1. I’ve Got Nothin’ (2017) READING FOR Monday: Chapter 8 sections 1 – 5
HOMEWORK – DUE Monday 6/26/17
HW 6: CH 6 #’s 7, 9, 13, 15, 17, 25, 28, odd, 59, odd
Chapter 6 Extra Credit: DUE Monday 6/26
HW 11: CH 11 #’s 36, 45, 47, (all), 59, 60, 63, 64, 65, 67, 99
No Extra Credit for CH 11
Lab Monday: Dry lab, no prelab
Lecture Quiz Monday (stupid copier)
Beacon with Chris
Monday and Wednesday from 3:00 – 5:00 in LRC 107

2. Redox Reactions 3 Cl2(g) + 2 Al(s)  2 AlCl3(s)+3 –1
Gain Electrons REDUCED
oxidizing agent
3 Cl2(g) + 2 Al(s)  2 AlCl3(s)
reducing agent
Lost Electrons OXIDIZED

3. Types of reactions Decomposition One thing  more than one thing
A  B + C…
H2CO3(aq)  H2O(l) + CO2(g)
C3H5(NO3)3(l)  CO2(g) + H2O(g) + N2(g) + O2(g)
Look for one reactant and multiple products

4. Types of reactions Predictable decompositions:
metal hydrogen carbonates with heat
metal hydrogen carbonate
metal hydrogen carbonate
metal hydrogen carbonate
metal hydrogen carbonate
metal carbonate + carbon dioxide + water
metal carbonate
metal carbonate + carbon dioxide
metal carbonate + carbon dioxide + water
metal carbonate + carbon dioxide + water
metal carbonate + carbon dioxide + water
metal carbonate + carbon dioxide + water
Ca(HCO3)2(s)
Ca(HCO3)2(s)
Ca(HCO3)2(s)
Ca(HCO3)2(s)
CaCO3(s) + CO2(g) + H2O(g)
CaCO3(s) + CO2(g) + H2O(g)
CaCO3(s) + CO2(g) + H2O(g)
CaCO3(s) + CO2(g) + H2O(g)
CaCO3(s) + CO2(g) + H2O(g)
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water
calcium hydrogen carbonate is heated and decomposes in to
calcium carbonate, carbon dioxide, and water

5. Types of reactions Predictable decompositions:
metal carbonates with heat
metal carbonate
metal carbonate
metal carbonate
metal oxide + carbon dioxide
metal oxide
metal oxide + carbon dioxide
metal oxide + carbon dioxide
metal oxide + carbon dioxide
Al2(CO3)3(s)
Al2(CO3)3(s)
Al2(CO3)3(s)
Al2O3 + 3 CO2(g)
Al2O3 + 3 CO2(g)
Al2O3 + 3 CO2(g)
Al2O3 + 3 CO2(g)
aluminum carbonate is heated and decomposes in to
aluminum oxide and carbon dioxide
aluminum carbonate is heated and decomposes in to
aluminum oxide and carbon dioxide
aluminum carbonate is heated and decomposes in to
aluminum oxide and carbon dioxide
aluminum carbonate is heated and decomposes in to
aluminum oxide and carbon dioxide
aluminum carbonate is heated and decomposes in to
aluminum oxide and carbon dioxide
aluminum carbonate is heated and decomposes in to
aluminum oxide and carbon dioxide
aluminum carbonate is heated and decomposes in to
aluminum oxide and carbon dioxide

6. Types of reactions Unpredictable decomposition reactions:
metal oxides with heat
metal oxide
metal(?) + O2(g)
Fe2O3(s)
Fe(s) + O2(g)
Fe2O3(s)
FeO(s) + O2(g)

7. Types of reactions Unpredictable decomposition reactions:
metal ___ates with heat
metal ___ate
something
+ something else
KClO3(s)
KCl + O2(g)
Mg(NO3)2(s)
Mg(NO2)2(s) + O2(g)
Al2(SO4)3(s)
Al2O3(s) + SO3(g)

8. Types of reactions Combination reactions Two things to one thing
A + B…  C
N2(g) + 3 H2(g)  2 NH3(l)
Look for multiple reactants and a single product

9. Types of reactions Predictable combination reactions:
non–VOS metals and non–metals
Li(s) + S(s)
Li2S(s)
Ba(s) + P(s)
Ba3P2(s)

10. Types of reactions Unpredictable combination reactions:
VOS metals and non–metals
Pb(s) + Se(s)
PbSe(s)
Pb(s) + Se(s)
PbSe2(s)

11. Types of reactions Unpredictable combination reactions:
non–metals and non–metals
N2(g) + O2(g)
N2O3(g)
N2(g) + O2(g)
NO2(g)
N2(g) + O2(g)
N3O2(g)

12. Types of reactions Combustion reactions A + O2(g)  H2O(g) + CO2(g)
C5H12(l) + O2(g)  H2O(g) + CO2(g)
Look for O2(g) as a reactant and H2O(g) and CO2(g) as products!!

13. Types of reactions Single replacement reactions A + BX  B + AX
Ca(s) + HCl(aq)  H2(g) + CaCl2(aq)
Look for one element and one compound or ion as reactants
There tends to be a transfer of electrons in a single replacement reaction
These are NOT NOT NOT ions!!!!!!

14. Activity Series Mg(s) + CdCl2(aq)  MgCl2(aq) + Cd (s)
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS
The more reactive metal will “want” to be the ion.
Mg(s) + CdCl2(aq)
 MgCl2(aq) + Cd (s)
Mg > Cd so it WILL react!
neutral atom
+2 ion
The MORE reactive metal will always be an ion or in a compound!!

15. Activity Series AuNO3(aq) + Ag(s)  AgNO3(aq) + Au(s)
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS
The more reactive metal will “want” to be the ion.
AuNO3(aq) + Ag(s)
 AgNO3(aq) + Au(s)
Ag > Au so it WILL react!
+1 ion
neutral atom
The MORE reactive metal will always be an ion or in a compound!!

16. Activity Series Al(s) + Sr(ClO3)2(s)  N.R.
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS
The more reactive metal will “want” to be the ion.
Al(s) + Sr(ClO3)2(s)
 N.R.
Sr > Al so NO REACTION!
neutral atom
+2 ion
The MORE reactive metal will always be an ion or in a compound!!

17. Activity Series Cu(s) + HBr(aq)  N.R. means in acid
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS
The more reactive metal will “want” to be the ion.
Cu(s) + HBr(aq)
 N.R.
H > Cu so NO REACTION!
neutral atom
+1 ion
The MORE reactive metal will always be an ion or in a compound!!

18. Activity Series HCl(aq) + Zn(s)  ZnCl2(aq) + H2(g)
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS
The more reactive metal will “want” to be the ion.
HCl(aq) + Zn(s)
 ZnCl2(aq) + H2(g)
Zn > H so it WILL react!
+1 ion
neutral atom
The MORE reactive metal will always be an ion or in a compound!!

19. Activity Series Ba(s) + H2O(l)  Ba(OH)2(aq) + H2(g) ^
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS
The more reactive metal will “want” to be the ion.
Ba(s) + H2O(l)
 Ba(OH)2(aq) + H2(g)
Ba > H2O so it WILL react!
neutral atom
The MORE reactive metal will always be an ion or in a compound!!

20. Activity Series Mn(s) + H2O(l)  N.R. ^
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS
The more reactive metal will “want” to be the ion.
Mn(s) + H2O(l)
 N.R.
H2O > Mn so NO REACTION!
neutral atom
The MORE reactive metal will always be an ion or in a compound!!

21. Activity Series H2SO4 + Hg  NR Ca + HOH  Ca(OH)2(aq) + H2(g)^
H2O
Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
H2SO4 + Hg
 NR
H > Hg so it will NOT react!
Ca + HOH
 Ca(OH)2(aq) + H2(g)
Ca > H2O so it WILL react!
Mn(ClO4)2 + Mg
 Mg(ClO4)2(aq) + Mn(s)
Mg > Mn so it WILL react!

22. Types of reactions Neutralization reactions
bases have a hydroxide – OH – in them
NaOH(aq) – Ca(OH)2(aq)
HA(aq) + BOH  BA + HOH(l)
H2S(aq) + Sr(OH)2(aq)  SrS(aq) + HOH(l)
look for an acid and a base

23. Types of reactions
Double Replacement (look for 2 ionic compounds as reactants)
AX + BY  AY + BX
Fe2(SO4)3(aq) + Li3AsO4(aq)  FeAsO4(s) + Li2SO4(aq)
Look for two ionic compounds or an ionic compound and an acid as reactants

24. Solubility Rules All ammonium and group 1 metal salts are SOLUBLE
NO EXCEPTIONS
All nitrate, chlorate, perchlorate, and acetate salts are SOLUBLE
Most chloride, bromide, and iodide salts are SOLUBLE
EXCEPTIONS! Compound containing silver, mercury (I), and lead (II)
Most fluoride salts are SOLUBLE
EXCEPTIONS! Compounds containing magnesium, calcium, strontium, barium, and lead (II)
Most sulfate salts are SOLUBLE
EXCEPTIONS! Compounds containing strontium, barium, mercury (I), and lead (II)
Most sulfide, oxide, and hydroxide salts are INSOLUBLE
EXCEPTIONS! Compounds containing calcium, strontium, and barium
Most sulfite, carbonate, phosphate, oxalate, and chromate salts are INSOLUBLE

25. Solubility and Reactions
Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s)
Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s)
Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s)
Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s)
Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s)
3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l)
3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l)
3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l)
3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l)
3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l)
2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s)
2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s)
2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s)
2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s)
2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s)
2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l)
2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l)
2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l)
2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l)
2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l)
K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g)
K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g)
K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g)
K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g)
K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g)
K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g)
2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq)
2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq)
2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq)
2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq)
2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq)

26. Predicting Reaction Products

27. Predicting Reactions – Double Replacement
Step 1: Write ONE of each ion directly above the reactants
Write the balanced chemical reaction for the reaction of aluminum chloride and magnesium sulfate.
Al+3
Cl–1
Mg+2
SO42–
Step 1:
AlCl3 + MgSO4 

28. Predicting Reactions – Double Replacement
Step 1: Write ONE of each ion directly above the reactants
Step 2: Copy ONE of each ion above the products, but swap the anions
Write the balanced chemical reaction for the reaction of aluminum chloride and magnesium sulfate.
Al+3
Cl–1
Mg+2
SO42–
Al3+
SO42– +
Mg2+
Cl–1
Step 2:
Step 1:
AlCl3 + MgSO4 

29. Predicting Reactions – Double Replacement
Step 1: Write ONE of each ion directly above the reactants
Step 2: Copy ONE of each ion above the products, but swap the anions
Step 3: Combine cations and anions to form neutral compounds
Write the balanced chemical reaction for the reaction of aluminum chloride and magnesium sulfate.
Al+3
Cl–1
Mg+2
SO42–
Al3+
SO42– +
Mg2+
Cl–1
Step 3:
Step 2:
AlCl3 + MgSO4 
Al2(SO4)3
+ MgCl2

30. Predicting Reactions – Double Replacement
Step 1: Write ONE of each ion directly above the reactants
Step 2: Copy ONE of each ion above the products, but swap the anions
Step 3: Combine cations and anions to form neutral compounds
Write the balanced chemical reaction for the reaction of calcium oxalate with nickel (III) acetate
Ca+2
C2O4–2
Ni+3
C2H3O2–1
Ca2+
C2H3O2–1 +
Ni3+
C2O4–2
Step 2:
Step 1:
Step 3:
CaC2O4 + Ni(C2H3O2)3 
Ca(C2H3O2)2
+ Ni2(C2O4)3