Ozone: Laboratory preparation, Properties, Uses, structure, layer

Ozone

Ozone is an allotropic form of oxygen and its molecular formula is O₃. It is an unstable dark blue diamagnetic gas. The presence of ozone in extremely small quantities has been observed in the atmosphere in places near the seaside (or) big lakes. It is present in sufficient quantities in the atmosphere at attitudes of 12 to 15 miles above the earth's surface. Ozone is particularly important since there is a layer of ozone in the upper atmosphere which absorbs harmful UV radiations from the sun and protect the people and other living organisms on the earth.

Laboratory preparation

Ozone is prepared in the laboratory by passing silent electrical discharges through dry oxygen in an apparatus known as the ozoniser. The commonly used ozoniser is Siemen's ozoniser

(i)  Siemen's ozoniser

It consists of two concentric metal tubes sealed together at one end. The inner side of the inner tube and the outer side of the outer tube are coated with tin foil and connected to one terminal each of an induction coil. A current of pure dry oxygen at low temperature is passed through annular space between the two tubes and by the silent action of electric discharge, the oxygen is partially converted into ozone. The sample of gas escaping from ozoniser is called ozonised oxygen and contains about 12% ozone.

Properties

(i)  Physical properties

It is a light blue gas which condense at 160.6 K into a dark blue liquid. This liquid freezes at 23.3 K.

Chemical properties

1) Decomposition : Pure ozone decomposes with an explosive violence.

 2O3 -- >  3O2

2) Oxidising action : Since it can liberate an atom of nascent oxygen easily (O3 -- >  O2 + O) it acts as a powerful xidizing agent.

i)Lead sulphide is oxidised to lead sulphate PbS + 4O3 -- >  PbSO4 + 4O2

ii) Potassium manganate is xidized to potassium permanganate

2K2MnO4 + H2O + O3 -- >  2KmnO4 + 2KOH + O2

3) Ozone reacts with peroxides and reduces it to oxides with the liberation of oxygen.

BaO2 + O3 -- >  BaO + 2O2

H2O2 + O3  -- >  H2O + 2O2

Uses of ozone

1.     It is used as germicide and disinfectant.

2.     It is used for bleaching oils, ivory, flour, starch, etc.

3.     Used in the manufacture of artificial silk and synthetic camphor.

Ozone structure

The ozone molecule consists of three oxygen atoms having a bent  structure

Each O atom contributes six valence electrons and so the total 3x6=18 electrons.

Ozone molecule is said to be resonance hybrid of the two contributing forms I & II.

Ozone layer

Ozone is produced in the upper atmosphere through absorption of a

SKRWRQ  K# RI XOWUDYLROHW OLJKW E\ DQ 2₂ molecule.

O2(g)   K# -- >  2O(g)

O(g) + O2(g) -- >  O3(g)

The ozone molecule formed has an excess of energy and dissociates back to O2 and O and it reacts with another molecule (M) such as CO2, N2 or O2, which causes the excess energy thus stabilizes the ozone molecule

O^*3(g) + M(g)        -- > O3(g)+ M^*(g)

Factors affecting ozone layer

The ozone in the upper atmosphere is important in shielding us from the intense ultraviolet radiation coming from the sun. The so-called ozone shield is a shell about 30 km altitude which contains enough ozone to absorb short wavelength UV radiation (less than 300 nm). Hence ozone is considered to be 'earth's protective umbrella'. The absorption causes dissociation of O3 to reform O2.

O3(g)   K^# -- >  O2(g) + O(g)

2O(g) -- >  O^·2(g)

O^·2(g) + M(g) -- > O2(g)+ M^·(g)

Existence of ozone shield owes to the life on the earth, since living tissues are very sensitive to wavelengths of ultraviolet absorbed by ozone. In recent years, the shield is damaged mainly by supersonic aircraft and chlorofluorocarbon products in the jet exhaust reduce ozone, and decreases its concentration in the shield.

Chlorofluorocarbons react with O₃ and causes a hole in the ozone layer. CFC's are used as refrigerants and as propellants in some "aerosol sprays". The lifetime of CFCs are so long that in another decades, the extent of ozone depletion in the upper atmosphere will be tremendous. It is reported that the holes caused in the ozone layer over the Antarctic and Arctic ocean are due to the use of CFCs in aerosols and refrigerators. It is feared that this will allow an excessive amount of UV light to reach the earth which will cause skin cancer (melanoma) in human.

UV

CFC -- >          Cl_(g)

Cl(g) + O3(g) -- >  ClO(g) + O2(g)

ClO + O(g)  -- >  Cl(g) + O2(g)

O3(g) + O(g) -- >  2O2(g)

It is also seen that the oxides of nitrogen (from car exhausts) and the halogen can damage the ozone layer. Therefore the protecting shield of the earth must be protected by taking immediate steps over the control of pollution.