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Types of Reactions

Types of Reactions. Unit C – Chemical Reactions. Chemical equations. Chemical reaction: a process in which substances interact, causing new substances with different properties to form Reactant: a starting substance in a chemical reaction

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Types of Reactions

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  1. Types of Reactions Unit C – Chemical Reactions

  2. Chemical equations • Chemical reaction: a process in which substances interact, causing new substances with different properties to form • Reactant: a starting substance in a chemical reaction • Product: a substance that is formed in a chemical reaction

  3. Chemical equations • Chemical equation: a condensed statement that expresses chemical change using symbols and chemical names or formulas • Word equation: a chemical equation in which the reactants and products in a chemical reaction are represented by their chemical names; their relative quantities or states of matter are not included

  4. Chemical equations • Skeleton equation: a chemical equation in which the reactants and products in a chemical reaction are represented by their chemical formulas; their relative quantities or states of matter are not included • Balanced chemical equation: a statement that uses chemical formulas and coefficients to show the identities and ratios of the reactants and products in a chemical reaction

  5. Chemical equations • Coefficient: in a balanced chemical equation, a positive number that is placed in front of a formula to show the relative number of particles of the substance that are involved in the reaction Example #1 iron + oxygen  iron(III) oxide Fe(s) + O2(g)  Fe2O3(s)

  6. Chemical reactions • There are generally 5 types of chemical reactions: • Synthesis • Decomposition • Combustion • Single displacement • Double displacement

  7. Synthesis • Synthesis reaction: a chemical reaction in which two or more reactants combine to produce a single compound • There are 3 general types of synthesis reactions: • 2 elements react to form a binary compound • 1 element reacts with 1 compound to form a new compound • 2 compounds react to form a new compound

  8. Synthesis • 2 elements react to form a binary compound • A univalent metal reacts with a non-metal to form an ionic compound Example #1 2 Na(s) + Cl2(g)  2 NaCl(s)

  9. Synthesis • 2 elements react to form a binary compound • A multivalent metal reacts with a non-metal to form various ionic compounds Example #1 2 Cu(s) + Cl2(g)  2 CuCl(s) Example #2 Cu(s) + Cl2(g)  CuCl2(s)

  10. Synthesis • 2 elements react to form a binary compound • Two non-metals react to form a molecular compound Example #1 C(s) + O2(g)  CO2(g) Example #2 2 C(s) + O2(g)  2 CO(g)

  11. Synthesis • 1 element reacts with 1 compound to form a new compound Example #1 2 SO2(g) + O2(g)  2 SO3(g) Example #2 PCl3(ℓ) + Cl2(g)  PCl5(s)

  12. Synthesis • 2 compounds react to form a new compound • A non-metal oxide reacting with water to form an acid Example #1 CO2(g) + H2O(ℓ)  H2CO3(aq) Example #2 SO3(g) + H2O(ℓ)  H2SO4(aq)

  13. Synthesis • 2 compounds react to form a new compound • A metal oxide reacting with water to form a base Example #1 Na2O(s) + H2O(ℓ)  2 NaOH(aq) Example #2 MgO(s) + H2O(ℓ)  Mg(OH)2(aq)

  14. Decomposition • Decomposition reaction: a chemical reaction in which a compound breaks down into elements or simpler compounds • There are 4 general types of decomposition reactions (and a few special ones): • A binary compound decomposing into its elements • A metal nitrate decomposing into a metal nitrite and oxygen gas • A metal carbonate decomposing into a metal oxide and carbon dioxide • A metal hydroxide decomposing into a metal oxide and water • Special reactions

  15. Decomposition • A binary compound decomposing into its elements Example #1 2 NaCl(s)  2 Na(s) + Cl2(g) Example #2 2 HgO(s)  2 Hg(ℓ) + O2(g) • A metal hydroxide decomposing into a metal oxide and water Example #1 Ca(OH)2(s) CaO(s) + H2O(g)

  16. Decomposition • A metal nitrate decomposing into a metal nitrite and oxygen gas Example #1 2 NaNO3(s)  2 NaNO2(s) + O2(g) • A metal carbonate decomposing into a metal oxide and carbon dioxide Example #1 CaCO3(s) CaO(s) + CO2(g) Sr(OH)2 (s)  H2O(l) + SrO(s)

  17. Decomposition • Special reactions • TNT (tri-nitro-toluene), dynamite Example #1 2 C7H5N3O6(s)  3 N2(g) + 5 H2O(g) + 7 CO(g) + 7 C(s) • Air bags (sodium azide): Example #1 2 NaN3(s)  2 Na(s) + 3 N2(g)

  18. Decomposition • Special reactions • Rocket thrusters (hydrazine): Example #1 3 N2H4(ℓ)  4 NH3(g) + N2(g) N2H4(ℓ)  N2(g) + 2 H2(g)

  19. Combustion • Combustion reaction: the reaction of a substance with oxygen, producing one or more oxides, heat, and light • Hydrocarbon: a compound that is composed only of the elements carbon and hydrogen • There are 2 general types of combustion of hydrocarbon reactions: • Complete combustion • Incomplete combustion

  20. Combustion

  21. Combustion • Complete combustion occurs when the only products are carbon dioxide (CO2) and water (H2O) Example #1 C3H8(g) + O2(g)  CO2(g) + H2O(ℓ)

  22. Combustion • Incomplete combustion occurs when the products are carbon dioxide (CO2) and water (H2O) AS WELL AS carbon monoxide (CO) and carbon/soot (C) • Soot: fine particles consisting mostly of carbon, formed during the incomplete combustion of a hydrocarbon Example #1 2 C3H8(g) + 7 O2(g)  2 CO2(g) + 8 H2O(ℓ) + 2 CO(g) + 2 C(s) 2 C3H8(g) + 7 O2(g)  CO2(g) + 8 H2O(ℓ) + 4 CO(g) + C(s) 2 C3H8(g) + 6 O2(g)  CO2(g) + 8 H2O(ℓ) + 2 CO(g) + 3 C(s)

  23. Combustion • Combustion reactions can also occur between oxygen and many other substances • Some of these reactions are not only combustion reactions, but synthesis reactions as well Example #1 2 H2(g) + O2(g)  2 H2O(g) Example #2 2 Mg(s) + O2(g)  2 MgO(s)

  24. Combustion • Combustion also occurs inside living organisms • An example of this is the combustion of glucose which is a chemical reaction necessary for life (cellular respiration) Example #1 C6H12O6(s) + O2(g)  6 CO2(g) + 6 H2O(g) • Although both combustion and cellular respiration are similar chemical reactions, there are some notable differences among the two processes

  25. Combustion

  26. Single displacement • Single displacement reaction: a chemical reaction in which one element in a compound is replaced (displaced) by another element • Activity series (metal & non-metal): a ranking of the relative reactivity of metals or halogens in aqueous reactions • There are 3 general types of single displacement reactions: • A metal displacing another metal from an ionic compound (involves activity series of metals) • A metal displacing hydrogen from acid or water (involves activity series of metals) • A non-metal displacing another non-metal from an ionic compound (involves activity series of non-metals)

  27. Single displacement • A metal displacing another metal from an ionic compound (involves activity series of metals) Example #1 Cu(s) + 2 AgNO3(aq)  Cu(NO3)2(aq) + 2 Ag(s) Example #2 Cu(s) + Al(NO3)3(aq) No reaction

  28. Single displacement • A metal displacing hydrogen from acid or water (involves activity series of metals) Example #1 Mg(s) + 2 HCl(aq)  MgCl2(aq) + H2(g) Example #2 Na(s) + H2O(ℓ) NaOH(aq) + H2(g) Example #3 Cu(s) + HCl(aq)  No reaction

  29. Single displacement • A non-metal displacing another non-metal from an ionic compound (involves activity series of non-metals) Example #1 Cl2(g) + 2 NaBr(aq)  2 NaCl(aq) + H2(g)

  30. Chemical reactions • [organizational chart summarizing all 5 types and subcategories]

  31. References • [include 2010 and 2003 MHR Chemistry 11 textbooks]

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