So we're going to have one electron in one of these p orbitals. To fill the first shell, 1s2, now the second two are then going to go to the second shell andįill up the s subshell 2s2, and then we're going to startįilling up the p subshell. A neutral boron would have five electrons. But what about boron? Boron gets interesting. Notice, we have four total electrons which would be the case inĪ neutral beryllium atom. Going to fill up the s subshell in the second shell. Go into the first shell, 1s2, and then the next two are Now what about beryllium? Well, that's gonna look a lot like lithium but now it has four electrons. In the first shell and one electron in the second shell. So then it'll go to the second shell and start filling up the s subshell. It's going to fill first is the s subshell. To the first energy level, the first shell, so theįirst two will go 1s2, and then the third electron is going to go into the second shell, and the subshell that Now what do you think is going to happen when we go to lithium? Well lithium, a neutral lithium will have three electrons in it, so the first two could go So its electronĬonfiguration would be 1s2. So instead of just having oneĮlectron in that first shell, we can fit up to two there. Now what happens if we go to helium? Well, a neutral helium atom is going to have two electrons. So we would say itsĮlectron configuration 1s1, in the first shell which is made only of an s subshell, it has one electron. It only has an s subshell,Īnd so that one electron in that neutral hydrogenĪtom would go over there.
The lowest energy level or the first shell, and that first shell has only one subshell in it. Now where would that one electron be? Well it would be in Has an atomic number of one which tells us it has one proton, and if it's neutral, that If we're talking aboutĪ neutral hydrogen atom, a neutral hydrogen atom, it And so first, let's just think about the electron configuration And to help us with that, we will look at a periodic table of elements. Now the goal of this video is to think about electron configurationsįor particular atoms. So if you're thinking about the subshell, the s subshell could fit two electrons, the p subshell can fit six electrons, the d subshell can fit 10 electrons, and the f subshell can fit 14 electrons, two per orbital. That has one, two, three, four, five different orbitals in it. So you have the s subshell, the p subshell that has threeĭifferent orbitals in it, you have the d subshell The various subshells which are found in the various shells. Us the types of orbitals which can be found in And an orbital is a description of that, where is it more or In a previous video, we've introduced ourselves to the idea of an orbital, that electrons don't just orbit a nucleus the way that a planet might orbit a star, but really, in order to describe where an electron is atĪny given point in time, we're really thinking about probabilities, where it's more likely to be found and less likely to be found. This means that we have a total of 8 electrons in the 2nd energy level (2 from the s subshell, and 6 from the p subshell).Īs you go further, you will get practice with identifying and conceptualizing electron configuration. In every p subshell there are 3 p orbitals. In the 2nd energy level, we have a p subshell in addition to the s subshell. This specific type of orbital is called the s orbital, and we have 1 s orbital for every s subshell. In the 1st energy level, we have 1 subshell, which basically means we have 1 type of orbital. Each orbital then has 2 electrons, which are said to have different and opposite spins. Finally, within each subshell there are individual orbitals referencing a specific region of space around the atom's nucleus. We can organize these electrons into different subshells based upon the shape of the region they occupy.
The pattern that we observe results in 3 classifications as follows (there are other considerations that you will learn about later as well).Ī Shell / Energy Level is a region or set of regions that have the same energy.Īlthough we cannot predict the exact location of the electrons at any time, we can map out the regions of space that they occupy. As electrons are added to the space around the atom's nucleus they are arranged in a way as to minimize repulsions.
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