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Initiation
Formation of a reactive intermediate
Propagation
Reactive intermediate reacts with stable molecule to produce another reactive intermediate or a product molecule
Termination
Side reactions that destroy the reactive intermediates, often resulting in nonradical product
Free Radicals
Species with odd numbers of electrons, stability determined by compound structure
Homolytic Cleavage
Bond cleavage resulting in free radicals, with electrons going to different atoms
Heterolytic Cleavage
Bond cleavage resulting in ions, with electrons going to the same atom
Primary
Halide bonded to a carbon atom bonded to only one other carbon atom, weak and least preferred
Secondary
Halide bonded to a carbon atom bonded to two other carbon atoms, slightly more stable
Tertiary
Halide bonded to a carbon atom bonded to three other carbon atoms, highly stable and preferred
Resonance
Increases stability of intermediate, preferred when exhibiting resonance
Exothermic Reaction
Weak bonds broken/strong bonds formed, releases energy
Endothermic Reaction
Strong bonds broken/weak bonds formed, requires input of energy
Chlorination Process
Highly exothermic process
Transition States
Highest position on the graph, where reactants change into products
Activation Energy
Difference between starting reactants energy and transition states energy
Rate-Limiting Step
Hump in the graph with highest energy, determines the overall reaction rate
Electronegativities
Higher values lead to quicker reactions, inversely proportional to size
Bond Dissociation Energy (+BDE)
Energy input required, useful in assessing energetics of a chemical reaction
Bond Formation Energy (-BDE)
Energy released, useful in assessing energetics of a chemical reaction
Hammond's Postulate
Related species similar in energy must be similar in structure, transition state resembles nearest stable molecule
Bromination
Highly selective reaction
Chlorination
Non-selective reaction