We say electrons must jump from the valence band to conduction band in order to be conductive. Why is that the case and why can't electrons in the valence bands themselves be conductive?

Is it because more energy levels are available unoccupied in the conduction band and electrons literally have a lot more room to roam around? If that is the case, then why doesn't the valence band of Silicon (3p band) be conductive despite being just 33% occupied ? What core concept of conductivity and/or band theory am I missing? Please elucidate.

Also can we explain the drift of electrons in a metal under an electric field in terms of transition between various close energy levels within the same conductive band?

  • $\begingroup$ 3p orbitals form several bands - some of which are fully occupied and others are empty. So it is not 33% occupied. $\endgroup$
    – Roger V.
    Oct 13, 2021 at 13:17
  • $\begingroup$ All three 3p orbitals (namely 3px, 3py, and 3pz) are of equal energy levels. So would it be wrong to label the band these orbitals form as a single 3p band? $\endgroup$
    – user316403
    Oct 13, 2021 at 13:25
  • 2
    $\begingroup$ @alex599 - it would be wrong to directly link any atomic energy levels to solid state energy levels. That mapping just does not work. $\endgroup$
    – Jon Custer
    Oct 13, 2021 at 13:29
  • $\begingroup$ see the answer by @JonCuster here... in fact, this might be a duplicate physics.stackexchange.com/q/278844/247642 $\endgroup$
    – Roger V.
    Oct 13, 2021 at 13:40
  • $\begingroup$ @RogerVadim - thanks for finding that for me. I was heading in that direction but actual work interfered... $\endgroup$
    – Jon Custer
    Oct 13, 2021 at 13:42

2 Answers 2


As @Custer explained previously,

it would be wrong to directly link any atomic energy levels to solid state energy levels. That mapping just does not work.

Here, I will try to elucidate it with an intuitive example.

One form of elemental carbon is diamond, where every tetrahedral carbon center combines with 4 other carbon atoms as shown below.

enter image description here

A total of 8 electrons are involved in the above bonding (4 from central $C$ atom and 1 each from the $C$ atoms in the corners). Likewise, 8 atomic orbitals are involved in the process, giving rise to 8 new molecular orbitals.

enter image description here

The 8 electrons occupy the molecular orbitals in the order of increasing energy levels. Thus, 4 bonding orbitals are filled with electrons and the 4 anti-bonding orbitals are empty. Also note, there is a big difference in energy between the bonding and anti-bonding orbitals.

Just as one central $C$ atom and 4 corner $C$ atoms gave rise to 4 $\phi$ and 4 $\phi^{*}$ molecular orbitals at 4 different energy levels, increasing the number of $C$ atoms in the material would form multitude of $\phi$ and $\phi^{*}$ molecular orbitals at varied energy levels, as shown below. In a group of $n$ carbon atoms bonded together, each atom will contribute 4 orbitals and 4 electrons. There will be 2n bonding molecular orbitals, each filled with 2 electrons, and 2n empty anti-bonding orbitals. When the number of carbon atoms in the material approaches infinity ($n → ∞$), the energy differences between bonding molecular orbitals becomes vanishingly small, essentially becoming a continuum. The same is true for the energy differences between the anti-bonding orbitals. Thus, the filled molecular orbitals and the empty molecular orbitals become two, separated bands with a gap in between.

enter image description here

Note that $1s$ atomic orbitals of $C$ also form bonding and anti-bonding orbitals during covalent bonding. Their bands, which are not shown above, occur below the filled band. Also note, since, $C-C$ bond has a considerable bond strength, the band gap between the filled and empty bands shown above is considerably large. Silicon, whose crystalline form also assumes diamond like molecular configuration, has a relatively weaker $Si-Si$ bond due to which its band gap is smaller than diamond's.

I hope this gives you an intuition on why one-to-one mapping of atomic energy levels with solid state energy levels would be wrong. For e.g., carbon's $2s, 2p_{x}, 2p_{y}$, and $2p_{z}$ atomic orbitals, all contribute to both of its filled and empty bands, i.e., the same set of atomic orbitals contribute to two different bands. Likewise, it might also be possible that bands contributed by two different sets of orbitals overlap, in which case it technically is a single band.

In the case of metals, although no such covalent $\sigma$ bonds occur between the atoms as in diamond or silicon, the core concept of band formation remains essentially the same.

Density of states

We know each band is composed of multitude of states, where no two electrons can occupy the same state. Also for some value of energy in a band, there exists more states than the other. The density of states function $g(E)$ is a probability distribution function such that,

$$\int_{E_1}^{E_2}g(E).dE$$ gives the number of states in the energy range $E_1$ to $E_2$ per unit volume of material. It should come no surprise that for energies inside a band gap, $g(E) = 0$.

Filling of electrons in bands

At thermodynamic equilibrium, the probability that a state of energy $E$ is filled with an electron is given by the Fermi-Dirac distribution

$$f(E)=\frac {1}{1+ e^{(E-\mu)/(k_{B}T)}}$$

The number of electrons in the energy range $E_1$ to $E_2$ per unit volume of material should be


And, the density of electrons in the material should be

$$\frac{N}{V} = \int _{-\infty }^{\infty }g(E).f(E)\,dE$$

The function $f(E)$ looks as follows at $T=0K$, i.e., when the electrons in the solid assume their ground states due to no possible thermal excitation.

for $E>\mu$, $f(E) = 0$
for $E<\mu$, $f(E) = 1$
for $E=\mu$, $f(E) = indeterminate$

This value of $\mu$ is called Fermi level, below which all electronic states must be filled at $0K$ and above which all states must be empty.
N.B. No states are allowed in band gaps, i.e., the gaps are always empty.

When $T ≠ 0K$, at Fermi level, function $f(E)$ returns $\frac{1}{2}$, implying that if there are electronic states allowed at Fermi level, half of the states must be occupied at all temperatures.

If the Fermi level lies in a band gap, the band immediately below it is called the valence band. Valence in the sense that it is the highest energy band electrons occupy at ground state of the solid. Similar terminologies are valence shell, the highest energy shell occupied by electrons in an atom at ground state, and valence orbitals, the highest energy orbitals occupied by electrons. Likewise, if the Fermi level lies within a band, then this band would be the valence band.
Please note, it would be wrong to blindly map the valence orbitals of an atom to the valence band of the solid formed of those atoms as discussed previously.

The basis of conductivity

We talked about band as essentially being a continuum of energy eigenstates. It can also be talked about as an almost continuous collection of momentum eigenstates (i.e., just as energy levels, only certain momenta are allowed for an electron). For every eigenstate there is an another with an equal and opposite momentum, i.e., if we populate every momentum eigenstate in a band, the net momentum of electrons will be zero.

If a band is not that populated, then under the influence of electric field, the electrons can redistribute themselves to appropriate unoccupied energy/momentum eigenstates within that band. Whereas, if the band is densely populated, there are not much free states available for redistribution. The more free states are available within a band, the more conductive it becomes.

Note that electrons can also lose their energy/momenta as thermal losses due to collisions with kernels in the lattice. This causes them to shift to a lower energy state within the band, and they can drift under the field once again. Likewise, electrons whose momenta are directed such that they decelerate under the field also will have their energy/momenta lost.

All in all, this net motion of electrons (drift velocity) is what's needed to sustain an electric current.

What determines the conductivity of a band? enter image description here

In metals, the fermi level $(E_F)$ passes through the valence band. As $T$ becomes greater than $0$, the electrons just below $E_F$ surpass the level and shift to higher energy states within the band. As there are a lot of unoccupied eigenstates within the band allowing redistribution under an electric field, the valence band is the conduction band for metals.

In semi-metals, $E_F$ passes through the trough of the valence band which has bimodal density of states. So, they need to be at somewhat a higher temperature than metals to be conductive (so that the electrons under $E_F$ can shift to energy levels with greater density of states allowing them to be more conductive). Technically, this bimodal valence band is also the conduction band.

In semi-conductors, $E_F$ lies in the band gap. All states in the band below $E_F$ (the valence band) are filled at $0K$ and the band is not conductive. At higher temperatures, however, the electrons can have enough energy to surpass the band gap and shift to the immediately higher unoccupied band. The electrons in this higher band, now become conductive, and so the band is called the conduction band.

In insulators (e.g., diamond), the $E_F$ passes through a very large band gap. The valence band is filled and non-conductive, and the occupancy of electrons in the band immediately higher than $E_F$, even at higher temperature, is almost null because of the very large band gap that needs to be surpassed. This higher band is what we refer to as conduction band, although no appreciable conduction takes place here. This should be an example to the fact that just as extremely populated bands, extremely non-populated bands are non-conductive too.

  • $\begingroup$ Why the bonding and anti-bonding $s$ orbital's don't have the same energy difference from their $s$ atomic orbitals (like $p$ orbitals have)? $\endgroup$
    – Anton
    Nov 28, 2021 at 12:25

A useful way to visualize the difference between conductors, insulators and semiconductors is to plot the available energies for electrons in the materials. Instead of having discrete energies as in the case of free atoms, the available energy states form bands. Crucial to the conduction process is whether or not there are electrons in the conduction band. In insulators the electrons in the valence band are separated by a large gap from the conduction band, in conductors like metals the valence band overlaps the conduction band, and in semiconductors there is a small enough gap between the valence and conduction bands that thermal or other excitations can bridge the gap. With such a small gap, the presence of a small percentage of a doping material can increase conductivity dramatically.

An important parameter in the band theory is the Fermi level, the top of the available electron energy levels at low temperatures. The position of the Fermi level with the relation to the conduction band is a crucial factor in determining electrical properties.

italics mine


The vertical variable is the energy levels of the bands.


I think this extract answers your questions within the band theory.

One can also visualize the electrons energy of the conduction band as solutions on the whole lattice, whereas in the valence band the electrons are tied to individual atoms , that is why it is called "valence".

  • $\begingroup$ I personally think that this answer is of the form: because those conductive electrons are in a magic band named the conductive band. OP might retaliate with: what specifically makes the conduction band conductive?. Having addressed that, I quite like the rest of your explanation. (Photons are also a great source of energy for those electrons to jump between bands, specially in semiconductors. $\endgroup$ Oct 13, 2021 at 14:15
  • $\begingroup$ @FriendlyLagrangian It clearly says that the electrons need a lot of energy to get in the conduction band from the valence band in insulators, and no energy for conductors. They can live in the conduction band, i.e. the whole lattice is available to them in conductors. In insulators they cannot get there , a very large thermal energy ( temperature) needed , and high temperatures melt lattices. $\endgroup$
    – anna v
    Oct 13, 2021 at 14:38

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