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Understanding Chemical Reactions: Types, Predictions, and Stoichiometry

This overview of chemical reactions explains how substances transform into new products through various types: synthesis, decomposition, single displacement, double displacement, neutralization, and combustion. It includes examples and balanced equations for each reaction type, along with insights on predicting products using the activity series. The document concludes with practical stoichiometry problems, emphasizing the relationship between reactants and products, highlighting the importance of mole ratios and the ability to calculate masses involved in chemical reactions.

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Understanding Chemical Reactions: Types, Predictions, and Stoichiometry

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  1. Test 4 Review

  2. Chemical Reaction • A process by which one or more substances are changed into one or more different substances. Reactants  Products

  3. Symbols NaHCO3(s) + HCl(aq) NaCl(aq) + H2O(l) + CO2(g) Yield sign (s) Solid (l) Liquid (g) Gas (aq) aqueous (dissolved in water)

  4. Complete the balanced equation • Nitrogen gas and oxygen gas react to produce dinitrogenpentoxide. • 2 N2(g) + 5 O2(g)  2 N2O5

  5. Potassium reacts with water to form potassium hydroxide and hydrogen gas. • 2 K + 2 H2O  2 KOH + H2(g)

  6. 6 Types of Reactions • Synthesis (Combination) • Decomposition • Single Displacement (Single Replacement) • Double Displacement (Double Replacement) • Neutralization • Combustion

  7. Synthesis • Also known as Combination • Two substances (usually elements) comvine to form a new compound. • A + B  AB • 2Ca(s) + O2(g)  2CaO(s)

  8. Decomposition • A compound breaks into its component parts • AB  A + B • 2NaCl  2Na(s) + Cl2(g)

  9. Single Displacement • Also known as Single Replacement • An element replaces an anion or a cation of a compound. • A + BC  B + AC • A + BC  C + BA • Mg(s) + H2SO4(aq)  MgSO4(aq) + H2(g)

  10. Double Displacement • Also known as Double Replacement • Cations from two compounds exchange partners • AB + CD  AD + CB • BaCl2(aq) + Na2SO4(aq)  BaSO4(g) 2 NaCl(g)

  11. Neutralization • An acid and a base react to form a salt and water. • Cation from base pairs with anion from acid to form a salt. • Hydroxide from base pairs with hydrogen from acid to form water. • This is also a Double Displacement (Replacement) • HX + YOH  H2O + YX • HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq)

  12. Combustion • Also known as oxidation • Oxygen is a reactant • Products always contain carbon dioxide and water • Typically produces heat • CxHyOz + O2 CO2 + H2O • CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)

  13. Practice problems • Will nickel replace hydrogen from water? • NO • Will lithium replace hydrogen from water? • YES • Will lead replace hydrogen from steam? • NO • Will magnesium replace hydrogen from steam? • YES • Will silver replace hydrogen from acids? • NO • Will sodium react with oxygen to form oxides? • YES

  14. Practice Problem • Will potassium replace zinc within a compound? • YES • Will lead replace aluminum within a compound? • NO • Will gold replace lithium within a compound? • NO • Will iron replace copper within a compound? • YES

  15. Predicting Products • Using what you know about types of reactions and the activity series, you can predict products for a reaction. • Ex: • Li + AgNO3 • Na + MgSO4  LiNO3 + Ag Mg + Na2SO4

  16. More practice • Barium chloride reacts with silver nitrate • Type of reaction: Double Displacement • BaCl2 + Cu(NO3)2 Ba(NO3)2 + CuCl2 • Aluminum oxide decomposes • Type of reaction: Decomposition • Al2O3 Al + O2 • 2 Al2O3 4 Al + 3 O2

  17. Soluble • If compounds are soluble, they have the ability to dissolve. • If they dissolve, they dissociate or “break apart” into their ions. • Ex: • NaCl Na+1 + Cl-1 • BaF2 Ba+2 + 2 F-1

  18. 2 AgNO3 + H2S  Ag2S + 2 HNO3 • Q: How many moles of Ag2S will be produced from 3.5 moles of AgNO3? • What happens if grams is involved? • Use Molar Mass! 1.75 mol Ag2S

  19. Q: How many grams of Ag2S will be produced from 3.5 moles of AgNO3? A balanced chemical equation tells the mole:mole ratio between different compounds in the equation.

  20. Tell-tale sign of Stoichiometry • If you are given information about one substance and asked about a different substance, it is a stoichiometry problem.

  21. Practice • What is the mass of Mg(OH)2 that will react with 1.20g of HCl? Mg(OH)2 + HCl MgCl2 + H2O 2 2 0.956g Mg(OH)2

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