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The 1827 Christmas Lectures
of Michael Faraday
Lecture #6
Metals and their Oxides -- Earths, Fixed Alkalines and Salts, &c
Chemists of the first half of the nineteenth century were engaged in an attempt to classify
the known substances. Chemistry was carried out exclusively on the macroscopic level and
because little was known of basic structure, all of the information was discussed in
macroscopic terms. Classification was achieved by making observations of physical
properties and of chemical reactions. In this sixth lecture of the Christmas series, Faraday
illustrated common characteristics of metals and organized and classified the various types
of compounds that metals form with oxygen.
Faraday believed that everything could be well understood if it could be directly observed.
For him, there was nothing too simple or too trivial to demonstrate to his audience. His
energy was boundless, his enthusiasm was contagious, and audiences flocked to his
demonstrations.
A lecturer should exert his utmost effort to gain completely the mind and attention of his
audience, and irresistibly make them join in his ideas to the end of the subject. He should
endeavor to raise their interest at the commencement of the lecture and by a series of
imperceptible graduations, unnoticed by the company, keep it alive as long as the subject
demands it.... A flame should be lighted at the commencement and kept alive with
unremitting splendor to the end.
The pedagogy used by Faraday in 1827 is still one of the most effective ways of teaching.
For the corresponding modern demonstrations, click on the icons
NOTE: In this lecture, the numbering of the original experiments
does not exactly match that of the modern demonstrations.
Metals - Oxides
.
Exp. 1: Metals
A table with an array of samples and materials is arranged near the speaker for
reference during the lecture. A chart with the printed names of some common
metals is displayed.
Exp. 2: Lustre
The lustre of clean pieces of silver, mercury, lead, gold, and steel is displayed. They
are placed near a piece of stone for comparison.
Exp. 3: Opacity
The opacity of metal is shown using a sheet of tin, tin foil, and the even thinner gold
leaf.
Exp. 4: Malleability
Malleability is shown using gold and silver leaf and ordinary metallic (tin) foil.
Copper wire is used as an example, also.
Exp. 5: Brittleness
Very fine wire of the type manufactured by Wollaston is exhibited. The reaction of
samples of antimony, bismuth, zinc, and lead to hammer blows illustrates brittleness.
Exp. 6: Tenacity
Iron and steel wires are hung with weights to show tensile strength. The strength of
inch square iron rods that support a bridge is shown.
Exp. 7: Conducting Power
Metal, wooden, and paper rods are placed in very hot and very cold water to show
conductivity.
Exp. 8: Weight
Samples of iron, lead, and gold are observed as heavy for their volume. They are
compared with samples of mercury and marble. Balls of iron and marble and a piece
of platinum are placed in a container of mercury.
Exp. 9: Heat
Crystals of lead, zinc, and antimony are heated and the changes observed.
Metals - Oxides
Exp. 10: Potassium in air
A piece of potassium is placed in air and ignited.
Exp. 11: Potassium in water
A piece of potassium is reacted with water.
Exp. 12: Zinc in candle flame
Zinc is placed in a crucible and heated in a candle flame. Powdered zinc is sprinkled
in a candle flame.
Exp. 13: Iron filing in lamp flame
Iron filings are sprinkled into the flame of a lamp.
Exp. 14: Oxides of silver and lead
Samples of silver and lead are heated on a charcoal block using a blowpipe flame.
Exp. 15: Tin oxide and rust compared
A sheet of tin is heated and the tarnish compared to the rusting of iron.
Exp. 16: Lead compared to lead sulfide
Lead sulfide is compared to lead.
Exp. 17: Iron in oxygen
Iron filings are heated in oxygen.
Exp. 18: Zinc foil in oxygen
Zinc foil is heated in oxygen.
Alkalies - Earths - and Acids
Exp. 19: Iron in oxygen
Iron is burnt in oxygen.
Exp. 20: Observe rust
A sample of rust is displayed and described.
Exp. 21: Oxides of copper
A sheet of copper is held in the fire and the colors of the oxides formed are
observed.
Exp. 22: Oxides of metals
Oxides of lead, tin, copper, and iron are exhibited.
Exp. 23: Table of oxides
Table of some oxides displayed.
Exp. 24: Observe oxides in water
Oxides of iron, copper, and tin are placed in water and lack of reaction observed.
Exp. 25: Metallic Acid
A solution of arsenious acid (oxide of arsenic) in water is tested with litmus paper.
Exp. 26: Zinc Oxide in acid
Oxide of zinc is dissolved in dilute sulfuric acid.
Exp. 27: White Vitriol, Blue Vitriol, Green Vitriol
Zinc sulphate, copper(II) sulphate, and iron(II) sulphate are exhibited in solid form.
Exp. 28: Copper sulphate precipitated by base
A solution of copper(II) sulphate is reacted with a solution of potassium hydroxide
precipitating copper hydroxide.
Exp. 29: Iron in Copper Sulfate
Iron is added to a solution of copper sulfate, and displacement demonstrated.
Neutralization of Metallic Acids
Exp. 30: Chromate Tungstate
Examples of chromates and tungstates are exhibited as examples of the salts of
metallic acids.
Exp. 31: Chromates Precipitated
Chromates of silver, mercury, lead, etc. are precipitated using solutions of metallic
acetates and potassium chromate.
Exp. 32: Properties of Potassium in water
A solution produced by the reaction of potassium with water is tested with turmeric
paper and is shown to be alkaline like ammonia. It feels soapy and neutralizes acids.
Exp. 33: Neutralization
An acid solution is neutralized with the potassium hydroxide solution using an
indicator.
Exp. 43: Properties of Hydrate of Potassium
Exhibit pure solid hydrate of potassium and compare to gaseous ammonia.
Exp. 44: Ashes of charcoal
Ashes of charcoal are extracted with water and the filtrate tested with turmeric
paper.
Exp. 45: Wood Ashes
Ashes from a wood fire are extracted with water and the filtrate tested with turmeric
paper.
Exp. 46: Display Nitre
A specimen of nitre, potassium nitrate, is exhibited.
Earths
Exp. 47: Forming oxides
Samples of marble and flint, are heated to form the oxide.
Exp. 48: Observe the oxides
Calcium oxide and flint, products of above calcination, are displayed and described.
Exp. 49: Basic properties of calcinate solutions
Solutions of lime and flint are tested with turmeric paper.
Exp. 50: Solubility of sand and limestone
Acid is added to sand and to limestone separately.
Exp. 51: Indicators in Sulfate solutions
Solutions of calcium sulfate, magnesium sulfate, and barium nitrate are tested with
indicator.
Exp. 52: Alkaline earths reacted with potassium carbonate
Solutions of alkaline earth salts are reacted with potassium carbonate.
Go to the modern lab demonstrations
.
Editors
Julianne Shepelavy, Michael Sixtus, Eric Stelter, Anne Stowe, Susana Suarez, Gail
Thompson, Kathleen Thompson, Robert Van Milligan and Alice Veyvoda.