Oxidation Reduction Reaction (Redox): A reaction in which electrons are transferred from one...
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Transcript of Oxidation Reduction Reaction (Redox): A reaction in which electrons are transferred from one...
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Oxidation Reduction Reaction (Redox):A reaction in which electrons are
transferred from one substance to another.
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Oxidation cannot occur without reduction Definition of Oxidized:
1. Losing of electrons (LEO)2. Increasing the ox. number, ie: 0 to +1
-2 to -13. Gaining oxygen
Definition of Reduced:1. Gaining of electrons (GER)2. Reducing the ox. number, ie: -1 to -2
1 to 03. Losing oxygen
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2Mg + O2 2MgO Mg atom transfers two electrons to each
oxygen atom. As a result 2 Mg atoms become Mg2+ and
two oxygen atoms become O2-
Mg loses two electrons O gains two electrons
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2Mg + O2 2MgO Mg atom transfers two electrons to each
oxygen atom. As a result 2 Mg atoms become Mg2+ and
two oxygen atoms become O2-
Mg loses two electrons O gains two electrons
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Can oxidation occur without reduction? What are the three definitions of oxidation? What are the three definitions of reduction? What is a way to remember oxidation/reduction in
terms of transfer of electrons? Does the oxidation number increase or decrease
when there is oxidation? Does the oxidation number increase or decrease
when there is reduction?
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When an electron is lost (An electron is found on the product side) there is oxidation◦ X0 X+1 + e-
When an electron is gained (An electron is found on the reactant side) there is reduction◦ e- +Y+1 Y0
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Ex5 Na0Na+1
Ex6 Fe+3Fe+2
Ex7 N+1N+2
Ex8 Mg+2Mg0
+1e-
1e-+
+1e-
2e-+
(LEO)oxidized
(GER)reduced
(LEO)oxidized
(GER)reduced
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Whatever is oxidized is called the reducing agent
Whatever is reduced is called the oxidizing agent
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Ex5 Na0Na+1
Ex6 Fe+3Fe+2
Ex7 N+1N+2
Ex8 Mg+2Mg0
+1e-
1e-+
+1e-
2e-+
oxidized
reduced
oxidized
reduced
reducing agent
oxidizing agent
reducing agent
oxidizing agent
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What is a reducing agent?
What is a oxidizing agent?
Are metals generally oxidized or reduced?
Are nonmetals generally oxidized or
reduced?
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Redox Rules to LearnFor Ionic and Covalent bonds
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Definition: Electonegativity is the atom’s ability to attract electrons.
Fluorine is the most electronegative element
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Increase ENMore protons to attract electrons
Decrease ENelectrons get further away from protons
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Oxidation number of an uncombined atom = zero(no compounds or ions)
i.e . Mg, H2, Na
ie. All H2 O2 N2 Cl2 Br2 I2 F2 ’s ox. # are zero
0 0 0
0 0 0 0 0 0 0
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Oxidation number of a monatomic ion = charge of the ion
i.e. Mg2+ , O2- , Al3+ , Br-
+2 +3 -1-2
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The sum of the oxidation numbers of a neutral compound = 0
i.e. H2O CO2 CO NaCl+1
2(+1)
-2
- 2 = 0
-2
2(-2)
+4
4 + = 0
-2+2
=0
-1+1
=0
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The oxidation number for H is +1 Exception: when bonded to a less electronegative element (metal), then it is -1.
i.e. LiH, NaH, MgH2 Exception
i.e. HF, HCl
+1 -1 -1+1 +2 -1
+1 -1 +1 -1
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Oxygen’s oxidation number is -2, in a compound
Two exceptions: peroxides and fluorine
in H2O2
with OF2
+1
2(+1) + 2( ?) = 0
? = -1
where O is -1
-1
2(-1)? + = 0
+2 where O is +2
fluorine (more electronegative)
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Oxidation number ofpolyatomic compound = zero polyatomic ion = the charge of the ion
i.e. compounds:
NH3 SiCl4 K3PO4
i.e. ions:
NH4+ CO3
2- SO42- NO3
-
+1
3(+1)
-3
-3 + = 0
+1
4(1)
-3
-3+ = +1
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Oxidation numbers for metals in:
Group 1A metal compound +1 2A metal compound +2 3A Aluminum compound +3
i.e. NaCl MgSO4 AlPO4
+1 -1
= 0
+2 +3
= 0
-2
+2 + ? + 4(-2)
+6
= 0
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The most electronegative element fluorine ALWAYS has an oxidation number of -1 when it is bonded to another element.
i.e. HF
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Assign oxidation numbers to each element
1.Cl2
2.Cl-
3.MgCl2
4. NaH
5. HCl
6. K3PO4
7. CaSO4
8. KF
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If oxidation number goes up it is oxidized. If oxidation number goes down it is reduced.
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Balance the reactions, write the oxidation numbers for each atom and write the oxidizing and reducing agents.
Ex1 HCl + Zn ZnCl2 + H22-1+1 0 0-1
2(-1)
+2
+2 + =0
Loss of electron oxidation (LEO)
Gain of electron reduction (GER)
Oxidizing agent
Reducing agent
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Ex2 Mg + N2 Mg3N2
Ex3 H2S + Cl2 HCl + S
Ex4 Fe + O2 Fe2O3
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There are three definitions of oxidation and reduction:
Oxidation Reduction1. 1.
2. 2.
3. 3.
Losing of electrons (LEO)
Gaining oxygen
Increasing oxidation #
Losing oxygen
Decreasing oxidation #
Gaining of electrons (GER)
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L E O goes G E R O I L R I G OSE
LECTRONS
XIDATION
AIN
LECTRONS
EDUCTION
XIDATION
S OSING
EDUCTION
S AINING