Thermochemical principles

Thermochemical principles

1. Shapes of molecules

   • Replusion pairs of electrons
     • Bonded/non-bonded
   • Common shapes (must learn w/ angle

2. Bonding (Lewis structure)

   • Ionic bonding
   • Covalent bonding

3. Periodic trends

   • Atomic radii
     • DOwn a group
     • Across a period
   • Ionic radii
     • Negative ions
     • Positive ions
   • Electronegativity (to determine polarity)

4. Electronic structure

   • Ionisation energy
     • Factors
     • Defination
     • Equation
     • Endothermic processess
   • Removal of electrons
   • Electron configuration

5. Intermolecular forces

   • Solubility (in water)
     • Able to hydrogen bond with water molecules (pg 43)
       • Ammonia gas (NH3)
       • Simple sugars
       • Lower molar mass alcohols
   • Bond strength
     • Energy required to break bonds
   • Forces (pg 39)
     • Temporary dipole (Weaker)
     • Hydrogen bonding (strongest)
     • Permanent dipole (Stronger)
   • Heats of reaction (change in enthalpy) (pg 46)
     • Endothermic
       • Heat is absorbed
       • More energy required to break exisiting bonds
     • Exothermic
       • Heat is released
       • More energy is required to form new bonds
     • Activation energy
     • Entropy, enthalpy and spontaneous reactions
       • Phases changes
         • Definations of different types of enthalpy
       • Denfinations
       • Balancing reactions
       • Measuring enthalpy changes (pg 52)
         • Using Hess's law (pg 62)