1. Why is Ammonia (NH3) a Weak Base?
An Arrhenius Base is a substance that, when dissolved in water, increases the concentration of hydroxide ions.
NH3(aq) H2O(l) NH4+(aq) OH-(aq) H H +1 H N H H N H H
Remember also that
An Arrhenius Acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions.

2. Acid and Base Anhydrides
Acid Anhydrides: a compound (such as an oxide) that reacts with water to give acidic solutions
Basic Anhydrides: a compound (such as an oxide) that reacts with water to give basic solutions
Acidity Increases
Oxides
Increasing Basicity
Basic Anhydride
Increasing Acidity
Acidic Anhydride
Basicity Increases

3. Acid-Base Titrations
Titrations are used to determine the amounts of substance present in a sample (solution).
End point
Known conc of acid V
Unknown amount
(concentration) of base
Could we reverse the order?

4. The End Point HA(g) H+(aq) + A-(aq) BOH(s) B+(aq) + OH-(aq)
The End Point for a good titration is the EQUIVALENCE point, i.e., the point at which the amount of base in the beaker equals the amount of acid disposed from the buret, i.e., nA = nB if both acid and base are one-equivalent, i.e.,
HA(g) H+(aq) A-(aq)
BOH(s) B+(aq) OH-(aq)
In contrast, a two-equivalent acid given by:
H2A(g) H+(aq) A2-(aq)
would result in 2 nA = nB.
The concentration of the base simply follows as nB/VB.

5. Do Acids Do More than Neutralize Bases?
Discuss/Demonstrate
Acid on a carbonate
Acid on a metal
Acid on a metal oxide

6. Do Bases Do More than Neutralize Acids?
Discuss/Demonstrate
Base (except ammonia) on an ammonium salt
Base on the oxide of a nonmetal

7. Redox Reactions or Oxidation-Reduction Reactions
Loss of Electrons = Oxidation
Gain of Electrons = Reduction
How do I remember this?
LEO, the lion, says GER

8. Oxidation and Reduction
Loss of 2 electrons = Oxidation
Mg(s) Cl2(g) MgCl2(s)
Each chlorine atom gains one electron
= Reduction
Loss of 2 electrons = Oxidation
2 Mg(s) O2(g) MgO(s)
Each oxygen atom gains two electrons
= Reduction

9. Reducing Agent: A substance that causes the reduction of another substance while being oxidized itself. Good reducing agent: H2.
Oxidizing Agent: A substance that causes the oxidation of another substance while being reduced itself (gains electrons). Strong oxidizing agents: O2, F2, Cl2, Br2 ±0 ±0 +2 -2
2 Mg(s) O2(g) MgO(s) ±0 ±0 +1 -1
2 Na(s) Cl2(g) NaCl(s)
reducing
agent
oxidizing
agent

10. Oxidation Number
Oxidation Numbers is a parameter obtained by exaggerating the ionic character of a bond. It can be understood as the charge that an atom would have if the more electronegative atom in a bond acquired the two electrons of the bond completely. +2 -2 +5 -2
MgO +6 -2
NO3-
SO3 +1 -1 +7 -2
HCl
MnO4-

11. The sum of the oxidation numbers of all atoms in the species is equal to its total charge.
For atoms in their elemental form 0
For atoms of group
For atoms of group
For atoms of group
For atoms of group , +2
For hydrogen (with non-metals)
-1 (with metals)
For fluorine (always)
For oxygen (unless with F)
-1 (in peroxides, O22-)
-1/2 (in superoxides, O2-)
For halogens (not F) in most compounds (unless with O or a more electronegative halogen)

12. Determining Oxidation Numbers
SO2
CCl4
COCl2
H2O2 O2
OH-
MgH2
CaCO3 I2

13. Electron Transfer Reactions = Redox Chemistry
An atom is oxidized (loses an electron) when its oxidation number increases in a chemical reaction.
An atom is reduced (gains an electron) when its oxidation number decreases in a chemical reaction.
C O CO2 ±0 -2
reduced
oxidized +4