Double-Slit Experiment
I believe you are describing the double slit experiment with electrons (as opposed to with light). The pattern you are describing is called an interference pattern (much like two pebbles producing ripples in a pond and there are parts where the ripples cancel out). Below is a diagram of the double slit experiment.
One way of showing the interference pattern is shown below:
To summarize how this experiment works, an electron gun is used to fire electrons one by one at a screen with two slits in it. Behind the double slit screen is another screen where the electrons build up. The importance of this experiment is that the electrons build up in an interference pattern (as shown below, where a is the beginning and e is the end) which proves that electrons have a wave-particle duality like light, as de Broglie predicted. This phenomenon has been shown to occur with photons, electrons, atoms, and some molecules (such as buckyballs, though, referencing the comments, I'm not sure about water).
There are two other important things to note about the double slit experiment. The first is the idea behind quantum mechanics - the probability wave. In quantum mechanics (unlike in Newtonian mechanics) nothing can be predicted exactly. A baseball will probably end up at home plate, but there's always a chance, however minuscule, that it'll end up over in the Andromeda Galaxy. The probabilities of where things will be are represented by what is called a probability wave. You can think of a probability wave like the one in the picture below (which isn't the probability wave of the baseball).
The basic idea is that where the probability wave is high, the particle represented is likely to end up; where it is low, it is not likely to end up. The reason I'm bringing up probability waves is because they are in the experiment. The electron's probability wave goes through both slits at once (interestingly, if you close one slit, the results are not at all what you'd expect with Newtonian mechanics, but it makes sense in the context of the electron going through both slits at once) and produces the interference pattern.
The second is an interesting thought experiment. The idea of this thought experiment is that if particle detectors are placed behind each slit to show how many photons/electrons/particles come through, the interference pattern will disappear, because of the fact that particles cannot be observed as both wave and particle at once, resulting in the wavefunction collapsing and the particle settling on a single slit. This can be somewhat represented by the diagram below.
The one difference is that the screen would have two slits with detectors A and B in front of those two slits; otherwise, the basic idea is the same.
Here is a website that the double slit experiment further.
Emission Spectrum
The emission spectrum of a chemical element or chemical compound is the spectrum of frequencies of electromagnetic radiation (e.g., visible light, microwaves, radio waves, gamma waves, etc) emitted due to an atom or molecule making a transition from a higher energy state to a lower energy state. The photon energy of the emitted photon (the photon is the carrier of the electromagnetic force) is equal to the energy difference between the two energy levels. Below shows the electromagnetic spectrum:
In the context of the video, when one of the electrons makes a quantum leap to one of the lower energy levels closer to the nucleus, it emits electromagnetic radiation at certain wavelengths. This emitted electromagnetic radiation is its emission spectrum.
The experiment is done by heating gases up until they glow - agitating the electrons in the process - and then observing the light they gave off through a prism, which produces very defined lines - the emission spectrum. This could not be explained with the Newtonian picture of the atom (which, honestly, wasn't really defined - definitive proof of atoms was only provided by Einstein during his annus mirabilis in 1905, with his paper on Brownian Motion) but could be explained with the Bohr picture of the atom. Though Bohr's picture turned out to be partially incorrect (never, ever picture an atom as a miniature solar system, or physicists will pull their hair out) one idea remained the same, and was further emphasized by the Pauli Exclusion Principle. This idea was that electrons couldn't be in just any spot - they had to be in certain shells, like layers of an onion. They could never, ever be in the spots between the shells.
This was kind of important because one, electrons couldn't spiral into the nucleus (always good to keep the fundamental structure of matter from collapsing) and two, it explained this experiment. When electrons do a little quantum leap between the energy levels, they either have to gain energy (to move away from the nucleus, toward the outer energy levels) or lose energy (to move towards the nucleus and the inner energy levels). Now, because of the Law of Conservation of Energy, the energy lost cannot just vanish - it has to go somewhere. Enter the emission spectrum. The electrons emit electromagnetic radiation, the energy of that radiation depending on how much energy the electrons are losing, and the wavelength of that radiation depending on the atom - which is where the science of spectroscopy comes from. Below is a diagram of an atom's shells and how electrons emit or absorb energy when moving between these.
Emission spectrums vary from atom to atom. Below shows the emission spectrums of a few elements.
Hope this helps!
