∆H: Change in chemical energy under conditions of constant pressure.̵� :00� Standard conditions of pressure of 1x10 Pa and stated temperature. Also, the standard

states of reactants and products.Standard Enthalpy of Formation: The enthalpy change when 1 mole of a substance is formed

from its elements with all reactants and products in their standard states.

Standard State: The most stable form of a substance under standard conditions.Standard Enthalpy of combustion: The enthalpy change when 1 mole of a substance burns

completely in oxygen with all reactants and products in their standard states.

Hess’s Law: The enthalpy change for a chemical reaction is independent of the route followed.Specific Heat Capacity: This is the amount, in joules, of energy required to raise the temperature

of 1ml of water 1oc.∆H: -(4.18×Mass×∆T÷1000)/MOLES Bond Enthalpy: The mean enthalpy change when 1 mole of covalent bonds is broken

homolytically in the gaseous phase. Nucleophile: Electron pair donor.Electrophile: Electron pair acceptor.Reagent: Chemical/chemicals that react with an organic molecule.Substrate: The organic molecule that undergoes the reaction.Addition Reacton: An unsaturated molecule (alkene) becomes saturated.Elimination Reaction: Saturated (alkane) becomes unsaturated.Substitution Reaction: Saturated (alkane) remains saturated, condition: aqueous reagent.Base: Curly arrow begins here but goes to Hydrogen, condition: alcoholic reagent.Dynamic Equilibrium: Forwards and backwards reactions proceeding at equal rates with the

concentration of reactants and products as constant.Le Chatelier’s Principle: If we change the external condition of a reaction at equilibrium, the

position of equilibrium will move so as to oppose the external change.Compromise: 450oc temperature and 200atms pressure.Activation Energy (Ea): The minimum energy the colliding particles must have for a chemical

reaction to occur.Most Probable Energy (Emp): This is the hump that takes place on the Maxwell Distribution

Graph.Catalyst: What: A substance which speeds up a chemical reaction but remains chemically

unchanged by the reaction. How: A catalyst provides an alternative reaction pathway of lower activation

energy.Reaction Rate: Change in concentration of a substance in a unit of time.Reagent of Oxidating Alcohols: Acified Potassium Dichromate (orange)Product of Oxidating Alcohols: Cr3+ (green)-it is an oxidising agent, therefore it is reduced.Bio-Fuels: Fuel produced from biological or renewable sources.Carbon Neutral: No net increase to the CO2 level in the atmosphere.Major Product: The most stable intermediate forms more often giving the major product.Polymerisation: Reaction which turns many small molecules into long chain molecules.How isomers found in Infa-red Spectrum: Finger print region unique to all compounds

comparison to authentic sample.Primary Alcohols: Oxidised to Aldehydes, then to Carboxylic Acid.Seconday Alcohols: Oxidised to Ketones.Reducing Agents: Gains Oxygen, Loses Electrons, Loses Hydrogen.Oxidising Agents: Loses of Oxygen, Gains of Electrons, Gains Hydrogen.Electronegativity: Ability to attract a pair of shared electrons in a covalent bond.Ores: Naturally occurring materials from which we can extract a metal commercially.Alloys: Mixture of metals.Stereoisomerism: Compounds with the same structural formula with bonds arranged differently

in space.Structural Isomers: Have the same molecular formula but different structural formulae.Hydrolysis: Splitting C-X bonds using waterMolecular Ion: The molecule with an electron knocked offRadical: An unpaired electron.Substitution: Replacement of the Halogen.