Gases are everywhere, and this is good news and bad news for chemists. The good news: when they are behaving themselves, it's extremely easy to describe their behavior theoretically, experimentally, and mathematically. The bad news is they almost never behave themselves.
In this episode of Crash Course Chemistry, Hank tells how the work of some amazing thinkers combined to produce the Ideal Gas Law, how none of those people were Robert Boyle, and how the ideal gas equation allows you to find out pressure, volume, temperature, or number of moles. You'll also get a quick introduction to a few jargon-y phrases to help you sound like you know what you're talking about.

Chapters:
Ideal Gas Law Equation
Everyone But Robert Boyle
Ideal Gas Law to Figure Out Things
Jargon Fun Time

We don't live in a perfect world, and neither do gases - it would be great if their particles always fulfilled the assumptions of the ideal gas law, and we could use PV=nRT to get the right answer every time. Unfortunately, the ideal gas law (like our culture) has unrealistic expectations when it comes to size and attraction: it assumes that particles do not have size at all and that they never attract each other. So the ideal gas "law" often becomes little more than the ideal gas estimate when it comes to what gases do naturally. But it's a close enough estimate in enough situations that it's very valuable to know. In this episode, Hank goes through a bunch of calculations according to the ideal gas law so you can get familiar with it.

Chapters:
Large Size + Attraction to Others
Mendeleev to the Rescue
The Hindenburg Disaster
Helium vs. Hydrogen
Making Fire with Cotton and Your Fist

Have you ever been to a Demolition Derby? Then you have an idea of how molecular collisions happen. In this episode, Hank talks about collisions between molecules and atoms, activation energy, writing rate laws, equilibrium expressions, reactions mechanics, and rate-determining steps. And funnel cakes are AWESOME!

Chapters:
Collisions Between Molecules and Atoms
Activation Energy
Writing Rate Laws
Rate Laws and Equilibrium Expressions
Reaction Mechanisms
Rate-Determining Steps

In this episode of Crash Course Chemistry, Hank gives you the low down on things like London Dispersion Forces, Hydrogen Bonds, Cohesion, Adhesion, Viscosity, Capillary Action, Surface Tension, and why liquids are just... WEIRD!

Chapters:
London Dispersion Forces
Dipole-Dipole Forces
Hydrogen Bonds
Cohesion
Adhesion
Viscosity
Capillary Action
Surface Tension

In this episode, Hank talks about Network solids and Carbon and how you can actually create a Diamond from plain old Carbon... well, YOU probably can't unless you own a bunch of elephants. It's a long story. BUT, within you will learn about Solid Networks, Diamond and Graphite Network Structures, as well as Sheet and 3D Networks. It's not making diamonds from scratch, but it's still pretty cool!

Ever feel like there's an international team of bad guys changing all of the easily remembered chemical names and turning them into test-failing, number-infused, pain-in-the-neck names? Well... you're not wrong. IUPAC exists, but try to keep in mind that they're doing it for the greater good. In this episode, Hank talks about IUPAC, prefixes, suffixes, ranking, numbers for carbon chains, and cis or trans double bonds.

Chapters:
IUPAC
Every Organic Compound Has Only One Name
Prefixes
Suffixes
Ranking Functional Groups
Lowest Possible Numbers for Carbon Chains
Cis or Trans for Double Bonds

In this episode, Hank welcomes you to the new age, to the new age, welcome to the new age. Here he'll talk about transmutation among elements, isotopes, calculating half-life, radioactive decay, and spontaneous fission.

Continuing our look at Nuclear Chemistry, Hank takes this episode to talk about Fusion and Fission. What they mean, how they work, their positives, negatives, and dangers. Plus, E=mc2, Mass Defect, and Applications of Fission and Fusion in the real world!

Hank does his best to convince us that chemistry is not torture, but is instead the amazing and beautiful science of stuff. Chemistry can tell us how three tiny particles - the proton, neutron, and electron - come together in trillions of combinations to form ... everything. In this inaugural episode of Crash Course Chemistry, we start out with one of the biggest ideas in chemistry ever - stuff is made from atoms. More specifically, we learn about the properties of the nucleus and why they are important to defining what an atom actually is.

Chapters:
Intro
Einstein & Atoms
Composition of Atoms
Atomic Number
Isotopes
Relative Atomic Mass
Mass Number

In this episode of Crash Course Chemistry, Hank discusses what molecules actually look like and why, some quantum-mechanical three-dimensional wave functions are explored, he touches on hybridization, and delves into sigma and pi bonds.

Chapters:
Molecules: Clumpy Globs...
Quantum-Mechanical Three-Dimensional Wave Functions
S & P Orbital Hybridization
Sigma & Pi Bonds
Hybridized Orbitals

This week we continue to spend quality time with gases, more deeply investigating some principles regarding pressure - including John Dalton's Law of Partial Pressures, vapor pressure - and demonstrating the method for collecting gas over water.

Chapters:
Theory of the Atom
Adding up the Pressures
Mixing Vinegar & Baking Soda
Collecting Gas Over Water

We have learned over the past few weeks that gases have real-life constraints on how they move here in the non-ideal world. As with most things in chemistry (and also in life), how a gas moves is more complex than it seems at first. In this episode, Hank describes what it means when we talk about the velocity of a gas - to understand gas velocity, we have to know what factors affect it, and how. Hank also teaches you about effusion, diffusion, and concentration gradients, before showing off a cool experiment that physically demonstrates the things you have just learned. Sound exciting enough for you? Let's get started.

Chapters:
Net Velocity vs. Average Velocity
Effusion
Graham's Law
Diffusion
Concentration Gradients
Precipitation Reaction with Gases

Molecules come in infinite varieties, so in order to help the complicated chemical world make a little more sense, we classify and categorize them. One of the most important of those classifications is whether a molecule is polar or non-polar, which describes a kind of symmetry - not just of the molecule, but of the charge. In this edition of Crash Course Chemistry, Hank comes out for Team Polar and describes why these molecules are so interesting to him.

You'll learn that molecules need to have both charge asymmetry and geometric asymmetry to be polar, and that charge asymmetry is caused by a difference in electronegativities. You'll also learn how to notate a dipole moment (or charge separation) of a molecule, the physical mechanism behind like dissolves like, and why water is so dang good at fostering life on Earth.

Chapters:
Charge Asymmetry & Geometric Asymmetry
Difference in Electronegatives
Hank is Team Polar
Dipole Moment
Charge Separation of a Molecule
Like Dissolves Like
Water is Awesome

Did you know that Polymers save the lives of Elephants? Well, now you do! The world of Polymers is so amazingly integrated into our daily lives that we sometimes forget how amazing they are. Here, Hank talks about how they were developed, and the different types of Polymers that are common in the world today, including some that may surprise you.

A lot of ionic compounds dissolve in water, dissociating into individual ions. But when two ions find each other and form an insoluble compound, they suddenly fall out of the solution in what's called a precipitation reaction. In this episode of Crash Course Chemistry, we learn about precipitation, precipitates, anions, cations, and how to describe and discuss ionic reactions.

Chapters:
Precipitate Reactions
Determining Precipitates
Writing Precipitate Reactions
Calculating Molar Mass Equation

Hank bursts our ideal gas law bubble, er, balloon, and brings us back to reality, explaining how the constants in the gas law aren't all that constant; how the ideal gas law we've spent the past two weeks with has to be corrected for volume because atoms and molecules take up space and for pressure because they're attracted to each other; that Einstein was behind a lot more of what we know today than most people realize; and how a Dutch scientist named Johannes van der Waals figured out those correction factors in the late 19th century and earned a Nobel Prize for his efforts.

Chapters:
Constants in the Gas Laws Aren't all that Constant
The Ideal Gas Law has to be Corrected for Volume and Pressure
Einstein was the Bomb
Van Der Waals Equation
Never Give Up!

All the magic that we know is in the transfer of electrons. Reduction (gaining electrons) and oxidation (the loss of electrons) combine to form Redox chemistry, which contains the majority of chemical reactions. As electrons jump from atom to atom, they carry energy with them, and that transfer of energy is what makes all life on Earth possible.

In this episode, we talk about Silicon Valley's namesake and how network solids are at the heart of it all. Hank also discusses Solid-State Semiconductors, N-Type and P-Type Semiconductors, Diodes, Transistors, Computer Chips, and Binary Code. All from the same thing that makes up sand!

This week, Hank elaborates on why Fugu can kill you by illustrating the ideas of solutions and discussing molarity, molality, and mass percent. Also, why polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes. All that plus Henry's Law and why Coke = Burps.

Chapters:
Molarity, Molality, and Mass Percent
Polar Solvents Dissolve Polar Solutes
Nonpolar Solvents Dissolve Nonpolar Solutes
Henry's Law
Coke=Burps
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Chemists need stoichiometry to make the scale of chemistry more understandable - Hank is here to explain why and to teach us how to use it.

Chapters:
Atomic Mass Units
Moles
Molar Mass
Equation Balancing
Molar Ratios