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Understanding Redox Reactions: Oxidation and Reduction Processes

Redox reactions involve the transfer of electrons between substances. Oxidation is defined as the loss of electrons, while reduction is the gain of electrons. In a redox reaction, these processes must occur simultaneously through half-reactions. The oxidizing agent causes oxidation, whereas the reducing agent causes reduction. Oxidation states help determine the electron transfer and are essential for understanding chemical reactions. This guide explains the principles and examples of redox reactions, including the roles of oxidizing and reducing agents, as well as oxidation state rules.

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Understanding Redox Reactions: Oxidation and Reduction Processes

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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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