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Oxidation-Reduction Reaction:
an oxidation-reduction or redox reaction refers to a reaction where electrons are transferred between reactants;
Oxidation refers to the loss of electrons.
Reduction refers to the gaining of electrons.
An Oxidizing Agent is an element which causes oxidation (and is reduced as a result) by removing electrons from another species.
A Reducing Agent is an element which causes reduction (and is oxidized as a result) by giving electrons to another species.
Oxidation Number:
Monoatomic ions: actual charge of the atom that results from the loss or gain of electrons
Atoms (not in ionic form):
o charge tthat the atom would develop if combined with other atoms by electron transfer
o hypothetical charge assigned to the atom using a set of rules
Examples:
Element Compound/Ion Oxidation State
Mg Mg(NO3)2 +2
I I2 0
S Na2S2O3 +2
S Na2S4O6 +5, +5, 0, 0
Objectives:
1. To recognize the visible indications of a redox reaction2. To assign oxidation states to different elements in a compound3. To identify the reducing and oxidizing agents of a reaction4. To balance redox reactions using a change-in-oxidation-state
methodActivity Series:
METHODOLOGY
Four test tubes were labelled A, B, C, and D
The ff. were mixed in test tube D:
2 drops 0.1M KMnO4
6 drops 6M H2SO4
6 drops 0.1M Na2C2O4
The ff. were mixed in test tube C:
2 drops 0.1M I2 in KI
2 drops 0.1M Na2S2O3
The ff. were mixed in test tube B:
2 drops 0.1M K2Cr2O7
6 drops 6M H2SO4
4 drops 3% fresh H2O2
The ff. were mixed in test tube A:
5 drops 0.1M Cu(NO3 )2
Mg ribbon
Each test tube was observed for evolution of gas and other visible reactions.
RESULTS
Test Tube Balanced Equation Observations
A Cu(NO3)2+ Mg Mg(NO3 )2 + Cu
Liquid: blue to yellow (colorless)
Solid: Silvery white ribbon to black(reddish brown) specks
B K2Cr2O7 + 4 H2SO4 + 3 H2O2 K2SO4 + Cr2(SO4)3 + 3 O2 + 7 H2O
Effervescence
C 2Na2S2O3 + I2 Na2S4O6 + 2 NaIYellow(reddish brown) to colorless
D2KMnO4 + 8 H2SO4 + 5 Na2C2O4
2 MnSO4 + 10 CO2 + 8 H2O + 5Na2SO4 + K2SO4
Purple to colorless
DISCUSSION
lost e-; oxidized; R.A.
+2 +5 -2 0 +2 +5 -2 0
Cu ( NO3 ) 2 + Mg Mg ( NO3 )2 + Cu
gained e-; reduced; O.A.
Mg is more reactive and more likely to be oxidized than Cu.
+1 +6 -2 +1+6 -2 +1 -1 lost e-
K2 Cr2 O7 + 4 H2SO4 + 3 H2O2 oxidized
R.A.
gained e- +1+6-2 +3 +6 -2 0 +1-2
reduced; O.A. K2SO4 + Cr2 (SO4)3 + 3 O2 + 7 H2O
lost e-; oxidized; R.A.
+1 +2 -2 0 +1+2.5-2 +1 -1
2 Na2S2O3 + I2 Na2S4O6 + 2 NaI
gained e-; reduced; O.A.
+1 +7 -2 +1+6-2 +1 +3 -2 lost e-; oxidized; R.A.
2 KMn O4 + 8 H2SO4 + 5 Na2C2O4
gained e-; reduced; O.A.
+2+6-2 +4 -2 +1 -2 +1+6-2 +1+6-2
2 MnSO4 + 10 CO2 + 8 H2O + 5 Na2SO4 + K2SO4
Sources:
http://ibchem.com/IB/ibnotes/brief/red-sl.htm