- #1
nitsuj
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Why do Electrons "want" 8 Electrons on the outter "shell"? What is so special about 8?
Why do Electrons "want" 8 Electrons on the outter "shell"
In summary, the shell model is a summary of what is going on, and it is not the only model that exists.
- #2
Quantum Defect
Homework Helper
Gold Member
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nitsuj said:
The old charge-size argument.
Adding electrons:
You have a compact nucleus with a large positive charge. You can add electrons to a neutral atom and the process will be exothermic -- i.e. electron affinity is positive. The tricky part of this is that quantum mechanics only allows a limited number of electrons to occupy comparable regions of space. Once this space is taken up, the next electrons will go into the atom at a distance much farther away. There will not be much attraction for these new electrons as the inner electrons effectively shield the nucleus.
Taking electrons away:
If you have something like sodium, the valence electrons is all by itself, farther away from the nucleus than the other electrons. This electron feels something close to a +1 charge, and it is relatively easier to ionize. However, the remaining electrons are, as a group, closer to the nucleus and feel a much larger nuclear charge. Since the potential energy goes like Z*e^2/r (and Z* is larger and r is smaller) these inner electrons will be quite a bit more difficult to remove.
Longstory short -- it is a combination of quantum mechanics -- which limits occupancy of different regions of space around the nucleus and the coulomb potential (e-nuclear attractions and e-e repulsions.)
- #3
sk1105
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Actually, that shell model of 2, 8, 18 etc. is only a summary of what is going on, and I'm afraid the real picture is a bit more complicated. The populations of electron shells stem from a phenomenon in quantum mechanics known as the Pauli Exclusion Principle, which says that two fermions (a type of particle that includes electrons) cannot share the same energy state unless they have different spins. Only two different spins are possible, so only two electrons can occupy one state. We also need to consider a property of the electrons in an atom called orbital angular momentum ##l##, and the z-component of orbital angular momentum, denoted ##m_l##.
In the first shell, ##l = 0##, and quantum mechanics says that ##m_l = 0## also. The energy states are labelled by the values of ##m_l##, so as we only have one value of ##m_l## here, that means one energy state and so from the exclusion principle we have two electrons in the first shell.
In the second shell, ##l = 1##, and quantum mechanics gives us ##m_l = -1, 0, 1##. So now we have 3 values of ##m_l##, and therefore 3 energy states. As before, we put two electrons in each state, giving six in this shell.
For the third shell, ##l=2## and ##m_l = -2, -1, 0, 1, 2##; perhaps now you can see the pattern. This means we have 5 energy states, so 10 electrons in total for this shell if we put two in each state.
As you can see, the picture derived from quantum mechanics looks a bit more complicated than the first model, but it doesn't mean you should throw your model away. I will now introduce a quantity ##n##, known as the principal quantum number. It is a positive integer, related to ##l## by ##l < n##, where ##l## is also an integer as we see above. The lowest value of ##n## is 1, and this corresponds to the lowest value of ##l## i.e. ##0##. As there are only two electrons corresponding to this value, this gives us the 2 electrons in the first shell as predicted by the more basic model.
Next, we have ##n = 2##, but we see from the relation with ##l## that this means ##l = 0## and ##l = 1## are both allowed for this value of ##n##. This means that in addition to the 3 states (and therefore 6 electrons) coming from ##l = 1##, we can have another two electrons in a second ##l = 0## state. Putting these together, we get
2 + 6 = 8 electrons in the next shell, agreeing with the simpler model.
Moving up to ##n = 3##, ##l = 0, 1, 2##, so you now get two electrons from ##l = 0##, six electrons from ##l = 1## and ten electrons from ##l = 2##. Put these together and you have 18 electrons in this shell, again in agreement with the simpler model.
I hope I've managed to explain this clearly enough, but if it all seems a bit daunting, the simple model works fine, and you may just have to wait until you learn quantum mechanics
In the first shell, ##l = 0##, and quantum mechanics says that ##m_l = 0## also. The energy states are labelled by the values of ##m_l##, so as we only have one value of ##m_l## here, that means one energy state and so from the exclusion principle we have two electrons in the first shell.
In the second shell, ##l = 1##, and quantum mechanics gives us ##m_l = -1, 0, 1##. So now we have 3 values of ##m_l##, and therefore 3 energy states. As before, we put two electrons in each state, giving six in this shell.
For the third shell, ##l=2## and ##m_l = -2, -1, 0, 1, 2##; perhaps now you can see the pattern. This means we have 5 energy states, so 10 electrons in total for this shell if we put two in each state.
As you can see, the picture derived from quantum mechanics looks a bit more complicated than the first model, but it doesn't mean you should throw your model away. I will now introduce a quantity ##n##, known as the principal quantum number. It is a positive integer, related to ##l## by ##l < n##, where ##l## is also an integer as we see above. The lowest value of ##n## is 1, and this corresponds to the lowest value of ##l## i.e. ##0##. As there are only two electrons corresponding to this value, this gives us the 2 electrons in the first shell as predicted by the more basic model.
Next, we have ##n = 2##, but we see from the relation with ##l## that this means ##l = 0## and ##l = 1## are both allowed for this value of ##n##. This means that in addition to the 3 states (and therefore 6 electrons) coming from ##l = 1##, we can have another two electrons in a second ##l = 0## state. Putting these together, we get
2 + 6 = 8 electrons in the next shell, agreeing with the simpler model.
Moving up to ##n = 3##, ##l = 0, 1, 2##, so you now get two electrons from ##l = 0##, six electrons from ##l = 1## and ten electrons from ##l = 2##. Put these together and you have 18 electrons in this shell, again in agreement with the simpler model.
I hope I've managed to explain this clearly enough, but if it all seems a bit daunting, the simple model works fine, and you may just have to wait until you learn quantum mechanics
Related to Why do Electrons "want" 8 Electrons on the outter "shell"
1. Why do electrons "want" 8 electrons on the outer shell?
Electrons "want" 8 electrons on the outer shell because it follows the octet rule, which states that atoms tend to gain, lose, or share electrons in order to achieve a full outer shell of 8 electrons. This is a stable configuration that makes the atom more energetically favorable.
2. What is the significance of the outer shell in electron configuration?
The outer shell, also known as the valence shell, is the most important shell in electron configuration because it determines the reactivity and chemical properties of an atom. It is the outermost shell where electrons are involved in bonding with other atoms.
3. Can elements have more or less than 8 electrons on the outer shell?
Yes, elements can have more or less than 8 electrons on the outer shell. This applies to elements in periods 2 and higher on the periodic table. Some elements, such as helium, only have 2 electrons on the outer shell, while others, such as sulfur, can have up to 12 electrons on the outer shell.
4. How do atoms achieve a full outer shell of 8 electrons?
Atoms can achieve a full outer shell of 8 electrons through various processes, such as gaining, losing, or sharing electrons. This can occur through the formation of chemical bonds with other atoms, or through the transfer of electrons in ionic bonding.
5. What happens when an atom does not have a full outer shell of 8 electrons?
When an atom does not have a full outer shell of 8 electrons, it is considered to be unstable and more reactive. These atoms will often undergo chemical reactions to gain, lose, or share electrons in order to achieve a full outer shell and become more stable.
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