PODCAST · education
CHEMDUNN
by CHEMDUNN
The podcast that brings your chemistry textbook to life through lively conversations! Our dynamic hosts break down complex topics and concepts into relatable, everyday terms, making learning chemistry accessible and enjoyable for everyone—especially for those that are needing to ace that next exam.Each episode features insightful discussions about common core topics in the typical chemistry curriculum. Say goodbye to monotonous lectures. Get ready to laugh, learn, and ... maybe ... enjoy chemistry—one conversation at a time!
Episodes
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Topic: Le Chatelier's Principle
This episode covers Le Chatelier's Principle, explaining how a chemical system at equilibrium will always shift its position to counteract and undo an external "stress." It explores three primary stressors: concentration changes, where the system shifts away from what is added and toward what is...
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Topic: pH Scale
This episode breaks down the fundamentals of the pH scale, explaining its concept, mathematics, and real-world applications. It defines pH as the "power of hydrogen," a logarithmic measurement of hydrogen ion concentration ([H+]) where each unit represents a tenfold change in acidity or basicity....
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Topic: K vs Q
This episode introduce the Reaction Quotient (Q) and explain how it serves as a "GPS" to predict whether a chemical reaction will shift toward products or reactants to reach its destination, the Equilibrium Constant (K). While both share the identical mathematical expression of products over...
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Topic: ICE Tables
This episode introduce the ICE table (Initial, Change, Equilibrium) as a foundational tool for tracking concentration changes and calculating the equilibrium constant (K) in chemical reactions. It explain how to construct the table by using initial concentrations, applying stoichiometry and a...
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Topic: Differential Rate Law
In this episode, we explore the fundamentals of differential rate laws — the mathematical expressions that describe how the speed of a chemical reaction depends on the concentration of its reactants. We break down the general rate law equation, Rate = k[A]^m[B]^n, explaining the role of the rate...
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Topic: Molecular Polarity
This episode explores molecular polarity, explaining how electronegativity differences create polar bonds and why molecular geometry determines overall polarity. The hosts distinguish between bond polarity and molecular polarity, showing how symmetrical molecules like CO₂ and CH₄ are nonpolar...
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Topic: Faraday's Law
Faraday's Law relates the amount of chemical change in an electrolytic cell to the total electric charge passed through it. The amount of product is directly proportional to the charge. Using Faraday's constant (96,485 C/mol/e-), the charge converts to moles of electrons, which then relates to...
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Topic: Electrolysis
Electrolysis uses electrical energy to drive a nonspontaneous redox reaction, the opposite of a voltaic cell. An electrolytic cell requires a power source, where the anode is positive and the cathode is negative (reversed polarity from voltaic). The process is used to split molten salts or…
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Topic: Cell potential (NON-standard conditions) / Nernst Equation
This episode explains how to calculate non-standard cell potentials (voltage) using the Nernst equation. Real-life batteries operate under non-standard conditions where concentrations change, causing voltage to drop. The equation shows that as the reaction quotient Q increases (more product)…
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Topic: Cell Potential (Standard Conditions)
The standard cell potential (E°cell) for a voltaic cell is calculated using E°cell = E°cathode − E°anode, where E° values come from standard reduction potential tables. A positive E°cell indicates a spontaneous reaction capable of producing electricity. Reduction occurs at the cathode (higher...
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Topic: Voltatic (or Galvanic) Cells
Voltaic (or Galvanic) cells convert chemical energy into electrical energy using a spontaneous redox reaction. The reaction is split into two half-cells: the anode (where oxidation occurs) and the cathode (where reduction occurs). Electrons flow through an external wire from the anode to the...
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Topic: Balancing Redox Reactions
To balance redox reactions, they are split into oxidation and reduction half-reactions. The goal is to conserve both mass and charge. In acidic solutions, H2O balances oxygen, and H+ balances hydrogen. In basic solutions, the reaction is first balanced as if it were acidic, and then OH- ions are...
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Topic: Intro Redox & Oxidation Numbers
Redox (Oxidation-Reduction) reactions involve the transfer of electrons. Oxidation is the loss of electrons (LEO), and Reduction is the gain of electrons (GER). These processes always occur simultaneously. Oxidation numbers are bookkeeping tools used to track this transfer. An increase in the...
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Topic: Gibb's Free Energy
Gibbs Free Energy (ΔG) predicts reaction spontaneity using the equation: ΔG = ΔH - TΔS. A negative ΔG means the reaction is spontaneous (happens on its own). This value combines enthalpy (ΔH), which is heat change, and entropy (ΔS), which is disorder. The reaction is spontaneous only at certain...
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Topic: Entropy
This episode defines entropy (S) as a measure of the disorder or the number of ways energy and matter can be arranged in a system. Entropy naturally increases when a substance changes phase from solid to liquid to gas, as temperature increases, or when a reaction produces more gas molecules. The...
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Topic: pH of Salts
This episode explains that not all salts are neutral; their pH depends on the origin of their ions. A salt is formed from an acid-base neutralization reaction. When dissolved, ions from weak acids or weak bases can undergo ion hydrolysis—reacting with water to form H3O+ (acidic) or OH- (basic)...
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Topic: Indicators
Indicators are weak acids or bases that change color based on the solution's pH. The color change happens because the indicator exists in an equilibrium between two forms, each having a different color. The goal is to choose an indicator whose transition range closely matches the equivalence…
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Topic: Titrations
This episode introduces titration, a technique used to determine an unknown concentration (analyte) using a solution of known concentration (titrant). The focus is the strong acid–strong base titration, where reactants fully dissociate. The equivalence point is reached when moles of H+ equal…
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Topic: Buffers
A buffer is a solution that resists changes in pH when small amounts of acid or base are added. It must contain a weak acid and its conjugate base (or a weak base and its conjugate acid). When acid (H+) is added, the conjugate base absorbs it; when base (OH-) is added, the weak acid neutralizes…
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Topic: Ka and Kb
Weak acids and bases partially dissociate in water, establishing equilibrium. Their strength is measured by the acid dissociation constant (Ka) and the base dissociation constant (Kb). A larger Ka or Kb indicates a stronger species. The constants are linked by the vital relationship: Ka x Kb =…
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Topic: Strong Acids & Strong Bases
The episode defines strong acids and strong bases as those that completely ionize (dissociate) in water, meaning 100% of the molecules break apart. This strength is independent of concentration. Memorizing the few common strong acids (like HCl and H2SO4) and strong bases (Group 1 and 2…
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Topic: Autoionization of Water
The autoionization of water, where H2O acts as both an acid and a base, is the focus of this episode. This process generates H3O+ and OH- ions. The equilibrium constant for this reaction is the Ion-Product Constant for Water, Kw, expressed as Kw = [H3O+][OH-]. At 25°C, the value of Kw is 1.0 x...
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Topic: Conjugate Acids & Bases
This episode discusses Conjugate Acid-Base Pairs as a necessary outcome of the Brønsted-Lowry definition. When an acid donates a proton (H+), it forms its conjugate base; when a base accepts a proton, it forms its conjugate acid. These pairs always differ by exactly one proton. Crucially, the...
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Topic: Definitions of Acids & Bases
Acids and bases are fundamental chemical concepts defined by how they behave in solution. The Arrhenius definition states that acids produce H+ ions and bases produce OH- ions in water. A broader view is the Brønsted-Lowry definition, where an acid is a proton (H+) donor and a base is a proton...
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Topic: Calculating Equilibrium Constant (K)
This episode focuses on the Equilibrium Constant (K), which mathematically quantifies the position of a chemical equilibrium. K is defined by the expression: Products over Reactants, where the molar concentration of each substance, represented by brackets [ ], is raised to the power of its...
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Topic: Chemical Equilibrium
This episode introduces chemical equilibrium, defining it as the point where the rate of the forward reaction equals the rate of the reverse reaction. This process is dynamic, meaning the reaction hasn't stopped, but the concentrations of all substances have become constant, though not…
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Topic: Rate Comparisons
This episode explains rate comparisons in chemical kinetics, focusing on how the rate of change for each substance in a chemical reaction is related through the stoichiometry of the balanced equation. It introduce a general rate expression where the rate of change in concentration for each…
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Topic: Integrated Rate Law
This episode demystifies the Integrated Rate Laws, the essential chemical kinetics equations that allow chemists to predict the exact concentration of a reactant at any given time. While standard rate laws show instantaneous speed, the integrated versions, derived using calculus, link...
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Topic: Bond Enthalpies
This episode explains how to calculate the enthalpy of a reaction (ΔHrxn) using average bond enthalpies. This method is based on the principle that breaking old bonds requires energy and forming new bonds releases energy. The core formula is ΔHrxn=Σ(bonds broken)−Σ(bonds formed), where "bonds...
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Topic: Enthalpies of Formation
This episode explains how to calculate the enthalpy change of a reaction using standard enthalpies of formation, which are values representing the energy required to form one mole of a compound from its elements. The episode introduces the "products minus reactants" formula. It emphasizes a key...
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Topic: Calorimetry
This episode explains calorimetry, the science of measuring heat transfer, based on the Law of Conservation of Energy. It demonstrates how to use the formula q=m⋅c⋅ΔT to solve for unknown variables in two common scenarios. First, the specific heat of an unknown metal is determined by measuring…
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Topic: Hess's Law
This episode explains Hess's Law, a method for calculating the enthalpy change of a reaction by treating it as a sum of other known reactions. It presents three key rules for manipulating these equations: reversing an equation changes the sign of its ΔH, multiplying an equation by a coefficient...
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Topic: Specific Heat Capacity
This episode provides a clear, concise summary of specific heat capacity and its use in thermochemistry. It introduces the fundamental concept that specific heat capacity, represented by the symbol c, is a measure of how much thermal energy a substance can store. The episode focuses on the key...
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Topic: Heating & Cooling Curves
A heating or cooling curve graphically represents the relationship between heat, temperature, and the physical state of a substance. The curve has sloped sections where the temperature changes as heat is added, and the substance remains in a single phase (solid, liquid, or gas). The formula…
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Topic: Thermochemical Equations
Enthalpy (ΔH) is the heat change in a chemical reaction and can be shown in two ways: either written with the equation or included as a reactant or product. A negative ΔH signifies an exothermic reaction that releases heat, which can be shown as a product in the equation. A positive ΔH signifies…
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Topic: Energy Diagrams
Energy diagrams are a visual tool to understand the energy changes in chemical reactions. They map the reaction from reactants to products, with the vertical axis showing potential energy. The difference in energy between the start and end points is the enthalpy change (ΔH). A peak in the diagram...
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Topic: Heat Flow
Heat transfers in three primary ways: conduction, convection, and radiation. Conduction is direct heat transfer through physical contact, common in solids like a metal spoon in hot soup. Convection is heat transfer through the movement of fluids (liquids or gases), where warmer, less dense fluid...
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Topic: Colligative Properties
Colligative properties are solution properties that depend on the number of solute particles, not their identity. The episode focuses on freezing point depression and boiling point elevation. In these calculations, m is molality (moles of solute per kilogram of solvent), Kf and Kb are...
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Topic: Complete and Net Ionic Equations
Ionic equations provide a more accurate view of reactions in solution than a simple chemical equation. A complete ionic equation shows all dissolved ionic compounds as separate ions, while solids, liquids, and gases remain intact. From this, a net ionic equation is derived by removing spectator...
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Topic: Dilution
Dilution is the process of lowering a solution's concentration by adding more solvent while keeping the amount of solute constant. This process is governed by the equation M1V1=M2V2, where M is molarity and V is volume, with subscripts 1 and 2 referring to the initial stock solution and the...
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Topic: Real vs. Ideal Gases
Real gases deviate from ideal behavior under high pressure and low temperature because the assumptions of the ideal gas law break down. At high pressure, the volume of gas molecules themselves becomes significant, making the gas less compressible than predicted. At low temperature, weak…
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Topic: Maxwell-Boltzmann Distribution
The Maxwell-Boltzmann distribution shows that molecules in a gas don't all move at the same speed, but rather follow a predictable statistical pattern. The curve representing this distribution shows a peak for the most probable speed and a long tail indicating that some molecules move very fast....
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Topic: Graham's Law
Graham's Law states that a gas's rate of diffusion or effusion is inversely proportional to the square root of its molar mass. In simple terms, lighter gases move faster than heavier ones. This relationship comes from the fact that all gases at the same temperature have the same average kinetic...
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Topic: Dalton's Law of Partial Pressure
This episode explains Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of each gas's individual pressure. This works because, at the molecular level, each gas acts independently. The episode gives examples, including collecting a gas over water,...
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Topic: Kinetic Molecular Theory
This episode on kinetic molecular theory (KMT) explains gas behavior through five fundamental postulates. These are: gas molecules are in constant, random motion; they have negligible volume; there are no intermolecular forces between them; all collisions are perfectly elastic; and their average...
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Topic: Ideal Gas Law
This episode explains the Ideal Gas Law as a universal equation that combines all the individual gas laws. It introduces the equation's components—pressure (P), volume (V), moles (n), the universal gas constant (R), and absolute temperature (T) in Kelvin—and emphasize the importance of using the...
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Topic: Gas Laws (Part 2)
This episode explains three additional gas laws including the unifying Combined Gas Law. It first introduces Gay-Lussac's Law, which states that pressure is directly proportional to absolute temperature at constant volume. Next, it covers Avogadro's Law, which describes the direct relationship...
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Topic: Gas Laws (Part 1)
This episode explains two fundamental gas laws: Boyle's Law and Charles's Law. It explains that Boyle's Law describes the inverse relationship between pressure and volume at constant temperature, using a scuba diving example to illustrate how an increase in pressure causes a decrease in volume....
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Topic: Solution Stoichiometry
This episode explains how to perform solution stoichiometry using molarity as the key conversion factor. It breaks down the process into a simple flow: use molarity to convert solution volume to moles, apply the mole ratio from the balanced equation, and then convert to the final requested units....
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Topic: Gas Stoichiometry (Non-Standard Conditions)
This episode explains how to perform non-STP gas stoichiometry using the Ideal Gas Law (PV=nRT). It emphasizes that this method is crucial for real-world applications where gases are not at standard conditions, rendering the 22.4 L/mol conversion factor invalid. The episode demonstrates how to…
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ABOUT THIS SHOW
The podcast that brings your chemistry textbook to life through lively conversations! Our dynamic hosts break down complex topics and concepts into relatable, everyday terms, making learning chemistry accessible and enjoyable for everyone—especially for those that are needing to ace that next exam.Each episode features insightful discussions about common core topics in the typical chemistry curriculum. Say goodbye to monotonous lectures. Get ready to laugh, learn, and ... maybe ... enjoy chemistry—one conversation at a time!
HOSTED BY
CHEMDUNN
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How many episodes does CHEMDUNN have?
CHEMDUNN currently has 119 episodes available on PodParley. New episodes are automatically indexed when they're published to the podcast feed.
What is CHEMDUNN about?
The podcast that brings your chemistry textbook to life through lively conversations! Our dynamic hosts break down complex topics and concepts into relatable, everyday terms, making learning chemistry accessible and enjoyable for everyone—especially for those that are needing to ace that next...
How often does CHEMDUNN release new episodes?
CHEMDUNN publishes regularly with 119 episodes available. Check the episode list for the typical release schedule.
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You can listen to CHEMDUNN on PodParley by clicking any episode. We provide an embedded audio player for direct listening, and you can also subscribe via your preferred podcast app using the RSS feed.
Who hosts CHEMDUNN?
CHEMDUNN is created and hosted by CHEMDUNN.
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