| The-Nisk wrote: | | I'll have to look up what's all the rage with "quantum" is, as it stands I'm shamefuly ignorant on it it would seem. |
Well, since you asked. ^_^;
In the mid-1800s, physicists started making real leaps and bounds studying energy. They were getting to the point where they thought they pretty much almost had physics "solved". But they came to a point where they were just totally stuck. According to theory, if you take a perfect blackbody and heat it up, it should emit light at any frequency - or in plain English, if you take a hunk of steel and heat it up to 2000 degrees, it should glow at all colours equally. The result is that the high frequencies should be emitting at infinite intensity. Of course, that's not what happens in practise. In practise, the hunk of steel will glow a certain colour (red-hot, white-hot... various different colours at different temperature), and the high frequencies were certainly not infinitely intense. To picture that, see here:
(The vertical axis is intensity, graph from here). As you can see, according to the classical model, the intensity just shoots off into infinity. In reality (labelled "quantum" in the graph), it peaks, and then drops.
Now this was a major problem for physics - so major they labelled it the "ultraviolet catastrophe". But at the time they still believed they had physics mostly solved, and this was just a detail that wouldn't change the fundamentals.
In 1900, Max Planck said, "screw this" (possibly not his actual words), and instead of trying to explain why the curve was shaped the way it was, he tried to explain what was happening. Classical theory assumed that every frequency had an equal chance of being emitted. Planck said, "obviously not, so what is the probability distribution if it is not all equal probabilities?" He tried to match various distributions... and found a match. He found that if he used a formula that assumed that the only frequencies emitted were frequencies that satisfied ℎf = n (where ℎ is a constant, f is frequency and n is 1,2,3,4...), it worked. Now Planck never tried to explain why that was so - he just admitted he had no clue - but it worked.
Five years later was 1905, Einstein's annus mirabilis, in which he published 4 papers that changed the course of physics. 2 were the foundation for relativity, 1 was on Brownian motion (which proved that atoms were real and not hypothetical) and the last was on the photoelectric effect. While studying the relationship between light frequency and voltage in photoelectric materials, Einstein found that they only accepted and emitted light in specific amounts. This led Einstein to hypothesize that light came in discrete packets: photons. Going a step further, he realized that this solved Planck's problem, too. That led to the first great breakthrough in (what would become) quantum mechanics: energy is quantized.
(Just to clear up the mystery of the word "quantized", if you're not familiar with it: when a value is quantized, that means it can only take up specific values, not just any value. For example, a crowd of people is quantized, because you can have a crowd of 100 or a crowd of 101 people... never a crowd of 100.326 people. Energy is quantized because you can emit 1 photon, or 2 photons... never 1.4 photons.)
To give you an idea of how controversial this was, when Einstein received his Nobel prize, they explicitly excluded his work on the photoelectric effect and photons. ^_^;
The next piece of the puzzle came from Niels Bohr. He created a model of the atom that was a kind of intermediary step between classical and quantum. You probably learned about the Rutherford model of the atom in high school physics, where negatively charged electrons orbit around a positively charged nucleus rather like planetary motion. The problem is... this model doesn't work. Whenever an electric charge is in motion, it radiates electromagnetic radiation (according to Maxwell's laws). But if the electron is constantly radiating EM radiation - which is energy - while orbiting the nucleus, the orbit would eventually decay. All atoms would collapse. Clearly... this is a problem.
Bohr created a model where electrons could only orbit in specific orbits - in other words, the orbit is quantized. To jump from one orbit to another took a fixed, specific amount of energy - Bohr refused to admit this implied photons (he didn't believe in them)... but it sure sounds like it, doesn't it?
The final piece of the puzzle was supplied by a man named Louis de Broglie. Since it was widely held at the time that light was a wave (from Maxwell's equations, for example), a photon must be both a particle and a wave. That duality was the reason Einstein's photons were so highly controversial. de Broglie was the guy who - depending on your view - solved the problem, or made it worse. de Broglie argued that not only photons, but all matter, was really wave-like in nature. He even drafted the equation to give the wavelength for any amount of matter.
Now if you're not seeing how all of this fits together, here's the key!
All matter is not tiny spheres, it is actually wave packets that look like this:
You can see how that can kinda seem like a particle when viewed from the side - it is sort of contained. Because they're not tiny spheres, particles don't actually bounce off of each other - the waves interfere.
The reason why electrons can only travel in certain orbits is because those orbits are the only ones were the orbital length is a multiple of the wavelength. In other words, if you take the orbital path and unfold it into a straight line, it will fit one complete electron wave (or two, or three, etc). This is the only way the wave pattern will stay stable, because if the path was a different length, the wave would interfere with itself on a second pass around.
All matter interactions become wave functions - not mechanical functions like balls bouncing off of each other. And because they are wave functions, you get neat effects like tunnelling (the wave passes through another wave intact), entanglement (the waves become codependent), and so on. And because matter is waves, it does not exist at a single point as it would if it were a tiny ball - it can exist over an area of space - a cloud (it can appear to be in multiple places at once).
Quantum physics can be difficult to grasp because we don't think in waves - we can easily picture tiny balls bouncing around, but wave forms interacting... it gets tricky. To make things worse, the wave nature of matter leads to wackiness like electrons being in multiple places at once, or electrons travelling from point A to point C without every crossing point B between them, and so on. These things are easy to see from the math... but the math is gross. Unless you want to solve the Shrödinger equation (and trust me, you don't ^_^), you just have to trust that things that make no sense to you are really happening at the atomic scale.
| ocalhoun wrote: | | (As a side note, It'll help you understand that there really is such a thing as a 'maybe', that not everything is a 'yes' or a 'no'... You seemed to have a problem with that on another thread.) |
That is not a particularly rational interpretation of QM. QM works in probabilities, but that doesn't imply uncertainty in the layperson sense. Consider a coin flip, which can be heads or tails, and call heads "yes" and tails "no". Before the coin is flipped you don't know whether you're getting "yes" or "no", so if someone asks if you are going to get "yes", you can say "maybe". But that doesn't mean that there is no "yes" or "no", it just means you don't know whether it will be "yes" or "no" yet. Once the coin is flipped, it will be either "yes" or "no"... not "maybe".
Similarly in QM, there is only uncertainty until interaction. Once there is interaction, all you have is "yes" or "no".
So, really, there is no "maybe" in QM. There is only "we don't know yet", but eventually it will boil down to either "yes" or "no". |