![]() ![]() So for helium right? An s orbital in the firstĮnergy level, like that. Talking about an s orbital in the first energy level right? So we're still talking about an s orbital in the first energy level. Ml must be equal to zero, and so we're still We're still in the first shell, we're still in the first energy level. So atomic number of two, so two protons and two electrons. ![]() Let's move on to helium now, so two electrons to worry about. One s one, or we could draw orbital notation like that for hydrogen. So the fourth quantum number ms we could say that's positive 1/2 spin. So this arrow pointing up is representing one electron with an up spin. And let's say the electronĮnters the orbital spin up. And we put the one electron of hydrogen into that one s orbital. We're talking about an s orbital in the first energy level, so we could label this orbitalĪs being the one s orbital. So you draw a line here, which represents an orbital. There's another way to writeĪn electron configuration, or to draw one out, it's called orbital notation. So one s one means one electron in an s orbital in the first energy level. And this superscript one here, this is telling us how many electrons are in that orbital. S says the electron for hydrogen goes into an s orbital. The energy level right? The shell, n is equal to one. We write the electronĬonfiguration as one s one. And so the electron for hydrogen is going to go into an s orbital. Like a sphere right? So in this sphere, in this three dimensional volume here, this is the most likely place, the most likely region we're going to find this one electron. So l is equal to zero tells us we're talking about an s orbital, and this tells us how many orientations. Value for ml right? So the magnetic quantum number, that's equal to zero. If l is equal to zero, there's only one allowed Only one allowed value for l, and that's equal to zero. Quantum numbers earlier, if n is equal to one there's So therefore, the electron goes into the lowest energy level possible. So where's the best place to put the one electron for hydrogen? Well, we wanna put that electron as close to the nucleus as possible, in order to maximize the attractive force between the positive chargeĪnd the negative charge. Here we have only oneĮlectron to worry about. Because as you writeĮlectron configurations you're thinking about theīest way to build up an atom. And we're gonna use the Aufbau principle. So our goal is to writeĪn electron configuration for that one electron of hydrogen. In a neutral atom, the number of protons is equal to the number of electrons. So if there's an atomic number of one, that means there's one So let's start with hydrogen, atomic number of one. Period in the periodic table, and we have only twoĮlements to worry about. Let's look at how to write electron configurationsįor the first period.
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