Unit 3 Chemistry Summary
- Created by: Lolo23
- Created on: 14-05-18 10:06
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- Unit 3 Chemistry
- Redox Reactions
- Interconversion Reaction
- Acidified Manganate
- Potassium Dichromate
- Reduction of Iodine via Thiosulphate
- Redox and Standard Electrode Potential
- Oxidation Numbers
- Electrodes
- Standard Hydrogen Electrode
- Hydrogen Fuel Cells
- Advantages and Disadvantages
- Electrochemical Series
- Standard Electrode Potential
- Chemistry of the P Block
- Key Ideas in the P Block
- Electron Configuration
- Oxidation States
- Maximum Covalency
- Amphoteric Behaviour
- Group III
- Electron Deficiency
- Boron Nitride
- Group IV
- Acid-Base Properties of Oxides
- Oxidation States
- Group VII
- Reaction of Chlorine with NaOH
- Uses of Halogen containing compounds
- Reaction of H2SO4 on NaX
- Patterns in Group VII
- Key Ideas in the P Block
- D Block Transition Metals
- Electron Configuration
- Ligands
- D block characteristics
- Catalysts
- Colouring of Transitions Metals
- Kinetics
- Measuring Rate of Reactions
- Sampling and Quenching
- Calculating Rates
- Rate Equation
- Units of Rate Constant
- Arrhenius Equation
- Finding the Activation Energy
- Effects on Rate
- Temperature
- Catalysts
- Rate determing Step
- Enthalpy Changes
- Principle of Conserving Energy
- Atomisation
- Lattice Formation
- Lattice Breaking
- Hydration
- Solution
- Born Haber Cycles
- Affects of Factors
- Lattice Enthalpy
- Hydration Enthalpy
- Stability of Compounds
- Principle of Conserving Energy
- Entropy Changes
- Factors
- Physical State
- Amount of Energy a Substance has
- Number of Particles
- Calculating Standard Entropy Changes
- Free Energy
- Factors
- Equilibria Constants
- Kc
- Kp
- Le Chatelier's Principles
- Relationship between Kc/Kp and Gibbs
- Kinetic and Equilibrium Data
- Acid-Base Equilibria
- Lowry-Bronsted Theory
- Strength and Concentrations of Acids and Bases
- Ka
- pH
- Kw
- Titration Curves
- Strong v Strong
- Weak A v Strong B
- Strong A v Weak B
- Indicators
- Buffers
- Weak Acid and Salt
- Weak Base and salt
- pH of equivalence point
- Strong v Strong
- Weak A v Strong B
- Strong A v Weak B
- Redox Reactions
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