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Types of Chemical Reactions: Synthesis, Decomposition, Single-Displacement, Double-Displacement, and Combustion

Learn about the different types of chemical reactions including synthesis, decomposition, single-displacement, double-displacement, and combustion. Understand the characteristics and equations for each type and how to balance chemical equations.

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Types of Chemical Reactions: Synthesis, Decomposition, Single-Displacement, Double-Displacement, and Combustion

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  1. Chapter 8 Notes Types of Chemical Reactions p.261 - 284

  2. 8.1 Chemical Reactions (p.261-269) • Starting on p.261 at the top, find the definitions for the following: • Chemical reaction, Reactant, Product • Chemical reactions are written like this: Reactant Product • p. 261, write the 4indications of a chemicalreaction (only the italicized section) • p.262, write the 3characteristics of a chemical equation (only the italicized section) • p. 263, copy down Table 1 (7 diatomic molecules) • What is the difference between a word equation and a formula equation? • How does the law of conservation of mass apply to chemical reactions? • What does the term yield mean in the context of chemical reactions? • p.266, Copy down the following 7 symbols from the chart • Yields, reversible reaction, (s), (l), (aq), (g), and heated • p.269, copy down the italicized portion of number 2.

  3. 8.1 section review • Complete questions 1 - 3

  4. 8.2 Types of Chemical Reactions • Synthesis (or Composition) reactions • Decomposition reactions • Single-displacement reactions • Double-displacement reactions Acid/Base reactions: Acid + Base  salt + water • Combustion reactions

  5. 1. Synthesis Reactions • aka: composition or addition • What happens: two or more substances combine to form a new compound • General Equation: A+X  AX • Example: Zn + O  ZnO • Specific examples – p.278-9 Synthesis Reactions with Oxides

  6. 2. Decomposition Reactions • What Happens: a compound is broken down in a reaction which makes two or more simpler compounds • Key words to indicate decomposition: • Electrolysis, heated, • General Equation: AXA+X • Example:CaCO3 CaO + CO2 • Specific examples – p.280 Metal Carbonates, Metal Hydroxides, and Metal Chlorates

  7. 3. Single-Displacement Reactions • AKA: Single-replacement • What happens: one element replaces a similar element in a compound • General equation: AX+B BX + A • Example:Zn + 2 HCl  ZnCl2 + H2 • According to the activity series, only a more reactive metal or nonmetal will replace a cation or anion in a compound. • There are several versions of an activity series, we will use the one on p.286 in your textbook. • Practice p.287 #1-3, then section review #2-3 on your own.

  8. 4. Double-Displacement reactions • AKA:double-replacement • What Happens: ions from two compounds change places to produce two new compounds • General Eq: AX + BY  AY + BX • Ex:HCl + NaOH  H2O + NaCl • Formation of a precipitate p.282 • Formation of water in acid/base reactions.

  9. 5. Combustion Reactions • aka: burning • What Happens: reaction of oxygen gas (O2), which releases heat and light • Production of water p.283 • General: CXHY + O2 H2O + CO2 • Example: CH4 + 2 O2 CO2 + 2 H2O

  10. How can you tell which type of reaction? • Composition: 2 elements (only 1 product) • Decomposition: 1 reactant (2+ products) • Single-displacement:1 element and 1 compound • Double-displacement: 2 compounds • Combustion:CXHY and O2

  11. Balancing Chemical Equations (8.1) • What is a Balanced Equation? • same number of each type of atom on both sides of the equation • This equation isNOT balanced: N2 + H2 NH3 N = 2 N = 1 H = 2 H = 3 • This equation IS balanced: N2 + 3 H2 2 NH3 N = 2 N = 2 H = 6 H = 6

  12. Steps to balance an equation: • Write the chemical reaction: Mg + O2 MgO • Count how many of each type of atom are on the reactant side and the product side Mg + O2 MgO Mg = 1 Mg = 1 O = 2 O = 1

  13. Steps to balance an equation: • Add coefficients to balance the equation • Remember, you can only add coefficients, you can’t change subscripts! 2 Mg + O2 2 MgO Mg = 1x2= 2 Mg = 1x2= 2 O = 2 O = 1x2= 2

  14. H2SO4 + Mg  MgSO4 + H2 H = 2 H = 2 SO4= 1 SO4= 1 Mg = 1 Mg = 1 Note: polyatomic ions are a single item in your inventory – DO NOT separate them into individual elements Polyatomic Ions

  15. Practice Na + Br2  NaBr Al(NO3)3 + Li LiNO3 + Al C3H8 + O2 CO2 + H2O

  16. Summing it up • Practice p.272 (#1ab, 2) • Practice p.274 (#1abc)

  17. Predicting Products of Reactions • Step 1: Identify reaction type • Step 2: Label cations and anions on the reactant side. • Step 3: Determine how cations and anions will recombine on the product side. • Step 4: Consult activity series to determine if reaction will occur. • Step 5:Cross charges on any compounds and determine if anything is diatomic.

  18. Examples • Ex1: Na + Cl _______ • Ex2: H2 + O2

  19. Examples • Ex1: MgBr2 ______ + ______ • Ex2: CaCO3 ______ + ______

  20. Examples • Ex1: Li + SrO ______ + ______ • Ex2: KOH + Ba ______ + ______

  21. Examples • Ex1: AgNO3 + BeCl2 • Ex2: FePO4 + ZnS

  22. Examples • Ex1: C2H6 + O2 CO2 + H2O • Ex2: C6H12O6 + O2

  23. 8.2 section review p. 284 (1-4)

  24. Activity Series of the Elements Section 8.3 Pages 285-287

  25. Activity Series An activity series organizes elements by how easily they react, or how active they are in a chemical reaction. Metals: easier loss of electrons Nonmetals: easier gain of electrons ONLY MATTERS IN SINGLE and DOUBLE DISPLACEMENT!

  26. Rules • There is only one rule – an element will replace (or displace) another element only if the second element is below it on the chart. • Ex: Lithium is at the top of the chart, so it will displace any metal in a compound that it is reacting with. • Complete the activity series worksheet (front side only)

  27. Solubility in chemical reactions • How does one know what state of matter a compound is in? How does one know if a precipitate is formed or not? • Use the solubility guidelines chart to determine if a compound is soluble (aqueous, or dissolved in solution) or insoluble (solid, or forms a precipitate) • Complete the worksheet on the back

  28. Homework • Complete both sides of the worksheet titled “Double Displacement Reactions”. • Use your activity series and solubility chart to determine: if a reaction will occur and if any precipitates are formed. • If the reaction will occur, write the products formed. If not, write no reaction.

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