Sunday, June 29, 2008

Why is SO3 is Lewis Acid?

I remember somebody asking this question in comments. I could not locate the answer at that time in the books that I referred to at that time.

Today I came across the issue in Inorganic Chemistry by Dr.O.P.Tandon, 2007 edition, page 120.

It says

Molecules haivng a multiple bond between atoms of dissimilar electronegativity act as Lewis acids. Typical examples of molecules belonging to this class of Lewis acids are CO2, SO2 and SO3. Under the influence of attacking Lewis base, one π-electron pair will be shifted towardsmore negative atom.

In page 128 question (viii) is more direct.

So# has acidic behaviour. Explain

Hint:Sulphur atom is attached with three very highly electronegative oxygen atoms. As a result, electrons are drawn towards oxygen atoms and S-atom remains wiht electron density and thus has the tendency to accept electrons. So it acts as a Lewis acid.

Wednesday, June 18, 2008

Organic Chemistry the Easy Way

Organic Chemistry the Easy Way

Bruce A. Hathaway, Bruce A. Hathaway Ph.D.

YOu can have a limited preview of it in google books

Monday, June 9, 2008

Blog status

Revision points of spectrum of hydrogen atom are updated.

Saturday, June 7, 2008

Acquired NCERT Books

Today I acquired the NCERT books of Chemistry Class XI and XII to help me in JEE studies.

Monday, June 2, 2008


Molecular Formula Si

Silicon Si;

Atomic weight 28.0855
Atomic number 14;
valence 4
Melting point 1414 deg C;
Boiling point 3265 deg C;
sp. gr. 2.33 (25 deg C);

Berzelius, generally credited with the discovery, in 1824 succeeded in preparing amorphous silicon by removing the fluosilicates by repeated washings. Deville in 1854 first prepared crystalline silicon, the second allotropic form of the element.

Silicon is present in the sun and stars and is a principal component of a class of meteorites known as "aerolites". It is also a component of tektites, a natural glass of uncertain origin.

Natural silicon contains three isotopes.

Fourteen other radioactive isotopes are recognized.

Silicon makes up 25.7% of the earth's crust, by weight, and is the second most abundant element, being exceeded only by oxygen.

Silicon is not found free in nature, but occurs chiefly as the oxide and as silicates. Sand, quartz, rock crystal, amethyst, agate, flint, jasper, and opal are some of the forms in which the oxide appears. Granite, hornblende, asbestos, feldspar, claymica, etc. are but a few of the numerous silicate minerals.

Silicon is prepared commercially by heating silica and carbon in an electric furnace, using carbon electrodes. Several other methods can be used for preparing the element.

Amorphous silicon can be prepared as a brown powder, which can be easily melted or vaporized.

Crystalline silicon has a metallic luster and grayish color.

The Czochralski process is commonly used to produce single crystals of silicon used for solid-state or semiconductor devices. Hyperpure silicon can be prepared by the thermal decomposition of ultra-pure trichlorosilane in a hydrogen atmosphere, and by a vacuum float zone process.

This product can be doped with boron, gallium, phosphorus, or arsenic to produce silicon for use in transistors, solar cells, rectifiers, and other solid-state devices which are used extensively in the electronics and space-age industries.

Hydrogenated amorphous silicon has shown promise in producing economical cells for converting solar energy into electricity.

Silicon is a relatively inert element, but it is attacked by halogens and dilute alkali. Most acids except hydrofluoric, do not affect it.

Silicones are important products of silicon. They may be prepared by hydrolyzing a silicon organic chloride, such as dimethyl silicon chloride. Hydrolysis and condensation of various substituted chlorosilanes can be used to produce a very great number of polymeric products or silicones, ranging from liquids to hard, glasslike solids with many useful properties.

Elemental silicon transmits more than 95% bf all wavelengths of infrared, from 1.3 to 6.7 um.

Silicon is one of man's most useful elements. In the form of sand and clay it is used to make concrete and brick; it is a useful refractory material for high-tempemture work, and in the form of silicates it is used in making enamels, pottery, etc.

Silica, as sand, is a principal ingredient of glass, one of the most inexpensive of materials with excellent mechanical, optical, thermal, and electrical properties. Glass can be made in a very great variety of shapes, and is used as containers, window glass, insulators, and thousands of other uses.

Silicon tetrachloride can be used to iridize glass. Silicon is important in plant and animal life. Diatoms in both fresh and salt water extract silica from the water to build up their cell walls.

Silica is present in ashes of plants and in the human skeleton. Silicon is an important ingredient in steel;

silicon carbide is one of the most important abrasives and has been used in lasers to produce coherent light of 4560 A.

Miners, stonecutters, and other engaged in work where siliceous dust is breathed in large quantities often develop a serious lung disease known as silicosis.