Nguồn ngoài

CHM2047: One-Semester General Chemistry

The course is designed for entering (not transfer) students who wish to move more quickly into advanced course work. Topics include electronic structure and bonding, gases, liquids, solids, kinetics, equilibria, acids and bases, thermodynamics, oxidation-reduction, metals and non-metals.

Chemistry

Tác giả: Valeria Kleiman
Nhà xuất bản: University of Florida
Nguồn: LibreTexts
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

Đọc trực tuyến Tải PDF (nguồn mở)

Mục lục· 168 mục

01: Introduction
1.01: Hypothesis Theories and Laws
1.02: The Scientific Method - How Chemists Think
1.03: Radiation and the Wave Nature of Light
1.04: The failures of Classical Mechanics- the Particle Nature of Light
1.05: Early Experiments to Characterize the Atom
1.06: First attempts to model the H atom
1.07: Matter as Waves
02: Describing Quantum systems
2.01: Describing Matter-Waves
2.02: The Uncertainty Principle
2.03: The Schrodinger Equation for a Wave
2.04: Operators Observables and Wavefunctions
2.05: Overview of Particle in a box
2.06: A Particle in a Multidimensional Box
03: Atoms Orbitals and Electronic Configurations
3.01: The Schroedinger equation for the H atom
3.02: Quantum Numbers for Atomic Orbitals
3.03: Atomic Orbitals
3.04: Many-Electron Atoms
3.05: Electron Configurations
3.06: Electron Configurations and the Periodic Table
04: Periodic Trends in Elements and Compounds
4.01: Development of the Periodic Table
4.02: Electronic Structure
4.03: Sizes of Atoms and Ions
4.04: Ionization Energy
4.05: Electron Affinity
4.06: Electronegativity
05: Molecular Structure and Geometry
5.01: Lewis Structures and the Octet Rule
5.02: Formal Charge and Resonance
5.03: Oxidation number
5.04: VSEPR Geometry
5.4.01: 5.4.1-Limitations of VSPER
5.05: Geometry and Molecular Polarity
06: Understanding Molecules with QM
6.01: Prelude to Covalent Bonding
6.02: The Born-Oppenheimer Approximation
6.03: The H Prototypical Species
6.04: The Overlap Integral
6.05: Bonding and Antibonding Orbitals
6.06: Molecular Orbitals Can Be Ordered According to Their Energies
6.07: Molecular-Orbital Theory Does not Predict a Stable Diatomic Helium Molecule
6.08: Molecular Orbital Theory Predicts that Molecular Oxygen is Paramagnetic
6.09: Summary of Molecular Orbital Theory
6.10: Valence Bond Theory
6.E: Advanced Theories of Covalent Bonding (Exercises)
07: Models for Polyatomic Molecules
7.01: Orbital Hybridization
7.02: Hybrid Atomic Orbitals
7.03: Multiple Bonding and Molecular Orbitals
08: 8 Coordination Chemistry
01: Nomenclature
02: Oxidation States of Transition Metals
03: History of Coordination compounds
04: Coordination Number and Geometry
4.01: Isomers
05: Polydented Ligands
06: Hard and Soft Acids and Bases
07: Magnetic Moments
08: Spectroscopy (Needs addition)
08: Valence Bond and MO Ligand Field (needs addition)
09: Crystal Field Theory
10: Introduction to Ligand Field Theory (Octahedral complexes)
10.01: Tetrahedral and Octahedral Geometries
11: Ligand Field Stabilisation Energy (LFSE)
11.01: The Effect of the Metal Ion on d-Orbital Splitting
12: The Effect of Ligands and the Spectrochemical Series
13: Absorption Spectra and Magnetic Properties
13.01: Colors of Coordination Compounds (Electronic Absorption Spectra)
13.02: Predicting UV-visible Absorption
09: Gases
9.01: Review of Gases
9.1.01: Characteristics of Gases
9.1.02: Pressure
9.1.03: The Gas Laws
9.02: The Ideal Gas Equation
9.03: Further Applications of the Ideal-Gas Equations
9.04: Gas Mixtures and Partial Pressures
9.05: Kinetic-Molecular Theory
9.06: Equipartition of Energy (Needs addition)
9.07: Molecular Effusion and Diffusion
9.08: Real Gases - Deviations from Ideal Behavior
9.E: Exercises
9.S: Gases (Summary)
10: Thermochemistry
10.01: The Nature of Energy
10.02: The First Law of Thermodynamics
10.03: Enthalpy
10.04: Enthalpy of Reaction
10.05: Heat Capacity Enthalpy and Calorimetry
10.06: Calorimetry
10.07: Hess's Law
10.08: Enthalpies of Formation
10.09: Foods and Fuels
10.E: Thermochemistry (Exercises)
10.S: Thermochemistry (Summary)
11: Spontaneous Processes and Thermodynamic Equilibrium
11.01: The Nature of Spontaneous Processes
11.02: Entropy and Spontaneity - A Molecular Statistical Interpretation
11.03: Entropy and Heat - Experimental Basis of the Second Law of Thermodynamics
11.04: Entropy Changes in Reversible Processes
11.05: Entropy Changes and Spontaneity
11.06: The Third Law of Thermodynamics
11.07: The Gibbs Free Energy
11.08: Carnot Cycle Efficiency and Entropy
11.E: Spontaneous Processes (Exercises)
12: Chemical Equilibrium- Thermodynamics and General Considerations
12.01: The Nature of Chemical Equilibrium
12.02: Reaction Directions (Thermodynamic Explanation) (needs work on Q)
12.03: The Empirical Law of Mass Action
12.04: Thermodynamic Description of the Equilibrium State
12.05: The Law of Mass Action for Related and Simultaneous Equilibria
12.06: Equilibrium Calculations for Gas-Phase and Heterogenous Reactions
12.07: Reaction Directions (Empirical Explanation)
12.08: Distribution of a Single Species between Immiscible Phases - Extraction and Separation
12.E: Chemical Equilibria (Exercises)
13: Solutions
13.01: Solids Liquids and Phase Transitions
13.1.01: Bulk Properties of Liquids - Molecular Interpretation
13.1.02: Intermolecular Forces - Origins in Molecular Structure
13.1.03: Intermolecular Forces in Liquids
13.1.04: Phase Equilibrium
13.1.05: Phase Transitions
13.1.06: Phase Diagrams
13.1.E: Solids Liquids and Phase Transitions (Exercises)
13.02: Solutions
13.2.01: Composition of Solutions
13.2.02: Nature of Dissolved Species
13.2.03: Phase Equilibrium in Solutions - Nonvolatile Solutes
13.2.04: Phase Equilibrium in Solutions - Volatile Solutes
13.2.05: Colloidal Suspensions
13.2.E: Solutions (Exercises)
14: Chemical Equilibrium in Solutions
14.01: AcidBase Equilibria
14.1.01: Classifications of Acids and Bases
14.1.02: Properties of Acids and Bases in Aqueous Solutions
14.1.03: Acid and Base Strength
14.1.04: Equilibria Involving Weak Acids and Bases
14.1.05: Buffer Solutions
14.1.06: Acid-Base Titration Curves
14.1.07: Polyprotic Acids
14.1.08: Organic Acids and Bases - Structure and Reactivity
14.1.09: A Deeper Look - Exact Treatment of Acid-Base Equilibria
14.1.E: Acid-Base Equilibria (Exercises)
14.02: Electrochemistry
14.2.01: Electrochemical Cells
14.2.02: The Gibbs Free Energy and Cell Voltage
14.2.03: Concentration Effects and the Nernst Equation
14.2.04: Batteries and Fuel Cells
14.2.05: Corrosion and Its Prevention
14.2.06: A Deeper Look- Electrolysis of Water and Aqueous Solutions
14.03: Solubility and Precipitation Equilibria
14.3.01: The Nature of Solubility Equilibria
14.3.02: Ionic Equilibria between Solids and Solutions
14.3.03: Precipitation and the Solubility Product
14.3.04: The Effects of pH on Solubility
14.3.05: Complex Ions and Solubility
14.3.06: A Deeper Look- Selective Precipitation of Ions
14.3.E: Solubility and Precipitation (Exercises)
15: Chemical Kinetics
15.01: Rates of Chemical Reactions
15.02: Rate Laws
15.03: Reaction Mechanisms
15.04: Effect of Temperature on Reaction Rates
15.05: A Deeper Look- Reaction Dynamics
15.06: Kinetics of Catalysis