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Understanding Chemical Reactions: Types and Equations Explained

This chapter provides an overview of chemical reactions, highlighting the process of transforming substances into new ones with distinct chemical and physical properties. It explains the structure of chemical equations, including reactants and products, and discusses the significance of subscripts and coefficients. The chapter categorizes reactions into five types: synthesis, decomposition, single replacement, double replacement, and combustion, accompanied by examples for clarity. Additionally, it includes symbols used in equations to denote states of matter and catalysts, enriching the understanding of chemical reactions.

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Understanding Chemical Reactions: Types and Equations Explained

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  1. Chapter 10 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 atoms of an element 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. Word Equation • This indicates the reactants and products of chemical reactions. reactant 1 + reactant 2 → product 1 iron (s) + chlorine (g) → iron(III) chloride (s) This reads: “Iron and chlorine react to produce iron(III) chloride.”

  8. Skeleton Equation • Uses chemical formulas instead of words to identify your reactants and products. Word: iron (s) + chlorine (g) → iron(III) chloride (s) Skeleton: Fe (s) + Cl2 (g) → FeCl3 (s)

  9. Chemical Equation • A skeleton equation that shows that the number of atoms of each reactant and each product is equal on both sides of the arrow, also called balanced. Word: iron (s) + chlorine (g) → iron(III) chloride (s) Skeleton: Fe (s) + Cl2 (g) → FeCl3 (s) Chemical: 2Fe (s) + 3Cl2 (g) → 2 FeCl3

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

  11. 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 • 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.)

  12. 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?

  13. Types of reactions • There are five types of reactions • Synthesis • Decomposition • Single replacement • Double replacement • Combustion

  14. Synthesis Reaction • A synthesis 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

  15. 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

  16. 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

  17. 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

  18. 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

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

  20. Tell which of the five types of reactions the following are:

  21. 2Na + 2H2O a 2NaOH + H2 Single replacement

  22. Fe + S a FeS combination

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

  24. CH4 + 2O2a CO2 + 2H2O combustion

  25. KClO2a KCl + O2 decomposition

  26. NaOH + HCl a NaCl + H2O Double replacement

  27. 4Fe + 3O2a 2Fe2O3 combination

  28. 2C2H2 + 5O2a 4CO2 + 2H2O combustion

  29. H2 + Cl2a 2HCl combination

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

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

  32. 2PbO2a 2PbO + 3O2 decomposition

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

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

  35. 4Li + O2a 2Li2O combination

  36. 2Ag + 2HCl a 2AgCl + H2 Single replacement

  37. 2H2O2a 2H2O + O2 decomposition

  38. C2H2 + O2a CO2 + H2O combustion

  39. 2HBr a H2 + Br2 decomposition

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

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