REDOX REACTIONS.

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Oxidation-Reduction Reactions “Redox”

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Presentation transcript:

REDOX REACTIONS

A process in which a substance loses one or more electrons OXIDATION A process in which a substance loses one or more electrons

A process in which a substance gains one or more electrons REDUCTION A process in which a substance gains one or more electrons

Oxidation Is Losing electrons Reduction Is Gaining electrons OIL RIG Oxidation Is Losing electrons Reduction Is Gaining electrons

Oxidation and reduction always occur together!

OXIDATION-REDUCTION RXNS Reactions in which electrons are transferred between reactants (bka Redox Reactions)

The key to Redox is Oxidation Number!

A way of tracking electrons in redox reactions OXIDATION NUMBERS A way of tracking electrons in redox reactions

Assigning Oxidation Numbers (6 rules)

The oxidation # of an atom by itself is zero. Rule 1 The oxidation # of an atom by itself is zero.

The oxidation # of any monatomic ion is equal to its charge. Rule 2 The oxidation # of any monatomic ion is equal to its charge.

The oxidation # of elements in a compound are written per atom. Rule 3 The oxidation # of elements in a compound are written per atom.

The sum of the oxidation #s in a compound is zero. Rule 4 The sum of the oxidation #s in a compound is zero.

Rule 5 The sum of the oxidation #s in a polyatomic ion is equal to the ion’s charge.

Oxidation #s to remember: Rule 6 Oxidation #s to remember: Elements in Group 1A: always +1 Elements in Group 2A: always +2 Aluminum: always +3

Oxidation #s to remember: Rule 6 Oxidation #s to remember: Fluorine: always -1 Hydrogen: usually +1 Oxygen: usually -2

Remember: Oxidation #s are not charges Remember: Oxidation #s are not charges! (they are just a way to track electrons)

Oxidation: when the oxidation # increases Another Definition Oxidation: when the oxidation # increases

Reduction: when the oxidation # decreases Another Definition Reduction: when the oxidation # decreases

Remember that oxidation and reduction occur together…

Causes oxidation Is itself reduced Oxidizing Agent Causes oxidation Is itself reduced

Causes reduction Is itself oxidized Reducing Agent Causes reduction Is itself oxidized