Chemistry Video & Text Solutions For College

Ch.1 - Intro to General Chemistry

The Scientific Method Mixtures Filtration Scientific Notation Accuracy & Precision Standard Deviation, Mean, Median & Mode Metric Prefixes Significant Figures Energy, Heat and Temperature Physical & Chemical Changes Physical & Chemical Properties Types of Energy Dimensional Analysis Density

Ch.2 - Atoms & Elements

Periodic Table Mole Concept Calculating Molar Mass Isotopes Mass Spectrometry Subatomic Particles Atomic Theory Oil Drop Experiment Gold Foil Experiment

Ch.3 - Chemical Reactions

Ionic and Covalent Bonds Molecular Models Metal Alloys Polyatomic Ions Naming Covalent Compounds Naming Ionic Compounds Naming Acids Empirical Formula Combustion Analysis Mass Percent Formula Balancing Chemical Equations Functional Groups in Chemistry Stoichiometry Limiting Reagent Limiting Reactant Percent Yield

BONUS: Lab Techniques and Procedures

Laboratory Materials Distillation & Floatation Test for Ions and Gases

Ch.4 - Chemical Quantities & Aqueous Reactions

Molarity Normality & Equivalent Weight Solution Stoichiometry Dilution Solubility Rules Net Ionic Equations Net Ionic Equation Electrolytes Redox Reaction Balancing Redox Reactions Redox Reactions Oxidation Reduction (Redox) Reactions Calculate Oxidation Number Types of Chemical Reactions Activity Series

Ch.5 - Gases

Pressure Units Manometer Partial Pressure The Ideal Gas Law Chemistry Gas Laws Ideal Gas Law Ideal Gas Law Density Ideal Gas Law Molar Mass Standard Temperature and Pressure Gas Stoichiometry Collecting Gas Over Water Effusion Root Mean Square Speed Kinetic Molecular Theory Van der Waals Equation Kinetic Energy of Gases Velocity Distribution

Ch.6 - Thermochemistry

Units of Energy Internal Energy Endothermic & Exothermic Reactions Calorimetry Thermochemical Equation Hess's Law Enthalpy of Formation Enthalpy

Ch.7 - Quantum Mechanics

Electromagnetic Spectrum Wavelength and Frequency Diffraction vs Refraction The Particle Nature of Light Photoelectric Effect De Broglie Wavelength Heisenberg Uncertainty Principle Bohr Model Bohr and Balmer Equations Wave Function Introduction to Quantum Mechanics Dimensional Boxes

Ch.8 - Periodic Properties of the Elements

Electron Configuration Orbital Diagrams Paramagnetic and Diamagnetic Coulomb's Law Effective Nuclear Charge Quantum Numbers The Spin Quantum Number Orbital Shapes Periodic Trends Atomic Radius Periodic Trends: Atomic Radius Periodic Trends: Ionic Radius Periodic Trends: Ionization Energy Periodic Trends: Electron Affinity Periodic Trends: Metallic Character

Ch.9 - Bonding & Molecular Structure

Chemical Bonds Lattice Energy Lattice Energy Application Born Haber Cycle Dipole Moment Lewis Dot Structure Octet Rule Formal Charge Resonance Structures Bond Energy

Ch.10 - Molecular Shapes & Valence Bond Theory

Molecular vs Electron Geometry Bond Angles Electronegativity Hybridization Benzene Orbital Overlap Molecular Orbital Theory Bond Order Delocalized Electrons Homonuclear Diatomic Molecules Heteronuclear Diatomic Molecules

Ch.11 - Liquids, Solids & Intermolecular Forces

Molecular Polarity Intermolecular Forces Intermolecular Forces and Physical Properties Phase Diagram Heating and Cooling Curves Unit Cell Atomic, Ionic, and Molecular Solids Clausius-Clapeyron Equation

Ch.12 - Solutions

Solutions, Molarity and Intermolecular Forces Making Solutions Henry's Law Calculate Molarity Mass Percent Molality Mole Fraction ppm Boiling Point Elevation Freezing Point Depression Colloid The Colligative Properties

Ch.13 - Chemical Kinetics

Rate of Reaction Average Rate of Reaction Instantaneous Rate of Change Arrhenius Equation Energy Diagram Catalyst Michaelis-Menten Equation Reaction Mechanism Rate Law Integrated Rate Law Identifying Reaction Order Collision Theory

Ch.14 - Chemical Equilibrium

Chemical Equilibrium Equilibrium Expressions ICE Chart Le Chatelier's Principle The Reaction Quotient

Ch.15 - Acid and Base Equilibrium

Identifying Acids and Bases Strong Acids and Strong Bases Arrhenius Acid and Base Bronsted Lowry Acid and Base Conjugate Acids and Bases Amphoteric Lewis Acid and Base pH and pOH Strong Acid-Base Calculations Weak Acids Weak Bases Ka and Kb Ionic Salts Diprotic Acid Polyprotic Acid

Ch.16 - Aqueous Equilibrium

Buffer Henderson Hasselbalch Equation Acid and Base Titration Curves Weak Acid Strong Base Titrations Weak Base Strong Acid Titrations Equivalence Point Strong Acid Strong Base Titrations Titrations of Diprotic and Polyprotic Acids Acid Base Indicators Ksp Selective Precipitation Formation Constant

Ch. 17 - Chemical Thermodynamics

Spontaneous Reaction First Law of Thermodynamics Second and Third Laws of Thermodynamics Entropy Boltzmann Equation Gibbs Free Energy

Ch.18 - Electrochemistry

Redox Reaction Balancing Redox Reaction The Nernst Equation Faraday's Constant Galvanic Cell Cell Notation Standard Hydrogen Electrode Cell Potential Batteries and Electricity Electroplating Electrolysis of Water & Mixture of Ions

Ch.19 - Nuclear Chemistry

Radioactive Decay Alpha Decay Beta Decay Gamma Emission Electron Capture Positron Emission Band of Stability First Order Half Life Nuclear Fission Mass Defect Nuclear Fusion Nuclear Transmutation

Ch.20 - Organic Chemistry

Introduction to Organic Chemistry Structural Formula Stereoisomers Chirality Optical Isomers Hydrocarbon The Alkyl Group Naming Alkanes Naming Alkenes Naming Alkynes Organic Chemistry Nomenclature Alkenes and Alkynes Benzene Reactions Functional Groups Alcohol Reactions Polymer

Ch.22 - Chemistry of the Nonmetals

Hydrogen Atom Alkaline Earth Metals

Ch.23 - Transition Metals and Coordination Compounds

Transition Metals Transition Metals Electron Configuration Oxidation States of Transition Metals Coordination Complexes Naming Coordination Compounds Coordination Isomers Crystal Field Theory Colors of Complex Ions

Chemistry Solutions Library

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Q. How much heat (kJ) is needed to raise the temperature of 100.0 grams of water from 25.0°C to 50.0°C?

Q. In which reaction does kp = kc? a) NO(g) + O2(g) <--> N2O3(g) b) N2(g) + O2(g) <--> 2NO(g) c) CaCO3(s) <--> CaO(s) + CO2(g) d) N2...

Q. How do you balance CH3OH + O2 → CO2 + H2O?

Q. 1.95 g of H2 is allowed to react with 9.94 g of N 2, producing 1.56 g of NH 3. What is the theoretical yield in grams for this reaction under the g...

Q. What is the net ionic equation for the reaction between HF (a weak acid) and NaOH?

Q. How many electrons in an atom can have the n = 5, l = 2 designation?

Q. Which of the following set of quantum numbers is not allowed?a. n = 1, l = 0, m l = 0, ms = −1/2b. n = 3, l = 2, m l = −1, ms = 1/2c. n = 5, l = 2,...

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