Thermodynamics - Physical 2 Flashcards
What does Hess’s Law state?
The enthalpy change for a reaction is independent of the route taken
Define standard enthalpy of formation.
The enthalpy change when one mole of a compound is formed from its constituent elements in standard conditions, with all products and reactants in their standard states.
What is the standard enthalpy of an element?
Zero, by definition.
Define standard enthalpy of combustion
The enthalpy change when one mole of a substance is completely burnt in (excess) oxygen
Define standard enthalpy of atomisation
Enthalpy change when one mole of gaseous atoms is formed from a compound in its standard state in standard conditions.
Define first ionisation energy
Enthalpy change when one mole of electrons is removed from one mole of gaseous atoms to form one mole of gaseous 1+ ions.
Define second ionisation energy.
Enthalpy change when one mole of electrons is removed from one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
Define first electron affinity
Enthalpy change when one mole of gaseous atoms gains one mole of electrons to form one mole of gaseous 1- ions.
Define second electron affinity.
Enthalpy change when one mole of gaseous 1- ions gains one mole of electrons to form one mole of gaseous 2- ions
Define lattice enthalpy of formation
Enthalpy change when one mole of solid ionic lattice is formed from its constituent gaseous ions.
Define lattice enthalpy of dissociation.
Enthalpy change when one mole of solid ionic lattice is dissociated (broken into) into its gaseous ions
Define enthalpy of hydration.
Enthalpy change when one mole of gaseous ions become hydrated/dissolved in water to infinite dilution [water molecules totally surround the ion]
Define enthalpy of solution
Enthalpy change when one mole of solute dissolves completely in a solvent to infinite dilution.
Define mean bond dissociation enthalpy
Enthalpy change when one mole of (a certain type of) covalent bonds is broken, with all species in the gaseous state
Write example equations for:
Standard enthalpy of formation Standard enthalpy of combustion Standard enthalpy of atomisation First ionisation energy
Second ionisation energy First electron
Standard enthalpy of formation Mg (s) + 1⁄2 O2 (g) → MgO (s)
Standard enthalpy of combustion CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g) Standard enthalpy of atomisation 1/2I2 (g) → I (g)
First ionisation energy Li (g) → Li+ (g) + e-
Second ionisation energy Mg+ (g) → Mg2+ (g) + e-
First electron affinity Cl (g) + e- → Cl - (g)
Write example equations for:
Second electron affinity Lattice enthalpy of formation Lattice enthalpy of dissociation
Enthalpy of hydration Enthalpy of solution
Mean bond dissociation enthalpy
Second electron affinity O- (g) + e- → O2- (g)
Lattice enthalpy of formation Na+ (g) + Cl- (g) → NaCl (s) Lattice enthalpy of dissociation NaCl (s) → Na+ (g) + Cl- (g) Enthalpy of hydration Na+ (g) → Na+ (aq)
Enthalpy of solution NaCl (s) → Na+ (aq) + Cl- (aq)
Mean bond dissociation enthalpy Br2 (g) → 2Br (g)
What is a Born-Haber cycle?
Thermochemical cycle showing all the enthalpy changes involved in the formation of an ionic compound. Start with elements in their standard states (enthalpy of 0)
Draw a labelled Born-Haber cycle for the formation of sodium chloride lattice, including ionisation, electron affinity, formation, lattice formation etc.
check
What factors affect the lattice enthalpy of an ionic compound?
Size of the ions, charge on the ions
How can you increase the lattice enthalpy of a compound? Why does this increase it?
Smaller ions, since the charge centres will be closer together. Increased charge, since there will be a greater electrostatic force of attraction between the oppositely charged ions. N.B. Increasing the charge on the anion has a much smaller effect than increasing the charge on the cation, since increasing anion charge also has the effect of increasing ionic size.
How can Born-Haber cycles be used to see if compounds could theoretically exist?
Use known data to predict certain values of theoretical compounds, and then see if these compounds would be thermodynamically stable. Was used to predict the existence of the first noble gas containing compound.
What actually happens when a solid is dissolved in terms of interactions of the ions with water molecules?
Break lattice → gaseous ions; dissolve each gaseous ion in water. The aqueous ions are surrounded by water molecules (which have a permanent dipole due to polar O-H bond)
What is the perfect ionic model?
Assumes that ions are perfectly spherical and that there is an even charge distribution (100% polar bonds). Act as point charges.
Why is the perfect ionic model often not accurate?
Ions are not perfectly spherical. Polarisation often occurs when small positive ions or large negative ions are involved, so the ionic bond gains covalent character. Some lattices are not regular and the crystal structure can differ.
