1 / 7

Redox Reactions

Redox Reactions. What is redox?. Redox reactions involve a transfer of electrons. Oxidation – involves losing electrons (increase in oxidation number) Reduction – involves gaining electrons (reduction in oxidation number) LEO the lion says GER Losing electrons = oxidation

abel
Download Presentation

Redox Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Redox Reactions

  2. What is redox? • Redox reactions involve a transfer of electrons. • Oxidation – involves losing electrons (increase in oxidation number) • Reduction – involves gaining electrons (reduction in oxidation number) • LEO the lion says GER • Losing electrons = oxidation • Gaining electrons = reduction

  3. How do you know if a reaction is redox or not? • Oxidation numbers can be assigned to all atoms based on electronegativity relative to the other atoms to which they are bonded. • If oxidation numbers change from one side of the equation to the other, that indicates that the reaction is a redox reaction.

  4. Rules for Assigning Oxidation Numbers • The oxidation number of an atom in the elemental state is zero.Example: Cl2 and Al both are 0 • The oxidation number of a monatomic ion is equal to its charge.Example: In the compound NaCl, the sodium has an oxidation number of 1+ and the chlorine is 1-. • The algebraic sum of the oxidation numbers in the formula of a compound is zero.Example: the oxidation numbers in the NaCl above add up to 0 • The oxidation number of hydrogen in a compound is 1+, except when hydrogen forms compounds called hydrides with active metals, and then it is 1-.Examples: H is 1+ in H2O, but 1- in NaH (sodium hydride). • The oxidation number of oxygen in a compound is 2-, except in peroxides when it is 1-, and when combined with fluorine. Then it is 2+.Example: In H2O the oxygen is 2-, in H2O2 it is 1-. • The algebraic sum of the oxidation numbers in the formula for a polyatomic ion is equal to the charge on that ion.Example: in the sulfate ion, SO42-, the oxidation numbers of the sulfur and the oxygens add up to 2-. The oxygens are 2- each, and the sulfur is 6+.

  5. Examples • NaCl • HNO3 • CaCO3 • PO4-3

  6. Redox Reactions • Identify which of the following equations represent redox reactions. • For each redox equation identified, write the oxidation state above each element. • Indicate the element that has been oxidized and the one that has been reduced.

  7. examples • KClO3 KCl + O2 • NaOH+ HClNaCl + H2O k • CO2 + H2O  C8H12O2+ O2 • NaCl + AgNO3  NaNO3 + AgCl

More Related