Energy Flashcards
Hess law
States that if a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same for each route
Lattice enthalpy
The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
Enthalpy change of formation
The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions
Enthalpy change of atomisation
The enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state
First ionisation energy
The enthalpy change that accompanies the loss of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
First electron affinity
The enthalpy change accompanying the addition of one electron to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions
Standard enthalpy change of solution
The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions
Standard enthalpy change of hydration
The enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water forming one mole of aqueous ions under standard conditions
Entropy
The quantitative measure of the degree of disorder in a system
Entropy change of reaction
The entropy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states
Free energy change
The balance between enthalpy, entropy and temperature for a process
Oxidation
Loss of electrons
Reduction
Gain of electrons
Standard electrode potential
The emf of a half cell compared with a standard hydrogen half cell, measured at 298K with solutions of 1moldm and a gas pressure of 100 kpa
