Chapter 1: Introduction: Matter, Energy, and Measurement
- Burning Iron and Magnesium
- Contrast the results of holding an iron strip and a magnesium ribbon in a flame
- Burning Iron and Magnesium.pdf
- Changes of State
- Pour liquid nitrogen into a beaker to demonstrate a variety of physical changes: the boiling of N2 (ℓ), the deposition of H2O (g) as H2O (s) on the outside of the beaker, and the melting of H2O (s) to H2O (ℓ) as the beaker eventually warms up again
- Changes of State
- Combustion of Methane Bubbles
- Ignite large soap bubbles filled with CH4 – this gets a “wow!” even from jaded college students! Then ignite a tower of methane-filled soap bubbles to produce a pillar of flame 3-5m high. As seen on Mythbusters.
- Combustion of Methane Bubbles.pdf
- Methane Bubbles XTREME.pdf
- Density of Coke vs. Diet Coke
- Drop unopened cans of regular Coke and Diet Coke into an aquarium filled with water. Coke sinks and Diet Coke floats – challenge the class to postulate an explanation.
- Density of Coke vs. Diet Coke.pdf
- Dry Ice Sublimation
- Make the sublimation of dry ice “visible” by dropping a piece of dry ice in a beaker of water. Then place a piece of dry ice in a glove, tie it off, and allow the dry ice to sublime, inflating the glove.
- Dry Ice Sublimation.pdf
- Halogens
- Display flasks containing the halogens chlorine, bromine, and iodine. Freeze the bromine flask in liquid nitrogen to show condensation of the vapor and freezing of the liquid.
- Halogens.pdf
- Heterogeneous and Homogeneous Mixtures
- Add solid NaCl to solid CuSO4 in a beaker and stir – this is a heterogeneous mixture. Add water to the beaker and stir – a homogeneous mixture (a solution) results.
- Heterogeneous and Homogeneous Mixtures.pdf
- Precision and Accuracy
- Using the document camera, measure a brass rod using rulers divided every 5 units, every 1 unit, and every 0.1 unit to introduce the concepts of precision and accuracy or significant figures
- Precision and Accuracy.pdf
Chapter 2: Atoms, Molecules, and Ions
- Cathode Ray Tube and Pinwheel
- Demonstrate the deflection of an electron beam with a magnet (CRT), and the particle nature of electrons by using a beam of electrons to spin a pinwheel. (Use the Geiger counter to show students the radiation that the CRT emits radiation (x-rays))
- Cathode Ray Tube and Pinwheel.pdf
- Conservation of Mass
- Demonstrate the law of conservation of mass with the colorful reaction of Co(NO3)2 (aq) and Na2CO3 (aq), using the document camera to project the digital readout of a balance on the screen before and after the reaction.
- Conservation of Mass.pdf
- Detection of Radioactivity
- Use a Geiger counter to demonstrate the radioactivity (or lack thereof) of several substances, including NaI, NaCl and uranium salts. A sheet of lead is provided to display the ability of lead to block radiation.
- Fiesta ware, and Uranium plate also available
- Detection of Radioactivity.pdf
- Gas Discharge Tubes of the Noble Gases
- Show that different gases give different colors when subjected to an electric discharge (the noble gases and hydrogen)
- Gas Discharge Tubes of the Noble Gases.pdf
- Periodic Properties
- Add pieces of Li, Na, K, Mg, and Ca, to beakers of water to observe the reactivity of metals from different parts of the periodic table.
- Periodic Properties.pdf
Chapter 3: Chemical Reactions and Reaction Stoichiometry
- Avogadro’s Law
- Three flasks containing equal amounts of acetic acid are fitted with balloons containing different amounts of NaHCO3; mix the reagents by lifting and shaking the balloons: the balloons will inflate with CO2 to a volume proportional to the number of moles produced, in accordance with Avogadro’s law.
- Avogadro’s Law.pdf
- Burning Magnesium Ribbon
- Burn a piece of magnesium ribbon in air to produce MgO
- Burning Magnesium RIbbon.pdf
- Combustion of Ethanol Vapors
- Compare the combustion of ethanol in a small dish to the combustion of ethanol vapors. When liquids are flammable, their vapors are explosive!
- Combustion EtOH Vapor.pdf
- Combustion vs. Fire
- Contrast the burning of ethanol with the burning of magnesium ribbon. One is combustion and the other is not. Does fire always mean combustion?
- Combustion vs. fire.pdf
- Combustion of Magnesium in Dry Ice
- Once ignited, magnesium burns without oxygen in a block of dry ice. The single replacement reaction results in magnesium oxide and a ball of solid carbon.
- Combustion of Magnesium in Dry Ice.pdf
- Electrolysis of Water
- Electrolyze water (Na2SO4 solution with indicator) in the Hoffman apparatus to decompose it into its component elements, hydrogen and oxygen.
- Electrolysis of Water.pdf
- Mole Samples
- Show mole samples of various elements and compounds in bottles
- Potassium and Water
- Drop a piece of potassium into an aquarium containing water and phenolphthalein to produce H2 (g) and KOH (aq) – the heat of reaction ignites the H2 (g) and a lavender flame is observed (from the K+), while the indicator turns pink from the formation of KOH.
- Potassium and Water.pdf
Chapter 4: Reactions in Aqueous Solution
- Acids and Bases
- Add drops of 0.1 M NaOH to a magnetically stirred solution of water and universal indicator until it turns blue, then add drops of 0.1 M HCl until the solution turns orange.
- Acids and Bases.pdf
- Conductivity Tester Demos
- Sugar and Salt – Use two conductivity testers with light bulbs to contrast the conductivity of d-H2O, sugar solution, and NaCl (aq).
- Strong and Weak Acids and Bases – Use two conductivity testers with light bulbs to contrast the conductivity of weak and strong electrolytes: acetic acid and HCl (aq), and/or NH3 (aq) and NaOH (aq)
- Conductivity Tester Demos 1.pdf
- Lead Nitrate and Potassium Iodide – Solid and Liquid Reactions
- Mix equal amounts of Pb(NO3)2 (s) and KI (s) in a test tube and shake thoroughly to show formation of yellow PbI2 (s). Contrast this with the results of mixing Pb(NO3)2 (aq) and KI (aq)
- Lead Nitrate and Potassium Iodide.pdf
- Metal Redox Reactions
- Copper and Zinc – Immerse a strip of Cu in ZnSO4 (aq) and compare to a strip of Zn in CuSO4 (aq).
- Copper Star Oxidation – Immerse copper wire in AgNO3 (aq). This is best done on the document camera over a lengthy period of time so students can observe the continuing reaction.
- Metal Redox Reactions.pdf
- Multiple Oxidation States of Vanadium
- Shake a solution of ammonium meta-vanadate with a Zn-Hg amalgam to reduce the vanadium from +5 to +4 to +3 to +2 with different colors at each stage
- Multiple Oxidation States of Vanadium.pdf
- Precipitation Reactions
- mix two pairs of solutions to show that some combinations produce precipitate and some give no net reaction.
- Precipitation Reactions
Chapter 5: Thermochemistry
- Combustion of Candy
- Contrast the oxidation of sucrose in the body (by eating some candy) with the oxidation of sucrose by KClO3 (as shown by dropping some candy into molten KClO3, producing steam and a lavender flame. Body temperature is ~37°C, and the melting point of KClO3 is 368°C.
- Combustion of Candy.pdf
- Combustion of Methane Bubbles
- Ignite large soap bubbles filled with CH4 – this gets a “wow!” even from jaded college students! Then ignite a tower of methane-filled soap bubbles to produce a pillar of flame 3-5m high. As seen on Mythbusters.
- Combustion of Methane Bubbles.pdf
- Methane Bubbles XTREME.pdf
- Crystallization of Supersaturated Sodium Acetate
- Add a tiny crystal of sodium acetate to a 2 L flask of a super-saturated solution to cause the solid to crystallize out, leaving almost no liquid – this demonstration is beautiful and dramatic, as well as being quite exothermic.
- Crystallization of Supersaturated Sodium Acetate.pdf
- Endothermic Reaction
- Shake solid Ba(OH)2 • 8 H2O with solid NH4NO3 to produce an aqueous mixture of Ba(NO3)2 (s) and NH3 (aq). The reaction is endothermic enough to freeze the flask to a wet piece of cardboard. Alternatively, a digital thermometer can be used to record the temperature change.
- Endothermic Reaction.pdf
- Luminol
- Pour solutions of luminol and H2O2 into a tall glass spiral to produce a beautiful chemiluminescent reaction. The light-emitting species is the dicarboxylate ion, aminophthalate, the product of the oxidation of luminol with H2O2
- Luminol Reaction.pdf
- Sound
- Tap a very small pile of red phosphorus and KClO3 with a hammer to show a reaction that produces light, sound, and heat, and recreates on a larger scale the reaction that occurs when you strike a match.
- Thionine Reaction
- Hold a solution of thionine and FeSO4 in front of a bright light to show the reduction of thionine from a violet form to a colorless form; this is an endothermic reaction that absorbs light energy.
- Thionine.pdf
Chapter 6: Electronic Structure of Atoms
- Atomic Spectra: Flame Tests
- Introduce various metal salts (e.g. NaCl, SrCl2, CuCl2) into an open flame to produce brilliant colors associated with exciting metal cations
- Flame Tests.pdf
- Fireworks Balloons
- Balloons filled with hydrogen gas and various salts and elements produce colored fireballs when ignited.
- Fireworks Balloons.pdf
- Gas Discharge Tubes of the Noble Gases
- Show that different gases give different colors when subjected to an electric discharge (the noble gases and hydrogen)
- Gas Discharge tubes.pdf
- Pickle Electrocutor
- Run an electric current through a dill pickle using a special apparatus to show students that the brine in the pickle conducts electricity, and the current heats and excites the sodium atoms present to a higher energy level. The emission of photons as the sodium returns to the ground state accounts for the yellow color of the light.
- Pickle Electrocutor.pdf
- Orbital Models
Chapter 7: Periodic Properties of the Elements
- Acidic and Basic Oxides
- Dissolve several oxides (CaO, ZnO, CO2, P4O10) in water containing universal indicator to show a range of basic and acidic oxides
- Acidic and Basic Oxides.pdf
- Periodic Properties
- Add pieces of Li, Na, K, Mg, and Ca, to beakers of water and phenolphthalein to observe the reactivity of metals from different parts of the periodic table.
- Periodic Properties.pdf
Chapters 8 and 9: Basic Concepts of Chemical Bonding & Molecular Geometry and Bonding Theories
- Paramagnetic O2
- Demonstrate the paramagnetism of liquid oxygen by pouring first N2(ℓ), then O2(ℓ) between the poles of a powerful magnet on the overhead projector or document
camera. - Paramagnetic O2.pdf
- Demonstrate the paramagnetism of liquid oxygen by pouring first N2(ℓ), then O2(ℓ) between the poles of a powerful magnet on the overhead projector or document
- Polarity and Geometry
- Show the dependence of dipole-dipole forces on geometry by contrasting the effect of a charged rod on streams of H2O and “CCl4” (actually hexane) flowing from burets.
- Polarity and Geometry.pdf
- VSEPR Shapes
- Use ball-and-stick models to illustrate the VSEPR shapes and sub-shapes.
- Linear
- Trigonal Planar – trigonal planar and bent 120°
- Tetrahedral – tetrahedral, trigonal pyramidal, and bent 109°
- Trigonal Bipyramidal – trigonal bipyramidal, see-saw, T-shaped, and linear
- Octahedral – octahedral, square pyramidal, square planar
- Use ball-and-stick models to illustrate the VSEPR shapes and sub-shapes.
Chapter 10: Gases
- Avogadro’s Law
- Three flasks containing equal amounts of acetic acid are fitted with balloons containing different amounts of NaHCO3; mix the reagents by lifting and shaking the balloons: the balloons will inflate with CO2 to a volume proportional to the number of moles produced, in accordance with Avogadro’s law
- Avogadro’s Law.pdf
- Boiling Water at Room Temperature
- Show water boiling at room temperature in a beaker in an evacuated bell jar, then put your hand in the water after boiling to convince students of
its low temperature. - Boiling water at Room Temp.pdf
- Show water boiling at room temperature in a beaker in an evacuated bell jar, then put your hand in the water after boiling to convince students of
- Charles’ Law
- Pour liquid nitrogen over a balloon to show that a decrease in T is accompanied by a decrease in V.
- Charles’ Law.pdf
- Graham’s Law of Diffusion
- Allow concentrated NH3 and concentrated HCl to vaporize and meet in a horizontal glass tube, forming a ring of NH4Cl.
- Graham’s Law of Diffusion.pdf
- Marshmallow Snowman
- Demonstrate the effect a decrease in P has on V by placing a marshmallow snowman in a bell jar and then evacuate the jar.
- Marshmallow Snowman.pdf
- Molar Volume
- Place 28 g of liquid nitrogen in a special cube balloon and tie off; after the N2 has vaporized, compare the volume of the bag to the 22.4 L box
- Molar Volume.pdf
- Squashing pop cans with atmospheric pressure
- Use atmospheric pressure to squash pop cans
- Squashing pop cans with atmospheric pressure.pdf
- Lake Nyos Demo
- CO2 is heavier than air and can extinguish candle flames
- Lake Nyos.pdf
Chapter 11: Liquids and Intermolecular Forces
- Comparing the Vapor Pressure of Two Liquids
- Show the effect of intermolecular forces on the vapor pressure of liquids by contrasting the vapor pressures of two isomers, diethyl ether and 1-butanol
- Comparing the Vapor Pressure of Two Liquids.pdf
- Effect of Pressure on the Melting Point of Ice
- Hang a wire weighted at both ends over a cylinder of ice; eventually the wire passes through the ice and the weights fall, leaving the ice intact. The ice below the wire melts due to pressure from the weights, and the water above the wire refreezes as the pressure is relieved.
- Effect of Pressure on MP of ice.pdf
- Halogens
- Display flasks containing the halogens chlorine, bromine, and iodine.
- On request, you can order a special flask of bromine that can be frozen in liquid nitrogen
- Halogens
- Negative Volume of Mixing
- Because of hydrogen bonding between water and absolute ethanol, when two identical volumes are mixed, the total volume is less than the sum of the two volumes.
- Negative Volume of Mixing.pdf
- Polarity and Geometry
- Show the dependence of dipole-dipole forces on geometry by contrasting the effect of a charged rod on streams of H2O and “CCl4” (actually hexane) flowing from burets.
- Polarity and Geometry.pdf
- Triple Point Demo
- Demonstrate the existence of three phases of CO2 at the triple point by adding crushed dry ice to a clear acrylic tube fitted with a pressure gauge and a release valve.
- Triple Point Demo.pdf
- Viscosities of Liquids
- Compare the viscosity of various liquids with a viscosity apparatus and relate the differences to strength of attractive forces.
- Viscosities of Liquids
- Vapor Pressure Lowering of Solutions
- Raoult’s Law states that the vapor pressure of a solution is lower than the vapor pressure of the pure solvent. Use a manometer to compare the vapor pressure of water to that of a sodium sulfate (Na2SO4) solution
- Vapor Pressure Lowering of Solutions.pdf