1. Unit 4: Chemical Reactions

2. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive Mercury (II), Copper (I), Nickel (II), Tin (IV), Iron (III), Barium 1.Fe + CuCl 2  2.Hg + Sn(SO 4 ) 2  3.Ba + Ni 3 (PO 4 ) 2  (Hint: Start by figuring out if the metal in the compound will be kicked out, then figure out the new compound thinking about charges, then balance)

3. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive Mercury (II), Copper (I), Tin (IV), Iron (III), Barium 1.Fe + CuCl 2  FeCl 3 + Cu 2.Hg + Sn(SO 4 ) 2  3.Ba + Ni 3 (PO 4 ) 2  (Hint: Start by figuring out if the metal in the compound will be kicked out, then figure out the new compound thinking about charges, then balance)

4. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive Mercury (II), Copper (I), Tin (IV), Iron (III), Barium 1.2 Fe + 3 CuCl 2  2 FeCl 3 + 3 Cu 2.Hg + Sn(SO 4 ) 2  3.Ba + Ni 3 (PO 4 ) 2  (Hint: Start by figuring out if the metal in the compound will be kicked out, then figure out the new compound thinking about charges, then balance)

5. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive Mercury (II), Copper (I), Tin (IV), Iron (III), Barium 1.2 Fe + 3 CuCl 2  2 FeCl 3 + 3 Cu 2.Hg + Sn(SO 4 ) 2  HgSO 4 + Sn 3.Ba + Ni 3 (PO 4 ) 2  (Hint: Start by figuring out if the metal in the compound will be kicked out, then figure out the new compound thinking about charges, then balance)

6. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive Mercury (II), Copper (I), Tin (IV), Iron (III), Barium 1.2 Fe + 3 CuCl 2  2 FeCl 3 + 3 Cu 2.Hg + Sn(SO 4 ) 2  NO REACTION 3.Ba + Ni 3 (PO 4 ) 2  (Hint: Start by figuring out if the metal in the compound will be kicked out, then figure out the new compound thinking about charges, then balance)

7. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive Mercury (II), Copper (I), Tin (IV), Iron (III), Barium 1.2 Fe + 3 CuCl 2  2 FeCl 3 + 3 Cu 2.Hg + Sn(SO 4 ) 2  NO REACTION 3.Ba + Ni 3 (PO 4 ) 2  Ba 3 (PO 4 ) 2 + Ni (Hint: Start by figuring out if the metal in the compound will be kicked out, then figure out the new compound thinking about charges, then balance)

8. Warm Up Use the following Activity series to predict the products and balancing the equations Least ReactiveMost Reactive Mercury (II), Copper (I), Tin (IV), Iron (III), Barium 1.2 Fe + 3 CuCl 2  2 FeCl 3 + 3 Cu 2.Hg + Sn(SO 4 ) 2  NO REACTION 3.3 Ba + Ni 3 (PO 4 ) 2  Ba 3 (PO 4 ) 2 + 3 Ni (Hint: Start by figuring out if the metal in the compound will be kicked out, then figure out the new compound thinking about charges, then balance)

9. 1. I Can Translate between word equations and chemical equations

10. HOFBrINCl There are seven “diatomic” elements These elements always exist in pairs “HOFBrINCl” H 2 O 2 F 2 Br 2 I 2 N 2 Cl 2

11. Write formulas for the following: Chlorine Iron Iodine Zinc Lead Hydrogen Oxygen

12. Write formulas for the following: Chlorine Iron Iodine Zinc Lead Hydroge n Oxygen Cl 2 Fe I 2 Zn Pb H 2 O 2

13. Word Equations – Putting it all together! Reactants – what you react Products – what you produce

14. Examples Sodium and water react to form sodium hydroxide and hydrogen gas. Barium chloride reacts with sodium sulfate to form barium sulfate and sodium chloride. 2 NaCl + F 2  2 NaF + Cl 2 4 NH 3 + 6 NO  5 N 2 + 6 H 2 O

15. Examples Sodium and water react to form sodium hydroxide and hydrogen gas. Na + H 2 O  NaOH + H 2 Barium chloride reacts with sodium sulfate to form barium sulfate and sodium chloride. BaCl 2 + Na 2 SO 4  BaSO 4 + 2 NaCl 2 NaCl + F 2  2 NaF + Cl 2 Sodium chloride and fluorine react to form sodium fluoride and chlorine 4 NH 3 + 6 NO  5 N 2 + 6 H 2 O Nitrogen trihydride (ammonia) and nitrogen monoxide react to form nitrogen and water

16. Things to remember when translating equations 1.HOFBrINCl! (these are diatomic) 2.Ionic compounds must be neutrally charged 3.Name ionic versus molecular compounds appropriately. (ionic- possible roman numerals, molecular-prefixes)

17. 2. I Can Balance a Chemical Equation

18. Balancing Equations “Balancing Equations” – adding coefficients to chemical equations so that the number of each type of atom on the reacts side is the same on the products side Balance the previous equations.

19. 3. I Can Classify Chemical Reactions into the five Main Types

20. 4. I Can Predict the Products of a Chemical Reaction

21. Types of Reactions 1.Synthesis reactions 2.Decomposition reactions 3.Single displacement reactions 4.Double displacement reactions 5.Combustion reactions You need to be able to identify each type.

22. 1. Synthesis Example C + O 2 OO C +  OO C General: A + B  AB

23. Ex. Synthesis Reaction

24. Practice Predict the products. Na (s) + Cl 2(g)  Mg (s) + F 2(g)  Al (s) + F 2(g)  NaCl (s) MgF 2(s) AlF 3(s) 2 2 2 3 2 Now, balance them.

25. 2. Decomposition Example: NaCl General: AB  A + B  Cl Na Cl + Na

26. Ex. Decomposition Reaction

27. 3. Single Displacement Example: Zn + CuCl 2  Zn Cl Cu + General: AB + C  AC + B Cl Zn Cu +

28. Ex. Single Replacement Reaction

29. Single Replacement Reactions Write and balance the following single replacement reaction equation: Zn (s) + HCl (aq)  ZnCl 2 + H 2(g) 2 NaCl (s) + F 2(g)  NaF (s) + Cl 2(g) Al (s) + Cu(NO 3 ) 2(aq)  22 Cu (s) + Al(NO 3 ) 3(aq) 3 23 2

30. 4. Double displacement Example: MgO + CaS General:AB + CD  AD + CB S O  Mg Ca + O S Mg Ca +

31. Double Replacement Reactions Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Example: AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq)  KNO 3(aq) + BaSO 4(s) 2

32. Practice Predict the products. 1.HCl (aq) + AgNO 3(aq)  2.CaCl 2(aq) + Na 3 PO 4(aq)  3.Pb(NO 3 ) 2(aq) + BaCl 2(aq)  4.FeCl 3(aq) + NaOH (aq)  5.H 2 SO 4(aq) + NaOH (aq)  6.KOH (aq) + CuSO 4(aq) 

33. 5. Combustion Reactions Combustion reactions - a hydrocarbon reacts with oxygen gas. This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: 1) Fuel (hydrocarbon) 2) Oxygen 3) Something to ignite the reaction (spark)

34. Combustion Reactions In general: C x H y + O 2  CO 2 + H 2 O Products are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by-products like carbon monoxide) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 )

35. Combustion Example C 5 H 12 + O 2  CO 2 + H 2 O Write the products and balance the following combustion reaction: C 10 H 22 + O 2  56 8

36. Mixed Practice State the type & predict the products. 1.BaCl 2 + H 2 SO 4  2.C 6 H 12 + O 2  3.Zn + CuSO 4  4.Cs + Br 2  5.FeCO 3 

37. To Predict Products Determine which type of reaction is most likely to occur. 1.Synthesis – you start with two single elements Look at charges to combine 2.Decomposition – you start with one compound Separate the elements. Pay attention if you have a diatomic! 3.Single Displacement-you start with one element and one compound Look at charges when you write the new ionic compound 4.Double Displacement – you start with two compounds Look at charges when you write the new ionic compounds 5.Combustion – you start with oxygen and a hydrocarbon Form carbon dioxide and water.

38. 5. I Can Derive an Activity Series Based on Experimental Information