1. Chapter 10 Notes, Part I Parts of an equation Types of reactions

2. What is a chemical reaction? A chemical reaction is the act of changing substances into new substances with new and different chemical and physical properties.A chemical reaction is the act of changing substances into new substances with new and different chemical and physical properties.

3. A Chemical Equation A chemical equation shows what is going on in a chemical reaction.A chemical equation shows what is going on in a chemical reaction. Instead of writing down the entire sentence “hydrogen reacts with oxygen to form dihydrogen monoxide (water)”, you could write…Instead of writing down the entire sentence “hydrogen reacts with oxygen to form dihydrogen monoxide (water)”, you could write…

4. 2H 2 + O 2  2H 2 Oreactantsproducts The substances you have before a chemical reaction occurs The substances you have after a chemical reaction occurs (found on the left side of the equation) (found on the right side of the equation)

5. 2H 2 + O 2  2H 2 Osubscriptscoefficients How many atoms of an element are in a compound How many substances are in the reaction

6. 2H 2 + O 2  2H 2 O The arrow reads as “produces”, “yields” or “reacts to form”

7. Word Equation This indicates the reactants and products of chemical reactions. reactant 1 + reactant 2 → product 1 iron (s) + chlorine (g) → iron(III) chloride (s) This reads: “Iron and chlorine react to produce iron(III) chloride.”

8. Skeleton Equation Uses chemical formulas instead of words to identify your reactants and products. Word: iron (s) + chlorine (g) → iron(III) chloride (s) Skeleton: Fe (s) + Cl 2 (g) → FeCl 3 (s)

9. Chemical Equation A skeleton equation that shows that the number of atoms of each reactant and each product is equal on both sides of the arrow, also called balanced. Word: iron (s) + chlorine (g) → iron(III) chloride (s) Skeleton: Fe (s) + Cl 2 (g) → FeCl 3 (s) Chemical: 2Fe (s) + 3Cl 2 (g) → 2 FeCl 3

10. 4Fe + 3O 2  2Fe 2 O 3 Iron reacts with oxygen gas to produce iron (III) oxide

11. Other symbols in an Equation (s) = substance is solid (l) = substance is liquid (g) = substance is a gas (aq) = substance is dissolved in water  = heat A formula written above or below an arrow means it is a catalyst (a substance that speeds up a reaction without being used up by it.)

12. What is: The name of something that speeds a reaction, but is not used up? The name of what you have before a reaction takes place? The symbol for heat? The number that shows there are more than one of the entire compound?

13. Types of reactions There are five types of reactions –Synthesis –Decomposition –Single replacement –Double replacement –Combustion

14. Synthesis Reaction A synthesis reaction occurs when two or more elements or compounds combine to form a single substance. It will follow the form A + B  AB Example: Fe + S  FeS

15. Decomposition Reaction A decomposition reaction occurs when one substance breaks down into two or more substances. It will follow the pattern AB  A + B Example: CaCO 3  CaO+CO 2

16. Single Replacement Reaction One element replaces another element in a compound. Generally follows the formula: AB + C  A + BC Example: Mg+Zn(NO 3 ) 2  Zn+Mg(NO 3 ) 2

17. Double Replacement Reaction The exchange of two positive ions between two reacting compounds, forming two new compounds as a product. Generally follows the formula: AB + CD  AD + CB Example: Na 2 S+Cd(NO 3 ) 2  CdS+2NaNO 3

18. Combustion Reaction A compound reacts with oxygen to producing energy as heat and light. Most of the time, it is a hydrocarbon reacting with oxygen, and the outcome is always carbon dioxide and water Follows the form: A + O 2  CO 2 + H 2 O Example: CH 4 + O 2  CO 2 + 2H 2 O

19. What type of reaction is: NaCN + H 2 SO 4  2HCN + Na 2 SO 4 Zn + 2HCl  ZnCl 2 + H 2 2C 2 H 6 + 7O 2  4CO 2 + 6H 2 O 2H 2 + O 2  2H 2 O

20. Tell which of the five types of reactions the following are:

21. 2Na + 2H 2 O  2NaOH + H 2 Single replacement

22. Fe + S  FeS combination

23. Al(OH) 3 + 3NaCl  AlCl 3 + 3NaOH Double replacement

24. CH 4 + 2O 2  CO 2 + 2H 2 O combustion

25. KClO 2  KCl + O 2 decomposition

26. NaOH + HCl  NaCl + H 2 O Double replacement

27. 4Fe + 3O 2  2Fe 2 O 3 combination

28. 2C 2 H 2 + 5O 2  4CO 2 + 2H 2 O combustion

29. H 2 + Cl 2  2HCl combination

30. MgO + 2KF  MgF 2 + K 2 O Double replacement

31. Na + Al(NO 3 ) 3  NaNO 3 + Al Single replacement

32. 2PbO 2  2PbO + 3O 2 decomposition

33. Ba(CN) 2 + H 2 SO 4  BaSO 4 + HCN Double replacement

34. C 3 H 8 + 5O 2  3CO 2 + 4H 2 O combustion

35. 4Li + O 2  2Li 2 O combination

36. 2Ag + 2HCl  2AgCl + H 2 Single replacement

37. 2H 2 O 2  2H 2 O + O 2 decomposition

38. C 2 H 2 + O 2  CO 2 + H 2 O combustion

39. 2HBr  H 2 + Br 2 decomposition

40. CrSO 4 + 2AgNO 3  Cr(NO 3 ) 2 + Ag 2 SO 4 Double replacement