1 / 23

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.

tyanne
Télécharger la présentation

Chapter 10

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related