1. Chemical Reactions and Equations Chapter 8

2. What does a chemical formula represent?  The elements contained in a chemical substance  Indicates the number of atoms of the element just to the right of the element symbol  a whole number that appears in front of a formula in a chemical equation. What is a subscript? What does it indicate? What is a coefficient?

3. Chemical Formulas 2 C 8 H 18 indicates there are 8 Carbon atoms in the molecule indicates there are 18 hydrogen atoms in the molecule Coefficient means 2 molecules

4. Visualizing Compounds Example: H 2 O H atoms = ________ O atoms = ________ Model of H 2 O: 2 1

5. What is a diatomic element?  An element with two atoms when it is by itself H 2 O 2 F 2 Br 2 I 2 N 2 Cl 2 Hydrogen Molecule Oxygen Molecule

6. DIATOMIC ELEMENTS You can also mark them off on your periodic table as the SUPER SEVEN!

7. Chemical Reaction  When bonds are broken and new bonds are formed producing a new substance Chemical Equation Symbolizes or represents a chemical reaction

8. Reactants Original substances in a chemical reaction Products Substances formed in a chemical reaction REACTANTS yields PRODUCTS

9. H 2 + O 2  H 2 O Igniting a mixture of hydrogen and oxygen will form water. The symbol equation is: ReactantsProduct

10. How does a chemical reaction occur?  Atoms must collide for the reaction to occur  Atoms are rearranged in a chemical change - None are lost - None are gained

11. any reaction that gives off heat Example: 2H 2 (g) + O 2 (g) 2H 2 O (l) + heat Exothermic Reaction

12. Endothermic Reaction any reaction in which heat is added Example: heat + 2HgO (s) 2Hg (l) + O 2 (g)

13. Evidence of a Chemical Change 1. Color change (THAT YOU DID NOT CAUSE!!) 2. Temperature change 3. Odor change 4. Formation of a gas 5. Formation of a precipitate  precipitate: insoluble solid that separates out of solution

14. Balancing Chemical Equations Notes

15. A Chemical Reaction Potassium Iodide [KI] Lead Nitrate [Pb(NO 3 ) 2 ] Final Product

16. Did a chemical change occur? How do you know? Is matter conserved in this reaction?

17. According to the LAW OF CONSERVATION OF MATTER: the total atoms of reactants must equal the total atoms of products [matter can’t be created or destroyed!] When you have a chemical reaction, you must add coefficients to balance the reaction!

18. Atom Inventory __H 2 + __O 2  __H 2 O Reactant SideProduct Side Atom TypeNumber of Atoms Atom TypeNumber of Atoms HH OO 2 2 2 1 UNBALANCED !

19. To balance an equation, coefficients CAN be added in front of products or reactants. DO NOT CHANGE SUBSCRIPTS!

20. New Atom Inventory __H 2 + __O 2  __H 2 O Reactant SideProduct Side Atom TypeNumber of Atoms Atom TypeNumber of Atoms HH OO 4 2 2 2 2 UNBALANCED !

21. New Atom Inventory __H 2 + __O 2  __H 2 O Reactant SideProduct Side Atom TypeNumber of Atoms Atom TypeNumber of Atoms HH OO 2 4 2 2 2 4 BALANCED!

22. Balancing Equations ___ Mg + ___ N 2 ---> ___ Mg 3 N 2 ___ H 2 S + ___ Cl 2 ---> ___ S 8 + ___ HCl ___ Al + ___ HCl ---> ___ AlCl 3 + ___ H 2 ___ Fe 2 O 3 + ___ CO ---> ___ Fe + ___ CO 2

23. Classifying Chemical Reactions

24. Two or more reactants combine to form ONE product. (marriage) example: 2Mg (s) + O 2 (g) 2MgO (s) A + X AX Synthesis

25. ONE reactant breaks down into smaller parts. (divorce) AX A + X Decomposition example: 2H 2 O (l)  2H 2 (g) + O 2 (g)

26. A single element replaces an element that is part of a compound. example: 2 Al (s) + 3 Fe(NO 3 ) 2(aq) 3 Fe (s) + 2 Al(NO 3 ) 3(aq) A + BX B + AX Y + BX X + BY Single Displacement

27. Ions from two different compounds exchange places to form two new compounds. (wife swap) AX + BY AY + BX 2KI (aq) + Pb(NO 3 ) 2 (aq) PbI 2 (s) + 2KNO 3 (aq) Double Displacement

28. A compound (usually a hydrocarbon) reacts with oxygen, releasing carbon dioxide and water. example: combustion of propane C 3 H 8 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O (g) AB + O 2 CO 2 + H 2 O Combustion

29. Activity Series  What is the activity series?  When elements are ranked in order of their relative reactivities

30. Activity Series of the Elements

31. 1.Why is sodium not used for silverware? It is highly reactive and reacts with water.

32. It is unreactive with oxygen or water and therefore does not readily break down.

33. 3. Why is food canned in containers made from steel coated with a thin layer of tin? Steel makes a strong container and the tin lining does not react with the contents.

34. 4. Why are cars painted? To prevent the iron from rusting by being exposed to oxygen in air.

35. Writing Chemical Reactions Notes

36. word equation: equation in which the reactants and products in a chemical reaction are represented by words a word equation is qualitative example: methane + oxygen carbon dioxide + water Word Equations

37. formula equation: represents the reactants and products of a chemical reaction by their symbols or formulas a formula equation is quantitative example: CH 4(g) + 2O 2(g) CO 2(g) + 2H 2 O (g) Formula Equations

38. Symbols in a Chemical Reaction

39. Writing Chemical Reactions  Steps to writing a reaction: 1. Balance the equation. 2. Fill in the phases of matter. 3. Identify the reaction type.

40. Example 1 Aluminum metal reacts with a solution of hydrochloric acid to produce hydrogen gas and aluminum chloride solution.

41. Example 2 Magnesium metal burns in oxygen gas to produce solid magnesium oxide.

42. Example 3 Hydrogen peroxide (H 2 O 2 ) solution breaks down to produce oxygen gas and liquid water in the presence of the catalyst “catalase”.

43. Example 4 Iron (III) Chloride solution and sodium hydroxide solution react to produce solid iron (III) hydroxide and sodium chloride solution.

44. Example 5 A piece of zinc metal is placed in copper (II) nitrate solution producing copper metal and zinc nitrate solution.

45. Example 6 Copper (II) sulfate solution and sodium hydroxide solution react to produce solid copper (II) hydroxide and sodium sulfate solution.