ib chemistry on redox, oxidation states, oxidation number
TRANSCRIPT
http://lawrencekok.blogspot.com
Prepared by Lawrence Kok
Video Tutorial on Redox, Oxidation, Reduction and oxidation number.
Cations/Metals/+ve ions
Gp 1 Gp 2 Gp 3 Transition metals ions ( variable oxidation states)
Oxidation state
+1
Oxidation state+2
Oxidation state
+3
Sc+3
Ti+2+3
V+2+3
Cr+2+3+6
Mn+2+3+6+7
Fe+2+3
Co+2+3
Ni+2
Cu+1+2
Zn+2
Li 1+ Be2+ Sc 3+ Ti 2+
Ti 3+
V 2+
V 3+
Cr 2+
C r3+
Cr6+
Mn 2+
Mn 3+
Mn 6+
Mn 7+
Fe 2+
Fe 3+
Co2+
Co 3+
Ni2+ Cu1+
Cu2+
Zn2+
Na 1+ Mg2+ Al 3+
K 1+ Ca2+
Anion/Non metal
Gp 5 Gp 6 Gp 7
Oxidation state
Oxidation state
Oxidation state
-3 -2 -1
N3- O2- F-1
P3- S2- CI-1
Br-1
I-1
Metal/Cations/+ve ions
Non Metal/Anions/-ve ions
Ionic Compound
Li2O MgCI2 Al2O3 FeOIron(II) oxide
NiONickel(II) oxide
CuOCopper(II) oxide
Li3N Mg3N2 AlN Fe3N2
Iron(II) nitrideNi3N2
Nickel(II) nitrideCu3N2
Copper(II) nitride
Oxidation state/Charge ion → Li1+ O2-
Formula compound Li2 O
1
Video on polyatomic ions
Writing Chemical Formula
Step 1 : Write Oxidation state/charge
Step 2 : Balance it, (electrically neutral) by cross multiply – as subscript
Polyatomic ions
Group of non-metals bonded together
Oxidation state
Oxidation state
Oxidation state
-1/+1 -2 -3
(OH)-1
Hydroxide(SO4)2-
Sulphate(PO4)
3-
Phosphate
(CN)-1
Cyanide(SO3)
2-
Sulphite
(SCN)-1
Thiocyanate(CO3)
2-
Carbonate
(NO3)-1
Nitrate(S2O3)
2-
Thiosulphate
(NO2)-1
Nitrite(Cr2O7)
2-
Dichromate
(NH4)+1
Ammonium
Polyatomic ions
Li2(CO3) Mg(CO3) Al2(CO3)3 Fe(CO3) Ni(CO3) Cu(CO3)
Li(OH) Mg(OH)2 Al(OH)3 Fe(OH)2 Ni(OH)2 Cu(OH)2
Li2(SO4) Mg(SO4) Al2(SO4)3 FeSO4 Ni(SO4) Cu(SO4) Video on polyatomic ions
Ionic Compound
Writing Chemical Formula
Metal/Cations/+ve ions
Cations/Metals/+ve ions
Gp1 Gp 2 Gp3 Transition metals ions ( variable oxidation states)
Oxidation state
+1
Oxidation state+2
Oxidation state
+3
Sc+3
Ti+2+3
V+2+3
Cr+2+3+6
Mn+2+3+6+7
Fe+2+3
Co+2+3
Ni+2
Cu+1+2
Li 1+ Be2+ Sc 3+ Ti 2+
Ti 3+
V 2+
V 3+
Cr 2+
C r3+
Cr6+
Mn 2+
Mn 3+
Mn 6+
Mn 7+
Fe 2+
Fe 3+
Co2+
Co3+
Ni2+ Cu1+
Cu2+
Na 1+ Mg2+ Al 3+
K 1+ Ca2+
Oxidation state/Charge ion → Li1+ (CO3)2-
Formula compound Li2 (CO
3)1
Step 1 : Write Oxidation state/charge ion
Step 2 : Balance it, (electrically neutral) by cross multiply – as subscript
Redox (Oxidation and Reduction)
Oxidation – Gain of oxygen ↑
Oxidation – Loss of hydrogen ↓ Reduction – Gain of hydrogen ↑
Reduction – Loss of oxygen ↓
Oxidation Reduction
Gain oxygen ↑ Loss oxygen ↓
Gain oxidation Number ↑
Loss oxidation Number ↓
Loss hydrogen ↓ Gain hydrogen ↑
Loss electron ↓ Gain electron ↑
Ca + O2 CaO→ CH4 + 2O2 CO→ 2+ 2H2Ogain oxygen gain oxygen
Zn + CuO ZnO + Cu→ PbO + CO Pb + CO→ 2loss oxygen loss oxygen
H2S + CI2 S +2HCI →loss hydrogen
H2S + CI2 S + 2HCI →
Redox - Oxidation state change- Electron transfer
CH4 + 2O2 → CO2 + 2H2O
gain hydrogen
Zn + CuSO4 → ZnSO4 + Cu Zn + CI2 → ZnCI2
No gain/loss oxygen/hydrogen
Redox
gain oxygen
gain hydrogen
Reduction
Oxidation
Are these redox rxns?
Redox - Oxidation state change- Electron transfer
Zn + CuSO4 → ZnSO4 + Cu Zn + CI2 → ZnCI2 No gain/loss oxygen/hydrogen
Are these redox rxns?
Yes – change in oxidation numberYes – loss/gain of electron
Yes – change in oxidation numberYes – loss/gain of electron✓ ✓
• Assuming bond are ionic with diff EN values (unless bet same element)• Assign each atom, measure of electron control relative to atom in pure element• Apparent/imaginary charge it has when bonded to diff elements• Unequal sharing electron based on electronegativity• + means lose electron• - means gain electron
Oxidation State/Number/ON Rules
Oxidation Reduction
Gain oxygen ↑ Loss oxygen ↓
Gain oxidation Number ↑
Loss oxidation Number ↓
Loss hydrogen ↓ Gain hydrogen ↑
Loss electron ↓ Gain electron ↑
H CIxx
xx
•x
∂-∂+
+1 -1Oxidation number
Oxidation state (sign, number) +2 NOT 2+
Oxidation state and formal charge useful tool for electron book- keeping. They are not REAL!- Oxidation state -Assume bond ionic with diff EN values (unless bet same element)- Formal charge – Assume bond covalent
Redox (Oxidation and Reduction)
Redox (Oxidation and Reduction)
• Assuming bond are ionic with diffEN values (unless bet same element)• Assign each atom, measure of electron control relative to atom in pure element• Apparent/imaginary charge it has when bonded to diff elements• Unequal sharing electron based on electronegativity• + means lose electron• - means gain electron
Oxidation Number/ON Rules
H CIxx
xx
•x
∂-∂+
+1 -1Oxidation number
Oxidation state (sign, number) +2 NOT 2+
Oxidation state and formal charge useful tool for electron book- keeping. They are not REAL!- Oxidation state -Assume bond ionic with diff EN values (unless bet same element)- Formal charge – Assume bond covalent
xx
CI CI
Oxidation Number/ON Rules
H CI Na CI
Imagine electron move to more EN element
O C O
oo
oo
xxoo
oo xx
xxox
Equal sharing
xx
xx
xx
ox
+1 -1Unequal sharing
0 0
xx xx
xx
ox
+1 -1Complete transfer
oxox
oo
oo
oo
oo
oo
oo
xoxo
Unequal sharing
-2 +4 -2
H O H
CI2 H CI Na CI C O2
+1 -1 -1+1 +4 -2
oo
ox
ox
+1 -2 +1Unequal sharing
H N HH
ox
ox
o x
oo
+1 -3 +1
+1
Unequal sharing
H2 O N H3
H C H
H
H
o xo x
ox
ox
+1
+1
+1
+1 -4
C H4
+1 -2 -3 +1 -4 +1
CI C CI
CI
CI
-1
-1
-1
-1
xx
xx
xx
xx
xx xx
xx
xx
xx
xx
xx
xx
xo
xo
ox
ox
+4
C CI4
+4 -1
0
Exceptions
Element ON Exception Example
Hydrogen +1 H +1
-1 Bond to metalMetal hydride
NaHCaH2
Oxidation Number/States/ON Rules Imagine electron move to more EN element
• Assuming bond are ionic with diff EN values (unless bet same element)• Assign each atom, measure of electron control relative to atom in pure element• Apparent/imaginary charge it has when bonded to diff elements• Unequal sharing electron based on electronegativity
H CI
xx
∂-xx
•x
Oxidation number +1 -1
∂+
xx
H CIxx
xx
xx
+1 -1
ox
Unequal sharing
H CI+1 -1
Na Hox
+1 -1Complete transfer
Na H+1 -1
Exceptions
Element ON Exception Example
Oxygen -2 O -2
+2Bond to fluorine
F2O
Exceptions
Element ON Exception Example
Oxygen -2 O -2
-1Peroxide
(O-O)H2O2
H O H F O Foo
oo
ox
ox
+1 -2 +1Unequal sharing
H2 O+1 -2
oo
oo
xx
xx
xx
xx
xx
xxo x
o x
-1 +2 -1Unequal sharing
F2 O-1 +2
O O HH
O-O single bond
oo
oo
oo
oo
o x
o xoo
equal sharing
+1 -1 -1 +1Unequal sharing
H2 O2
+1 -1
EN fluorine higher ↑EN oxygen higher ↑
Oxidation Number/ON Rules Imagine electron move to more EN element
O O H O HOxidation state O different – depend element bond with – different EN values !
F O F O Oxx
xx
xx
xx
xxxx
Equal sharing
0 0
O20
oo
oo
oo
oo
o x
o x+1 -2 +1
Unequal sharing
H2 O+1 -2
xx xx
xx xx
xxxx
o x
o x
-1 +2 -1
F2 O-1 +2
H Hoo
oo
oo
oo
oo
o x
o x
+1 -1 -1 +1
H2 O2+1 -1
Unequal sharing Unequal sharing
Oxidation Number/ON Rules Imagine electron move to more EN element
• Assuming bond are ionic with diff EN values (unless bet same element)• Assign each atom, measure of electron control relative to atom in pure element• Apparent/imaginary charge it has when bonded to diff elements• Unequal sharing electron based on electronegativity
H CI
xx
∂-xx
•x
Oxidation number +1 -1
∂+
xx
Oxidation Number/ON Rules Imagine electron move to more EN element
O O H O HOxidation state O different – depend element bond with – different EN values !
F O F O Oxx
xx
xx
xx
xxxx
Equal sharing
0 0
O2
0
oo
oo
oo
oo
o x
o x
+1 -2 +1
Unequal sharing
H2 O+1 -2
xx xx
xx xx
xxxx
o x
o x
-1 +2 -1
F2 O-1 +2
H Hoo
oo
oo
oo
oo
o x
o x
+1 -1 -1 +1
H2 O2+1 -1
Unequal sharing Unequal sharing
Oxidation Number/ON Rules Imagine electron move to more EN element
Oxidation state N different – depend element bond with – different EN values !
H N HH
HH O N O H O N O N O N
O
O O
O
o x
o x
o x
x xx x
+1 -3 +1
+1
-2
[N H4 ]-3 +1 +1
Unequal sharing
xx
o x
o x xoxo
xx
oo
oo oo
oo
+1 -2 +3 -2
Unequal sharing
H N O2
+1 +3 -2
O
o x
o x xoxo
xx
oooo
oo
+1 -2 +5 -2
-2
Unequal sharing
H N O3
+1 +5 -2
o x
o x
xxoo
xxoo
oo
oo
oo
oo
oo
oo
oo
oo
oo oo -2
-2 -2
-5 -5-2
N2 O5
Unequal sharing
-5 +2
+1+
Oxidation Number/ON Rules
Atoms uncombined free element state = ON = 0
Ion form – ON same as charged on ion
1
2
Mg
Mg2+
Na
Na+
O2 S8
O2-
3 ON for element same as its most common ion/groupON metal from Gp 1 – 3ON non metal Gp 5 - 7
Anion/Non metal
Gp 5 Gp 6 Gp 7
Oxidation state
Oxidation state
Oxidation state
- 3 - 2 - 1
N 3- O 2- F 1-
P 3- S 2- CI 1-
Cation/Metal
Gp 1 Gp 2 Gp 3
Oxidation state
Oxidation state
Oxidation state
+1 +2 +3
Na 1+ Mg 2+ Al 3+
K 1+ Ca 2+ Ga 3+
4
CI20 0 0 0 0
+1 +2 -2 -1 -2
CI- S2-
ON for transition metal varies Transition metal ions
Transition metals ions (variable oxidation states)
Sc+3
Ti+2+3
V+2+3
Cr+2+3+6
Mn+2+3+6+7
Fe+2+3
Co+2+3
Ni+2
Cu+1+2
Zn+2
Sc 3+ Ti 2+
Ti 3+
V 2+
V 3+
Cr 2+
Cr 3+
Cr 6+
Mn 2+
Mn 3+
Mn 6+
Mn 7+
Fe 2+
Fe 3+
Co 2+
Co 3+
Ni 2+ Cu 1+
Cu 2+
Zn 2+
Oxidation number
Diff ONCharge on ion
Click here on oxidation rulesClick here view simple step
Notes
Sc3+
Charge on Sc
Oxidation number
+3
Oxidation state
-+3+
ON all atoms in polyatomic ion add up to charge of polyatomic ion
ON all atoms in neutral molecule add up to 0
CO3 2- SO4
2-
H2SO4 CO25
Oxidation Number/ON Rules
HNO3
(+1)2 + (+6) + (-2)4 = 0
+1 +6 -2
(+4) + (-2)2 = 0 (+1) + (+5) + (-2)3 = 0
+4 -2 +1 +5 -2
(+4) + (-2)3 = -2
+4 -2
(+6) + (-2)4 = -2
NO31-
+6 -2
(+5) + (-2)3 = -1
+5 -2
7 ON atom/molecule of element = 0 (NOT combined)
H2 CI2 O2 Fe Cu Mg0 0 0 0 0 0
8 Monoatomic ion – ON same as charged on ion
Ionic compound
Charge ion Oxidation number
MgF2 Mg 2+ F 1- Mg (+2) F (-1)
NaCI Na 1+ CI 1- Na (+1) CI (-1)
KBr K 1+ Br 1- K (+1) Br (-1)
CaI2 Ca 2+ I 1- Ca (+2) I (-1)
Li3N Li 1+ N 3- Li (+1) N (-3)
Al2O3 Al 3+ O 2- AI (+3) O (-2)
9Formula compound
Charge Oxidation number
Name using oxidation number
FeO Fe 2+ or 2+ +2 Iron (II) oxide
Fe2O3 Fe 3+ or 3+ +3 Iron (III) oxide
Cu2O Cu 1+ or 1+ +1 Copper (I) oxide
CuO Cu 2+ or 2+ +2 Copper (II) oxide
MnO2 Mn 4+ or 4+ +4 Manganese (IV) oxide
MnO4- Mn 7+ or 7+ +7 Manganese (VII) oxide
K2Cr2O7 Cr 6+ or 6+ +6 Potassium dichromate (VI)
Cr2O3 Cr 3+ or 3+ +3 Chromium (III) oxide
Click here view chemguide notes
6
Oxidation Number/ON Rules
9 Metal more than one oxidation states, Roman numeral used
Manganese ChromiumIonic
compoundMnSO4 MnO2 K2MnO4 KMnO4 K2Cr2O7 Cr2O3
OxidationNumber
(+2) + (+6) + (-2)4 = 0 Mn (+2)
(+4) + (-2)2 = 0Mn (+4)
(+1)2 + (+6) + (-2)4 = 0Mn (+6)
(+1) + (+7) + (-2)4 = 0Mn (+7)
(+1)2 + (+6)2 + (-2)7 = 0Cr (VI)
(+3)2 + (-2)3 = 0Cr (III)
IUPAC name
Manganese(II)
sulphate
Manganese (IV)
oxide
Manganese(VI)
Manganese(VII)
Chromium(VI)
Chromium(III)
Iron CopperIonic
compoundFeCI2 FeCI3 CuCI CuCI2
OxidationNumber
(+2) + (-1)2 = 0 Fe (+2)
(+3) + (-1)3 = 0 Fe (+3)
(+1) + (-1) = 0 Cu (+1)
(+2) + (-1)2 = 0 Cu (+2)
IUPAC name
Iron (II) chloride Iron (III) chloride Copper (I) chloride Copper (II) chloride
Vanadium
VO2 + VO 2+
(+5) + (-2)2 = +1 V (+5)
(+4) + (-2) = +2 V (+4)
Vanadium (V) Vanadium (IV)
ON for underlined element in ionic compound10
Na2SO3 Na2SO4 NaNO2 NaNO3 (SO3)2- (SO4)2-
(+1)2 + (+4) + (-2)3 = 0 (+1)2 + (+6) + (-2)4 = 0 (+1)+ (+3) + (-2)2 = 0 (+1)+ (+5) + (-2)3 = 0 (+4) + (-2)3 = -2 (+6) + (-2)4 = -2
ON for S = +4 ON for S = +6 ON for N = +3 ON for N = +5 ON for S = +4 ON for S = +6
+1 +4 -2 +1 +6 -2 +1 +3 -2 +1 +5 -2 +4 -2 +6 -2
Oxidation Number/ON Rules
11 ON for underlined element in compound
OH-1 PO4
3- S2O32- CN-1 OCI-1 H2O2 (HCO3)-1
(-2) + (+1) = -1 (+5) + (-2)4 = -3 (+2)2 + (-2)3 = -2 (+4) + (-5) = -1 (-2) + (+1) = -1 (+1)2 + (-1)2 = 0
ON for O = -2 ON for P = +5 ON for S = +2 ON for C = +4 ON for O = -2 ON for O = -1 ON for C = +4
(+1) + (+4) + (-2)3 = -1
-2 +1 +5 -2 +2 -2 +4 -5 -2 +1 +1 -1 +1 +4 -2
Oxidation Reduction
Gain oxygen ↑ Loss oxygen ↓
Loss hydrogen ↓ Gain hydrogen ↑
Redox (Oxidation and Reduction)
Rxn involve gain/loss of oxygen/hydrogen
CH4 + 2O2 → CO2 + 2H2O Gain hydrogen
Oxygen reduction
gain oxygen
Carbon oxidation
Rxn involve gain/loss of electron
Oxidation Reduction
Gain ON ↑ Loss ON ↓
Loss electron ↓ Gain electron ↑- broader definition- cover more rxn types
PbO + CO Pb + CO→ 2
Lead Reduction
gain oxygen
Carbon oxidation
(-4) (+4)
(0) (-2)
ON ↑
ON ↓oxygen reduced
carbon oxidized
PbO + CO Pb + CO→ 2
(+2) (0)lead reduced
(+2) (+4)
CH4 + 2O2 → CO2 + 2H2O
ON ↑carbon oxidized
ON ↓loss oxygen
Redox (Oxidation and Reduction)
• Assuming bond are ionic with diff EN values (unless bet same element)• Assign each atom, measure of electron control relative to atom in pure element• Apparent/imaginary charge it has when bonded to diff elements• Unequal sharing electron based on electronegativity
Oxidation Number/ON Rules
H CIxx
xx
•x
∂-∂+
+1 -1Oxidation numberOxidation state (sign, number) +2 NOT 2+
Oxidation state useful tool for electron book- keeping. They are not REAL!- Oxidation state -Assume bond ionic with diff EN values (unless bet same element)
xx
Na CI
Oxidation Number/ON Rules Imagine electron move to more EN element
xx
xx
xx
ox
+1 -1Complete transfer
Na CI+1 -1
Ionic compound
H CI
Covalent compound
xx
xx
+1 -1xx
ox
H CI
Unequal sharing+1 -1
Organic Covalent compound
H C O H
H
Hox
ox
o X
o X
ox
oo
-2+1
+1
+1
+1 -2
C H4 O
Unequal sharing
Still covalent bond
Treat as imaginary ionic (loss/gain of electron control)
Bonds are still covalent NOT ionic, keep track where electron going
-2 +1 -2
(+1) + (-1) = 0 (+1) + (-1) = 0
(-2) + (+1)4 + (-2) = 0
O S O
O
ooxx
ooxx
ooxx
-2 +6 -2
-2
S O3
+6 -2
(+6) + (-2)3 = 0Click here note ON for organic carbon
oo oo
oo
oo
oo
oo
ON for carbon is NOT -2
Oxidation Number/ON Rules• Assuming bond are ionic with diff EN values (unless bet same element)• Apparent/imaginary charge it has when bonded to diff elements• Unequal sharing electron based on electronegativity
- Oxidation state useful tool for electron book- keeping. They are not REAL!Oxidation state (sign, number) +2 NOT 2+
Click here here note ON carbon
H C C H
Oxidation state Carbon compound
-4 CH4
-3 C2H6
-2 CH3CI
-1 C2H2
0 CH2CI2
+1 CHCI2-CHCI2
+2 CHCI3
+3 C2CI6
+4 CCI4
ON carbon (Organic molecules)
Average oxidation number bet carbon is taken!
Different ON states
Don’t need to take average ON bet carbons
Oxidation state
Carbon compound
-3 and -1 CH3CH2OH
-3 and +1 CH3CHO
Different ON states
ox
ox
+1 -1 -1 +1
C2 H2
-1 +1
oxoxox
Equal sharing
(-1)2 + (+1)2 = 0
H C C O HH
H
o X
ox
o X o X oo
ox
ox
H
H
o X oo
ox
+1
+1
-2
+1
+1
+1
+1-1-3
C2 H6 O1
x +1 -2
2x + 6 -2 = 0 x = -2
ON C in CH3 = -3ON C in CH2 = -1Average ON C = -2
H C C OH
ox
+1
H
H
o Xo X
ox
o X oo
xoxo
oo
+1
+1 +1
-3 -2+1
C2 H4 O1
x +1 -2
2x + 4 -2 = 0 x = -1
ON for carbon is NOT -1
ON C in CH3 = -3ON C in CH = +1Average ON C = -1
ON C in CH3 = -3ON C in COOH = +1Average ON C = 0
+3
Oxidation Number/ON Rules• Assuming bond are ionic with different EN values (unless bet same element)• Apparent/imaginary charge it has when bonded to diff elements• Unequal sharing electron based on electronegativity
- Oxidation state useful tool for electron book- keeping. They are not REAL!Oxidation state (sign, number) +2 NOT 2+
Click here here note ON carbonON carbon (Organic molecules)
Average oxidation number bet carbon is taken!
Oxidation state carbon
Carbon compound
-3 and +3 CH3COOH
H C C O HH
H
o X
ox
o X o X oo
ox
ox
H
H
o X oo
ox
+1
+1
-2
+1
+1
+1
+1-1
C2 H6 O1
x +1 -2
2x + 6 -2 = 0 x = -2
ON C in CH3 = -3ON C in CH2 = -1Average ON C = -2
H C C OH
ox
+1
H
H
o Xo X
ox
o X oo
xoxo
oo
+1
+1 +1
-3 -2+1
C2 H4 O1
x +1 -2
2x + 4 -2 = 0 x = -1
ON for carbon is NOT -2
ON for carbon is NOT -1
ON C in CH3 = -3ON C in CH = +1Average ON C = -1
H C C O H
H O
H
+1
ox
o X
+1
+1
o X-3 -3
ox
+1
oo
oo
oo
ooxx
oo
ox
ox
-2
ON for carbon is NOT 0
C2 H4 O2
x +1 -2
2x + 4 -4 = 0 x = 0
Oxidation state carbon
Carbon compound
-3 and -1 CH3CH2OH
Oxidation state carbon
Carbon compound
-3 and +1 CH3CHO
NOT Redox rxn•NO Loss/gain electron•NO change in oxidation number
Concept Map
Type of chemical reaction
Combustion/Respiration rxn Displacement rxn
Synthesis rxn Decomposition rxn
Single Displacement
Double Displacement
Acid/Base rxn
Involve oxygen!!
CH4 + 2O2 CO→ 2+ 2H2O C6H12O6 +6O2 6CO→ 2+6H2O
Redox rxn•Loss/gain electron•Change in oxidation number
Zn + 2HCI H→ 2+ ZnCI2 Zn + CuO ZnO + Cu→
Redox rxn•Loss/gain electron•Change in oxidation number
KI + Pb(NO3)2 PbI→ 2 + KNO3
Type of chemical reaction
HCI + NaOH NaCI + H→ 2O MgO + 2HCI MgCI→ 2 + H2O 2H2 + O2 2H→ 2O 2KCIO3 2KCI + 3O→ 2
Redox rxn•Loss/gain electron•Change in oxidation number
Redox rxn•Loss/gain electron•Change in oxidation number
NOT Redox rxn•NO Loss/gain electron•NO change in oxidation number
H CI + Na O H NaCI + H→ 2 O+1 -1 +1 -2 +1 +1 -1 +1 -2
2H2 + O2 2H→ 2O0 0 +1 -2
2K CI O3 2K CI + 3O→ 2
+1 +5 -2 +1 -1 0
C6 H12 O6 + 6O2 6C O→ 2 + 6H2 O Zn + 2H CI H→ 2 + Zn CI2
0 +1 -1 0 +2 -1
K I + Pb (N O3)2 Pb I→ 2 + K N O3
+1 -1 +2 +5 -2 +2 -1 +1 +5 -2 0 +1 -2 0 +4 -2 +1 -2
Oxidation state
Carbon compound
-4 CH4
-3 C2H6
-2 CH3CI
-1 C2H2
0 CH2CI2
+1 CHCI2-CHCI2
+2 CHCI3
+3 C2CI6
+4 CCI4
Different ON/ states for Carbon Different ON/ states for sulphur
Carbon attach to H – ON lower ↓- Carbon less oxidized- Carbon attract electron
Carbon attach to CI/O (EN ↑) – ON higher ↑- Carbon more oxidized- Carbon lose electron
Oxidation state
Sulphur compound
-2 H4S
0 S8
+2 SCI3
+4 SO2
+4 SO3 2-
+6 SO3
+6 H2SO4
Sulphur attach to H /CI– ON lower ↓- Sulphur less oxidized- Sulphur attract electron
Sulphur attach to O (EN ↑) – ON higher ↑- Sulphur more oxidized- Sulphur lose electron
Oxidation numbers and name
Formula ion
Charge Oxidation number
Name using ON
CrO42- 2- ON for Cr +6 Chromate (VI)
Cr2O7 2- 2- ON for Cr +6 Dichromate (VI)
MnO4- 1- ON for Mn +7 Manganate (VII)
MnO42- 2- ON for Mn +6 Manganate (VI)
CIO - 1- ON for CI +1 Chlorate (I)
CIO3 - 1- ON for CI +5 Chlorate (V)
CIO2 - 1- ON for CI +3 Chlorate (III)
CIO4 - 1- ON for CI +7 Chlorate (VII)
Formula compound
Charge Oxidation number
Name using oxidation number
FeO Fe 2+ or 2+ +2 Iron (II) oxide
Fe2O3 Fe 3+ or 3+ +3 Iron (III) oxide
Cu2O Cu 1+ or 1+ +1 Copper (I) oxide
CuO Cu 2+ or 2+ +2 Copper (II) oxide
MnO2 Mn 4+ or 4+ +4 Manganese (IV) oxide
MnO4- Mn 7+ or 7+ +7 Manganese (VII) oxide
K2Cr2O7 Cr 6+ or 6+ +6 Potassium dichromate (VI)
Cr2O3 Cr 3+ or 3+ +3 Chromium (III) oxide
Period 2
Shared electron cloud closer to O
Electronegativity
Electronegativity (EN)•Tendency of atom to attract/pull shared/bonding electron to itself•EN value higher – pull/attract electron higher (EN value from 0.7 – 4)
EN highest EN lowest
Factors affecting EN value•Size of atom/distance – small size/distance – stronger attraction for electron•Nuclear charge – higher nuclear charge – stronger attraction for electron
Electronegativity•EN increase up a Group•EN increase across a Period
F
CI
Br
I
Size increase
Attraction electron decrease
EN lower
Size
Be+4
Li+3 B
+5 N+7
O+8 F
+9
EN increase across period 2
Nuclear charge
EN increase across period 2 Nuclear charge increase Strong attraction for electron
EN increase
Gp 17
C+6
EN decrease down gp 17
FORMAL CHARGE (FC)
Tool/Model for comparing which Lewis structures is more acceptable
Lewis structure SO2
Which is acceptable?
Lewis structure SO3
Formal Charge•Treats covalent bond with equal electron distribution no EN diff bet atom•Electronegative atom has negative while least electronegative atom has positive formal charge.
Formula formal charge
Click here video formal chargesClick here video formal charges
V - valence electrons of atom L – Lone pair electronB - electrons shared in covalent bonds in the molecule
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All resonance structure contribute to electronic structure. Real structure is combination of them.Lowest formal charge (stable), contribute more than less stable structure.Sum of formal charges must be zero for neutral or equal to charge on ion.
L +
Formal charge concept
Formal charge NOT real !!
Acknowledgements
Thanks to source of pictures and video used in this presentation
Thanks to Creative Commons for excellent contribution on licenseshttp://creativecommons.org/licenses/
Prepared by Lawrence Kok
Check out more video tutorials from my site and hope you enjoy this tutorialhttp://lawrencekok.blogspot.com