The heats of formation of halides (HfX
4 ZrX
4, TiX
4SiX
4CX
4), -ΔH°
298, are empirically expressed in terms of electronegativities (
xC and
xA) of cation and anion (halogen ion):
-ΔH°
298/(4e
2/
rC)=
axA+
b/
xC-
c+
dxA+
e,
where
a, b, c, d, and
e are empirical constants; factor 4,
e, and
rC represent the valence number of cation, the charge on the electron, and cation-radius, respectively. The value of 4
e2/
rC corresponds to electrostatic energy between effective nuclear charge of the M
4+ ion (4
e) and an electron at a distance from its nucleus equal to its ionic radius
rC. Although physical meaning is not clear, this empirical equation is useful in predicting electronegativity and/or ionic radius from the heat of formation, and vice versa. The electronegativity of Hf
4+ is revised to be 1.4 in Pauling's scale and the ionic radius of Th
4+ in tetrahedral site is estimated to be 0.77Å. The heats of formation of GeX
4, SnX
4 and PbX
4 (X: halogen) are related to both cation radius (
rC) and anion radius (
rA):
-ΔH°
298{(-
e2/
rA)/(-100kcal
thmol
-1)}1/2/(4
e2/
rC)=
axA+
b.
From this empirical equation the heat of formation of SnF
4, (g) is estimated to be 235 kcal
thmol
-1.
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