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radical
reactive intermediate with a single unpaired electron
classified at primary, secondary, tertiary (like others)
tertiary most stable & take least energy to break, primary least stable & takes most energy
radicals are sp2 hybridized & trigonal planar
features of radical reactions
need added energy (light or heat)
radical initiator (peroxides) contain extra weak bonds that source radicals
heating it causes homolysis of the weak OO bond, forming 2 RO radicals
three main steps of a radical reaction
initiation: 2 radicals formed by homolysis of a sigma bond
propagation: radical reacts with another reactant to form a new sigma bond and another radical
termination: two radicals combine to form a stable bond
monohalogenation
when a single H atom on a carbon has been replaced by a halogen
radical chlorination vs bromination
chlorination forms a 1:1 mixture of products (unselective)
bromination often yields one major (markovnikov) product
chlorination is faster
abstraction of a primary or secondary hydrogen by Cl is exothermic, by Br is endothermic
reactivity of C-H bonds
primary bonds are strongest and least reactive, take most energy to form
tertiary bonds are weakest and most reactive, take least energy to form
radical vs ionic addition
radical involves an initial attack by the radical
ionic involved an initial attack by a proton (H+)
polymers
large molecules made up of repeating units of monomers
polymerization
process of joining together monomers to make polymers
more substituted radical adds to less substituted end of monomer (head-to-tail polymerization)