hydrogens, just varying structure  Isomers all have the same chemical formula  When a number appears before the hydrocarbon that identifies where the double or triple bonds are located

 Branched chain- made from carbon atoms where at least one carbon atom is joined onto more than two other carbon atoms. Lower boiling points than straight chains.  Straight chain- made from carbon atoms joined onto no more than 2 other carbons

 Molecular Formula shows the number of carbons and hydrogens but not the structure or electrons. C4H10 Butane

 Structural shows where the carbons and hydrogens are located and the types of bonds

 Dot diagrams show where the electrons are between each carbon and hydrogen and also the types of bonds C C H H HH

 When monomer molecules are combined to create a polymer