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Chemistry 1210
Materials Needed for CHEM 1210
Chapter 1
1.1 The Study of Chemistry
1.3 Properties of Matter
1.4 Units of Measurement
1.5 Uncertainty in Measurement
1.6 Dimensional Analysis
Chapter 2
2.3 The Modern View of Atomic Structure
2.7 Ions
2.4 Atomic Weights
3.4 Avagadro’s Constant and the Mole
2.6 Molecules and Molecular Compounds
2.7 Ions and Ionic Compounds
2.8 Naming Inorganic Compounds
Chapter 3
3.1 Chemical Equations
3.2 Patterns of Chemical Reactivity
3.3 – 3.4 Formula Weights
3.4 Avagadro’s Number and the Mole Calculations
3.5 Empirical Formulas
3.6 Stoichiometry
3.7 Limiting Reactants
Stoichiometry Summary
Chapter 4
4.1 General Properties of Aqueous Solutions
4.2 Precipitation Reactions
4.3 Acids and Bases
4.4 Oxidation-Reduction Reactions
4.5 Concentrations of Solutions
4.6 Solution Stoichiometry and Chemical Analysis
CHEM 1210 Exam #1 Study Guide
CHEM 1210 Practice Exam #1
Chapter 5
5.1 The Nature of Energy
5.2 The First Law of Thermodynamics
5.3 & 5.4 Enthalpy and Enthalpies of Reaction
5.5 Calorimetry
5.6 Hess’s Law
5.7 Enthalpies of Formation
Chapter 6
6.1 The Electronic Structure of Atoms
6.2 Wave-Particle Duality
6.3 Line Spectra and the Bohr Model
6.4 The Wave Behavior of Matter
6.5 & 6.6 Quantum Mechanics and Atomic Orbitals
6.7 Many Electron Atoms
6.8 Electron Configurations and Orbital Block Diagrams
Chapter 7
7.1 Development of the Periodic Table
7.3 Atomic and Ionic Radii
7.3 Isoelectronic Species
7.4 Ionization Energy
7.5 Electron Affinity
8.4 Electronegativity
7.6 Magnetic Properties
CHEM1210 Exam #2 Study Guide
CHEM 1210 Practice Exam #2
Chapter 8
8.1 Lewis Symbols and the Octet Rule
8.2 Ionic Bonding
8.3 Covalent Bonding
8.4 Bond Polarity and Electronegativity
8.5 Drawing Lewis Structures
8.8 Strengths of Covalent Bonds
Chapter 9
9.1 – 9.2 Molecular Shapes and VSEPR
9.2 – 9.3 VSEPR Shapes and Molecular Polarity
9.4 Covalent Bonding and Orbital Overlap
9.5 Hybrid Orbitals
9.6 Multiple Bonds
9.7 Molecular Orbitals
9.8 Period 2 Diatomic Molecules
Chapter 10
10.1 Characteristics of Gases
10.2 Pressure
10.3 The Gas Laws
10.4 The Ideal Gas Equation
10.5 Further Applications of the Ideal-Gas Law
10.6 Gas Mixtures and Partial Pressures
10.7 The Kinetic-Molecular Theory of Gases
10.8 Molecular Effusion and Diffusion
10.9 Real Gases: Deviations From Ideal Behavior
CHEM 1210 Exam #3 Study Guide
CHEM 1210 Practice Exam #3
Chapter 11
11.1 Molecular Comparisons of Gases, Liquids, and Solids
11.2 Intermolecular Forces
11.3 Select Properties of Liquids
11.4 Phase Changes
11.5 Vapor Pressure
11.6 Phase Diagrams
Chapter 12
12.1 Classifications of Solids
12.2 Structures of Solids
12.3 Metallic Solids
12.4 Metallic Bonding
12.5 Ionic Solids
12.6 Molecular Solids
12.7 Covalent-Network Solids
CHEM 1210 Final Exam Study Guide
Chemistry 1220
Welcome to CHEM 1220
Chapter 13
13.1 The Solution Process
13.2 Saturated Solutions and Solubility
13.3 Factors Affecting Solubility
13.4 Expressing Solution Concentration
13.5 Colligative Properties
Chapter 14
14.1 Factors that Affect Reaction Rates
14.2 Reaction Rates
14.3 Concentration and Rate Laws
14.4 The Change of Concentration with Time
14.5 Temperature and Rate
14.6 Reaction Mechanisms
14.7 Catalysis
Chapter 15
15.1 The Concept of Equilibrium
15.2 The Equilibrium Constant
15.3 Understanding and Working With Equilibrium Constants
15.4 Heterogeneous Equilibria
15.5 & 15.6 Equilibrium Constants
15.7 Le Chatlier’s Principle
Chapter 16
16.1 Acids and Bases: A Brief Review
16.2 Bronsted-Lowry Acids and Bases
16.3 The Autoionization of Water
16.4 The pH Scale
16.5 Strong Acids and Bases
16.6 Weak Acids
16.7 Weak Bases
16.8 Relationship Between K
a
and K
b
16.9 Acid-Base Properties of Salt Solutions
16.10 Acid-Base Behavior and Chemical Structure
16.11 Lewis Acids and Bases
CHEM 1220 Exam #1 Study Guide
CHEM 1220 Alt. Exam Form
CHEM 1220 Review Session
Chapter 17
17.1 The Common Ion Effect
17.2 Buffered Solutions
17.3 Acid-Base Titrations
17.4 Solubility Equilibria
17.5 Factors that Affect Solubility
17.6 Precipitation and Separation of Ions
17.7 Qualitative Analysis for Metallic Elements
K
sp
Lab Experience
CHEM 1220 Exam #2 Study Guide
Chapter 19
19.1 Spontaneous Processes
19.2 Entropy and the Second Law of Thermodynamics
19.3 Molecular Interpretation of Entropy
19.4 Entropy Changes in Chemical Reactions
19.5 Gibbs Free Energy
19.6 Free Energy and Temperature
19.7 Free Energy and the Equilibrium Constant
Chapter 20
20.1 Oxidation States and Oxidation-Reduction Reactions
20.2 Balancing Redox Reactions
20.3 Voltaic Cells
20.4 Cell Potentials Under Standard Conditions
20.5 Free Energy and Redox Reactions
20.6 Cell Potentials Under Nonstandard Conditions
20.7 Batteries and Fuel Cells
20.8 Corrosion
20.9 Electrolysis
Electrochemistry Lab Experience
Chapter 23
23.1 The Transition Metals
23.2 Transition Metal Complexes
23.3 Common Ligands in Coordination Chemistry
23.4 Nomenclature and Isomerism in Coordination Chemistry
23.5 Colors and Magnetism in Coordination Chemistry
23.6 Crystal Field Theory
CHEM 1220 Exam #3 Study Guide
CHEM 1220 Alternate Exam #3 Form
Chapter 21
21.1 Radioactivity
21.2 Patterns of Nuclear Stability
21.3 Nuclear Transmutations
21.4 Rates of Radioactive Decay
21.6 Energy Changes in Nuclear Reactions
21.7 & 21.8 Nuclear Power
Blog
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Chemistry 1220
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Lecture #1: January 7-8
Lecture #2: January 9-10
Lecture #3: January 14-15
Lecture #4: January 16-17
Lecture #5: January 22-23
Lecture #6: January 24-28
Lecture #7: January 29-30
Lecture #8: January 31-February 1
Lecture #9: February 5-6
Lecture #10: February 7-10
Lecture #11: February 12
Lecture #12: February 13-14
Lecture #13: February 18-19
Lecture #14: February 20-21
Lecture #15: February 25-26
Lecture #16: February 27-28
Lecture #17: March 4-5
Lecture #18: March 6-7
Lecture #19: March 18-19
Lecture #20: March 20-21
Lecture #21: March 25-26
Lecture #22: March 27-28
Lecture #23: April 1-2
Lecture #24: April 3-4
Lecture #25: April 8-9
Lecture #26: April 10-11
Lecture #27: April 15-16
Last Lecture
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