Introduction to Soil Chemistry
Introduction to Soil Chemistry
Introduction to Soil Chemistry
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energy considerations 37<br />
side-by-side, as depicted in the p x–p x representation. This is possible because<br />
the p and d orbitals are directed in space along the x, y, and z axes.<br />
In some a<strong>to</strong>ms the p and s orbitals are mixed <strong>to</strong>gether <strong>to</strong> form several equivalent<br />
orbitals. The most common example is carbon, where four orbitals are<br />
formed by mixing one s orbital with three p orbitals <strong>to</strong> give four equivalent<br />
orbitals designated as sp 3 orbitals.<br />
Silicon as SiO 2, or its polymeric form [SiO 4] n, has only two types of orbitals<br />
available for bonding. In the following scheme, sp 3 bonding occurs in SiO 4 and<br />
[SiO 4] n; however they are tetrahedral, not planar as shown:<br />
O Si O O<br />
O<br />
Si<br />
(2.1)<br />
In SiO 2 the Si and O a<strong>to</strong>ms have sp 2 -hybridized orbitals 5 forming sigma bonds<br />
and p orbitals forming p bonds. The oxygen also has p orbitals containing lone<br />
pairs of electrons. Polymeric silicon has sp 3 -hybridized obitals available for<br />
bonding, while oxygen still has lone pairs of electrons in p orbitals. These then<br />
are the orbitals available for bonding <strong>to</strong> elements or compounds that come<br />
in<strong>to</strong> contact with the particle’s surface. This type of interaction could be of<br />
either end-on-end or p type (i.e., side-by-side). In all cases steric hindrances<br />
may limit the type of interaction occurring.<br />
Clays contain aluminum oxides in addition <strong>to</strong> silica as SiO 2 and its polymeric<br />
forms. Again there are the p orbitals of oxygen and sp-hybridized<br />
orbitals from aluminum, which may result in end-on-end or side-by-side<br />
bonding with the same restrictions encountered with silicon.<br />
For removal of compounds bonded <strong>to</strong> silicon, aluminum or oxygen bonded<br />
<strong>to</strong> silicon or aluminum p- and sp-hybridized orbitals must be broken and new<br />
bonds formed. This will require energy and the correct orientation of attacking<br />
groups along with an effective attacking species. In addition, the rate of<br />
species removal will depend on the reaction path and the steric fac<strong>to</strong>rs<br />
involved. All of these put <strong>to</strong>gether will determine the overall rate of the reaction<br />
and the time needed for extraction.<br />
2.4. ENERGY CONSIDERATIONS<br />
The first question in terms of the stability or strength of any bonding interaction<br />
is energy. A general equation for energy is DH = H i - He. This equation<br />
5 sp 2 -hybridized orbitals are formed by mixing one s orbital with two p orbitals <strong>to</strong> produce three<br />
sp 2 orbitals.<br />
O<br />
O