1. Warm Up 12/18 Write the formula of the following ionic compound: magnesium phosphide. Hint: A magnesium cation has a charge of +2, and a phosphorus anion has a charge of -3.

2. Warm Up 1/12 Put the chemical equation into words: H + O → H O 2 22 Hydrogen and oxygen react to produce dihydrogen monoxide.

3. Lesson: Balancing Chemical Equations

4. 1 st Law of Thermodynamics Matter and energy cannot be created or destroyed. They can only be converted into different forms. This means the total amount of matter and energy in the universe is constant.

5. Kinetic Electric Radiant Thermal &

6. 2 Na (s) + Cl (g) → 2 NaCl (s) 2  Notice there are the same numbers of each type of atom on both sides of the equation. NaClNa Cl + →

7. 2 Na (s) + Cl (g) → 2 NaCl (s) 2 Question: If 30 g of Na reacts with 50 g of Cl, how much NaCl should there be? NaClNa Cl + →

8. __K + __ O → __ K O 2

9. Steps to Balance Equations: 1.List each element and how many there are for both sides. 2.Place coefficients in the blanks to try to balance it (start with the most difficult one).

10. __K + __ O → __ K O 2

11. __H + __ O → __ H O 2 2 2

12. __Al + __ O → __ Al O 2 2 3

13. __H O → __ H O + __ O 2 2 22

14. __Al + __ H PO → __H + __ AlPO 324 4

15. __Ca(ClO ) → __ CaCl +__ O 322 2

16. Practice! 1)__ Fe + __ O → __ Fe O 2)__ Mg(OH) → __ MgO + __ H O 3)__ KBr + __Fe(OH) → __KOH + __FeBr 4)__ZnS + __AlP → __Zn P + __Al S 5)__ CaCO + __H PO →__Ca (PO ) + __H CO 33334422 3322 33 22 223

17. Warm Up 1/9 Label the parts of this chemical equation: 2 Na (s) + Cl (g) → 2 NaCl (s) 2

18. Chemical Equation: Symbolic representation of a chemical reaction. Reactants 2 Na (s) + Cl (g) → 2 NaCl (s) 2 State of matter Yield Sign Product Coefficient

19. A synthesis reaction starts with 2 reactants and ends up with 1 product. A + B → AB Types of Chemical Equations

20. A + B → AB + →

21. Synthesis H 2(g) + Cl 2(g)  2HCl (g)

22. Which reactions are synthesis reactions? a. 2 Na + 2 HCl  H 2 + 2 NaCl b. C + O 2  CO 2 c. 2 Na + Cl 2  2 NaCl d. 2 H 2 O  2 H 2 + O 2

23. A decomposition reaction starts with 1 reactant and ends up with 2 or more products. AB → A + B

24. → +

25. Decomposition 2H 2 O (l)  2H 2(g) + O 2(g)

26. Which reactions are decomposition reactions? a. 2 Na + 2 HCl  H 2 + 2 NaCl b. C + O 2  CO 2 c. 2 Na + Cl 2  2 NaCl d. 2 H 2 O  2 H 2 + O 2

27. A single replacement reaction starts with two reactants and ends up with two products. The uncombined element takes the place of the combined element in the compound. AB + C → AC + B

28. + → +

29. Single Replacement Cu (s) + 2AgNO 3(aq)  Cu(NO 3 ) 2(aq) + 2Ag (s)

30. Which reactions are single replacement reactions? a. K + AgCl  Ag + KCl b. 2 Na + Cl 2  2 NaCl c. 2 Na + 2 HCl  H 2 + 2 NaCl d. MgO + 2 Na  Na 2 O + Mg

31. A double replacement reaction starts with 2 reactants and ends up with 2 products. In this case both the reactants are compounds and both products are compounds. They simply change partners. AB + CD → AC + BD

33. Double Replacement Pb(NO 3 ) 2(aq) + K 2 CrO 4(aq)  PbCrO 4(s) + 2KNO 3(aq)

34. Which reactions are double replacement reactions? a. NaOH + HBr  HOH + NaBr b. 2 H 2 + O 2  2 H 2 O c. Ca + S  CaS d. MgI 2 + 2 NaCl  MgCl 2 + 2 NaI

35. A combustion reaction has O as a reactant and will have CO or H O (or both) as products. Energy is released in the form of light and heat. Gasoline in your car engine is a combustion reaction. 2 2 2

37. Which reactions are combustion reactions? a. C + O 2  CO 2 b. 2 H 2 + O 2  2 H 2 O c. Ca + S  CaS d. CH 4 + 2 O 2  CO 2 + 2 H 2 O

38. A + BC  B + AC To determine if A will replace B in compound BC, use the Activity Series An element can replace any element below it in the series.

39. Al (s) + ZnCl 2(aq)  ?  What is replacing what?  Al replacing Zn  Will this happen? Check to see if Al is more active than Zn.  Al is above Zn, so it is more active Al (s) + ZnCl 2(aq)  Zn (s) + AlCl 3(aq) (unbalanced) 2Al (s) + 3ZnCl 2(aq)  3Zn (s) + 2AlCl 3(aq)

40. Co (s) + 2NaCl (aq)  ?  What is replacing what?  Co replacing Na  Will this happen? Check to see if Co is more active than Na.  Co is NOT above Na in the activity series, so it will NOT replace Na. Co (s) + 2NaCl (aq)  no rxn (NR)

41. Using the activity series, predict whether each of the possible reactions will occur. For reactions that will occur, write the products & balance the eqn.  MgCl 2(aq) + Zn (s)   Al (s) + H 2 O (g)   K (s) + AgCl (aq)   MgO + Na  No Rxn Al O + H KCl + Ag Na O + Mg 2 2 2

42. AB + CD → AD + CB Example: Both reactants have to be aqueous One product has to be a solid, one aqueous To find out which is s & aq, use the Solubility Rules saq AgNO3(aq)+ NaCl(aq) → AgCl( ) + NaNO3( )

43. AgNO 3 (aq) + KCl(aq) --> KNO 3 ( ) + AgCl( ) BaCl 2 (aq) + Na 2 SO 4 (aq) --> BaSO 4 ( ) + 2NaCl( ) s s aq

44. Practice 1. Pb(NO3)2 + 2KI → PbI2( ) + 2KNO3( ) 2. CaCl2 (aq) + Na2CO3 (aq) → NaCl ( ) + CaCO3( ) 3. K 2 CO 3 (aq)+ BaCl 2 (aq)---> BaCO 3 ( ) + KCl( ) 4. Pb(NO 3 ) 2 + K 2 S ---> K(NO 3 )( ) + PbS ( ) s s s aq s

45. PreAP Practice 1)K 2 CO 3 + BaCl 2 ---> 2) Al 2 (SO 4 ) 3 + Ca 3 (PO 4 ) 2 ---> 3) Pb(NO 3 ) 2 + K 2 S ---> 4) Pb(NO 3 ) 2 + CuSO 4 --->