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Types of Chemical Reactions

Types of Chemical Reactions. The Five Reactions: synthesis, decomposition, single replacement, double replacement, and combustion reactions. Types of Reactions. There are millions of reactions. Can ’ t remember them all Fall into several categories. We will learn 5 types.

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Types of Chemical Reactions

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  1. Types of Chemical Reactions The Five Reactions: synthesis, decomposition, single replacement, double replacement, and combustion reactions

  2. Types of Reactions • There are millions of reactions. • Can’ t remember them all • Fall into several categories. • We will learn 5 types. • Will be able to predict the products. • For some we will be able to predict whether they will happen at all. • Will recognize them by the reactants

  3. #1 Synthesis Reactions • Combine - put together • 2 elements, or compounds combine to make one compound • Ca +O2® CaO • We can predict the products if they are two elements. • Mg + N2®

  4. Write and balance • Ca + Cl2® • Fe + O2® iron (II) oxide • Al + O2® • Remember that the first step is to write the formula • Then balance

  5. #2 Decomposition Reactions • decompose = fall apart • one reactant falls apart into two or more elements or compounds. • NaCl Na + Cl2 • CaCO3CaO+ CO2

  6. #2 Decomposition Reactions • Can predict the products if it is a binary compound • Made up of only two elements • Falls apart into its elements • H2O • HgO

  7. #2 Decomposition Reactions • If the compound has more than two elements you must be given one of the products • The other product will be from the missing pieces • NiCO3 • H2CO3(aq)

  8. #3 Single Replacement • One element replaces another • Reactants must be an element and a compound. • Products will be a different element and a different compound. • Na + KCl® K + NaCl • F2 + LiCl®LiF + Cl2

  9. #3 Single Replacement • Metals replace metals (and hydrogen) • K + AlN® • Zn + HCl® • Think of water as HOH • Metals replace one of the H, combine with hydroxide. • Na + HOH ®

  10. #3 Single Replacement • We can tell whether a reaction will happen • Some are more active than other • More active replaces less active • Use the list • Higher on the list replaces lower. • If the element by itself is higher, it happens, in lower it doesn’t (NR: no reaction)

  11. #3 Single Replacement • Note the * • H can be replaced in acids by everything higher • Only the first 5 (Li - Na) react with water. • Fe + CuSO4® • Pb + KCl® • Al + HCl®

  12. #3 Single Replacement • What does it mean that Au And Ag are on the bottom of the list? • Nonmetals can replace other nonmetals • Limited to F2 , Cl2 , Br2 , I2 • The order of activity is that on the table. • Higher replaces lower. • F2 + HCl® • Br2 + KCl®

  13. #4 Double Replacement • Two things replace each other. • Reactants must be two ionic compounds or acids. • Usually in aqueous solution • NaOH + FeCl3® • The positive ions change place. • NaOH + FeCl3® Fe+3 OH- + Na+1Cl-1 • NaOH + FeCl3® Fe(OH)3 + NaCl

  14. Complete and balance • assume all of the reactions take place. • CaCl2 + NaOH® • CuCl2 + K2S ® • KOH + Fe(NO3)3® • (NH4)2SO4 + BaF2®

  15. Examples • H2 + O2® • H2O ® • Zn + H2SO4® • HgO® • KBr +Cl2® • AgNO3 + NaCl® • Mg(OH)2 + H2SO3 ®

  16. #5 Combustion Reactions • A compound composed of only C H and maybe O is reacted with oxygen • the products will be CO2 and H2O.

  17. Examples • C4H10 + O2® • C6H12O6+ O2® Write a balanced equation for the complete combustion of each of these compounds. a) acetic acid, HC2H3O2 c) glycerol, C3H8O3 b) decane, C10H22 d) sucrose, C12H22O11

  18. Chapter 7 Summary

  19. The Process • Determine the type by looking at the reactants. • Put the pieces next to each other • Use charges to write the formulas • Use coefficients to balance the equation.

  20. How to recognize which type • Look at the reactants • E + E Combination • C Decomposition • E + C Single replacement • C + C Double replacement

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