Abstract
The sol-gel synthesis of metal oxides can be performed via the hydrolysis and condensation of metal cations in aqueous solutions. This inorganic route provides a cheap and reliable way for industrial uses. However, many hydrolyzed precursors can be present simultaneously in the precursor solution and very few data are available on the formation of condensed species. The so-called Partial Charge Model provides a useful guide to describe and predict hydrolysis and condensation reactions in aqueous solutions. A charge-pH diagram can be established. It shows how condensation can be initiated via acid-base or redox reactions. The two basic condensation processes, olation and oxolation, are then discussed in terms of a charge-electronegativity diagram. They can lead either to small solute condensed species (polyanions or polycations) or to the formation of an infinite network (colloids, gels, or precipitates). Complexation by anionic species is finally discussed in the frame of an electronegativity-pH diagram. It also plays an important role during the formation of solid phases.
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Abbreviations
- PCM:
-
Partial Charge Model
- χ:
-
Electronegativity
- Μ:
-
Chemical Potential
- δ:
-
Partial charge
- σ:
-
Chemical softness (= 1/η)
- η:
-
Chemical hardness
- χi, χx or χ(X):
-
Electronegativity of an atom or of a group of atoms
- δ(X) or δx :
-
Partial charge beared by an atom or a group of atoms
- r:
-
Covalent radius
- Zeff :
-
Nuclear effective charge
- k:
-
Constant linking hardness to electronegativity (k = 1.36 in this work)
- z:
-
Oxidation state (valency) of a cation (1≤z≤8)
- χ0 :
-
Pauling electronegativity
- N:
-
Coordination number of a cation (N ≤ 12)
- h:
-
Number of protons removed from an aquo-ion [M(OH2)N]z+
- χw :
-
Mean electronegativity of an aqueous solution given by Eq. (13)
- Β:
-
= RTLn 10 with R perfect-gas constant and T temperature
- cH :
-
Proton concentration
- λ:
-
Constant linking electronegativity to pH(= 0.035 according to Eq. (12))
- χ *+ :
-
Critical electronegativity for acid ionization given by Eq. (77) with Ω=1
- χ *− :
-
Critical electronegativity for basic ionization given by Eq. (77) with Ω=−1
- χ *0 :
-
Critical electronegativity for olation given by Eq. (77) with Ω=0
- χ *OH :
-
Critical electronegativity for oxolation given by Eq. (75)
- PZC:
-
Point of Zero Charge of a solid phase
- AcO− :
-
Acetate ion CH3COO−
- α:
-
Number of water molecules removed by a ligand upon coordination
- χP :
-
Mean electronegativity of a complexed precursor
- n:
-
Valency of an anion Xn−
- m:
-
Stoichiometric coefficient
- q:
-
Number of protons beared by an anion HqX(n−q)−
- χD :
-
Critical electronegativity for ionic dissociation given by Eq. (79)
- χH:
-
Critical electronegativity for hydrolysis given by Eq. (80)
- h *q :
-
Critical hydrolysis ratio associated to a HqX(n−q)− anion given by Eq. (83)
- pH *q :
-
Critical pH value associated to h *q through Eq. (58)
- χq :
-
Mean electronegativity of an anion HqXn−q)−
- δ:
-
Charge differential characteristic of an element given by Eq. (59)
- pHm :
-
Optimum pH for complexation by an anion Xn− given by Eq. (62)
- ox:
-
Oxalate anion C2O 2−4
- δ(χ,X):
-
Partial charge upon the X group when mean electronegativity is χ
- χS:
-
Mean electronegativity of the aquo ligand (2.491 using Table 5)
- Ω:
-
Index for Eqs. (76) and (77)
- σ(N,M):
-
Softness of the [M(OH2)N] complex given by Eq. (86)
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Henry, M., Jolivet, J.P., Livage, J. (1992). Aqueous chemistry of metal cations: Hydrolysis, condensation and complexation. In: Reisfeld, R., JJørgensen, C.K. (eds) Chemistry, Spectroscopy and Applications of Sol-Gel Glasses. Structure and Bonding, vol 77. Springer, Berlin, Heidelberg. https://doi.org/10.1007/BFb0036968
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