Chemistry Module 3
- Created by: Ellen2745
- Created on: 01-05-18 09:21
View mindmap
- 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
- Arrangement of elements
- 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
- Redox reactions and reactivity
- 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
- Decreasing ease forming 1- ions
- 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
- Characteristic physical properties
- 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
- Anions
- Test for ions
- 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
- Explain the role of a catalyst
- Boltzmann distribution
- Explanation of the proportion of molecules exceeding the activation energy and hence the reacction rate
- Temperature changes
- Catalytic behaviour
- Explanation of the proportion of molecules exceeding the activation energy and hence the reacction rate
- Simple collision theory
- 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
- Dynamic equilibruim exists:
- Equlilbrium constant
- Homogenous reactions and calculations of the equilibrium constant
- Estimation of the position of equilibrium from the magnitude of Kc
- Dynamic equilibrium and Le Chatelier's principle
- Periodicity
Comments
No comments have yet been made