1.  Complete the Warm up at your table (Synthesis Table)  Once you are done with the warm up, get a packet from the front of the room  Start the packet in class and finish it for H/W  Today we will be discussing: “How do you recognize and represent chemical changes?” Homework: Synthesis W/S Important Dates: 4/2: Reaction Test

2.  We will be taking the quiz first!  Complete the Warm up at your table (Balancing Reactions)  You will need paper and something to write with  Today we will be discussing: “How do you recognize and represent chemical changes?” Homework: Single and Combustion. W/S Important Dates: 4/2: Reaction Test

3.  Combustion Reactions:  Reactions in which oxygen combines with a hydrocarbon molecule and releases energy in the form of heat and light  C 3 H 6 O(s) + 3O 2 (g) → 3CO 2 (g) + 3H 2 O(g)  CH 4 (g) + 2O 2 (g) → CO 2 (g) + 2H 2 O(g)

4.  Products will ALWAYS be Carbon Dioxide and Water  All reactants and Products will be gasses  C 3 H 8 (g) + O 2 (g) → CO 2 (g) + H 2 O(g)  Balancing Trick!  1. Balance the carbons using carbons subscript  2. Balance the hydrogens using hydrogens subscript/2  3. Add up all the oxygens on the product side. Balance the oxygens using this number/2

5.  C 3 H 8 (g) + O 2 (g) → CO 2 (g) + H 2 O(g)  C 3 H 8 (g) + 10/2O 2 (g) → 3CO 2 (g) + 4H 2 O(g)  C 3 H 8 (g) + 5O 2 (g) → 3CO 2 (g) + 4H 2 O(g)  Balancing Trick!  1. Balance the carbons using carbons subscript  2. Balance the hydrogens using hydrogens subscript/2  3. Add up all the oxygens on the product side. Balance the oxygens using this number/2

6.  C 8 H 16 (g) + O 2 (g) → CO 2 (g) + H 2 O(g)  C 8 H 16 (g) + 12O 2 (g) → 8CO 2 (g) + 8H 2 O(g)  C 21 H 44 (g) + O 2 (g) → CO 2 (g) + H 2 O(g)  C 21 H 44 (g) + 32O 2 (g) → 21CO 2 (g) + 22H 2 O(g)  C 6 H 14 (g) + O 2 (g) → CO 2 (g) + H 2 O(g)  C 6 H 14 (g) + 19/2O 2 (g) → 6CO 2 (g) + 7H 2 O(g)  C 6 H 14 (g) + 19O 2 (g) → 12CO 2 (g) + 14H 2 O(g)  C 3 H 6 O(g) + O 2 (g) → CO 2 (g) + H 2 O(g)  C 3 H 6 O(g) + 4O 2 (g) → 3CO 2 (g) + 3H 2 O(g)

7.  Single Replacement Reactions:  A reaction in which the atoms of one element replace the atoms of another element in a compound  AB + C → CB + A  Cu(S) + 2AgNO 3 (aq) → 2Ag(s) + Cu(NO 3 ) 2 (aq)  F 2 (g) + 2NaBr(aq) → 2NaF(aq) + Br 2 (l)

8.  Lithium  Rubidium  Potassium  Calcium  Sodium  Magnesium  Aluminum  Manganese  Zinc  Iron  Nickel  Tin  Lead  Copper  Silver  Platinum  Gold  Fluorine  Chlorine  Bromine  Iodine  Page 293

9.  3 basic types of single replacement reactions  1. Metal replaced by a more active metals  2. Hydrogen in acids replaced by active metals  3. Nonmetals replaced by more active nonmetals  4. Hydrogen in water replaced by a metal

10.  MNM + AM → AMNM + M  Fe(s) + CuSO 4 (aq) → FeSO 4 (aq) + Cu(s)  Na(s) + SnCO 3 → ?  2Na(s) + SnCO 3 → Na 2 CO 3 + Sn(s)  Pt(s) + Zn 2 O → ?  Pt(s) + Zn 2 O → NR

11.  M(s) + HX → MX + H 2 (g)  Zn(s) + 2HCl(aq) → ZnCl 2 (aq) + H 2 (g)  Cu(s) + HNO 3 (aq) → Cu(NO 3 ) 2 (aq) + H 2 (g)  Cu(s) + 2HNO 3 (aq) → Cu(NO 3 ) 2 (aq) + H 2 (g)  Na(s) + H 2 SO 4 (aq) → Na 2 SO 4 (aq) + H 2 (g)  2Na(s) + H 2 SO 4 (aq) → Na 2 SO 4 (aq) + H 2 (g)

12.  NM(s,l,g) + MNM(aq) → MNM(aq) + NM(s,l,g)  Cl 2 (g) + 2NaBr(aq) → 2NaCl(aq) + Br 2 (l)  Br 2 (l) + MgI 2 (aq) → ?  Br 2 (l) + MgI 2 (aq) → MgBr 2 (aq) + I 2 (s)  F 2 (g) + FeBr 2 (aq) → ?  F 2 (g) + FeBr 2 (aq) → NR

13.  M(s) + H 2 O(l) → M(OH) x (aq) + H 2 (g)  2Na(s) + 2H 2 O(l) → 2NaOH(aq) + H 2 (g)  Fe(s) + H 2 O(l) → ?  Fe(s) + 2H 2 O(l) → Fe(OH) 2 (aq) + H 2 (g)  Sr(s) + H 2 O(l) → ?  Sr(s) + 2H 2 O(l) → Sr(OH) 2 (aq) + H 2 (g)

14.  Al(s) + H 2 SO 4 (aq) → ?  2Al(s) + 3H 2 SO 4 (aq) → 3H 2 (g) + Al 2 (SO 4 ) 3 (aq)  Br 2 (l) + MgI 2 (aq) → ?  Br 2 (l) + MgI 2 (aq) → MgBr 2 (aq) + I 2 (s)  Zn(s) + H 2 O(l) → ?  Zn(s) + 2H 2 O(l) → ZnOH(aq) +H 2 (g)  Ag(s) + CuCl 2 (aq) → ?  Ag(s) + CuCl 2 (aq) → NR  Fe(s) + CuSO 4 → ?  Fe(s) + CuSO 4 → FeSO 4 + Cu(s)  Br 2 (g) + KCl(aq) → ?  Br 2 (g) + KCl(aq) → NR