Nitrogen (N) and its Behaviour:
(1) Nitrogen is the lightest element of 15th group
with the symbol N and atomic number 7. It often
called the pnictogens.
The name pnictogens comes from the Greek πνίγειν "to
choke", directly referencing nitrogen's asphyxiating properties.
(2) The name Nitrogen gets its name from a
mineral known as “niter”
(potassium nitrate), from which it can be prepared. It was first discovered and
isolated by a Scottish physician Daniel Rutherford in 1770.
(3) Nitrogen is a fairly common element
in the earth’s crust. It is most important constituent of atmosphere, making up
to 78.08 %. Nitrogen is a colorless, odorless, non combustible and
nontoxic gas. Makes up the major portion of the atmosphere, but will not
support life by itself.
(4) The greatest use of nitrogen is in
ammonia which is used for fertilizer production and to produce nitric acid.
Nitrogen gas is used where inert atmosphere is needed, such as in an ordinary
light bulb. Nitrogen is also used in protecting historic documents. Nitrogen is
also used in storage of food stuff and in explosives.
(5) Nitrogen is use in purging air
conditioning and refrigeration systems, and in pressurizing aircraft tires. It May
cause asphyxiation by displacement of air. Under prolonged exposure to fire or
heat containers may rupture violently and rocket
(6) Nitrogen is absolutely essential to
all living organisms. It is important part of all protein molecules which,
among other functions, are the building materials in all kinds of cells.
Abnormal Behaviour of
Nitrogen:
(1) Nitrogen is a gas, while other
elements are solids.
(2) Nitrogen molecule is diatomic (N2)
while molecules of P, As and Sb are tetra atomic (P4, As4,
Sb4) and that of Bi is mono atomic.
(3) Halides of nitrogen except NF3
are highly explosive.
(4) N2O3 and N2O5
are monomeric while trioxides and pentoxides of P,As and Sb are dimeric.
(5) It is chemically inert due to the
presence of triple bond other elements are highly reactive due to presence of
single bond in their molecule.
(6) N2, CO, (CN)¯ are isoelectronic species but N2
is less reactive due to nonpolar nature and high ionisation energy.
(7) N does not form sulphides.
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