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Chemical Reactions

Chemical Reactions . Describing Chemical Reactions. Chemical Reaction – process where a new substance is produced Indications of a chemical reaction heat and light production of a gas formation of a precipitate Precipitate – a solid formed when two ionic solutions are mixed.

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Chemical Reactions

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  1. Chemical Reactions

  2. Describing Chemical Reactions • Chemical Reaction – process where a new substance is produced • Indications of a chemical reaction • heat and light • production of a gas • formation of a precipitate • Precipitate – a solid formed when two ionic solutions are mixed

  3. Types of Reactions • There are five types of chemical reactions we will talk about: • Combination • Decomposition • Single Replacement • Double Replacement • Combustion • You need to be able to identify the type of reaction and predict the product(s)

  4. Combination Reactions • aka Synthesis reactions • occur when two or more substances combine and form a compound • Reactant + Reactant  1 Product • Ex: Ca (s)+ Cl2 (g)  CaCl2 (s)

  5. Practice • Predict the products. Write and balance the following synthesis reaction equations. • Example #1 - Aluminum metal reacts with fluorine gas Al(s) + F2(g)  2 3 AlF3(s) 2

  6. Decomposition Reactions • occurs when a compound breaks up into the elements when heated • 1 Reactant  Product + Product • Ex: 2 KCl (s)  2K (s) + Cl2 (g)

  7. Practice • Predict the products. Then, write and balance the following decomposition reaction equations: • Example #2 – Solid lead (IV) oxide decomposes PbO2(s)  Pb(s) + O2(g)

  8. Single Replacement Reactions • occur when one element replaces another in a compound • a metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-) • Ex: 2K (s) + MgCl2 (aq)  2 KCl (aq) + Mg (s) • Ex: Br2 (g) + 2 LiCl (aq)  2 LiBr (aq) + Cl2 (g)

  9. Single Replacement Reactions • Write and balance the following single replacement reaction equation: • Example #3 - Zinc reacts with aqueous hydrogen monochloride Zn(s) + HCl(aq) ZnCl2(aq) + H2(g)Note: Zinc replaces the hydrogen ion in the reaction • Example #4 - Sodium chloride solid reacts with fluorine NaCl(s) + F2(g)  NaF(s) + Cl2(g) 2 2 2

  10. Double Replacement Reactions • Example: • AgNO3(aq) + NaCl(s)  • occur when a metal replaces a metal and a nonmetal replaces a nonmetal in a compound • Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together AgCl(s) + NaNO3(aq) • Another example: • K2SO4(aq) + Ba(NO3)2(aq)  2 KNO3(aq) + BaSO4(s)

  11. Practice • Predict the products. Balance the equation • Example # 5 – Aqueous calcium chloride reacts with aqueous sodium phosphate CaCl2(aq) + Na3PO4(aq)  • Example # 6 – Aqueous iron (III) chloride reacts with aqueous sodium hydroxide FeCl3(aq) + NaOH(aq)  3 2 6 NaCl (s) + Ca3(PO4)2(aq) NaCl (s) + Fe(OH)3(aq) 3 3

  12. Combustion Reactions • occur when a hydrocarbon or alcohol reacts with oxygen gas • CxHy + O2  CO2 + H2O • products are ALWAYS carbon dioxide and water • Ex : 2CH3OH + 3O2  4H2O + 2CO2

  13. Combustion • Write the products and balance the following combustion reaction: • Example #7 - • C5H12 + O2 H2O + CO2 8 5 6

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