constructing born haber cycles Flashcards
2 factors that effect strength of ionic bonding
size of ions and charge of ions
when does ionic bond strength increase
when ions smaller and have higher charges
what happens if ionic bonding is stronger
the lattice enthalpy is more exothermic
lattice enthalpy definition
enthalpy change when one mole of an ionic solid is formed from its constituent ions in the gas state
first step of alternative route for lattice enthalpies hess cycle
separation
-negative of enthalpy formation
second stage in hess law alternative route to
atomisation
-element in its standard state
-1/2cl2 —>CL
enthalpy change of separation
enthalpy change when one mole of an ionic compound is separated into its constituent ions in their gas phase
when can you link enthalpy of atomisation and bond dissociation
when elements in standard states are gaseous
-when they are covalently bonded
third step in alternative route in lattice enthalpies
electron affinity calculated using ionisation energies
fourth and last step of alternative route lattice enthalpies
adding electrons
electron affinities
is lattice enthalpy exo or endo
exothermic
equation for calculating lattice enthalpy
formation= everything else added together
then rearrange for lattice enthalpy
equation when lattice dissociation is used
formation+ lattice dissociation = everything else
perfect ionic model
all ions perfectly spherical and all bonding ionic
what does theoretical values not account for
covalent character in bonding
what suggest if something has larger covalent character or not
the difference between theoretical and experimental values
what happens to anion as it bonds with cation
its electron cloud distorts and it becomes polarised by the cation
what makes ion more polarising
small and higher charge
which ions have highest polarising power
small
high charge
have positive charge
polarisability
larger and more highly charges ions
factors that affect polarisation
polarising power of cation
polarisability of anion
whats an exception exam question to polarization rules
silver halides
example of comparing bonding
NaCl has larger difference in theoretical and experimental lattice enthalpies
-NaCl has a larger amount og covalent character
-NaCl has larger amount of polarisation
-since anions comparing both Na- this mean Ag+ must have higher polarising power than Na+
how to answer silver halides question on polarization
AgBr has a larger difference in the theoretical and experimental lattice enthalpies
-AgBr has a larger amount of covalent character
what are hydrated ions held together by
ion dipole forces
enthalpy of solution
when one mole of a solute in its standard state dissolves in water to form aqueous ions
enthalpy of hydration
when one mole of gaseous ions are converted to aqueous ions
factors that determine strength between ions and polar water molecules
magnitude of ions charge and size of ion