Born-Haber Cycles
暂无描述。系统推荐的高质量记忆内容，适合每天坚持背诵学习。
卡片预览 (19 张)
Define standard enthalpy of formation
The enthalpy change when 1 mole of a compound is formed from its elements with all reactants and products in their standard states at 298K and 100kPa
Define standard enthalpy of combustion
The enthalpy change when 1 mole of a compound burns completely in oxygen at 298K and 100kPa with all reactants and products in their standard states
Define standard enthalpy of a reaction
The enthalpy change when the reactants react in stoichiometry shown in the equation at 298K and 100kPa
Define standard enthalpy of solution
The enthalpy change when 1 mole of a substance dissolves completely at 298K and 100kPa
Define standard enthalpy of hydration
The enthalpy change when 1 mole of gaseous ions are surrounded by water molecules and form a solution at infinite dilution at 298K and 100kPa
Define lattice enthalpy of association
The enthalpy change when 1 mole of a crystalline solid ionic compound is formed from its gaseous ions at 298K and 100kPa
Define lattice enthalpy of dissociation
The enthalpy change when 1 mole of a crystalline solid ionic compound dissociates into its gaseous ions
Define bond dissociation energy
The enthalpy change when 1 mole of a covalent bond is broken by homolytic fission at 298K and 100kPa
Define standard enthalpy of atomisation
The enthalpy change when 1 mole of gaseous atoms is formed from an element in its standard state at 298K and 100kPa
Define first ionisation energy
The enthalpy change where one mole of gaseous atoms loses an electron to form one mole of gaseous +1 ions
Define second ionisation energy
The enthalpy change where one mole of gaseous +1 ions loses an electron to form one mole of gaseous +2 ions
Define first electron affinity and state whether it is endothermic or exothermic
The enthalpy change where one mole of atoms gains an electron to form one mole of gaseous -1 ions Exothermic
Define second electron affinity and state whether it is endothermic or exothermic
The enthalpy change where one mole of gaseous -1 ions gain an electron to form one mole of gaseous -2 ions Endothermic due to repulsion
State the enthalpy changes used to calculate enthalpy of solution
Lattice dissociation enthalpy Enthalpy of hydration
Describe why there is a difference between the enthalpies of hydration of different ions
Different sizes and charge densities - more or less strongly attracted to δ+ H or δ- O in water
Describe the theoretical and experimental methods for finding lattice formation enthalpies
Theoretical - using a perfect ionic model Experimental - using a Born-Haber cycle
Describe the perfect ionic model
Ions are perfect spheres with full positive and negative charges They only experience electrostatic attraction
Describe why covalent character exists in ionic substances
Positive ions attracts electrons from negative ion Some electrons start to be shared between ions
State when covalent character is greatest
Small, highly charged positive ion (cation) Large, highly charged negative ion (anion)