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Chapter 10

Chapter 10. Chemical Reactions. Must Know. Diatomic molecules H 2 N 2 O 2 F 2 Cl 2 Br 2 I 2 Common Allotropes P 4 S 8. State of Element or Compound. Aqueous ( aq ) Dissolved in water Solid (s). Gas (g) Liquid (l). Writing Chemical Equation s.

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Chapter 10

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  1. Chapter 10 Chemical Reactions

  2. Must Know • Diatomic molecules • H2 • N2 • O2 • F2 • Cl2 • Br2 • I2 • Common Allotropes • P4 • S8

  3. State of Element or Compound • Aqueous • (aq) • Dissolved in water • Solid • (s) • Gas • (g) • Liquid • (l)

  4. Writing Chemical Equations • You will have word problems that you must write the skeleton equation for. • Be able to write formulas for ionic compounds, covalent compounds, acids, and bases. • You should know how to balance equations • Must be organized • Do it exactly how I do it

  5. Examples • ___KClO3 ___KCl + ___O2 • Pg 282 #4 - 6

  6. Types of Chemical Reactions • Synthesis reactions • A + B  AB • 2K + Br2  2KBr • Decomposition Reactions • AB  A + B • Ni(OH)2  NiO + H2O

  7. Combustion Reactions • Always contains oxygen • Oxygen combines with another substance to release huge amounts of energy and/or light • Usually have to put energy in in order to initiate the reaction. Get huge gains of energy out of the reaction. • Usually occurs with a hydrocarbon. • CxHy • Gasoline is a hydrocarbon • When a hydrocarbon is completely combusted your products will always be CO2 + H2O. • Example: __C2H6 + __O2 __CO2 + __H2O • You balance

  8. Replacement Reactions • 2 Types • Single Replacement Reactions • A + CB  AB + C • Determined by reactivity • Use the reactivity chart • If element A is more reactive than element C then the reaction will occur. If it is not then N.R. • __K + __ZnCl2  __KCl + __Zn (You balance)

  9. Single Replacement Reactions Practice • Determine if the reaction will occur and balance the equations. • RbI(aq) + F2(g)  • Fe + Na3PO4 

  10. Double Replacement Reactions • AB + CD  AD + CB • 2NaOH + CuCl2  2NaCl + Cu(OH)2 • Double Replacement Reactions forms • A solid (precipitate) • A liquid (H2O) • A gas

  11. Prediction Sheet Examples • CaCO3 CaO + CO2 • 2Na + 2H2O  2NaOH + H2 • SrO + H2O  Sr(OH)2 • Ba(OH)2  BaO + H2O • 2KClO3  2KCl + 3O2 • C6H8 + 8O2  6CO2 + 4H2O

  12. Terminology to Know • Soluble • Dissolves in a solution • Dissociate • Comes apart

  13. Rules for forming a precipitate in double replacement reactions • Solubility rules • Strong acids dissociate in water • HCl, HBr, HI, H2SO4, HNO3, HClO4, HClO3 • Example: HClO3 H+ and ClO3- • Strong bases dissociate in water • LiOH, NaOH, KOH, RbOH, CsOH • Example: LiOH Li+ and OH-

  14. Soluble Salt Rules • Ionic compounds (metal/nonmetal) • The anion of an acid and a cation of a strong base • Soluble salts dissociate

  15. Soluble Salt Rules Always soluble in a cpd. Exceptions None Ag, Pb, Hg22+ Ag, Pb, Hg22+, Ca, Sr, Ba • Group 1 metals, NH4, NO3, ClO4, ClO3, C2H3O2 • Cl-, Br-, I- • SO42-

  16. If the salt falls under one of the exceptions then it is insoluble and forms a precipitate. • Examples • NaCl – Rule 1. Soluble. • Fe(C2H3O2)2 – Rule 1. Soluble. • ZnCl2 – Rule 2. Soluble. • AgBr – Rule 2. Insoluble (forms precipitate) • MgSO4 – Rule 3. Soluble. • CaSO4 – Rule 3. Insoluble (forms precipitate)

  17. Remember that in a double replacement reaction 1 of 3 things must form or the reaction does not occur. At this point we have only looked at formation of precipitates. • Pg. 294 #33 • Will this happen? • Write the balanced chemical equation, complete ionic equation, and net ionic equation. You will be required to write all 3.

  18. D.R.R. Practice Problems (precipitate) • Determine if the reaction will occur. If the reaction occurs write the balanced chemical equation, complete ionic equation, and the net ionic equation. • Aqueous solutions of ammonium phosphate and sodium sulfate are mixed. • Aqueous solutions of lithium sulfate and calcium nitrate are mixed.

  19. Acid Base Reactions • Water forming • 1 of the 3 things that must happen in a double replacement reaction. • HCl(aq) + KOH(aq)  H2O(l) + KCl(aq) • Write the complete ionic equation and net ionic equation. • Diprodic reactions • Contains 2 hydrogen; also water forming • H2SO4(aq) + 2KOH(aq)  2H2O(l) + K2SO4(aq)

  20. Acid Base Reactions Practice Problem (liquid) • Pg. 296 # 40

  21. Production of gases • Final result used to determine double replacement reactions • Acid + carbonate (CO32-)  CO2(g) + H2O + ions • Acid + cyanide (CN-) HCN(g) + ions • Acid + sulfide (S2-)  H2S(g) + ions • Example: • 2HClO4(aq) + K2CO3(aq)  CO2(g) + H2O(l) + 2KClO4(aq)

  22. D.R.R. Practice Problems (gas) • Pg. 299 # 44

  23. Homework • Pg. 305 86-94

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