3.6 Enthalpy Changes 2 Flashcards
enthaply of atomisation?
the enthalpy change when 1 mole of gaseous atoms is formed from a compound in its standard state under sc
lattice enthalpy of formation??
the enthalpy change when 1 mole of solid ionic compound is formed frm its gaseous constituent ions under sc
lattice breaking enthalpy??
the energy req to break apart an ionic lattice into its gaseous constituent ions under sc
enthalpy of solution??
the enthalpy change when one mole of an ionic solid is dissolved in a solvent to infinite dilution so ions no longer interact under sc
enthalpy of hydration??
the enthalpy change when one mole of aq ions is formed from one mole of gaseous ions
what affects the solubility of ionic compounds in water??
the solubility of ionic compounds depends on the balance bet the hydration enthalpy of ions in the compound and the lattice breaking enthalpy of the compound
what factors affect enthalpy of hydration??
hydration enthalpy of an ion depends on the amnt of attraction bet ions and water molecules, the bigger the charge and the smaller the ion, the larger the enthalpy of hydration
Hess’s law??
the enthalpy change of a rctn is independent of the route taken
how can enthalpy change of a soln be calc using an energy cycle??
lattice breaking enthalpy & enthalpy change of hydration used in energy cycle to calc enthalpy change of soln using Hess’s kaw
Born-Haber cycle??
lattice enthalpy cant be calc directly so born-haber cycle used to calc lattice enthalpy by applying Hess’s law, by comparing enthaply of formation of the ionic compound to the enthalpy req to make gaseous ions from the elemnt
standard enthalpy of formation?
the enthalpy change when 1 mol of a compound is formed from its elements in their standard states in scs
1st IE??
the enthalpy change when 1 mole of gaseous atoms forms one mole of gaseous 1+ ions
1st EA??
the enthalpy change when 1 mole of gaseous atoms forms one moole of 1- ions
what is the perfect ionic model?
the perfect ionic model assumes that all ions are perfectly spherical and that the bonds have no covalent character
why are theoretical lattice enthalpies often diff from experimental ones??
theoretical lattice enthalpies use calculations based on a perfect ionic model of lattice, experimental values differ as most ionic compounds have some covalent character, the more polarisation in ionic bond, the more covalent character of compound