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Redox and Synthesis

Redox and Synthesis. Redox and Synthesis: At the conclusion of our time together, you should be able to:. Recognize a synthesis chemical reaction Show the change in oxidation numbers in this reaction type. Simple Reactions. Synthesis (Combination). Decomposition. Single Replacement.

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Redox and Synthesis

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  1. Redox and Synthesis

  2. Redox and Synthesis:At the conclusion of our time together, you should be able to: Recognize a synthesis chemical reaction Show the change in oxidation numbers in this reaction type

  3. Simple Reactions Synthesis (Combination) Decomposition Single Replacement Double Replacement

  4. Synthesis A + B A B Decomposition A + B A B Single Replacement + + A B C A C B Double Replacement + + A B C D A D C B

  5. Synthesis A + B A B Decomposition A + B A B Single Replacement + + A B C A C B Double Replacement + + A B C D A D C B

  6. 1. Synthesis reactions • Synthesis reactionsoccur when two substances (generallyelements) combine and form a compound. (Sometimes these are called combination or addition reactions.) reactant + reactant  1 product • Basically: A + B  AB • Example: 2H2 + O2  2H2O • Example: C+ O2  CO2

  7. Synthesis Reactions • Here is another example of a synthesis reaction

  8. Synthesis and Redox • Predict the products, balance the following reaction and give the change in oxidation numbers: Na + Cl2  NaCl 2 Na + Br2  2 NaCl Each Na loses 1e- oxidation, reducing agent Each Clgains 1e- reduction, oxidizing agent

  9. Redox and Synthesis:Let’s see if you can: Recognize a synthesis chemical reaction Show the change in oxidation numbers in this reaction type

  10. Practice • Predict the products. Write and balance the following synthesis reaction equations. • Sodium metal reacts with chlorine gas Na(s) + Cl2(g)  • Solid Magnesium reacts with fluorine gas Mg(s) + F2(g)  • Aluminum metal reacts with fluorine gas Al(s) + F2(g)  NaCl MgF2 AlF3

  11. Practice • State the type, predict the products, balance the following reactions and show the change in oxidation numbers: Cs + Br2  CsBr 2 Cs + Br2  2 CsBr Each Cs loses 1e- oxidation, reducing agent Each Br gains 1e- reduction, oxidizing agent

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