Pictures

4. Chemical Reactions

(Last Updated 01/28/2024, 15:30 MST)

Brown Chapter 3 Stoichiometry PowerPoint

Brown Chapter 4 Reactions in Aqueous Solution PowerPoint

4.1 Introduction for Reactions

Conservation of Mass

4.2 Net Ionic Equations

Molecular Equation

Ionic Equation

Net Ionic Equation

Writing Net Ionic Equation

4.3 Representations of Reactions

Chemical Equations

4.4 Physical and Chemical Changes

Chemical Equations

Physical vs Chemical Changes

4.5 Stoichiometry

Stoichiometry

Stoichiometry of Balanced Chemical Equation
0. Balanced chemical equation.
1. Given quantity and units.
2. Conversion from given units to moles.
3. Mole ratio between required and given quantities (coefficients from balanced chemical equation).
4. Conversion from moles to required units.
5. Calculate the requested quantity.

4.6 Introduction to Titration

Titration

Acid-Base Titration Calculations (Ma)(Va)(Na) = (Mb)(Vb)(Nb) Ma = Molarity of acid Va = Volume of acid Na = Number of protons donated per mole of acid Mb = Molarity of base Vb = Volume of base Nb = Number of protons accepted per mole of base Volume units must be identical.

Redox Titration

Oxidation-Reduction Titration Calculations (Mo)(Vo)(No) = (Mr)(Vr)(Nr) Mo = Molarity of oxidizer Vo = Volume of oxidizer No = Number of electrons accepted per mole of oxidizer Mr = Molarity of reducer Vr = Volume of reducer Nr = Number of electrons donated per mole of reducer Volume units must be identical.

Stoichiometry

4.7 Types of Chemical Reactions

Displacement Reactions

Element Replacement Activity Series

F₂ > Cl₂ > Br₂ > I₂
2HI + Br₂ → 2HBr + I₂
2HBr + Cl₂ → 2HCl + Br₂
2HCl + F₂ → 2HF + Cl₂

Halogen Activity Experiment

Metathesis (Exchange) Reactions

Element Replacement Activity Series

4.8 Introduction to Acid-Base Reactions

Strong and Weak Acids

Strong Acids

Acid Base Reaction

Gas-Forming Reactions

4.9 Oxidation-Reduction (Redox) Reactions

Oxidation-Reduction Reactions

Assigning Oxidation States (OS)

1. An element in a free form has OS = 0.

2. In a compound or ion, the sum of the oxidation states equals the total charge of the compound or ion.

3. Fluorine in compounds has OS = −1; this extends to chlorine and bromine only when not bonded to a lighter halogen, oxygen or nitrogen.

4. Group 1 and group 2 metals in compounds have OS = +1 and +2, respectively.

5. Hydrogen has OS = +1 but adopts −1 when bonded as a hydride to metals or metalloids.

6. Oxygen in compounds has OS = −2 but only when not bonded to oxygen (e.g. in peroxides) or fluorine.

-Thanks Wikipedia

Reaction Type	Redox?	Model	Guidelines
Synthesis/Combination	Maybe	A + B → C	-
Decomposition	Maybe	C → A + B	-
Single Displacement	Always	AB + C → AC + B	Activity Series (metals or halogens)
Double Displacement (Metathesis/Exchange)	Never	AB + CD → AD + CB	Solubility Table, Acid-Base Reactions (with or without gas), Complex Table (Metals and Ligands)
Combustion (Complete)	Always	CHO + O₂→ CO₂ + H₂O	Principle reactant is any compound of C and H, and sometimes O. Products are always CO₂and H₂O.
Combustion (Incomplete)	Always	CHO + O₂ → CO + H₂O	Products vary in an incomplete combustion reaction, but "half-way" is with CO and H₂O products.