Aurum Potestas Est

We as a race and a culture have a massive love affair with gold. It is the basis of our currency, the definitive mark of wealth and status, in some ways the bedrock of our society. We hoard it, we covet it, we hide it away except for special occasions, but we never really use it.

This is perhaps the strangest thing about gold; for something around which we have based our economy on, it is remarkably useless. To be sure, gold has many advantageous properties; it is the best thermal and electrical conductor and is pretty easy to shape, leading it to be used widely in contacts for computing and on the engine cover for the McLaren F1 supercar. But other than these, relatively minor, uses, gold is something we keep safe rather than make use of; it has none of the ubiquity nor usefulness of such metals as steel or copper. So why are we on the gold standard? Why not base our economy around iron, around copper, around praseodymium (a long shot, I will admit), something a bit more functional? What makes gold so special?

In part we can blame gold’s chemical nature; as a transition metal it is hard, tough, and a solid at room temperature, making it able to be mined, extracted, transported and used with ease and without degenerating and breaking too easily. It is also very malleable, meaning it can be shaped easily to form coins and jewellery; shaping into coins is especially important in order to standardise the weight of meta worth a particular amount. However, by far its most defining chemical feature is its reactivity; gold is very chemically stable in its pure, unionised, ‘native’ form, meaning it is unreactive, particularly with such common substances as; for this reason it is often referred to as a noble metal. This means gold is usually found native, making it easier to identify and mine, but is also means that gold products take millennia to oxidise and tarnish, if they do so at all. Therefore, gold holds its purity like no other chemical (shush, helium & co.), and this means it holds its value like nothing else. Even silver, another noble and comparatively precious metal, will blacken eventually and lose its perfection, but not gold. To an economist, gold is eternal, and this makes it the most stable and safe of all potential investments. Nothing can replace it, it is always a safe bet; a fine thing to base an economy on.

However, just as important as gold’s refusal to tarnish and protect is beauty is the simple presence of a beauty to protect. This is partly put down to the uniqueness of its colour; in the world around us there are many greens, blues, blacks, browns and whites, as well as the odd purple. However, red and yellow are (fire and a few types of fish and flower excepted) comparatively rare, and only four chemical elements that we commonly come across are red or yellow in colour; phosphorus, sulphur, copper and gold. And rusty iron but… just no. Of the others, phosphorus (red) is rather dangerous given its propensity to burst into flames, is also commonly found as a boring old white element, and is rather reactive, meaning it is not often found in its reddish form. Sulphur is also reactive, also burns and also readily forms compounds; but these compounds have the added bonus of stinking to high heaven. It is partly for this reason, and partly for the fact that it turns blood-red when molten, that brimstone (aka sulphur) is heavily associated with hell, punishment and general sinfulness in the Bible and that it would be rather an unpopular choice to base an economy on. In any case, the two non-metals do not have any of the properties that the transition metals of copper and gold do; those of being malleable, hard, having a high melting point, and being shiny and pwettiful. Gold edged out over copper partly for its unreactivity as explored above (after time copper loses its reddish beauty and takes on a, but also because of its deep, beautiful, lustrous finish. That beauty made it precious to us, made it something we desired and lusted after, and (combined with gold’s relative rarity, which could be an entire section of its own) made it valuable. This value allows relatively small amounts of gold to represent large quantities of worth and value, and justifies its use as coinage, bullion and an economic standard.

However, for me the key feature of gold’s place as our defining scale of value concerns its relative uselessness. Consider the following scenario; in the years preceding the birth of Christ, the technology, warfare and overall political situation of the day was governed by one material, bronze. It was used to make swords, armour, jewellery, the lot; until one day some smartarse figured out how to smelt iron. Iron was easier to work than bronze, allowing better stuff to be made, and with some skill it could be turned into steel. Steel was stronger as well as more malleable than bronze, and could be tempered to change its properties; over time, skilled metalsmiths even learned how to make the edge of a sword blade harder than the centre, making it better at cutting whilst the core absorbed the impact. This was all several hundred years in the future, but in the end the result was the same; bronze fell from grace and its societal value slumped. It is still around today, but it will never again enjoy its place as the metal that ruled the world.

Now, consider if that metal had, instead of bronze, been gold. Something that had been ultra-precious, the king of all metals, reduced to something that was merely valuable. It had been trumped by iron, and iron would have this connotation of being better than it; gold’s value would have dropped. In any economic system, even a primitive one, having the value of the substance around which your economy is based change in value would be catastrophic; when Mansa Musa travelled from Mali on a pilgrimage to Mecca, he stopped off in Cairo, then the home of the world’s foremost gold trade, and spent so much gold that the non-Malian world had never known about that the price of gold collapsed and it took more than a decade for the Egyptian economy to recover. If gold were to have a purpose, it could be usurped; we might find something better, we might decide we don’t need that any more, and thus gold’s value, once supported by those wishing to buy it for this purpose, would drop. Gold is used so little that this simply doesn’t happen, making it the most economically stable substance; it is valuable precisely and solely because we want it to be and, strange though it may seem, gold is always in fashion. Economically as well as chemically, gold is uniquely stable- the perfect choice around which to base a global economy.


The Red Flower

Fire is, without a doubt, humanity’s oldest invention and its greatest friend; to many, the fundamental example what separates us from other animals. The abilities to keep warm through the coldest nights and harshest winters, to scare away predators by harnessing this strange force of nature, and to cook a joint of meat because screw it, it tastes better that way, are incredibly valuable ones, and they have seen us through many a tough moment. Over the centuries, fire in one form or another has been used for everything from being a weapon of war to furthering science, and very grateful we are for it too.

However, whilst the social history of fire is interesting, if I were to do a post on it then you dear readers would be faced with 1000 words of rather repetitive and somewhat boring myergh (technical term), so instead I thought I would take this opportunity to resort to my other old friend in these matters: science, as well as a few things learned from several years of very casual outdoorsmanship.

Fire is the natural product of any sufficiently exothermic reaction (ie one that gives out heat, rather than taking it in). These reactions can be of any type, but since fire can only form in air most of such reactions we are familiar with tend to be oxidation reactions; oxygen from the air bonding chemically with the substance in question (although there are exceptions;  a sample of potassium placed in water will float on the top and react with the water itself, become surrounded surrounded by a lilac flame sufficiently hot to melt it, and start fizzing violently and pushing itself around the container. A larger dose of potassium, or a more reactive alkali metal such as rubidium, will explode). The emission of heat causes a relatively gentle warming effect for the immediate area, but close to the site of the reaction itself a very large amount of heat is emitted in a small area. This excites the molecules of air close to the reaction and causes them to vibrate violently, emitting photons of electromagnetic radiation as they do so in the form of heat & light (among other things). These photons cause the air to glow brightly, creating the visible flame we can see; this large amount of thermal energy also ionises a lot of atoms and molecules in the area of the flame, meaning that a flame has a slight charge and is more conductive than the surrounding air. Because of this, flame probes are sometimes used to get rid of the excess charge in sensitive electromagnetic experiments, and flamethrowers can be made to fire lightning. Most often the glowing flame results in the characteristic reddy/orange colour of fire, but some reactions, such as the potassium one mentioned, cause them to emit radiation of other frequencies for a variety of reasons (chief among them the temperature of the flame and the spectral properties of the material in question), causing the flames to be of different colours, whilst a white-hot area of a fire is so hot that the molecules don’t care what frequency the photons they’re emitting are at so long as they can get rid of the things fast enough. Thus, light of all wavelengths gets emitted, and we see white light. The flickery nature of a flame is generally caused by the excited hot air moving about rapidly, until it gets far enough away from the source of heat to cool down and stop glowing; this process happens all the time with hundreds of packets of hot air, causing them to flicker back and forth.

However, we must remember that fires do not just give out heat, but must take some in too. This is to do with the way the chemical reaction to generate the heat in question works; the process requires the bonds between atoms to be broken, which uses up energy, before they can be reformed into a different pattern to release energy, and the energy needed to break the bonds and get the reaction going is known as the activation energy. Getting the molecules of the stuff you’re trying to react to the activation energy is the really hard part of lighting a fire, and different reactions (involving the burning of different stuff) have different activation energies, and thus different ‘ignition temperatures’ for the materials involved. Paper, for example, famously has an ignition temperature of 451 Fahrenheit (which means, incidentally, that you can cook with it if you’re sufficiently careful and not in a hurry to eat), whilst wood’s is only a little higher at around 300 degrees centigrade, both of which are less than that of a spark or flame. However, we must remember that neither fuel will ignite if it is wet, as water is not a fuel that can be burnt, meaning that it often takes a while to dry wood out sufficiently for it to catch, and that big, solid blocks of wood take quite a bit of energy to heat up.

From all of this information we can extrapolate the first rule that everybody learns about firelighting; that in order to catch a fire needs air, dry fuel and heat (the air provides the oxygen, the fuel the stuff it reacts with and the heat the activation energy). When one of these is lacking, one must make up for it by providing an excess of at least one of the other two, whilst remembering not to let the provision of the other ingredients suffer; it does no good, for example, to throw tons of fuel onto a new, small fire since it will snuff out its access to the air and put the fire out. Whilst fuel and air are usually relatively easy to come by when starting a fire, heat is always the tricky thing; matches are short lived, sparks even more so, and the fact that most of your fuel is likely to be damp makes the job even harder.

Provision of heat is also the main reason behind all of our classical methods of putting a fire out; covering it with cold water cuts it off from both heat and oxygen, and whilst blowing on a fire will provide it with more oxygen, it will also blow away the warm air close to the fire and replace it with cold, causing small flames like candles to be snuffed out (it is for this reason that a fire should be blown on very gently if you are trying to get it to catch and also why doing so will cause the flames, which are caused by hot air remember, to disappear but the embers to glow more brightly and burn with renewed vigour once you have stopped blowing).  Once a fire has sufficient heat, it is almost impossible to put out and blowing on it will only provide it with more oxygen and cause it to burn faster, as was ably demonstrated during the Great Fire of London. I myself have once, with a few friends, laid a fire that burned for 11 hours straight; many times it was reduced to a few humble embers, but it was so hot that all we had to do was throw another log on it and it would instantly begin to burn again. When the time came to put it out, it took half an hour for the embers to dim their glow.