Thermodynamics

• Enthalpy of formation

  Energy required to form 1 mole of a substance from its elements in standard conditions and states
• Lattice enthalpy

  Enthalpy change to form 1 mole of an ionic lattice from its gaseous ions in SCS
• Enthalpy of neutralization

  When solutions of acid and base react to form 1 mole of water in Standard conditions and states
• Enthalpy change of hydration

  Enthalpy change to dissolve 1 mole of a substance in water
• Enthalpy change of solution

  Enthalpy change to form 1 mole of aqueous ions from its gaseous ions
• First ionisation energy

  Energy required to remove one electron from a gaseous ion in standard conditions
• Enthalpy of hydration calculation


  Hhyd= Hlatt + Hsol
• Effect of ionic charge on enthalpy

  As Ionic charge increases the charge density increases, enthalpy becomes more exothermic due to the stronger electrostatic forces of attraction between opposite ions
• Effect of ionic radius on enthalpy

  As ionic radius increases, charge density decreases so enthalpy becomes more exothermic as it has weaker electrostatic forces of attraction between ions
• Effect of concentration on equilibrum

  Increase in reactants = Right shift

  Decrease in reactands = left shift
• Effect of pressure on equilibrium

  Increase= shift to side with less moles

  Decreases = shift to side with more moles
• effect of temperature on equilibrium

  decrease = shift to the left

  increase = shift to the right
• Enthalpy of combustion

  The enthalpy change for the complete combustion of 1 mole of a substance
• Equilibrium constant calculation

  Kc = Moles of C X D / Moles of A X B
• Transition metal

  A D-block element that has an ion with an incomplete or partially complete d-sub shell
• Properties of transition metals

  Have multiple oxidation states for each element in its compound

  Form coloured ions

  Used as catalysts