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REDOX REACTIONS
BONDING
• Occurs in order for atoms to become stable
• Atoms need a full outer shell to be stable• Atoms may form :
Ionic bonds: gain/lose e- Covalent bonds: sharing electrons
Includes diatomic molecules – HOFBrINCl
Hydrogen bonds: due to polarity of molecules
REDOX REACTIONS
• Reduction – Oxidation Reaction• Most important energy changes occur
in living organisms via redox reactions (rxns)
• Involves the transfer of electrons between two atoms One atom is oxidized One atom is reduced
• They always occur together
REDUCTION
• Electrons are gained• Charge is negative hence the term
‘reduced’• Energy is absorbed – an ENDERGONIC rxn• Can be recognized in 3 ways:
1) removal of an oxygen 2) gaining a hydrogen 3) gaining an electron
OXIDATION
• Electrons are removed or lost• Molecule becomes less negative• Releases energy – an EXERGONIC rxn• Can be recognized in 3 ways:
Oxygen is added Hydrogen is removed Electron is removed Does not necessarily involve oxygen
Memory Tip
LEO (the lion says) GER
LEO: Lose Electrons OxidationGER: Gain Electrons Reduction
Redox Terminology
• Electron Donor: one that loses e-
• Electron Acceptor: one that gains e-
• Oxidizing Agent: one that is reduced but causes another
atom to be oxidized• Reducing Agent:
one that is oxidized but causes another atom to be reduced
TRY THIS
• Na+ + Cl- NaCl
• Which atom is oxidized? Na
• Which atom is the oxidizing agent? Cl
TRY THIS
Iron(III) oxide lost its oxygens – it has been reduced. Oxidizing agent
Carbon monoxide gains oxygen – it has been oxidized. Reducing agent.
Role of Electronegativity
• In order to oxidize an atom, energy is needed to force the electrons to leave their parent atom
• Substances with a high electronegativity do not let their e- go easily and therefore require more energy to be oxidized than those with low electronegavities
EXAMPLE
OTHER EXAMPLES
• Oxidation: Bleaching Corrosion Antiseptics
• Reduction: Photosynthesis Antioxidants (prevent oxidation by
reducing) Photography
Reading
• Read page 114 to120 of textbook