AS-Level Chemistry Module 2 - OCR A

AS-Level Chemistry Module 2 - OCR A

1. Atoms and Moles

   • The Atom
     • Structure
       • Protons, Neutrons, Electrons
     • Nuclear Symbols
       • Mass number
       • Atomic Number
     • Atoms and Ions
       • Positive or Negative Charge
     • Isoptoes
       • Same number of protons, different number of neutrons
   • Atomic Models
     • JJ Thomson
       • Plum Pudding Model
     • Rutherford's Model
       • Gold Foil Experiment
     • Bohr's Model
       • Four basic principles
   • Relative Mass
     • Atomic Mass
       • Calculating
     • Isotopic Mass
     • Molecular Mass
     • Formula Mass
   • The Mole
     • What is a mole?
     • Molar Mass
     • Calculations
   • Gas Volumes
     • Gas Volume
     • Ideal Gas Equation
       • pV=nRT
   • Concentration Calculations
     • Moles and Concentration
       • n=cxV(dm3)

2. Formulas and Equations

   • Formulas
     • Empirical and molecular formulas
   • Calculating Formulas
     • Empirical formula
       • Experimental data
       • Percentage compositions
     • Molecular formula
   • Chemical Equations
     • Balancing equations
     • Ionic Equations
   • Equations and Calculations
     • Calculating masses
     • Gas volumes
     • State symbols
   • Formulas of Ionic Compounds
     • Formation of ions
     • Formulas

3. Reactions and Calculations

   • Acids, Bases and Salts
     • What are they?
     • Strength of acids and bases
     • Reactions
       • Acid-base reactions
       • Acids and Oxides
       • Acid and metal oxides
       • Acid and metal hydroxides
       • Acids and carbonates
   • Anhydrous and Hydrous Salts
     • What are they?
     • Finding the formula of hydrated salts
   • Titrations
     • Performing titrations
     • Indicators
     • Practical Techniques
       • Measuring masses
       • Volumes of solutions
     • Standard Solutions
       • Preparing solutions
       • Calculations
   • Titrations Calculatons
     • Calculating concentration
     • Polyprotic acids
     • Calculating volumes
   • Chemical Yield
     • Theoretical yield
     • Percentage yield
   • Atom Economy
     • What is it?
     • Calculating it
     • Addition and substitution reactions
     • Atom economy and percentage yield
     • Atom economy in industry
   • Oxidation Number
     • Finding
       • From formulas
       • From systematic names
     • Assigning
     • Using
       • Working out systematic names
       • Working out formulas
   • Redox Reactions
     • What are they?
     • Changing oxidation numbers
     • Reactions with dilute acids and metals

4. Electrons, Bonding and Structure

   • Electronic Structure
     • Electron Shells
       • Sub-shells
         • s-shells
           • 2 electrons, 1 orbital
         • p-shells
           • 6 electrons, 3 orbitals
         • d-shells
           • 10 electrons, 5 orbitals
         • f-shells
           • 14 electrons, 7 orbitals
       • Shells
         • 1st shell
           • 2 electrons
         • 2nd Shell
           • 8 electrons
         • 3rd shell
           • 18 electrons
         • 4th shell
           • 32 shells
     • Orbitals
       • s-sub shells are spherical
       • p-sub shells are dumb-bell
     • Electron Configurations
       • Sub-shell notation
       • Electrons in boxes
       • Energy Level Diagrams
   • Ionic Bonding
     • Oppositely charged ions are attracted together
       • Ionic compound forms
         • Overall charge is 0
     • Dot and Cross diagrams
     • Giant Ionic Lattices
       • Regular shape
       • Attracted to oppositely charged ions in all directions
     • Behaviour of Compounds
       • Electrical Conductivity
         • Conduct when molten or dissolved
       • Melting and boiling points
         • High
           • Strong electrostatic forces
       • Solubility
         • Dissolves in water
   • Shapes of Molecules
     • Linear
       • Berylium Chloride/Carbon Doixide
       • 180 degrees
     • Trigonal Planar
       • 120 degrees
       • Boron Triflouride
     • Tetrahedral
       • 109.5 degrees
       • Methane, Ammonium ion
     • Trigonal Pyramidal
       • Ammonia
       • 107 degrees
     • Non-linear
       • 104.5 degrees
       • Water
     • Trigonal bipyramidal
       • Phosphorous Pentachloride
       • 120, 90 degrees
     • Octahedral
       • 90 degrees
       • Sulphur hexaflouride
   • Polarisation
     • Electronegativity
     • Polar and non-polar bonds
     • Polar molecules
     • Predicting bond types
   • Intermolecular Forces
     • Induced dipole-dipole interactions
     • Permanent dipole-dipole interactions
     • Hydrogen Bonding
     • Behaviour of simple covalent compounds
       • Electrical Conductivity
       • Melting and boiling points
       • Solubility
     • Trends in melting and boiling points
   • Covalent Bonding
     • Molecules
       • Non-metals
       • Share electrons, each atom gets 8 electrons in their outer shell
     • Dot and cross
       • Single, Double and triple bonds
     • Dative covalent
       • 1 atom provides both shared electrons
     • Special Cases
       • Boron Triflouride
       • Sulphur Hexaflouride
     • Covalent bond strength
       • Average bond enthalpy