1. Chapter 8 Chemical Reactions

2. I. Nature of Chemical Reactions  reactant – substance(s) that enters a reaction, on the left of a chemical equation  product – substance(s) produced by a reaction, on the right of a chemical equation  KI + Pb(NO 3 ) 2 ---> PbI 2 + KNO 3  Looking at the reaction here... –What are the reactants? –What are the products? –…and the blast from the past…. What is wrong with it?

3. II. Balancing Chemical Equations  Chemical reactions are described by chemical equations which must be balanced  A balanced equation has the same # of atoms of each element on each side of the arrow! –C + O 2 --> CO 2 –2H 2 + O 2 --> 2H 2 O

4. II. Balancing Chemical Equations  Matter can neither be created nor destroyed  We know that a chemical reaction must have the same amount of material after as it had before because of the conservation of mass  Def – the observation that mass remains constant in a chemical reaction is known as the conservation of mass

5. II. Balancing Chemical Equations  To balance a chemical equation: –Do an atom count. Count each element’s atoms on each side of the equation. WRITE THE ELEMENTS IN THE SAME ORDER ON BOTH SIDES!!! –Check to see if it’s already balanced. If it is, stop. –If not, find the most complicated compound. –Starting w/that compound, go element by element through that side of the equation, balancing each element by adding coefficients (“playing tennis”). –If an element is repeated more than once on one side of an arrow, save it for last.

6. II. Balancing Chemical Equations  Balance the following:  Na + MgF 2 --> NaF + Mg  N + O 2 --> NO 2  KCl + Pb(NO 3 ) 2 --> KNO 3 + PbCl 2

7. II. Balancing Chemical Equations  Balance the following:  2 Na + MgF 2 --> 2NaF + Mg  N + O 2 --> NO 2 BALANCED!!!  2KCl + Pb(NO 3 ) 2 --> 2KNO 3 + PbCl 2

8. Balance These! Mg + HCl --> MgCl 2 + H 2 N 2 + H 2 --> NH 3 H 2 O 2 --> H 2 O + O 2 Al + O 2 --> Al 2 O 3 HCl + NaOH --> NaCl + H 2 0 KClO 3 --> KCl + O 2 Al + NiBr 2 --> AlBr 3 + Ni CaSO 4 + AlBr 3 --> CaBr 2 + Al 2 (SO 4 ) 3

9. Balance These!  Mg + 2HCl --> MgCl 2 + H 2  N 2 + 3H 2 --> 2NH 3  2H 2 O 2 --> 2H 2 O + O 2  4Al + 3O 2 --> 2Al 2 O 3  HCl + NaOH --> NaCl + H 2 0  2KClO 3 --> 2KCl + 3O 2  2Al + 3NiBr 2 --> 2AlBr 3 + 3Ni  3CaSO 4 + 2AlBr 3 --> 3CaBr 2 + Al 2 (SO 4 ) 3

10. III. Types of Chemical Reactions  Synthesis Reaction - 2 or more simple substances coming together to form a new, more complex one –2Na + Cl 2 ---> 2NaCl –the Na and Cl came together to form NaCl –It’s kind of like two people getting married  Britney Spears married K-Fed  Britney Spears married K-Fed

11. III. Types of Chemical Reactions  Decomposition reaction - complex substance being broken down into 2 or more simpler ones –H 2 CO 3 ---> H 2 0 + CO 2 –the complex H 2 CO 3 broke up into the simpler H 2 0 and CO 2 –It’s kind of like 2 people getting a divorce  Britney and K-Fed split up 

12. III. Types of Chemical Reactions  Single-Replacement Reaction - an uncombined element replaces another element in a compound –2Na + 2H 2 0 ---> 2NaOH + H 2 –if you look, you’ll see that Na kicked the H out of water to form NaOH--it replaced it –It’s kind of like when one person breaks up with someone to go out with someone else.  Brad Pitt left Jennifer Aniston for Angelina Jolie

13. III. Types of Chemical Reactions  Double-Replacement Reaction - different atoms in 2 different compounds replace each other –2KCl + Pb(NO 3 ) 2 ---> 2KNO 3 + PbCl 2 –the K and Pb each switched partners! –the K had Cl, but it traded Cl for NO 3 –the Pb had NO 3, but it traded NO 3 for Cl –It’s kind of like if…  Jessica Simpson & Nick Lachey and Britney Spears & K-Fed decided that it would be better if Jessica was with K-Fed and Britney was with Nick

14. Balance and Classify: AlBr 3 + Ni ---> Al + NiBr 2 AlBr 3 + Ni ---> Al + NiBr 2 Al + O 2 ---> Al 2 O 3 Al + O 2 ---> Al 2 O 3 KCl + O 2 ---> KClO 3 KCl + O 2 ---> KClO 3 NaCl + H 2 0 ---> HCl + NaOH NaCl + H 2 0 ---> HCl + NaOH (NH 4 ) 2 SO 4 + Ba(NO 3 ) 2 ---> BaSO 4 + NH 4 NO 3 (NH 4 ) 2 SO 4 + Ba(NO 3 ) 2 ---> BaSO 4 + NH 4 NO 3 MgCl 2 + H 2 ---> Mg + HCl MgCl 2 + H 2 ---> Mg + HCl H 2 + O 2 ---> H 2 0 H 2 + O 2 ---> H 2 0 NaCl ---> Na + Cl 2 NaCl ---> Na + Cl 2 CaCl 2 + F 2 ---> CaF 2 + Cl 2 CaCl 2 + F 2 ---> CaF 2 + Cl 2 AgCl + KNO 3 ---> AgNO 3 + KCl AgCl + KNO 3 ---> AgNO 3 + KCl

15. Balance and Classify: 2AlBr 3 + 3Ni ---> 2Al + 3NiBr 2 4Al + 3O 2 ---> 2Al 2 O 3 2KCl + 3O 2 ---> 2KClO 3 NaCl + H 2 0 ---> HCl + NaOH (NH 4 ) 2 SO 4 + Ba(NO 3 ) 2 ---> BaSO 4 + 2NH 4 NO 3 MgCl 2 + H 2 ---> Mg + 2HCl 2H 2 + O 2 ---> 2H 2 0 2NaCl ---> 2Na + Cl 2 CaCl 2 + F 2 ---> CaF 2 + Cl 2 AgCl + KNO 3 ---> AgNO 3 + KCl

16. IV. Energy of Chemical Reactions  Exothermic Reactions - reactions that release energy –reactants have more energy than products –the energy released is often heat –CH 4 + 2O 2 ---> CO 2 + 2H 2 0 + energy  Endothermic Reactions - reactions in which energy is absorbed –products have more energy than reactants –2NaCl + energy ---> 2Na + Cl 2 Exothermic or Endothermic?

17. IV. Energy of Chemical Reactions  Activation Energy - energy required to “jump start” a reaction, it’s the hill on an energy diagram

18. Classify these as Exothermic or Endothermic  energy is released  reactants have more energy than the products  energy is a reactant  an explosion  the reaction’s beaker cools  products have more energy than the reactants  reactants have less energy than the products

19. V. Rates of Chemical Reactions  Reaction rate - how quickly reactants turn to products  Collision theory - molecules react when they collide (like bumper cars!)

20. V. Rates of Chemical Reactions  to make a reaction go faster, cause more collisions! –increase the concentration - the more molecules there are, the more collisions there are –increase the surface area - if you powder the reactants, then there are more molecules exposed on the surface rather than trapped inside a lump –increase the temp. - causes molecules to move faster, thus there are more collisions –add a catalyst - a catalyst is a chemical that lowers the activation energy (the hill on the energy diagram)

21. Fill in these graphs! concentration rxn rate temperature particle size rxn rate am’t of catalyst rxn rate

22. Fill in these graphs! concentration rxn rate temperature particle size rxn rate am’t of catalyst rxn rate

23. Fill in these graphs! concentration rxn rate temperature particle size rxn rate am’t of catalyst rxn rate

24. Fill in these graphs! concentration rxn rate temperature particle size rxn rate am’t of catalyst rxn rate

25. Fill in these graphs! concentration rxn rate temperature particle size rxn rate am’t of catalyst rxn rate