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Redox
Reaction
Redox reaction Group C
Oxidation is a reaction
where oxygen
combines with an
element/compound to
form another
substance
Oxidation – Gain of oxygen
When calcium burns in oxygen, the following
reaction takes place
calcium + oxygen  calcium oxide
2Ca(s) + O2  2CaO(s)

Since calcium has gained oxygen. It has be
oxidised. Hence this is oxidation.
Oxidation – Loss of Hydrogen
When ammonia is passed over heated copper(II)
oxide, the following reaction takes place.

ammonia + copper(II) oxide  nitrogen +
copper + water vapour
2NH3(g) + 3CuO(s)  N2(g) + 3Cu(s) + 3H2O(g)

Since ammonia has lost hydrogen, it has been
oxidised.
Oxidation – Loss of Electrons
Oxidation can still take place despite having no
oxygen/hydrogen. When a substance loses
electrons it is considered oxidation.

magnesium + chlorine  magnesium chloride
Mg(s) + Cl2(g)  MgCl2(s)
What is Reduction?
Definition Of Reduction

• Reduction is a chemical reaction where it loses
  oxygen, gain hydrogen, gain electron and have a
  decrease in oxidation state by a molecule, atom
  or ion.
• A reactant that reduces another substance is a
  reducing agent.
• The reducing agent transfers electrons to
  another substance, it reduces others, and is thus
  itself oxidized. And, because it "donates"
  electrons, it is also called an electron donor.
Reduction-Loss Of Oxygen

When zinc burns in copper(II) oxide, the
following reaction takes place.
Zinc + copper oxide  Zinc oxide + copper
Zn(s)+CuO(s)  ZnO(s)+Cu(s)

Since Zinc has gain oxygen,it is oxidised.
Copper(II) oxide loses oxygen,thus it is reduced.
Reduction-Gain Of Hydrogen

When nitrogen burns with hydrogen gas, the
following reaction takes place.
Nitrogen +Hydrogen  Ammonia
N2 + 3H2  2NH3

Nitrogen gain hydrogen, thus it is being reduced.
Reduction-Gain Of Electron
 When iron reacts with chloride acid, the
following reaction takes place.
Iron + chlorine  Iron(III) + Chloride
2Fe2++Cl2  2Fe3++2Cl-

Since iron loses electron, it is oxidised. Chlorine
gains electron, thus it is reduced.
Common Reducing Agent
•   Lithium aluminium hydride (LiAlH4)
•   Nascent (atomic) hydrogen
•   Sodium amalgam
•   Diborane
•   Sodium borohydride (NaBH4)
•   Compounds containing the Sn2+ ion, such as tin(II) chloride
•   Sulfite compounds
•   Hydrazine (Wolff-Kishner reduction)
•   Zinc-mercury amalgam (Zn(Hg)) (Clemmensen reduction)
•   Diisobutylaluminum hydride (DIBAL-H)
•   Lindlar catalyst
•   Oxalic acid (C2H2O4)
•   Formic acid (HCOOH)
•   Ascorbic acid (C6H8O6)
•   Phosphites, hypophosphites, and phosphorous acid
•   Dithiothreitol (DTT) – used in biochemistry labs to avoid S-S bonds
•   Compounds containing the Fe2+ ion, such as iron(II) sulfate
•   Carbon monoxide(CO)
•   Carbon (C)
Oxidation State
The oxidation state is the
charge an atom of an
element would have if it
existed as an ion in a
compound.
To work out the oxidation state of an atom,
      we apply the following rules:
Rule                          Example              Oxidation state
1. The oxidation state of a   Cu, S, Cl2           0, 0, 0
free element is zero.
2. The oxidation state of a   K+, Zn2+, Cl-, O2-   +1, +2, -1, -2
simple ion is the same as
the charge on the ion.
3. The oxidation states of    Ca, C, 3O            +2, +4, 3x(-2)=-6
the atoms present in the
formula of a compound                              All add up to zero.
add up to zero. The
example shown here is
CaCO3 .
4. The total of the           S, 4O                +6, 4x(-2)=-6
oxidation states of the
atoms in a polyatomic ion                          All add up to -2.
is equal to the charge on
the ion. The example
shown here is SO4 2- .
Solution to question: Find the
   oxidation state of each element in
          ammonium sulfate.
(NH4)2SO4
Since hydrogen in NH4 has an o.s of +1,
Ammonium has a charge of 1.
Let n be x
2(x+4(1))=2
2x-2-8
x=-3
Hence nitrogen has an o.s of -3
Since oxygen in SO4 has an o.s of -2,
Sulfate has a charge of -2.
Let s be y
y+4(-2)=-2
y-8=-2
y=6
Hence sulfur has an o.s of 6.
Source


CHEMISTRY Matters textbook

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Done by
•   Edwin
•   Kian Leong
•   Jeremy
•   Melvan

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Redox reaction Group C

  • 3. Oxidation is a reaction where oxygen combines with an element/compound to form another substance
  • 4. Oxidation – Gain of oxygen When calcium burns in oxygen, the following reaction takes place calcium + oxygen  calcium oxide 2Ca(s) + O2  2CaO(s) Since calcium has gained oxygen. It has be oxidised. Hence this is oxidation.
  • 5. Oxidation – Loss of Hydrogen When ammonia is passed over heated copper(II) oxide, the following reaction takes place. ammonia + copper(II) oxide  nitrogen + copper + water vapour 2NH3(g) + 3CuO(s)  N2(g) + 3Cu(s) + 3H2O(g) Since ammonia has lost hydrogen, it has been oxidised.
  • 6. Oxidation – Loss of Electrons Oxidation can still take place despite having no oxygen/hydrogen. When a substance loses electrons it is considered oxidation. magnesium + chlorine  magnesium chloride Mg(s) + Cl2(g)  MgCl2(s)
  • 8. Definition Of Reduction • Reduction is a chemical reaction where it loses oxygen, gain hydrogen, gain electron and have a decrease in oxidation state by a molecule, atom or ion. • A reactant that reduces another substance is a reducing agent. • The reducing agent transfers electrons to another substance, it reduces others, and is thus itself oxidized. And, because it "donates" electrons, it is also called an electron donor.
  • 9. Reduction-Loss Of Oxygen When zinc burns in copper(II) oxide, the following reaction takes place. Zinc + copper oxide  Zinc oxide + copper Zn(s)+CuO(s)  ZnO(s)+Cu(s) Since Zinc has gain oxygen,it is oxidised. Copper(II) oxide loses oxygen,thus it is reduced.
  • 10. Reduction-Gain Of Hydrogen When nitrogen burns with hydrogen gas, the following reaction takes place. Nitrogen +Hydrogen  Ammonia N2 + 3H2  2NH3 Nitrogen gain hydrogen, thus it is being reduced.
  • 11. Reduction-Gain Of Electron When iron reacts with chloride acid, the following reaction takes place. Iron + chlorine  Iron(III) + Chloride 2Fe2++Cl2  2Fe3++2Cl- Since iron loses electron, it is oxidised. Chlorine gains electron, thus it is reduced.
  • 12. Common Reducing Agent • Lithium aluminium hydride (LiAlH4) • Nascent (atomic) hydrogen • Sodium amalgam • Diborane • Sodium borohydride (NaBH4) • Compounds containing the Sn2+ ion, such as tin(II) chloride • Sulfite compounds • Hydrazine (Wolff-Kishner reduction) • Zinc-mercury amalgam (Zn(Hg)) (Clemmensen reduction) • Diisobutylaluminum hydride (DIBAL-H) • Lindlar catalyst • Oxalic acid (C2H2O4) • Formic acid (HCOOH) • Ascorbic acid (C6H8O6) • Phosphites, hypophosphites, and phosphorous acid • Dithiothreitol (DTT) – used in biochemistry labs to avoid S-S bonds • Compounds containing the Fe2+ ion, such as iron(II) sulfate • Carbon monoxide(CO) • Carbon (C)
  • 14. The oxidation state is the charge an atom of an element would have if it existed as an ion in a compound.
  • 15. To work out the oxidation state of an atom, we apply the following rules: Rule Example Oxidation state 1. The oxidation state of a Cu, S, Cl2 0, 0, 0 free element is zero. 2. The oxidation state of a K+, Zn2+, Cl-, O2- +1, +2, -1, -2 simple ion is the same as the charge on the ion. 3. The oxidation states of Ca, C, 3O +2, +4, 3x(-2)=-6 the atoms present in the formula of a compound All add up to zero. add up to zero. The example shown here is CaCO3 . 4. The total of the S, 4O +6, 4x(-2)=-6 oxidation states of the atoms in a polyatomic ion All add up to -2. is equal to the charge on the ion. The example shown here is SO4 2- .
  • 16. Solution to question: Find the oxidation state of each element in ammonium sulfate. (NH4)2SO4 Since hydrogen in NH4 has an o.s of +1, Ammonium has a charge of 1. Let n be x 2(x+4(1))=2 2x-2-8 x=-3 Hence nitrogen has an o.s of -3
  • 17. Since oxygen in SO4 has an o.s of -2, Sulfate has a charge of -2. Let s be y y+4(-2)=-2 y-8=-2 y=6 Hence sulfur has an o.s of 6.
  • 19. Done by • Edwin • Kian Leong • Jeremy • Melvan