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REDOX Reactions

REDOX Reactions. Oxidation – Reduction . Oxidation – Reduction Reaction. These reactions involve a transfer of electrons Half reactions MUST occur simultaneously Oxidation – loss of electrons Oxidizing agent – a substance that has the potential to cause another substance to be oxidized.

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REDOX Reactions

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  1. REDOX Reactions Oxidation – Reduction

  2. Oxidation – Reduction Reaction • These reactions involve a transfer of electrons • Half reactions MUST occur simultaneously • Oxidation – loss of electrons • Oxidizing agent – a substance that has the potential to cause another substance to be oxidized

  3. Oxidation – Reduction Reaction • Reduction – involves the gain of electrons • Reducing agent – a substance that has the potential to cause another substance to be reduced (gain electrons)

  4. Oxidation States • The oxidation number of a pure element is 0 • The oxidation number of a monatomic ion equals the charge on the ion • The more electronegative element in a binary compound is assigned the number equal to the charge it would have it were an ion • The oxidation number of fluorinein a compound is always -1 • Oxygen has an oxidation number of -2 unless it is combined with Fluorine, in which it is +1 or +2, or it is in a peroxide, in which it is -1

  5. Oxidation States • Hydrogen’s oxidation state in most of its compound is +1, unless it is combined with a metal, in which case it is -1 • In compounds, Group1 and Group 2 elements and aluminum have oxidation numbers of +1, +2, and +3 respectively • The sum of the oxidation numbers of all atoms in a neutral compound in 0 • The sum of the oxidation numbers of all atoms in a polyatomic ion equals the charge of the ion

  6. Oxidation • Oxidation is the process in which atoms or ions of an element experience an increase in oxidation states 2 Na (s) + Cl2 (g) 2 NaCl(s) • Sodium undergoes an oxidation process because the sodium atoms loses an electron and become a sodium ion – sodium is an oxidized to a sodium ions • Electrons are on the right side of the arrow) • A species whose oxidation number increases is oxidized • 0 +1 • Na  Na+ + e-

  7. Reduction • Reduction is the process in which the oxidation state of an element decreases 2 Na (s) + Cl2 (g) 2 NaCl(s) •  Each chlorine atom accepts an electrons and becomes a chloride ion • Electrons are on the left side of the arrow Cl2+ 2e- 2Cl- • A species that undergoes a decrease in oxidation state is reduced

  8. Oxidation – Reduction Reaction Lose Gain Electrons Electrons OxidationReduction • “Leo” the lion says “Ger”

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