Oxidation Numbers, ox # - SCH4U1-CCVI - home + 3 e- Au +1.50 Ce4+ + e-1 Ce3+ +1.44 ClO4 1- + 8 H+ +...
Transcript of Oxidation Numbers, ox # - SCH4U1-CCVI - home + 3 e- Au +1.50 Ce4+ + e-1 Ce3+ +1.44 ClO4 1- + 8 H+ +...
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Oxidation Numbers, ox #
are _____ or _____ numbers assigned to each _______ or
____ assuming that the _____________ are transferred
________________ from the ______ electronegative
element to the _______ electronegative element.
________________ now mimic ________ systems.
ox# are written _______ followed by _________ and are
assigned using the following:
Oxidation Number Rules
The ox# of an ______ in it’s pure form, (eg. Pb(s), O2(g) )
is ____.
The ox# of a ____________ _____ is equal to the _________ on that ______.
eg. Cl1-
The algebraic ____ of the oxidation numbers in a ________ polyatomic compound is ___.
eg. Mg3N2 Fe(NO3)3
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The most common ox# for O is ___, in peroxides it is ___,
and in compounds with fluorine it is ___. The most common ox# of H is ___, in metal hydrides it is
___. The algebraic ______ of the oxidation numbers in a
polyatomic _____ is equal to the _________ on the ____.
eg. Cr2O
7
2-
Assign the ox# to the most _______________ element __ Determine the ______ charge for that element Considering the charge on the ion or neutral compound,
find the total charge for the other element, then its ox #. In compounds of _______________, the ox# of the
______ electronegative atom is ______ and the ox# of the
______ electronegative atom is _______.
eg. CO2 In a covalent bond, the more ________________ atom
takes _____ the ____________ in the bond.
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Energy Transfer Theory
Chemical reactions _________ with the ______________
of __________.
Often, this energy is _____ noticeable as it doesn’t
involve a ___________ change or the production of
________ or _______.
This is true of ____________ reactions, where the
___________ switch between entities with no
___________ change in _________.
To examine the energy ____________ we _________ the
chemical reaction into ___ separate reactions called _____
____________.
For:
Net ionic equation
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Half reactions
The energy _________ is the electron ______________ –
______________
Redox reactions require the ______________ reaction
_________________________ to occur simultaneously
with the _______________ reaction
_________________________
Redox – ____________________________
_________ goes __________
______ _______
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Balancing REDOX Reactions 1. Assign ___________ ____________ (ox. #) to ______ element in the
rxn and __________ the species being ____________ and ____________.
2. Write separate ______ ____________ (1/2 rxn), for the
______________ (ox.) and _____________ (red.) processes. 3. Balance the ___________ that undergo _____________ or
______________. 4. Add the total _________ gained or lost in _______ ox. or red. rxn.
5. Multiply each _________ so that once combined, the total # of e-s ______ out.
6. Combine the _________. 7. Balance the net ___________ (due to ions) using _____ ions to one
side (for acidic sol’n) or with _______ ions (for basic sol’n). 8. Add _______ to balance ____ and ____. 9. Check that the final eq’n is ________________.
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Predicting Redox Reactions
Redox Rxn
occur due to the ____________ of e- from ________
substance to _______________.
is a ________________ of e- between _____________.
if ______ substance ________ e- from another, a
_______________________ rxn _____________. eg. Cu + 2Ag+ ↔ Cu2+ + 2Ag
Reducing agents (RA)
a substance that __________ e- to another substance and
undergoes __________________. Oxidizing agents (OA)
a substance that __________ e- to another substance and
undergoes __________________. eg. Cu + 2Ag+ ↔ Cu2+ + 2Ag
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rxns are listed as ____________, S = Strong, W = Weak.
SOA OA1 + ne- ↔ RA1 WRA
WOA OA2 + ne- ↔ RA2 SRA spontaneous rxns occur only if the ______ is
____________ and to the _________ of the ______. For spontaneous rxn:
eg. Will a mixture of aqueous chromium (II) nitrate and tin (II) nitrate react and if so what is the overall equation?
List all species ________ determine the ________, _____________ on the _______ and the ________, ________ on the _________ on the REDOX table
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eg. Create ½ rxns from the following reaction data and place in order of strongest to weakest OA:
Ion/metal Zn Pb Ag I1-
Zn2+
Pb2+
Ag+
I2
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eg. Create ½ rxns from the following reaction data and place in order of strongest to weakest OA:
Cu2+ + Pb Cu + Pb2+ Ag + Br2 AgBr
Ag+ + Cu Ag + Cu2+ Au + Br2 no rxn
eg. Create ½ rxns from the following reaction data and place in order of strongest to weakest OA:
W + M2 W2+ + M1- Y2+ + Z Y + Z2+
X + M2 no rxn W + Y2+ no rxn
X2+ + Z X + Z2+
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Standard Reduction Potentials ( also p 805) E° (volts)
F2 + 2 e- 2 F-1 +2.87
S2O82- + 2 e- 2 SO4
2- +2.01
Co3+ + e-1 Co2+ +1.81
Pb4+ + 2 e-1 Co2+ +1.80
H2O2 + 2 H+ + 2 e- 2 H2O +1.77
Au+ + e-1 Au +1.69
PbO2 + SO42- + 4 H+ + 2 e- PbSO4 + 2 H2O +1.69
MnO41- + 8 H+ + 5 e- Mn2+ + 4 H2O +1.51
Au3+ + 3 e- Au +1.50
Ce4+ + e-1 Ce3+ +1.44
ClO41- + 8 H+ + 8 e- Cl1- + 4 H2O +1.39
Cl2 + 2 e- 2 Cl- +1.36
2 HNO2 + 4 H+ + 4 e- N2O + 3 H2O +1.30
Cr2O72- + 14 H+ + 6 e- 2 Cr3+ + 7 H2O +1.23
O2 + 4 H+ + 4 e- 2 H2O +1.23
MnO2 + 4 H+ + 2 e- Mn2+ + 2 H2O +1.22
2 IO31- + 12 H+ + 10 e- I2 + 6 H2O +1.20
Br2 + 2 e- 2 Br-1 +1.07
AuCl41- + 3 e- Au + 4 Cl- +1.00
Hg2+ + 2 e- Hg +0.85
ClO1- + H2O + 2 e- Cl1- + 2 OH-1 +0.84
Ag+ + e- Ag +0.80
NO31- + 2 H+ + e- NO2 + H2O +0.80
Hg22+ + 2 e- 2 Hg +0.79
Fe3+ + e- Fe2+ +0.77
O2 + 2 H+ + 2 e- H2O2 +0.70
MnO41- + 2 H2O + 3 e- MnO2 + 4 OH-1 +0.60
I2 + 2 e- 2 I- +0.54
Cu+ + e- Cu +0.52
O2 + 2 H2O + 4 e- 4 OH- +0.40
Cu2+ + 2 e- Cu +0.34
SO42- + 4 H+ + 2 e- SO2 + 2 H2O +0.18
SO42- + 4 H+ + 2 e- H2SO3 + H2O +0.17
Sn4+ + 2 e- Sn2+ +0.15
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Cu2+ + e- Cu+ +0.15
S + 2 H+ + 2 e- H2S +0.14
AgBr + e- Ag + Br-1 +0.07
2 H+ + 2 e- H2 +0.00
Fe3+ + 3 e- Fe -0.04
Pb2+ + 2 e- Pb -0.13
Sn2+ + 2 e- Sn -0.14
AgI + e- Ag + I-1 -0.15
Ni2+ + 2 e- Ni -0.26
Co2+ + 2 e- Co -0.28
H3PO4 + 2 H+ + 2 e- H3PO3 + H2O -0.28
Tl+ + e- Tl -0.34
PbSO4 + 2 e- Pb + SO42- -0.36
Se + 2 H+ + 2 e- H2Se -0.40
Cd2+ + 2 e- Cd -0.40
Cr3+ + e- Cr2+ -0.41
Fe2+ + 2 e- Fe -0.45
S + 2 e- S2- -0.48
Ga3+ + 3 e- Ga -0.53
Ag2S + 2 e- 2 Ag + S2- -0.69
Cr3+ + 3 e- Cr -0.74
Zn2+ + 2 e- Zn -0.76
Te + 2 H+ + 2 e- H2Te -0.79
2 H2O + 2 e- 2 OH-1 + H2 -0.83
Cr2+ + 2 e- Cr -0.91
Se + 2 e- Se2- -0.92
SO42- + H2O + 2 e- SO3
2- + 2 OH-1 -0.93
Te + 2 e- Te2- -1.14
Mn2+ + 2 e- Mn -1.18
V2+ + 2 e- V -1.19
Al3+ + 3 e- Al -1.66
Ti2+ + 2 e- Ti -1.75
Mg2+ + 2 e- Mg -2.37
Ce3+ + 3 e- Ce -2.48
Na+ + e- Na -2.71
Ca2+ + 2 e- Ca -2.87
Ba2+ + 2 e- Ba -2.91
Cs2+ + 2 e- Cs -2.92
Ra2+ + 2 e- Ra -2.92
K+ + e- K -2.92
Li+ + e- Li -3.00
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Electrochemical Cells
(Galvanic, Voltaic, Electric)
the ___________ reactions are occurring _____________
and are _________ by a _______
the e- _________ occurs through this ___________ circuit
the ______ difference ______________ is manifested as
__________ __________.
X+Y+
K+ NO3-
Salt Bridge
As the cell proceeds:
Cathode Anode
mass of electrode
Solution electrical charge
Ions from salt bridge
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Cell Shorthand Notation eg. For the Zn/Cu cell: ____________________________ Conventions: the │ notation indicates a phase ______________ where
the _______________ and _________________ are in
physical contact. the ║ notation represents the ______ __________ or
_________ ____________ if additional _____________ are ____________ or
specific ___________ are ___________, they are written
with the _____________ separated by a ___________ or
a _______________. if the cell has no _______ for the electrode, __________
electrodes _________ or __________ are used:
___________________________________________ standard cells are __________ at _________ all ______ sets of information – REDOX equation, cell
diagram and the cell notation are related and if ___ is
provided, the other ____ should be able to be _________.
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Calculating Cell Potential, E°cell for each _____ ___________ the ____________
_______________ is listed on the chart on p. 805 or the
reference sheet. the complete ______ is a combination of the
____________ and _____________ half reactions - the
_______ of the two is the _______ potential, _________ this is the usable energy given by:
______________________________________________ as all half reactions are listed as ____________ rxns, the
oxidation reaction ________ the sign, so:
______________________________________________
eg. Calculate the E° cell for the following unbalanced
equation:
Br2 + Cu 2 Br¯ + Cu+
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eg. a) Determine the anode, cathode and calculate the standard cell potential produced by a galvanic cell consisting of a Sn
electrode in contact with a solution of Sn2+ ions and a Cr
electrode in contact with a solution of Cr3+ ions.
b) Write the shorthand cell notation.
eg. Use complete half-reactions and potentials to predict whether the following reaction is spontaneous or non-spontaneous in aqueous solutions. If the cell is spontaneous, write the cell shorthand notation.
O2 + 2 SO
2 + 4 OH1- 2 SO
4
2- + 2 H2O
YOU MUST READ 9.6 Corrosion p.710 – 713 before the next lesson
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Reactions of Metals with Water The _______ is the _______ and will be ____________.
The ______ and ___________ in it will be the __________.
Need to consider:
i) __________ ________ - _____ of the 3
ii) ________________ _________ this requires a very long ____
_____, or an _______________, as O2 is not very water ________
iii) ________ ______________ - as with ______ ______
• Metals _______ the _____________ _______ _______ will be
________________
That’s why:
• Not ___ metals _______ with __________ ________
eg. ones that _____: ones that ______:
• Not ___ metals _______ with _____________ _______
eg. ones that _____: ones that ______:
• Not ___ metals _______ with _________ ________
eg. ones that _____: ones that ______:
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Metals with Metals • Alloys are _______ to change a metal’s ____________. • As _____ _______ undergo ____________ – rust,
corrosion, patina – _______ metals are _______ to stop
the ____________. eg. ___ or ___ need protection. • The ____________ metal, called a ___________ ______,
is ______ on the table _________ to the _______ in
_________. It will __________ the ____________ and
______ the _______.
eg. Which metals will ________ Zn?
eg. Which metals will ____ ________ Zn?
eg. a) Pick a metal that will protect Zn and determine the
cell potential if the cathode is oxygenated water.
b) Do the same for the case where Zn is not protected.
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Cells and Spontaneity
Reactants Products
ΔEcell Cell Type Spontaneity
Electrolytic cells, ΔE < 0
requires _____________ source of ______ to ________
the ____ __________ within the cell.
e- are __________ from the _________ and __________
to the ____________ by the ________________. rxn is then the _____________ of the ________________
rxn. used to __________________ and to produce _________
__________. Solution rxns so _____+ could be the ____________
and/or the ____________ reaction.
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eg. KI solution and battery
Cathode (red): Erº (V)
Anode (ox): Erº (V)
e- from the __________ (-ve) ____________ of the
_______________ reduce the ________
e- from the _____ flow to the ___________ (+ve) __________ of the ____________ to complete the _____________.
forms ______ and _______ from an ____________ sol’n!
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versus
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eg. Given the following molten system, AgCl, predict the products at each electrode. Assume inert electrodes and sufficient voltage to cause a reaction to take place. Consider all possible rxns.
eg. Given a 1.00 M solution of ZnI2 at 25°C, predict the anode and
cathode half cell reactions. What is the minimum voltage required for each cell to operate?
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Stoichiometry of Cell Reactions
Basic Concepts 1. q = It where:
q = _____________________
I = _____________________
t = _____________________
1C = _______________
2. Faraday’s Law: the ________ of a substance
__________ or ______________ is __________ related to the ____________ transferred
3. Faraday = ___________________________
F = ________________
4.
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eg.1 Calculate the amount of charge which passes
through an electrolytic cell with a current of 1.80A for 5.0 min.
eg. 2 Calculate the mass of Zn deposited by a
current of 2.50 A operating over 30.0 min in an electrolytic cell containing Zn(NO3)2(aq).
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Free Energy & Electrochemistry ΔGº = ___________ and ΔGº = __________ and… ΔGº = ______________
eg. Calculate ΔGº and Ke for the electrolytic Zn/Al
cell, Zn │ Al3+│Al.
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RT
0cell
EnF Keqln