lecture 20.2- oxidation numbers
DESCRIPTION
Section 20.2 lecture for Honors & Prep ChemistryTRANSCRIPT
Bellwork- Redox
Which species is oxidized? Which one is reduced? What acts as the oxidizing agent?
H+ (aq) + Li(s) Li+(aq) + H2(g)
N2(g) + O2(g) 2NO2(g)
Bellwork- Redox
Which species is oxidized? Which one is reduced? What acts as the oxidizing agent?
H+ (aq) + Li(s) Li+(aq) + H2(g)
C(s) + O2(g) 2CO2(g)
Cations in compounds or solutions are reduced to elemental metals
ex. Na+ + e- Na(s) reduction half-reaction
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Metals are oxidized into cationsex. Al(s) Al3+ + 3e- oxidation half-reaction
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Combustion reactions are redox reactions.
Ex. CH3 + O2 CO2 + H2O
Carbon & hydrogen are oxidized.
Oxygen is reduced.
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The attachment of oxygen is oxidation.
Ex. C becomes part of CO2
Carbon is oxidized.
Oxygen is always reduced.
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Assign an oxidation number to each
atom using the rules:
1. Elements are 0. ex. O2(g) , H2(g), Li(s)
Monatomic ions are their charge. ex. Na+ is +1 and Cl- is -1
2. For compounds
Oxygen is -2 Hydrogen is +1
The sum of the oxidation numbers must equal the charge on the compound.
Ex.
CO2
Oxygen is -2 and there are two, so carbon is +4.
2(-2) + _____ = 0+4
Ex.
NO3-
O is -2.
3(-2) = -6
-6 + _____ = -1-5
An increase in oxidation number is oxidation
A reduction in oxidation number is reduction
An element has been oxidized if..
• Electrons are lost
• Oxidation number increases
• Oxygen is gained Ex. S SO2
• Hydrogen is lost C2H6 C2H4