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Types of Chemical Equations

Types of Chemical Equations. https://www.youtube.com/watch?v=tE4668aarck. Types of Reactions.

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Types of Chemical Equations

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  1. Types of Chemical Equations https://www.youtube.com/watch?v=tE4668aarck

  2. Types of Reactions Chemists know that elements and compounds undergo particular types of chemical reactions. Just as all members of a chemical family react in a similar way, compounds have definite patterns of chemical properties.

  3. Types of Reactions Chemists use these patterns to classify groups of chemical changes. Most chemical reactions can be grouped into five categories: 1. synthesis 2. decomposition 3. single displacement 4. double displacement 5. combustion

  4. Synthesis Reactions Synthesis reactions involve the combination of smaller atoms and/or molecules into larger molecules. These reactions are sometimes also called combination reactions. Often the reactants are elements that combine chemically to form compounds.

  5. Synthesis Reactions A + B  AB

  6. Synthesis Reactions Description A chemical reaction in which two or more reactants combine to produce a new product.

  7. A+BAB Example: • The “Haber” process to produce ammonia • N2(g) + 3H2(g)  2NH3(g)

  8. A+BAB Example: • The shuttle “blast off” • 2H2(l) + O2(l) 2H2O(g)

  9. A+BAB Example: • The production of “smog” • N2(g) + O2(g) 2NO2(g) • 2NO(g) + O2(g) 2NO2(g)

  10. Synthesis Reactions Synthesis reactions can also involve combinations of small molecules. For example, when ammonia and hydrogen peroxide combine, they form a white smoke as solid particles of ammonium chloride are formed. hydrogen chloride + ammonia  ammonia chloride HCl + NH3 NH4Cl

  11. Decomposition Reactions Description A a chemical reaction in which a compound breaks down into two or more simpler compounds or elements.

  12. Decomposition Reactions AB  A + B

  13. AB  A + B Example: • The electrolysis of water • 2H2O(l) 2H2(g) + O2(g)

  14. AB  A + B Example: A TNT Explosion 2C7H5N3O6 (s)  3N2(g) + 5H2O(g) + 7CO(g) + 7C(s)

  15. AB  A + B Example: • Decomposition of sodium azide (air bags) • 2NaN3(s)  3N2(g) + 2Na(s)

  16. Displacement Reactions Many industrial processes, such as the one used to isolate nickel from the deposits found around Sudbury, rely on a series of chemical reactions that include the displacement of one element by another to form a new compound.

  17. Single Displacement Description A chemical reaction in which one element takes the place of an element in a compound to produce another element and another compound.

  18. Single Displacement A + BC  AC + B (where A is a metal) A + BC  BA + C (where A is a non-metal)

  19. A + BC  AC + B Example: Producing zinc chloride (ZnCl2) and hydrogen gas (H2) Zn(s) + 2HCl(aq)  ZnCl2 (aq) + H2(g)

  20. A + BC  AC + B Example: Producing copper (Cu) metal Mg(s) + CuSO4(aq)  MgSO4 (aq) + Cu (s)

  21. A + BC  AC + B Example: • Displacing silver (Ag) from silver nitrate (AgNO3) • Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)

  22. Activity Series The activity series is a list of elements organized according to their chemical reactivity. The most reactive element appears on the top, and the least reactive appears at the bottom. Remember! Metals can only replace other metals in a reaction, and non-metals can only replace other non-metals. Metals higher up on the activity series list will replace metals lower on the list during a single displacement reaction.

  23. Double Displacement Description A chemical reaction in which the positive ions of two different compounds exchange places, resulting in the formation of two new compounds.

  24. Double Displacement AB + CD  AD + CB

  25. AB + CD  AD + CB Example: Sulfur dioxide (SO2) is used to preserve the colour of dried fruit. A double displacement reaction followed by a decomposition reaction releases the sulfur dioxide gas required for the process. Na2SO3(aq) + 2HCl(aq) 2NaCl (aq) + H2SO3(aq) The decomposition reaction H2SO3(aq) H2O(l) + SO2(g)

  26. AB + CD  AD + CB Example: A double displacement reaction between two soluble salts may produce an insoluble salt, causing a precipitate to form. Eg: Lead (II) nitrate solution reacts with sodium chloride solution, forming a precipitate. Pb(NO3)2 (aq) + 2NaCl (aq) 2NaNO3(aq) + PbCl2(s)

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