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Types of Chemical Reactions

Learn about the five general types of chemical reactions, including synthesis, decomposition, single displacement, double displacement, and combustion. Understand the characteristics and examples of each reaction type.

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Types of Chemical Reactions

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  1. Types of Chemical Reactions • There are five general types of reactions: • Synthesis • Decomposition • Single Displacement • Double Displacement • Combustion

  2. Synthesis Reactions Synthesis Reactions

  3. synthesis reactions • The word synthesis means to bring together separate parts into a new whole. • Chemical synthesis reactions take two elements or polyatomic ions and combine them into a new compound. • Have the form A + B = AB

  4. A. Synthesis • the combination of 2 or more simpler substances to form a more complex compound • only one product forms A+ BAB 2P + 3Br2 2PBr3

  5. Synthesis Reactions • Synthesis reactions are also called combination reactions • A synthesis reaction occurs when two substances combine to form a new compound

  6. Real life please…. Rust is a synthesis reaction 4Fe + 3O2 Fe2O3

  7. Synthesis Reactions Fe + O2 FeO2

  8. Examples of Synthesis Reactions • 2 Mg (s) + O2 (g)  2 MgO (s) • Fe (s) + Cl2 (g)  FeCl2 (s) • U (s) + 3 F2 (g)  UF6 (g)

  9. synthesis reactions: • __ H2 + __ O2__ H2O • __ C + __ H2__ C3H8 • __ S8+ __ O2__ SO3 • __ P + __ O2__ P2O5

  10. synthesis reactions: • 2 H2 + O2 2 H2O • 3 C + 4 H2C3H8 • S8+ 12 O28 SO3 • 4 P + 5 O22 P2O5

  11. Decomposition Reactions

  12. decomposition reactions • The word decompose means to break a compound apart into its pieces. • Decomposition reactions take a compound reactant and break it into two separate elements or polyatomic ion products. • Have the form AB  A + B

  13. B. Decomposition • a complex compound breaks down into 2 or more simpler substances • only one reactant ABA+B 2H2O2 2H2O + O2

  14. Decomposition Reactions Electrolysis Animations An example decomposition reaction 2H2O 2H2 + O2

  15. Decomposition Reactions Write the equation for the break down of marble (Calcium Carbonate) into Calcium Hydroxide which then further breaks down into Carbon Dioxide and Calcium Oxide.

  16. Decomposition Reaction • In decomposition reactions, one substance breaks down (decomposes) into two or more simpler substances

  17. Examples of Decomposition Reactions • 2 HgO (s)  2 Hg (l) + O2 (g) • Ca(OH)2  CaO (s) + H2O (g) • H2SO4 (aq)  SO3 (g) + H2O (l) 

  18. decomposition reactions: • __ KClO3__ KCl+ __ O2 • __ Fe(OH)3__ Fe2O3+ __ H2O • __ Ag2O __ Ag + __ O2

  19. decomposition reactions: • 2 KClO32 KCl+ 3 O2 • 4 Fe(OH)32 Fe2O3+ 6 H2O • 2 Ag2O 4 Ag + O2

  20. Replacement Reactions

  21. replacement reactions Oh noes! • Replacement reactions are where one element replaces the other in a pair. • For example: Mr. Goober and Halle Barry are dancing in the club, when suddenly…

  22. Single Replacement Reaction • In a single replacement reaction (also called a displacement reaction), an element reacts with a compound • A + BX AX + B

  23. C. Single Replacement • one element replaces another in a compound; an uncombined element replaces one in the compound • metal replaces metal (+) • nonmetal replaces nonmetal (-) A +BCAC+B Zn + 2HCl  ZnCl2 + H2

  24. Real life please… • Never store acids in metal containers because 2Al + 6HCl 2AlCl3 + 3H2 The metal container will dissolve, leaking the acid everywhere…

  25. Examples of Single Replacement Reactions • Mg + Zn(NO3)2  Mg(NO3)2 + Zn • Mg + 2 AgNO3  Mg(NO3)2 (aq) + 2 Ag

  26. Single Replacement Reactions NaF Cl2 NaCl + F2 _____ + _____ FeCl2 + K  _____ + _____ HCl + Zn  _____ + _____ H2O + Na  _____ + _____ AgNO3 + Cu  _____ + _____ KCl Fe ZnCl2 H2 H2 NaOH CuNO3 Ag

  27. Replacement

  28. Double Replacement

  29. Double Replacement Definition AB + CD  AD + CB + + 

  30. Double Displacement Reactions • In a double displacement reaction, two compounds react • The compounds swap elements with each other

  31. Double Displacement • Compounds contain a positive and negative part • In a double displacement, the positive parts swap places with each other as do the negative parts

  32. D. Double Replacement • ions in two compounds “change partners” • cation(+) of one compound combines with anion(-) of the other AB +CDAD +CB 2KOH + CuSO4 K2SO4 + Cu(OH)2

  33. Double replacements • Double replacements are similar to single, except in a double replacement, two ionic “couples” switch partners! AB + CD  AD + CB

  34. Double Replacement TlKs + RpTs RpKs + TlTs AD + CB AB + CD

  35. Real life please… 2HCl + Mg(OH)2 MgCl2 + 2H2O When your stomach is upset (heartburn, ect) and there is excess stomach acid, TUMS or milk of magnesia is used to neutralize the excess stomach acid.

  36. replacement reactions: • __AlBr3+ ___ K2SO4___ KBr + ___ Al2(SO4)3 • __ FeCl3 + ___ NaOH___ Fe(OH)3 + __NaCl • __ CF4 + __ Br2 __ CBr4 + __ F2 • __ Pb(OH)2 + ___ HCl___ H2O + ___ PbCl2

  37. replacement reactions: • 2 AlBr3+ 3 K2SO46 KBr+ Al2(SO4)3 • FeCl3+ 3 NaOHFe(OH)3+ 3 NaCl • CF4+ 2 Br2CBr4+ 2 F2 • Pb(OH)2+ 2HCl 2H2O + PbCl2

  38. Predicting Product Rules • Identify your Cations and Anions • Decide what new things will bond together • DO the ionic or covalent bonding process • Finish your equation • Balance • Identify what type of reaction

  39. Practice • Predict the products. • Balance the equation • Identify the type of reaction for each of the following • HCl + AgNO3  • CaCl2 + Na3PO4  • Pb(NO3)2 + BaCl2  • FeCl3 + NaOH • H2SO4 + NaOH  • KOH + CuSO4 

  40. Practice Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N2 + O2 BaCO3  Co(III)+ S NH4 + H2CO3  NI3 

  41. Predict the Products of the following reactions and balance • BaCl2 (aq) + KClO4 (aq)  • HCl (aq) + NaOH (aq)  • RbBr (aq) + AgCl (aq) 

  42. Review – Balance/identify type • 1. FeCl3 + NaOH  Fe(OH)3 + NaCl • 2. CuCl2 + NaI  CuI2 + NaCl • 3. H2O2  H2O + O2

  43. Review-Write Skeleton Equations • 1. Magnesium metal reacts with Chlorine to form Magnesium Chloride. • 2. Silver Nitrate reacts with Sodium Chloride to form Silver Chloride and sodium nitrate

  44. Balance the following/identify type • H2 + O2 H2O • Na + Br2 NaBr • AgNO3 + Cu  Cu(NO3)2 + Ag

  45. Review-Write Balanced Equations • 1. Hydrogen reacts with chlorine to form hydrogen chloride • 2. Carbon monoxide gas reacts with gaseous oxygen to form carbon dioxide

  46. Write Balanced Equations • 1) Na + Cl2 • 2) HgCl2 • 3) Fe(OH)3

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