Chemistry Module 3

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  • Created by: Ellen2745
  • Created on: 01-05-18 09:21
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  • Module 3
    • Periodicity
      • Arrangement of elements
        • Increase in atomic number
        • Define periodicity
        • Groups having the same chemical properties
      • Electron configuration
        • Periodic trends in electron configuration across Periods 2&3
        • ,s-, p- & d- blocks
      • First ionisation
        • Define first ionisation
        • Across Periods 2&3, and down a group
          • Attraction
          • Nuclear charge
          • Atomic radius
        • Prediction of successive ionisation energies
          • Number of electrons in each shell of an atom and the group of the element
      • Trend in structure and melting point
        • Define metallic bonding
        • Explanation of giant metallic lattice structure
        • Solid giant covalent lattices of carbon and silicon
          • Diamond
          • Graphite
          • Graphene
        • Physical properties of giant metallic and giant covalent lattices
          • melting and boiling point
          • Solubility
          • Electrical conductivity
    • Group 2
      • Redox reactions and reactivity
        • Loss of electrons, in redox reactions, form 2+ ions
        • Relative reactivities Mg-Ba, redox reactions with:
          • Oxygen
          • Water
          • Dilute acids
        • Trend in reactivity- first and second ionisation energies down the group
      • Reactions
        • Water and Group 2 oxides- trend of increasing alkalinity
        • Group 2 compounds as bases
          • Ca(OH)2 in agriculture- neutralise acid soils
          • Mg(OH)2 and CaCO3 as 'antacids'- treating indigestion
    • Halogens
      • Characteristic physical properties
        • Diatomic molecules
        • Explain the bp in terms of London forces
      • Redox reactions and reactivity
        • Gain one electron in redox reactions to form 1- ions
        • Trend in reactivity of the halogens by reacting with other halide ions
        • Explanation of the trend
          • Decreasing ease forming 1- ions
            • Attraction
            • Atomic radius
            • Electron shielding
        • Define disproportionation
          • Reaction of chlorine with water- water treatment
          • Reaction of chlorine with cold, dilute aqueous sodium hydroxide- bleach
        • Benefits of using chlorine to kill bacteria contrasted with associated risks- water treatment
      • Characteristic reactions
        • precipitation reactions
        • test with aqueous silver ions and then aqueous ammonia
    • Qualitative analysis
      • Test for ions
        • Anions
          • CO3 2- reacting with H+ forming CO2
          • SO4 2-, by precipitation with Ba 2+
          • Halides, Acidified silver nitrate and ammonia
        • Cations
          • NH4+ reacting with warm NaOH forming NH3
    • Enthalpy changes
      • Chemical reactions are exothermic or endothermic
      • Define:
        • Activation energy
        • Standard conditions
        • Enthalpy change of formation
        • Enthalpy change of combustion
        • Enthalpy change of neutralisation
      • q=mcT
      • Bond enthalpies
        • Define average bond enthalpy
        • Explanation of exothermic and endothermic reactions- bond breaking and making
        • Average bond enthalpies to calculate enthalpy changes and realted quantities
      • Hess' law and enthalpy cycles
        • Enthalpy change of reaction from enthalpy change of combustion
        • Enthalpy change of reaction from enthalpy change of formation
        • Enthalpy changes from unfamiliar enthalpy cycles
    • Reaction rates
      • Simple collision theory
        • Effect of concentration, including pressure of gases, on the rate of reaction- frequency of collisions
        • Calculation of reaction rates from the gradients of graphs measuring how a physical quantity changes with time
      • Catalysts
        • Explain the role of a catalyst
          • Increasing reaction rate without being used up by the overall reaction
          • Allowing a reaction to proceed via a different route with lower activation energy- enthalpy profile diagrams
        • Define homogenous and heterogenous catalysts
        • Catalysts have a great economic importance
          • Increase sustainability by lowering temperatures and reducing energy demand from combustion of fossil fuels with resulting reduction in CO2 emissions
      • Boltzmann distribution
        • Explanation of the proportion of molecules exceeding the activation energy and hence the reacction rate
          • Temperature changes
          • Catalytic behaviour
    • Chemical equilibrium
      • Dynamic equilibrium and Le Chatelier's principle
        • Dynamic equilibruim exists:
          • Closed system
          • Rate of the forward reaction equals the rate of the reverse reaction and the concentration don't change (products and reactants)
        • Effect of temperature, pressure and concentration
        • A  catalyst increases the rate of reaction, both directions, doesn't change the position of equilibrium
        • Importance to the chemical industry and the compromise between the equilibrium and rate
      • Equlilbrium constant
        • Homogenous reactions and calculations of the equilibrium constant
        • Estimation of the position of equilibrium from the magnitude of Kc

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