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Classifying Chemical Reactions

Classifying Chemical Reactions. CP Chemistry. 5 Reaction Types. Composition / Synthesis/ Combination Decomposition Single Replacement (cationic or anionic) Double Replacement (or displacement) Combustion.

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Classifying Chemical Reactions

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  1. Classifying Chemical Reactions CP Chemistry

  2. 5 Reaction Types • Composition/ Synthesis/ Combination • Decomposition • Single Replacement (cationic or anionic) • Double Replacement (or displacement) • Combustion

  3. Synthesis reaction is a reaction in which two or more substances react to produce a single product.

  4. Composition/ Synthesis/ Combination • GENERAL FORMATS • A + B AB • Two single elements combine to make ONE PRODUCT

  5. Practice 1 • Write the balanced equation for the synthesis of sodium chloride salt from sodium metal and chlorine gas. • Solid silver(I) oxide can be produced from silver metal and oxygen gas. Write the balanced equation for this reaction.

  6. Practice 2 • Write the balanced equation for the synthesis of solid potassium chloride from potassium metal and chlorine gas. • Write the balanced equation for the synthesis of sulfur trioxide gas from solid sulfur and gaseous oxygen.

  7. Decomposition reaction = a single compound breaks down into two or more elements or compounds They often require an energy source (heat, light, or electricity) Ex: The decomposition of gold(III) oxide to its elements:

  8. Decomposition(Opposite of Composition) • GENERAL FORMATS • AB  A + B • SINGLE Reactant is identifying factor

  9. Practice 3 a. Write the balanced equation for the decomposition of chromium(III) oxide salt to gaseous oxygen and chromium metal. b. Write the balanced equation for the decomposition of mercury(II) oxide salt to solid mercury and oxygen gas.

  10. Single replacement reaction = one element replaces another element in a compound A + BX → AX + B Sodium replaces the silver ion in silver nitrate by the following reaction: Na(s) + AgNO3(aq)  NaNO3(aq) + Ag(s)

  11. The Activity Series Higher on the activity series = the more the metal wants to be in a compound! Use the activity to predict if a rxn will occur  the higher metal will always kick a lower metal out of a compound (replacing the lower metal)

  12. Single Replacement • To use activity series…. • Compare the metals in each compound (positive ions) • Higher metal ends up in compound • If already in the compound…NO REACTION will occur

  13. Practice 4 SR Example 1 Use the activity series to determine if the following reactions will occur and write the products if they do: a) Li(s) + AgNO3(aq)  react? b) Cu(s) + KNO3(aq)  react? c) Mg(s) + Zn(NO3)2(aq)  react? d) Au(s) + Ca(NO3)2(aq)  react?

  14. SR Example 1 Use the activity series to determine if the following reactions will occur: a) Li(s) + AgNO3(aq)  react? b) Cu(s) + KNO3(aq)  react? c) Mg(s) + Zn(NO3)2(aq)  react? d) Au(s) + Ca(NO3)2(aq)  react?

  15. Halogens • A higher halogen can replace a halogen that is below it in a compound • Activity increases up the group of halogens AX + Y  AY + X • Fluorine gas will react with sodium chloride salt…

  16. Practice 5 Use the activity series to determine if the following reactions will occur: • F2(g) + AgBr(aq)  • Br2(l) + KF(aq)  • I2(s) + ZnCl2(aq)  • Cl2(g) + CaI2(aq) 

  17. Combustion reaction (burning) = oxygen combines with another reactant and releases energy in the form of heat and light Whenever a hydrocarbon (a compound containing only C and H) combusted, the products are always CO2(g) and H2O(g).

  18. Combustion Reactions

  19. Practice 6 • Write the balanced equation for the combustion of gaseous ethane, C2H6. • Write the balanced equation for the combustion of solid sulfur to produce sulfur trioxide gas.

  20. Double replacement reactions = ions exchange between two compounds. Identify… Two compounds as reactants The metals will swap the cations…Does not matter who is stronger…They both swtich!

  21. Double Replacement • GENERAL FORMAT • AB + CD  AD + CB • Identifying Factor: Two compounds as reactant

  22. Double Replacement Precipitate = solid product produced during a chemical reaction All double replacement reactions produce water, a precipitate, or a gas.

  23. Reaction from Video

  24. Practice 7 The reaction between calcium nitrate and sodium hydroxide produces calcium hydroxide and sodium nitrate. • Write the complete balanced equation • Identify which reactant will be the precipitate.

  25. Practice 7 The reaction between calcium nitrate and sodium hydroxide produces calcium hydroxide and sodium nitrate. • Identify the precipitate

  26. Practice 8: Classify the following reactions

  27. Classify the following reactions

  28. Solubility: Solubility Rules

  29. Solutions • Solution = homogeneous mixtures of two or more pure substances. • Solute = the dissolved substance • seems to “disappear” • solvent = the substance solute dissolves in • does not appear to change state Tro's Introductory Chemistry, Chapter 13

  30. Aqueous Solutions • Aqueous Solution: one or more substances (solutes) are dissolved in water • Polar molecules & ionic compounds can dissolve in water • Dissociation: when ionic compounds dissolve in water they separate into ions NaCl(s) Na+(aq) + Cl-(aq)

  31. How Does a Solution Form? As a solution forms, the solvent pulls solute particles apart and surrounds, or solvates, them.

  32. Remember Conductivity?? Moving Ions = Carry Electricity

  33. Insoluble • Things that do NOT dissolve in water. • Examples: • Solid: Will precipitate or fall out of solution • Liquid: pure liquid like water or mercury • Gas: will bubble out of solution

  34. Which Compounds are Soluble?? • We have certain rules that help us determine which compounds are able to dissolve (dissociate) in water • It is also helpful to know which of the products will be the solid precipitate

  35. Solubility Rules • Solubility Rules help us determine whether or not a precipitate will form when two aqueous solutions are mixed • Soluble  (aq) • Insoluble  (s)

  36. Practice 9: Using the Solubility Rules Predict the states of matter in the equations below. • Zinc(II) acetate is mixed with sodium phosphate. The reaction produces zinc(II) phosphate and sodium acetate. • Write the equation for this reaction and balance it. • Add the states of matter for each compound based on the solubility rules

  37. Practice 10 Predict if the following ionic compounds are soluble or insoluble in water by writing their formula then (s) or (aq) after: • Ammonium nitrate • Nitric acid • Iron(III) sulfate • Silver bromide • Magnesium chloride

  38. Practice 11 Write the balanced equation for the reaction of aqueous lithium sulfate with aqueous lead(II) nitrate.

  39. Practice 13 Write the balanced equation when solutions of sodium hydroxide and copper(II) chloride are mixed.

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