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Understanding Chemical Reactions: Types and Equations

This chapter covers the fundamentals of chemical reactions, explaining what they are and how they are represented through chemical equations. It introduces key concepts such as reactants and products, the use of subscripts and coefficients, and the symbols indicating the states of matter. The chapter also outlines the five main types of chemical reactions: combination, decomposition, single replacement, double replacement, and combustion. Each type is defined and exemplified, ensuring a thorough understanding of the fundamental reactions that govern chemical processes.

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Understanding Chemical Reactions: Types and Equations

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  1. Chapter 8 Notes, Part I Parts of an equation Types of reactions

  2. What is a chemical reaction? • A chemical reaction is the act of changing substances into new substances with new and different chemical and physical properties.

  3. A Chemical Equation • A chemical equation shows what is going on in a chemical reaction. • Instead of writing down the entire sentence “hydrogen reacts with oxygen to form dihydrogen monoxide (water)”, you could write…

  4. reactants The substances you have before a chemical reaction occurs (found on the left side of the equation) products The substances you have after a chemical reaction occurs (found on the right side of the equation) 2H2 + O2a2H2O

  5. subscripts How many elements are in a compound coefficients How many substances are in the reaction 2H2 + O2a2H2O

  6. 2H2 + O2a2H2O The arrow reads as “produces”, “yields” or “reacts to form”

  7. Iron reacts with oxygen gas to produce iron (III) oxide 4Fe + 3O2a2Fe2O3

  8. Other symbols in an Equation • (s) = substance is solid • (l) = substance is liquid • (g) = substance is a gas • (aq) = substance is dissolved in water • D = heat

  9. Other symbols in an Equation • (A formula written above or below an arrow means it is a catalyst (a substance that speeds up a reaction without being used up by it.)

  10. What is: • The name of something that speeds a reaction, but is not used up? • The name of what you have before a reaction takes place? • The symbol for heat? • The number that shows there are more than one of the entire compound?

  11. Types of reactions • There are five types of reactions • Combination • Decomposition • Single replacement • Double replacement • Combustion

  12. Combination Reaction • A combination reaction occurs when two or more elements or compounds combine to form a single substance. • It will follow the form A + B a AB • Example: Fe + S aFeS

  13. Decomposition Reaction • A decomposition reaction occurs when one substance breaks down into two or more substances. • It will follow the pattern AB a A + B • Example: CaCO3aCaO+CO2

  14. Single Replacement Reaction • One element replaces another element in a compound. • Generally follows the formula: AB + C a A + BC • Example: Mg+Zn(NO3)2aZn+Mg(NO3)2

  15. Double Replacement Reaction • The exchange of two positive ions between two reacting compounds, forming two new compounds as a product. • Generally follows the formula: AB + CD a AD + CB • Example: Na2S+Cd(NO3)2aCdS+2NaNO3

  16. Combustion Reaction • A compound reacts with oxygen to producing energy as heat and light. • Most of the time, it is a hydrocarbon reacting with oxygen, and the outcome is always carbon dioxide and water • Follows the form: A + O2a CO2 + H2O • Example: CH4 + O2a CO2 + 2H2O

  17. What type of reaction is: • NaCN + H2SO4a 2HCN + Na2SO4 • Zn + 2HCl a ZnCl2 + H2 • 2C2H6 + 7O2a 4CO2 + 6H2O • 2H2 + O2a 2H2O

  18. ON THE WHITEBOARDS: • Tell which of the five types of reactions the following are:

  19. 2Na + 2H2O a 2NaOH + H2 Single replacement

  20. Fe + S a FeS combination

  21. Al(OH)3 + 3NaCl aAlCl3 + 3NaOH Double replacement

  22. CH4 + 2O2a CO2 + 2H2O combustion

  23. KClO2a KCl + O2 decomposition

  24. NaOH + HCl a NaCl + H2O Double replacement

  25. 4Fe + 3O2a 2Fe2O3 combination

  26. 2C2H2 + 5O2a 4CO2 + 2H2O combustion

  27. H2 + Cl2a 2HCl combination

  28. MgO + 2KF a MgF2 + K2O Double replacement

  29. Na + Al(NO3)3aNaNO3 + Al Single replacement

  30. 2PbO2a 2PbO + 3O2 decomposition

  31. Ba(CN)2 + H2SO4a BaSO4 + HCN Double replacement

  32. C3H8 + 5O2a 3CO2 + 4H2O combustion

  33. 4Li + O2a 2Li2O combination

  34. 2Ag + 2HCl a 2AgCl + H2 Single replacement

  35. 2H2O2a 2H2O + O2 decomposition

  36. C2H2 + O2a CO2 + H2O combustion

  37. 2HBr a H2 + Br2 decomposition

  38. CrSO4 + 2AgNO3a Cr(NO3)2 + Ag2SO4 Double replacement

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