For those wondering about why the article says "Two atoms alone can’t form a molecule, it takes at least three to do chemistry", here's another explanation from the reddit thread [0]
> Each atom has some amount of energy associated with it. If you just bring two atoms together, the total energy is simply the sum of their individual energies. This state is typically referred to as an excited state. However, the stable bonded form of the two atoms actually has a lower energy. So to go from two separate atoms to two bonded atoms, the atoms have to first collide and form the excited state and then lose some amount of energy to go to the stable state. If they don’t lose that energy, then they can and will break apart again. One way to lose that energy is via collision with the third atom.
> In normal systems where you have tons of atoms flying around, collisions happen very frequently, so you can typically assume that the stabilization will happen immediately following the reaction. This is why the idea that stabilization is an important step in a chemical reaction is typically not covered in intro chemistry. However, it’s not uncommon to have conditions where that assumption does not hold. This then gets into the concept of pressure dependent reaction kinetics, which studies the effect of having slow stabilization.
Interesting. Is this how catalysts work? By bringing the atoms/molecules reacting together and providing a path for taking away the excess energy more easily?
There are lots of different types of catalysts: Homogeneous (molecule, typically small, in solution), heterogeneous (solid or porous surface) and enzymes (biological molecules.) Many do work by bringing reactants together so that the relevant fragments can combine. Chemical reactions are usually described as going through an energetic transition state and many catalysts stabilize this state so that the reaction can "get over the hill" and become product. Of course, it also stabilizes it for the reverse reaction so the products can become reactants again. The overall equilibrium is not changed. Both reactions speed up. If, however, one extracts the product as it is formed, more product will be formed and hence catalysts are incredibly useful since, by definition, they are not consumed by the reaction - i.e. you get the catalyst back so it can continue to do its work.
The last 1/3 of this old video from Shell describes how catalytic cracking, a crucial part of oil refining, works. It covers practical reactor considerations, including getting the products out so more are formed and 'poisoning' where a catalyst's efficiency is reduced by contamination and how that's dealt with in a continuous process.
https://www.youtube.com/watch?v=hC1PKRmiEvs
That doesn't seem right. Cars have catalysts where the air flows through. Also 2 H2 + O2 -> 2 H2O (+ a characteristic bang :-)) at room temperature and pressure (initially) using a platinum catalyst is shown in school chemistry classes.
Just learned on Wikipedia (en/Platinum) that the 2007 Nobel price in Chemistry was awarded for explaining how that works. doi:10.1002/anie.200800480
Car's catalyst work at high temperatures, not at room temperature.
In fact, at room temperature they don't work at all, which is exactly the problem with catalysts, they don't work when you start your car.
They need to heat with the hot combustion gases to start working, and that takes a while.
This is one of the reasons that laboratory's measurements of particles and gases like nitrogen oxides do not apply to real emissions in cities, because most people in cities will use the cars, for example, diesels in Europe, for very short periods of time, then let the car cool down and use it again to go back less than 10 kilometers away.
There are many kinds of catalysts beyond materials surfaces. Organic chemists use metal complexes as catalysts in organic synthesis. This is especially important in asymmetric catalysis where you want to form high excesses of one isomer of a molecule, which can have drastically different effects in medicine for example. Catalysis also plays an important role in biology I believe.
Can they? Normally[1] emission of a photon would be a result of an electron moving from a high-energy shell to a low-energy shell. Going from two Cl to one Cl_2 is also a transition to a lower-energy state, but it's not immediately obvious that this would be able to generate a photon in the same way as an electron shell transition. You can do the molecule merge with atoms that already had their electrons in the lowest state... can't you?
Yeah I was thinking that too. Given the observations they describe I can only assume that releasing a photon is too slow of a process compared to the speed in which the molecule breaks apart.
If you smash them together faster, you just increase their energy, i.e. the opposite of what you want. If electrons fly off, you are likely to be left with an unstable molecule.
I sort of see what you are trying to say, but I think you're slightly misunderstanding what is going on. It is true that you are sharing electrons in a covalent bond, but it is not correct to therefore say that you need less electrons than in the atom state. A simple example: say you have to H atoms. Each has one electron. You put them together and form H2, which has two electrons combined. In both cases you need a total of two electrons, in order to have a neutral system. If you change that in any way, you will end up with highly reactive species (e.g. H+, H-, H2+, H2-). H+ is of course just an acid.
What you are probably thinking of, is the fact that if you put NaOH, or HCl in water, you get Na+, OH-, etc., and these are more stable than their neutral counterparts. But this is because they are stabilised by (polar) water molecules. Outside of water (or some other stabilising solvent), Na+, OH-, H+ and Cl- are all very reactive species.
> It appears you need the energy from 3 in order for the 2 to make a bond.
> It's the other way around. Two atoms alone will release a bunch of energy when they form a molecule; exactly enough energy to rip the molecule back apart. That energy has to go somewhere, and where it goes is the third atom.
In other atomic physics experiments it's a problem - three-body collisions are able to dump energy into one of the three atoms and that atom has enough energy to escape the trap. These are "three-body losses".
Whereas with two-body collisions, neither atom can be going any faster afterwards than the fastest one was before the collision. So they remain trapped.
Since the three-body collision rate is proportional to the cube of the density of atoms, and the two-body collision rate only to the square of density (for obvious reasons), this phenomenon limits the density of atomic clouds we can do experiments with. If we increase the density to the point where three-body collisions are significant, we rapidly lose atoms.
> Each atom has some amount of energy associated with it. If you just bring two atoms together, the total energy is simply the sum of their individual energies. This state is typically referred to as an excited state. However, the stable bonded form of the two atoms actually has a lower energy. So to go from two separate atoms to two bonded atoms, the atoms have to first collide and form the excited state and then lose some amount of energy to go to the stable state. If they don’t lose that energy, then they can and will break apart again. One way to lose that energy is via collision with the third atom.
> In normal systems where you have tons of atoms flying around, collisions happen very frequently, so you can typically assume that the stabilization will happen immediately following the reaction. This is why the idea that stabilization is an important step in a chemical reaction is typically not covered in intro chemistry. However, it’s not uncommon to have conditions where that assumption does not hold. This then gets into the concept of pressure dependent reaction kinetics, which studies the effect of having slow stabilization.
[0] https://www.reddit.com/r/science/comments/f7mqwl/physicists_...