Thermochemical principles

Shapes of molecules
1. Replusion pairs of electrons
  1. Bonded/non-bonded
2. Common shapes (must learn w/ angle
Bonding (Lewis structure)
1. Ionic bonding
2. Covalent bonding
Periodic trends
1. Atomic radii
  1. DOwn a group
  2. Across a period
2. Ionic radii
  1. Negative ions
  2. Positive ions
3. Electronegativity (to determine polarity)
Electronic structure
1. Ionisation energy
  1. Factors
  2. Defination
  3. Equation
  4. Endothermic processess
2. Removal of electrons
3. Electron configuration
Intermolecular forces
1. Solubility (in water)
  1. Able to hydrogen bond with water molecules (pg 43)
    1. Ammonia gas (NH3)
    2. Simple sugars
    3. Lower molar mass alcohols
2. Bond strength
  1. Energy required to break bonds
3. Forces (pg 39)
  1. Temporary dipole (Weaker)
  2. Hydrogen bonding (strongest)
  3. Permanent dipole (Stronger)
4. Heats of reaction (change in enthalpy) (pg 46)
  1. Endothermic
    1. Heat is absorbed
    2. More energy required to break exisiting bonds
  2. Exothermic
    1. Heat is released
    2. More energy is required to form new bonds
  3. Activation energy
  4. Entropy, enthalpy and spontaneous reactions
    1. Phases changes
      1. Definations of different types of enthalpy
    2. Denfinations
    3. Balancing reactions
    4. Measuring enthalpy changes (pg 52)
      1. Using Hess's law (pg 62)

Resource summary

	Created by Billie Sims-Fowler over 7 years ago