Term | Definition |
Endothermic Reaction | A reaction that (overall) takes in energy from the surroundings. +ve delta H value |
Exothermic Reaction | A reaction that (overall) gives out energy into the surroundings. -ve delta H value |
Enthalpy Change | Temperature change caused by a reaction at constant pressure |
Activation Energy | The minimum energy required for a reaction to occur successfully/for collisions to be succesful |
Nucleopile | An electron pair donor |
Primary Alcohol | An alcohol in which the OH group is bonded to a carbon that is bonded to one other carbon |
Secondary Alcohol | An alcohol in which the OH group is bonded to a carbon that is bonded to two other carbons |
Tertiary Alcohol | An alcohol in which the OH group is bonded to a carbon that is bonded to three other carbons |
Standard Molar Enthalpy Change of Bond Dissociation | The enthalpy change required to break one mole of the same covalent bonds under standard conditions, all species in the gaseous state |
Standard Molar Enthalpy of Combustion | The enthalpy change when one mole of compound is completely burned in oxygen under standard conditions, all reactants and products in their standard states |
Standard Molar Enthalpy of Formation | The enthalpy change when one mole of compound is formed under standard conditions from its elements in their standard states |
Hess' Law | The total enthalpy change of a reaction is independent of the route taken |
Dynamic Equilibrium | When the forward and backward reactions are occurring at the same rate and so the concentration of the reactants and products remains constant. It occurs in a closed system. |
Le Chatelier's Principle | If a system at equilibrium is disturbed, the centre of equilibrium moves in the direction that tends to reduce the disturbance and minimise the change. |
Catalyst | Reduces the activation energy by providing an alternative route for the reaction. |
Reduction | Gain of electrons and a decrease in oxidation state |
Oxidation | Loss of electrons and an increase in oxidation state |
Reducing Agent | Reducing agents donate electrons (and so cause reduction) |
Oxidising Agent | Oxidising agents accept electrons (and so causes oxidation) |