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Noble gas configuration

How to write electron configurations for atoms and monatomic ions using noble gas configuration.

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  • male robot hal style avatar for user RandomDad
    Why do shells name by letters S, P, D, F?
    (40 votes)
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    • old spice man green style avatar for user Matt B
      Great question and good trivia for any Chemistry enthusiasts:

      The line groups (subshells) were called sharp, principal, diffuse, and fundamental. When the angular momentum quantum number was used to describe and explain these groups of lines, s became an abbreviation for = 0, p meant = 1, d meant = 2, and f meant = 3.

      Luckily, this is now meaningless, so don't worry what they really mean :-)
      (92 votes)
  • leaf yellow style avatar for user fryercar76
    What would the noble gas electron configuration for an element look like if the element is a noble gas? Would it be
    [Ne]3s^23p^6 ?
    (16 votes)
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  • leaf green style avatar for user Marcela Cruz
    What does it mean "Full Octet" ?
    (4 votes)
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  • spunky sam blue style avatar for user Albert Chhab
    Please help, I did not understand what happened after we wrote Neon at . Why did we write 3s^2 and 3p^2.
    (5 votes)
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    • piceratops seed style avatar for user RogerP
      What she was doing was writing the electron configuration of silicon. Written in full this is 1s2 2s2 2s6 3s2 3p2. However, the first part of this long expression, 1s2 2s2 2s6, is the electron configuration of neon. Therefore, to shorten the configuration for silicon she wrote [Ne] 3s2 3p2.

      All that this means is that silicon has a core structure that is the same as neon, but then has four more electrons (3s2 3p2). It's just a short cut and it is commonly used. Furthermore, it is helpful because the outer electrons (3s2 3p2) are the valence electrons and these are the ones that are of most importance.
      (10 votes)
  • blobby green style avatar for user zshhade99
    For Calcium, why is the electron configuration not contain "d", for the 3rd subshell section, before writing 4s2?
    (6 votes)
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  • leaf green style avatar for user Prakriti Marwah
    How can we tell what shell can fit what number of electrons? From the examples i figured- the 's' shells can take a maximum of 2 electrons and 'p' shells can take a maximum of 6 electrons. Is this right?
    (3 votes)
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  • male robot johnny style avatar for user Yuganes warman
    So the first shell consists of s orbitals, second shell s and p orbitals , third shell s,p and d orbitals and fourth shell s,pd,and f orbitals, what about the other shells like the fifth shell and beyond, does it remains as s p d and f orbitals only or it extends to g h and so on ? Also correct me if I am wrong about the shell part,thanks in advance !
    (3 votes)
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  • leaf green style avatar for user nehaarika.shridhar
    what exactly are valence electrons?
    (2 votes)
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  • starky sapling style avatar for user ₦Ɇ฿ɄⱠ₳
    Can someone please remind me why she has written another s after the p at and then another p.

    Also, why does she have a 6 at the top of the first p at ?
    Why not a 2?
    (2 votes)
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  • starky sapling style avatar for user Lina333
    So we must remember the noble gas electronic configuration,isn't it?or do we just need to remember the positions of the different elements in the periodic table ?
    (3 votes)
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Video transcript

- [Voiceover] In this video, we're going to be talking about how you can write electron configurations using noble gas notation. And to be more specific, in this video we're also going to be focusing on examples using main group elements. So, we're doing that because the transition metals, right here, and the lanthanides, are a little bit more complicated, so we won't be doing that in this particular video. So the rule for writing the noble gas notation for something is pretty simple. It is, you take the noble gas immediately preceding your atom or ion, so what do I mean by immediately preceding? That means we want the noble gas that comes right before it, so you go up a row, and you go over to here, where the noble gases live. And you put that in brackets and then you write your other electrons, and you write your other electrons using the same notation that you normally write electron configurations in. If you don't remember what that is, we'll go through a couple examples right now. So hopefully it will become more clear. So before we get started, I'm just going to remind you why we call the noble gases noble, and that is because they have a full octet of electrons. And so, since they have a full octet, they're not very reactive, they have all of the electrons they want, and as a result, you will see in chemistry that a lot of chemistry, chemical reactions will be driven by other non-noble gases trying to get a full octet. So the first example we're going to talk about and write the configuration for is silicon. Silicon is right below carbon in the Periodic Table, and we can write its full electron configuration, just for comparison, so if we start up here, with hydrogen, silicon has the electron configuration 1s2 2s2 2p6, so as a reminder, these are our S electrons because they're in S orbitals. These are our P electrons because they're in P orbitals, and then once we're through our 2p6 electrons, we go to 3s2 and we have two more electrons, so it's 3p2. So that's the electron configuration for silicon. Now, we can write it out using noble gas notation. And compare, so, the noble gas immediately preceding silicon, if we go up a row and then move over, we see that it's neon. So we write neon in brackets. And then, the other electrons are the ones that come after neon. So we go down, and the electrons that aren't included in neon would be our 3s2 electrons, right here, and the 3p2 electrons. So if we compare these two ways of writing our electron configuration, you can see that these electrons right here, so everything up to 3s2 3p2, that gives us the electron configuration for neon. And so we don't have to write that, we just write neon, and assume that whoever's reading it knows what the electron configuration for neon is. The other thing you might notice is that these other electrons here, that we wrote outside of the brackets, these are our valence electrons. So, writing your electron configuration this way, using noble gas notation, makes it really obvious where your valence electrons are and what kind they are, so that's helpful. We are going to go through one more example and that will be calcium. So calcium is over here, and so, we're not going to write the full electron configuration this time. We're just going to write the noble gas notation. So calcium, the noble gas immediately preceding it, we go up a row and then over and we see that the noble gas is argon, so we write argon in our brackets, and then, what electrons are not in argon? So we move down and we see that we have our 4s electrons, and we have two of them. So this is the noble gas configuration for calcium. So does calcium have a full octet? And we know that these are the valence electrons and we also know that if it did have a full octet, it would actually already have a noble gas configuration, so it would either have krypton or argon and in this case, it turns out that calcium prefers to lose two electrons, as opposed to gaining a bunch. It would be gaining 10 plus six. So, lose two electrons, and when calcium loses two electrons, it becomes the calcium 2-plus cation. And then we can write the electron configuration really short, or it'll be really short because we know it's going to lose these two valence electrons and then, it will have the electron configuration which is just the same as argon. And we can tell, really easily, looking at this, that calcium 2-plus has a full octet. So, one of the many pros of writing things in noble gas notation, besides the fact that it, you know, makes your hand less tired, is that it makes it really easy to see where your valence electrons are, and whether or not your ion or atom has a full octet.