Chemistry

Chemistry

1. Miss Hayden

   • Formulae, equations and amount of substance
     • The Mole
       • How to count atoms
       • One Mole = 6.02x10^23
       • Mass --> Moles
         • Mass/MolesxRFM
         • Moles=Mass/RFM
     • Actual and Percentage yield
       • Percentage yield=Actual mass/theoretical yield x 100
     • Solutions
       • volume=moles/conc x 1000
       • Moles=Volume/1000 x conc
       • conc=moles/volume x 1000
     • Gases
       • moles=volume/24000
       • volume=moles x 24000
     • Calculating formula using moles.
       • 1) Symbols
         • 2) Masses
           • 3) Moles
             • 4) Mass/Moles
               • 5) Ratio
                 • 6) Formula
       • Empirical formula
         • 7) Weight
         • 1) Symbols
     • Converting molarity, masses and ppm
       • ppm=mass/total mass x 1,000,000
       • ppm to mass
         • Mass=ppm/1,000,000 x total mass
           • ppb=same, but divide by 1,000 after main calculation
     • Atom Economy
       • Mass of desired product/mass of all reactants

2. Mr Turton

   • Atomic Structure and the Periodic Table
     • Mass Spectrometry
       • 1) Vapoursation
         • 2) Ionization
           • 3) Acceleration
             • 4) Deflection
               • 5) Detection
                 • The ions are fired towards a detector where they pick up electrons and become stable atoms. The number of electrons collected is detected and determines which isotope(s) is/are present
               • The particles are deflected inside a magnetic field which can be varied in order to detect specific isotopes
             • The gas is accelerated through magnefied metal sheets round the spectrometer
           • The gas is ionized by having electrons fired at it
         • A material is vapourised and put into the spectrometre
     • Ionisation energies
       • All are Endothermic
         • Positive enthalpy change
       • Energy required to remove the most loosely held electron from one mole of gaseous atoms to produce 1 mole of gaseous ions, each with a charge of 1+
       • Ionisation energy is affected by 3 things:
         • Effect of shielding from the other shells
         • Distance from the nucleus
         • Effective nuclear charge
     • Electron configurations
       • Orbitals
         • Orbital energies, up in increasing energy
           • 1s
             • 2s
               • 2p
                 • 3s
                   • 3p
                     • 4s
                       • 3d
                         • 4p
                           • 4d
                             • 4f
                       • n=4
                   • n=3
               • n=2
             • n=1
       • Electron configuration rules
         • 1) The aufbau Principle
           • 2) Hund's rule
             • 3) The Pauli Exclusion Principle
               • Up and down pairs
             • Fill singly, then double up
           • start at bottom, work upwards
       • First ionization energies of the first 20 elements
         • First Ionization energies of the first 20 Elements

3. Miss Delegate

   • Formulae, equations and amounts of substance
     • Polyatomic ions
       • 1+ NH4
       • 3- PO4
       • 2- SO4 and CO3
       • 1-OH and NO3
     • Ionic equations
       • Pb(NO3)2 (aq) + 2KI (aq) --> PbI2 (s) + 2KNO3 (aq) Pb2+ (aq) +2I- --> PbI2 (s)
     • OIL RIG
       • Oxidation is loss of electrons
       • Reduction is gain of electrons
     • Making a salt
       • Reactions of Acids
         • Acid + Alkali-->Salt + Water
           • Acid + Metal-->Salt + Hydrogen
         • Acid + Metal Oxide-->Salt+Water
           • Acid + Metal Carbonate-->Salt + Carbon Dioxide + Water