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I have a little question I hope someone could answer.

I'm reading some Solid State Physics and I have come across energy bands and energy gaps. As far as I understand the energy band is where the electrons are able to occupy space, and the gap is space where there are no states to occupy.

Now, in my book they have examples with energy bands and gaps forming from Na and Si. For Na it's just normal where you have your band and then a gap between that and the next band. But for Si they have 3s and 3p orbitals which seem to form filled bands for 3s and unfilled bands for 3p - and that is, at least I think, what makes it good for a semiconductor.

Now, my question is: Is the only difference between the band formation for Na and Si, that the energy gap between the energy bands in Na is much larger than that of Si?

Don't know if I have explained it okay, but hopefully, someone understands what I mean.

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  • $\begingroup$ your explanation is clear but question is not clear so have a another look on it and make a appropriate language. $\endgroup$
    – Rahul
    Aug 8, 2013 at 18:14
  • $\begingroup$ I'll try again: According to my book when Si make a band formation, it will create a energy band for the 3s orbital and 3p orbital. The 3s orbital will be filled, and the 3p orbital will not. In between there is a band gap. Now, if I look at Na it will form only 3s energy bands which is also separated by energy gaps. So basically, both of them have energy gaps. My question then was: Is the reason why Si is considered a semiconductor and not Na, that the energy gap between the 3s and 3p bands is much smaller than the energy gap between the energy bands for Na, which is between the 3s bands. $\endgroup$ Aug 8, 2013 at 18:24

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Electrons are fermions, which mean that no two electrons may have exactly the same state. This statement is called Pauli Exclusion Principle.

Each atom has discrete energy levels which may be occupied by electrons (in fact, the correct statement will be that electrons in the atom can have discrete values of potential energy). These discrete potential energy levels represent atom's Orbitals.

Imagine some atom being ripped of all its electrons (a nucleus). When the first electron is returned to the atom, it occupies the least energetic state available. When the second electron is returned to the atom it can not have the same state as the first one. It seems like this electron must occupy the second lowest energy level, however electrons have "spin". Two electrons may occupy the same energy level in the atom if they have different spins (therefore their state is not the same). This is the reason why the lowest orbital can accommodate two electrons - one having "spin up" and other having "spin down".

atom's orbitals

We won't discuss why the second orbital may be represented as four sub-orbitals and can accommodate a total of 8 electrons - this requires a quantum mechanical analysis which is not directly related to your question.

Now, suppose that you brings two Na atoms close together. They have exactly the same number of electrons at exactly the same orbitals. However, non-valence orbitals are filled by the maximum number of electrons which accommodate all allowed electronic states in the atoms. This should lead to existence of pairs of electrons having exactly the same states in these atoms, right? No, the Pauli exclusion principle is not broken here. What happens is that due to electrons' interactions, each orbital is being split - the corresponding orbitals in these atoms change their energies a bit, leading to creation of two orbitals having slightly different energies. The difference between new orbitals' energies is called covalent energy.

Orbitals splitting

When you add third atom to the existing two, the orbitals split once more, and the covalent energy reduces. The process continues with each additional atom. By the time you have a macroscopic cluster of Na atoms, each orbital was split a huge number of times and the covalent energy became exceedingly small - the energy levels of orbitals became indistinguishable from each other (the separation is well below measurement limit of any existing technique).

Energy band formation

In this case there is no more reason to treat each altered energy level of a particular orbital separately, and the notation of "bands" come in handy. Energy band represents all energies of (initially) the same orbital. The electrons may transit freely between energy levels in the same band.

Bands are formed for each orbital of the element. The number of bands is equal to the number of orbitals in the elementary atom of Na.

Pauli exclusion principle still applies, therefore the number of electrons in a single band has an upper bound. Electrons tend to occupy the lowest energy bands first. When there are no more electronic states in a band, any additional electron will occupy the next energy band.

The energy level of the most energetic electrons in a material (material, not atom anymore) is called Fermi level (this definition is a bit simplified, but correct in general). All the electronic states below Fermi level will be occupied by electrons, and all the states above will be empty.

The highest energy band which is completely filled with electrons is called Valence Band. The lowest energy band which has unoccupied electronic states in it is called Conduction Band.

The last piece of information we need in order to understand the distinction between conductors, semi-conductors and insulators, is that an energy band which is full with electrons (valence band is one of them) can not carry current (i.e. electrons in this band can't contribute to current flow). The explanation for this is again a bit tricky, therefore just get this fact as granted (and you are welcome to find additional info on the Web). Completely empty band can't contribute to current too because there are no electrons which can gain energy in it at all.

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Conductors

Conductors are characterized by overlapping valence and conduction bands (otherwise stated: Fermi level lies inside conduction band of conductors, and this band is partially filled with electrons). Valence electrons can freely transit to higher energy states in the conduction band, therefore applied voltage will cause their drift - electrical current.

Insulators

Insulators are characterized by Fermi level lying in between valence and conduction band. Valence band is therefore full and its electrons can't contribute to current. Conduction band is therefore empty and there are no electrons which can contribute to current at all.

Does this mean that an insulators can't conduct current at all? Well, no. It means that if you want to see current flow in insulator, you must transfer huge energy to electrons in order to transit them from valence band into conduction band (the energetic separation between these bands is called band gap).

Semi-conductors

Semi conductors have the same band structure as insulators, with Fermi level lying inside the band gap. The only difference is that the band gap of semiconductors is relatively small, which allows for low energy transitions of electrons from the valence band into the conduction bands. The energy for this transition may be gained from electrostatic energy, optical energy, heat energy etc...

Yes, semiconductors are just bad insulators :)

Hope this clarifies the energy bands concept.

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