1. Chemical Equations synthesis decomposition combustion of a hydrocarbon single replacement double replacement

2. Parts of a chemical equation

3. Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)

4. Parts of a chemical equation Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)

5. Parts of a chemical equation Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)

6. Parts of a chemical equation Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)

7. Parts of a chemical equation Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)

8. Parts of a chemical equation Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)

9. Parts of a chemical equation Mg(s) + 2 HCl(aq)  H 2 (g) + MgCl 2 (aq)

10. In a chemical reaction, existing atoms are simply rearranged. The atoms on both sides of the equation must balance. N 2 + H 2  NH 3 (not balanced)

11. In a chemical reaction, existing atoms are simply rearranged. The atoms on both sides of the equation must balance. N 2 + 3 H 2  2 NH 3 (balanced)

12. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. Example: CO 2 + H 2  C 2 H 6 + H 2 O

13. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. Example: CO 2 + H 2  C 2 H 6 + H 2 O Balance the carbons and oxygens first.

14. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. Example: 2 CO 2 + H 2  C 2 H 6 + 4 H 2 O Balance the carbons and oxygens first.

15. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. Example: 2 CO 2 + 7 H 2  C 2 H 6 + 4 H 2 O Finally, balance the hydrogens.

16. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. 2.When the same polyatomic ion is present on both sides of an equation, balance the entire ion rather than the individual elements. Example: CaCl 2 + AgNO 3  Ca(NO 3 ) 2 + AgCl

17. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. 2.When the same polyatomic ion is present on both sides of an equation, balance the entire ion rather than the individual elements. Example: CaCl 2 + 2 AgNO 3  Ca(NO 3 ) 2 + AgCl The nitrate ions can be balanced as if they are a single element.

18. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. 2.When the same polyatomic ion is present on both sides of an equation, balance the entire ion rather than the individual elements. Example: CaCl 2 + 2 AgNO 3  Ca(NO 3 ) 2 + 2 AgCl Balance the Ca, Cl, and Ag to complete.

19. Tips for balancing reactions. 1.Start by balancing elements that are only found once on each side of the reaction. 2.When the same polyatomic ion is present on both sides of an equation, balance the entire ion rather than the individual elements. 3.When balancing combustion reactions for hydrocarbons, always start with a 2 in front of the hydrocarbon (more on this later).

20. Synthesis Reactions (A + B  AB) Two or more substances combine to form a larger compound.

21. Synthesis Reactions (A + B  AB) Two or more substances combine to form a larger compound. Example: 2 H 2 (g) + O 2 (g)  2 H 2 O(l)

22. Synthesis Reactions (A + B  AB) Two or more substances combine to form a larger compound. Example: 2 H 2 (g) + O 2 (g)  2 H 2 O(l) Example: MgO(s) + CO 2 (g)  MgCO 3 (s)

23. Decomposition (AB  A + B) A single compound breaks down into two or more smaller substances.

24. Decomposition (AB  A + B) A single compound breaks down into two or more smaller substances. Example: 2 NaHCO 3 (s)  CO 2 (g) + H 2 O(g) + Na 2 CO 3 (s)

25. Combustion of a hydrocarbon (C x H y O z + O 2  CO 2 + H 2 O) Any hydrocarbon that burns in the presence of oxygen will produce carbon dioxide and water vapor.

26. Combustion of a hydrocarbon (C x H y O z + O 2  CO 2 + H 2 O) Any hydrocarbon that burns in the presence of oxygen will produce carbon dioxide and water vapor. Balance by giving the hydrocarbon a coefficient of 2, then balance C, H, and then O. Check to see if the coefficients can be simplified.

27. Combustion of a hydrocarbon (C x H Y O z + O 2  CO 2 + H 2 O) Any hydrocarbon that burns in the presence of oxygen will produce carbon dioxide and water vapor. Balance by giving the hydrocarbon a coefficient of 2, then balance C, H, and then O. Check to see if the coefficients can be simplified. Example: C 3 H 8 (g) + 5 O 2 (g)  3 CO 2 (g) + 4 H 2 O(g)

28. Chemical Equations synthesis decomposition combustion of a hydrocarbon single replacement double replacement

29. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound.

30. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound. Metals replace the positive ion, nonmetals replace the negative ion.

31. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound. Metals replace the positive ion, nonmetals replace the negative ion. Example: Ca(s) + AlCl 3 (aq) →

32. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound. Metals replace the positive ion, nonmetals replace the negative ion. Example: Ca(s) + AlCl 3 (aq) → Al(s) + CaCl 2 (aq)

33. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound. Metals replace the positive ion, nonmetals replace the negative ion. Example: 3 Ca(s) + 2 AlCl 3 (aq) → 2 Al(s) + 3 CaCl 2 (aq)

34. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound. Metals replace the positive ion, nonmetals replace the negative ion. Example: 3 Ca(s) + 2 AlCl 3 (aq) → 2 Al(s) + 3 CaCl 2 (aq) Example: F 2 (g) + SrBr 2 (aq) →

35. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound. Metals replace the positive ion, nonmetals replace the negative ion. Example: 3 Ca(s) + 2 AlCl 3 (aq) → 2 Al(s) + 3 CaCl 2 (aq) Example: F 2 (g) + SrBr 2 (aq) → Br 2 (l) + SrF 2 (aq)

36. Single Replacement (A + BC → B + AC) A pure element replaces a similar element in a compound. Metals replace the positive ion, nonmetals replace the negative ion. Example: 3 Ca(s) + 2 AlCl 3 (aq) → 2 Al(s) + 3 CaCl 2 (aq) Example: F 2 (g) + SrBr 2 (aq) → Br 2 (l) + SrF 2 (aq) H, O, N, Cl, Br, I, F form diatomic molecules in their pure form and require a subscript of 2

37. Chemical Equations synthesis decomposition combustion of a hydrocarbon single replacement double replacement

38. Double Replacement (AB + CD → AD + CB) Two elements in compounds switch places. One of the two products will be a solid precipitate (insoluble compound).

39. Double Replacement (AB + CD → AD + CB) Two elements in compounds switch places. One of the two products will be a solid precipitate (insoluble compound). It is important to include states of matter (s, l, g, aq) when writing these equations.

40. Double Replacement (AB + CD → AD + CB) Two elements in compounds switch places. One of the two products will be a solid precipitate (insoluble compound). It is important to include states of matter (s, l, g, aq) when writing these equations. Use your solubility table (bottom right of periodic table) to determine whether a compound is soluble (aq) or insoluble (s).

41. sodium chloride + silver nitrate → ?

42. The reactants in a double replacement reaction will always be aqueous.

43. sodium chloride + silver nitrate → ? The reactants in a double replacement reaction will always be aqueous. NaCl(aq) + AgNO 3 (aq) →

44. sodium chloride + silver nitrate → ? The reactants in a double replacement reaction will always be aqueous. Switching the metals will give you the correct partners for the products. NaCl(aq) + AgNO 3 (aq) →

45. sodium chloride + silver nitrate → ? The reactants in a double replacement reaction will always be aqueous. Switching the metals will give you the correct partners for the products. NaCl(aq) + AgNO 3 (aq) → AgCl( ) + NaNO 3 ( )

46. sodium chloride + silver nitrate → ? The reactants in a double replacement reaction will always be aqueous. Switching the metals will give you the correct partners for the products. The solubility table shows that silver chloride is the precipitate (insoluble). NaCl(aq) + AgNO 3 (aq) → AgCl(s) + NaNO 3 (aq)

47. lithium carbonate + calcium bromide → ?

48. Reactants must be aqueous. Li 2 CO 3 (aq) + CaBr 2 (aq) 

49. lithium carbonate + calcium bromide → ? Reactants must be aqueous. Switch the metals to obtain new compounds. Li 2 CO 3 (aq) + CaBr 2 (aq)  CaCO 3 ( ) + LiBr( )

50. lithium carbonate + calcium bromide → ? Reactants must be aqueous. Switch the metals to obtain new compounds. Check the solubility table to determine which compound is the precipitate. Li 2 CO 3 (aq) + CaBr 2 (aq)  CaCO 3 (s) + LiBr(aq)

51. lithium carbonate + calcium bromide → ? Reactants must be aqueous. Switch the metals to obtain new compounds. Check the solubility table to determine which compound is the precipitate. Balance the equation. Li 2 CO 3 (aq) + CaBr 2 (aq)  CaCO 3 (s) + 2 LiBr(aq)