Energetics 2 Flashcards
Lattice energy
The energy change when one mole of an ionic solid is formed from its gaseous ions
Atomisation energy
The energy change for the formation of one mole of gaseous atoms from an element in its standard state at 298K and 100kPa
Eg 1/2Br2(l)=>Br-(g)
Electron affinity
First electron affinity is the energy change for the addition of one electron for each mole of atoms in the gas phase
Second electron affinity
Energy change for the addition of one electron for each mole of ions with a negative charge in the gas phase
Lattice energy provides a measure of
Ionic bond strength
Always exothermic as is the energy of bonds being made
Experimental lattice energy value is
From a born-Haber cycle
Theoretical lattice energy value is
Obtained from electrostatic theory
Based on: ionic charges and ionic radii
Assumes perfect ionic bonding
Comparing experimental and theoretical lattice energy values indicates
The degree of covalent bonding
Possible covalent character?
Polarising power
Based on the strength of the pull of cations on the electrons and how much the anion allows the electrons to be pulled
Factors that increase polarisation in ionic compound are
- increased charge on anion or cation
- increased size of anion
- decreased size of cation
The greater the polarisation effect on covalent character
The greater the covalent character
Hydration of ions
When ionic substances in water, polar water highly attracted to ions
The process of water molecules linking to ions
Water molecules are vibrating, s as they bond to the ions they the ions free from the lattice
Enthalpy of hydration
Heat energy change when one mole of gaseous ions dissolve in an excess of water to form an infinitely dilute solution under standard conditions
Enthalpy of solution
Heat energy change when one mole of ionic solid dissolved in excess water in standard conditions
Enthalpy of hydration is affected by
Ionic radii
Ionic charges
Greater attraction more energy released