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TOPIC: OXYGEN
CONTENTS:
PERIOD 1: GENERAL PROPERTIES OF OXYGEN
Oxygen is the most abundant element on earth. It is prepared in the laboratory by catalytic decomposition of Potassium trioxochlorate(V) or hydrogen peroxide. Industrially, it is prepared by the liquefaction of air followed by fractional distillation of liquefied air.
Oxygen, being strongly electronegative, is chemically very reactive. It reacts with most metals to form basic oxides which are ionic, they also reacts with most non- metals to form acidic oxides which are covalent molecules and they reacts with hydrocarbons, fuels [to form CO2 and H2O. It rekindles a glowing splint to indicate its presence in any place.
The oxides of oxygen can be classified into basic, acidic, amphoteric and neutral oxides. Peroxide is prepared by the action of a dilute acid on the peroxides of certain metals. It is a strong oxidizing agent. However, in the presence of more powerful oxidizing agents, ozone, O3, is an unstable allotrope of oxygen. The ozone layer in the atmosphere acts as a protective shield by preventing too much ultra-violet radiation from falling on earth and harming living organism.
Electronic Structure and Bonding Capacity of Oxygen
Oxygen is an element in group (VIA) of the periodic table. Its atomic number is 8, and has an electronic configuration of 1S2 2S2 2P4 ————-Electronic structure
Thus, oxygen forms a complete octet by either accepting two electrons from a donor to form O2-in an ionic substance, or by sharing two electrons with other atoms to form a covalent substance. At room temperature and pressure, oxygen exists as a discrete gaseous diatomic molecule, O2 the two toms are joined together by double covalent bond, O=O.
EVALUTION
PERIOD 2: LABORATORY AND INDUSTRIAL PREPARATION OF OXYGEN
LABORATORY PREPARATION
There are two general and common methods for the laboratory preparation of oxygen
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