2.1. STRUCTURE
17
of the large anions A"- with the small cations C"+ located in the tetrahedral sites of
the anion FCC lattice. If the anions touch each other, their radii have the value
a. = a/21/2, where a is the lattice parameter, and the radius aT of the tetrahedral site
aT = 0 . 2 2 4 7 ~ ~
is given by Eq. (2.2). This is the case for the very small Ai3+ cation
in the AlSb structure. In all other cases the cations in Table B.2 are too large to fit in
the tetrahedral site so they push the larger anions further apart, and the latter no
longer touch each other, in accordance with Fig. 2.9. In a covalent model for the
structure consisting of neutral atoms A and C the atom sizes are comparable, as the
data in Table B.2 indicate, and the structure resembles that of Si or Ge. To compare
these two models, we note that the distance between atom A at lattice position 0 0 0
and its nearest neighbor C at position
is equal to t a u , and in Table B.3 we
compare this crystallographically evaluated distance with the sums of radii of ions
A"-, C"+ from the ionic model, and with the sums of radii of neutral atoms A and C
of the covalent model using the data of Table B.2. We see from the results on Table
B.3 that neither model fits the data in all cases, but the neutral atom covalent model
is closer to agreement. For comparison purposes we also list corresponding data for
several alkali halides and alkaline-earth chalcogenides that crystallize in the cubic
rock salt or NaCl structure, and we see that all of these compounds fit the ionic
model very well. In these compounds each atom type forms a FCC lattice, with the
atoms of one FCC lattice located at octahedral sites of the other lattice. The
octahedral site has the radius aoct = 0.4141 la, given by Eq. (2.1), which is larger
than the tetrahedral one of Eq. (2.2).
Since the alkali halide and alkaline-earth chalcogenide compounds fit the ionic
model so well, it is significant that neither model fits the structures of the
semiconductor compounds. The extent to which the semiconductor crystals exhibit
ionic or covalent bonding is not clear from crystallographic data. If the wavefunction
describing the bonding is written in the form
where the coefficients of the covalent and ionic wavefunction components are
normalized
2
acov +ai?,, = 1
then a:ov is the fractional covalency and ai?,, is the fractional ionicity of the bond. A
chapter (Poole and Farach 2001) in a book by Karl Boer (2001) tabulates the
effective charges e* associated with various 11-VI and 111-V semiconducting
compounds, and this effective charge is related to the fractional covalency by the
expression
8 - N + e *
8
4 o v =
17
of the large anions A"- with the small cations C"+ located in the tetrahedral sites of
the anion FCC lattice. If the anions touch each other, their radii have the value
a. = a/21/2, where a is the lattice parameter, and the radius aT of the tetrahedral site
aT = 0 . 2 2 4 7 ~ ~
is given by Eq. (2.2). This is the case for the very small Ai3+ cation
in the AlSb structure. In all other cases the cations in Table B.2 are too large to fit in
the tetrahedral site so they push the larger anions further apart, and the latter no
longer touch each other, in accordance with Fig. 2.9. In a covalent model for the
structure consisting of neutral atoms A and C the atom sizes are comparable, as the
data in Table B.2 indicate, and the structure resembles that of Si or Ge. To compare
these two models, we note that the distance between atom A at lattice position 0 0 0
and its nearest neighbor C at position
is equal to t a u , and in Table B.3 we
compare this crystallographically evaluated distance with the sums of radii of ions
A"-, C"+ from the ionic model, and with the sums of radii of neutral atoms A and C
of the covalent model using the data of Table B.2. We see from the results on Table
B.3 that neither model fits the data in all cases, but the neutral atom covalent model
is closer to agreement. For comparison purposes we also list corresponding data for
several alkali halides and alkaline-earth chalcogenides that crystallize in the cubic
rock salt or NaCl structure, and we see that all of these compounds fit the ionic
model very well. In these compounds each atom type forms a FCC lattice, with the
atoms of one FCC lattice located at octahedral sites of the other lattice. The
octahedral site has the radius aoct = 0.4141 la, given by Eq. (2.1), which is larger
than the tetrahedral one of Eq. (2.2).
Since the alkali halide and alkaline-earth chalcogenide compounds fit the ionic
model so well, it is significant that neither model fits the structures of the
semiconductor compounds. The extent to which the semiconductor crystals exhibit
ionic or covalent bonding is not clear from crystallographic data. If the wavefunction
describing the bonding is written in the form
where the coefficients of the covalent and ionic wavefunction components are
normalized
2
acov +ai?,, = 1
then a:ov is the fractional covalency and ai?,, is the fractional ionicity of the bond. A
chapter (Poole and Farach 2001) in a book by Karl Boer (2001) tabulates the
effective charges e* associated with various 11-VI and 111-V semiconducting
compounds, and this effective charge is related to the fractional covalency by the
expression
8 - N + e *
8
4 o v =