redox reactions electron transfer reactions electron transfer reactions are oxidation- reduction or...
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Redox Reactions
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Electron Transfer ReactionsElectron Transfer ReactionsElectron Transfer ReactionsElectron Transfer Reactions• Electron transfer reactions are oxidation-reduction or redox
reactions.
• Results in the generation of an electric current (electricity)
or be caused by imposing an electric current.
• Therefore, this field of chemistry is often called
ELECTROCHEMISTRY.
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2Mg (s) + O2 (g) 2MgO (s)
2Mg 2Mg2+ + 4e-
O2 + 4e- 2O2-
Oxidation half-reaction (lose e-)
Reduction half-reaction (gain e-)
Electrochemical processes are oxidation-reduction reactions in which:
• the energy released by a spontaneous reaction is converted to electricity.
0 0 2+ 2-
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Terminology for Redox ReactionsTerminology for Redox ReactionsTerminology for Redox ReactionsTerminology for Redox Reactions
• OXIDATIONOXIDATION—loss of electron(s) by a species; —loss of electron(s) by a species; increase in oxidation number; increase in oxygen.increase in oxidation number; increase in oxygen.
• REDUCTIONREDUCTION—gain of electron(s); decrease in —gain of electron(s); decrease in oxidation number; decrease in oxygen; increase oxidation number; decrease in oxygen; increase in hydrogen.in hydrogen.
• OXIDIZING AGENTOXIDIZING AGENT—electron acceptor; species is —electron acceptor; species is reduced. (an agent facilitates something; ex. reduced. (an agent facilitates something; ex. Travel agents don’t travel, they facilitate travel)Travel agents don’t travel, they facilitate travel)
• REDUCING AGENTREDUCING AGENT—electron donor; species is —electron donor; species is oxidized.oxidized.
• OXIDATIONOXIDATION—loss of electron(s) by a species; —loss of electron(s) by a species; increase in oxidation number; increase in oxygen.increase in oxidation number; increase in oxygen.
• REDUCTIONREDUCTION—gain of electron(s); decrease in —gain of electron(s); decrease in oxidation number; decrease in oxygen; increase oxidation number; decrease in oxygen; increase in hydrogen.in hydrogen.
• OXIDIZING AGENTOXIDIZING AGENT—electron acceptor; species is —electron acceptor; species is reduced. (an agent facilitates something; ex. reduced. (an agent facilitates something; ex. Travel agents don’t travel, they facilitate travel)Travel agents don’t travel, they facilitate travel)
• REDUCING AGENTREDUCING AGENT—electron donor; species is —electron donor; species is oxidized.oxidized.
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You can’t have one… without the other!
• Reduction (gaining electrons) can’t happen without an oxidation to provide the electrons.
• You can’t have 2 oxidations only or 2 reductions only in the same equation. Reduction has to occur at the cost of oxidation
LEOLEO the lion says the lion says GERGER!!oossee
lleeccttrroonnss
xxiiddaattiioonn
aaiinn
lleeccttrroonnss
eedduuccttiioonn
GER!GER!
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Another way to remember
•OIL RIGxxiiddaattiioonn
ss oossee
eedduuccttiioonn
ss aaiinn
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•
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Formation Silver Crystals
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Review of Oxidation numbers
The charge the atom would have in a molecule (or anionic compound) if electrons were completely transferred.
1. Free elements (uncombined state) have an oxidation number of zero.
Na, Be, K, Pb, H2, O2, P4 = 0
2. In monatomic ions, the oxidation number is equal to the charge on the ion.
Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2
3. The oxidation number of oxygen is usually –2. In H2O2
and O22- it is –1.
4.4
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4. The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds. In these cases, its oxidation number is –1.
6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion.
5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1.
HCO3-
O = -2 H = +1
3x(-2) + 1 + ? = -1
C = +4
Oxidation numbers of all the atoms in HCO3
- ?
4.4