Standard enthalpy of formation - the energy transferred when1 mole of the compoundis formed fromits elementsunderstandard conditions (298K and 100kpa), all reactants and products being in their standard states, Enthalpy of atomization - the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state, Sublimation - a solid metal turning to gaseous atoms, Bond dissociation - the standard molar enthalpy change when one mole of a covalent bond is broken into two gaseous atoms (or free radicals), Ionization energy - the enthalpy change required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous ions, Second ionization energy - the enthalpy changeto remove 1 mole of electrons from one mole of gaseous 1+ ions to produces one mole of gaseous 2+ ions., Electron Affinity - the enthalpy change that occurs when 1 mole of gaseous atoms gain 1 mole of electrons to form 1 mole of gaseous ions with a–1 charge, Lattice enthalpy - the standard enthalpy change when1 mole of an ionic crystal lattice is formed from its constituentions in gaseous form, Lattice dissociation - the standard enthalpy change when 1 mole of an ionic crystal lattice form is separated into its constituent ions in gaseousform., Enthalpy of hydration - when one mole of gaseous ions become aqueous ions., Enthalpy of solution - the standard enthalpy change when one mole of an ionic solid dissolves inalarge enough amount of water to ensure that the dissolved ions are well separated and do not interact with oneanother.,

Thermodynamics

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