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Overview
• Oxidation and reduction reactions always occur together (redox reactions)
• You can’t have one without the other
• Includes: extracting metal from an ore
• Salt on roads– Salt accelerates the reaction between oxygen
and metal– Makes electron transfer easier
Oxygen
• Most abundant element on Earth
• 21% of our atmosphere (pure)
• 89% of Earth’s water (compound)
• 45.5% of Earth’s crust (compound)
• 2/3rd’s of the human body (compound)
• Foods (compound)
• Rust
Chemical Properties of Oxygen
• Combines with many elements and compounds
• Rust (reacts with metals)
• Other oxides (reacts with nonmetals)
• Methane (reacts with other compounds)– Bunsen burner
Hydrogen
• In the universe, 95% of all atoms are hydrogen
• Seldom found alone
• Hydrocarbons
• Hindenburg…
3 ways of looking at oxidation and reduction
• 1. oxidation is a gain of oxygen atoms, reduction is a loss of oxygen atoms
• 2. oxidation is a loss of hydrogen atoms, reduction is a gain of hydrogen atoms
• 3. oxidation is a loss of electrons, reduction is a gain of electrons– Most fundamental explanation, what we will
be dealing with the most
Oxidation Reduction
Gains oxygen Lose Oxygen
Lose Hydrogen Gains hydrogen
Lose Electrons Gains electrons
Oxygen
Hydrogen
e-
In relation to our lab…
• Remember that reduction is a loss of oxygen from a compound
• We converted iron ore to metallic iron– We removed oxygen from the iron(III) oxide
– 2Fe2O3 + 3C 4Fe + 3CO2
– Carbon was oxidized because it gained an oxygen
Leo the Lion!
• LEO the lion says GER– Loss of electrons is oxidation, gain of
electrons is reduction
Examples
• Is the reactant oxidized or reduced?
• Pb PbO3
• SnO2 SnO
• KClO3 KCl
• C2H6O C2H4O
• C2H2 C2H6
Pertaining to LEO…
• Mg + S MgS• Mg + S Mg2+ + S2-
• Magnesium is oxidized– Said to be the reducing agent– Substance in the reaction that loses electrons
• Sulfide sulfur atom is reduced – Said to be the oxidizing agent– Substance in the reaction that gains electrons
Oxidation Numbers
• A count of the electrons transferred or shared in the formation or breaking of chemical bonds
• You must assign each element in the reaction an oxidation number
• Follow a set of rules…
Oxidation Number Rules
1. The total of the oxidation numbers of all the atoms in a neutral molecule, an isolated atom, or a formula unit is 0– Examples
2. In their compounds, the Group 1A metals all have an oxidation number of +1, and the Group 2A metals have an oxidation number of 2+.– Examples
Rules Con’t
3. In its compounds, hydrogen has an oxidation number of +1 (except in metal hydrides such as NaH, where it is -1)– Examples
4. In its compounds, oxygen has an oxidation number of -2 (except in peroxides such as H2O2, where it is -1)– Examples
5. In their binary compounds with metals, Group7A elements have an oxidation number of -1. Group 6A elements have an oxidation number of -2, and Groups 5A elements have an oxidation number of -3.– Examples
Identifying Redox Reactions
0 +3 -2 0 +3 -2
• 2 Al + Fe2O3 2 Fe + Al2O3
• Al increases from 0 to +3, it is ______
• Oxidized!
• Fe decreases from +3 to 0, it is _______
• Reduced!
Oxidizing and Reducing Agents
• Now the confusing part…
• CuO + H2 Cu + H2O
• Cu goes from +2 to 0– Cu is reduced, therefore it is called an oxidizing
agent because it causes some other substance to be oxidized
• H goes from 0 to +1– H is oxidized, therefore it is called a reducing agent
because it causes some other substance to be reduced.
Identifying Agents in an Equation
• CuO + H2 Cu + H2O
Reduction: CuO is the oxidizing agent
Oxidation: H2 is the reducing agent
Some common oxidizing agents
• Oxygen!– Oxidized coal in electric power– Gas in automobiles– Wood in campfires– Food we eat
• Antiseptics– Hydrogen Peroxide– Benzoyl peroxide
• Disinfectants– Chlorine