- What are macromolecules?
- What are some examples of inorganic macromolecules?
- How is the properties of sulfur related to its structure?
What are macromolecules?
A macromolecule is a very large molecule having a polymeric chain structure.
Proteins, polysaccharides, genes, ruber, and synthetic polymers consist of
For synthetic polymers, here are the abbreviations for some common polymers.
|HDPE: high density polyethylene
||LDPE: low density polyethylene
|PET: polyethylene terephthalate
||PVA: polyvinyl alcohol
|PVC: polyvinyl chloride
There are only a few known inorganic macromolecules. For example, when liquid
sulfur is poured into cold water, long chains of ...-S-S-S-S-S-... are formed.
These molecules are present in a phase known as elastic sulfur.
is an introduction to polymers, if you are interested.
What are some examples of inorganic macromolecules?
inorganic macromolecules can be divided into several categories: solids
formed mainly due to covalent bonds, organosilanes, siloxanes and organosiloxanes.
Solids formed mainly due to covalent bonds
We have mentioned diamond, graphite, silicon, germanium, etc as large
molecules. In this section, some more examples are given:
Zinc sulfide has two forms (or phases): the
wurtzite and the
zinc blende. These are typical structures, because many other
common compounds have the same structure. Knowing the bonding, geometry,
symmetry of these structures is important, because scientific discussion
and applications are based on their structures. The difference between
wurtzite and zinc blende illustrates some fundamental geometry and symmetry
Wurtzite is a typical mineral, often involving iron and zinc sulfide, and
For example: ZnO, SiC, AlN, CaSe, BN, C(Hexagonal Diamond) all have the same
crystal structure as wurtzite in terms of bonding, symmetry, packing
The zinc blende is cubic. It can be perceived as a f.c.c. lattice of S
with half of the tetrahedral sites occupied by Zn. A unit cell of the crystal
structure is shown in
Zinc blende, and you can see this structure from various perspective.
The diagram on the page can be manipulated by moving the mouse.
The same group has also got a
wurtzite structure that you can manipulate. By the way,
the zinc blende structure has the same bonding skeleton as the diamond
structure. Thus, the wurtzite and zinc blende structures are two typical
structural types for inorganic macromolecules.
Silanes and organosilanes
Since Si-Si is much weaker than C-C bonds, silanes SinH2n+2,
are not as stable as alkanes. Methane is a stable gas, but silane SiH4
explode as soon as it comes in contact with air. Silane is made by reacting
Mg2Si with dilute HCl, but the silane produced burns as soon
as it comes in contact with air at the surface of the solution:
Mg2Si + 4 HCl = 2 MgCl2 + SiH4
SiH4 + 2 O2 = SiO2 + 2 H2O
When an organosilane reacts with water, the Si-Si bonds break:
R3Si-SiR3 + 2 H2O = 2 R3SiOH + H2
where R is an alkyl or aryl group. Organosilanes have some unique applications, and
silane coupling agents, RnSiX4-n (X being a halogen)
Siloxanes and organosiloxanes
Siloxanes and organosiloxanes have Si-O-Si-O-Si linkage, and these are stable
polymers due to the strong Si-O-Si bonds. Since Si atoms tend to form four
bonds, these polymers form two- and three-dimensional networks, making them
| | |
R O O
The siloxane technologies
makes use of silicon polymers whereas
is a very common application.
Silicates are based on Si-O-Si linkages. Quartz for example is based on
three-dimensional frame work of these linkages. We will have another page
on silicates put on this site in the future. The picture shown here is
a picture of quartz.
How is the properties of sulfur related to its structure?
Sulfur is in the same group as oxygen, and its valence electrons have the
These six electrons usually occupy the four sp3 hybrid orbitals,
two of which have a pair of electrons each, and the other two have only
one electron each. Thus, sulfur usually form two bonds such as
H2S, its structure similar to H2O.
Sulfur atoms bond to each other forming the cyclic molecules such as
S6 and S8, a diagram of the latter is shown here.
The two bonds and the two lone pairs of electrons around the sulfur point
to the direction of a tetrahedron, making the -S- angle approximately 100
Sulfur has three allotropes: rhombic, monoclinic, and plastic sulfur.
At room temperature, monoclinic sulfur is the the stable form. When heated,
monoclinic sulfur melts to form a viscous liquid at 119 degree C at the
atmosphere pressure. At higher pressure, the monoclinic sulfur transforms into
the rhombic sulfur. Both crystalline forms have the S8 crown
shaped molecule and the plastic sulfur has a chain structure of unspecified
number of atoms Sn (n is a very large unspecified number).
Since we are talking about the element sulfur, we might include some
information on it. Sulfur occur as minerals: pyrite, FeS2
(also known as fool's gold); gypsum, CaSO4ºH2O,
(when dehydrated it is called paster of paris). Sulfur also occur as
an element in nature because some bacterial converts sulfur oxides and other
compounds to elemental sulfur. Elemental sulfur is extrated from under
ground by hot water and air in a process called the Frasch process.
Sulfur is easily oxidized to sulfur dioxide
S8 + 8 O2 = 8 SO2
The SO2 is a bent molecule with an O-S-O angle of 120 degrees.
It reacts further with water and with oxygen as examplified by the
SO2 + H2O = H2SO3 (sulfurous acid)
2 SO2 + O2 = 2 SO3 (catalyst required)
SO3 + H2O = H2SO4 (sulfuric acid)
Na2SO3 + S = Na2S(=S)O3 (known as hypo)
What are the properties and structures of phosphorus?
Phosphorus has only 5 valence electons, one less electron than sulfur. Thus
it tends to form three bonds around a P atom. The analogous of ammonia is
phosphine, PH3, which is air stable with a melting point of
White phosphorus can be obtained by reducing phosporus oxide with carbon:
P4O10 + 10 C = P4 + 10 CO
The crystals consist of P4 molecules as shown here, and
it undergoes natural combustion if not stored under water. The combustion
leads to the formation of P4O10.
White phosphorus converts to stable red, black, violet and scarlet phosphorus,
which have complicated network of
macromolecules. This link shows the images using CrystalMaker Software.
The bonding in P4 can be explained in the same manner as that
described for sulfur, but that is left as an exercise. As most other
non-metallic elements, phosphorus also form a complicated covalent solid.
This page is roughly set up, not polished yet. When given time, more needs
to be done.