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Dispersion of light is the phenomenon of splitting of a beam of white light into its seven constituent colours on passing through a glass prism. The band of coloured components of a light beam is called its spectrum. The cause of dispersion is that different colours of white light with different wavelengths undergo different deviations on passing through a glass prism.
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Difference between soaps and detergents:
|
Soaps |
Detergents |
|
(i)Soaps are biodegradable.
(ii) Soaps have relatively weak cleansing action. |
(i) Detergents are not biodegradable. (ii) Detergents have a strong cleansing action. |
Cleaning action of soap:
Soaps are molecules in which the two ends have differing properties, one is hydrophilic, that is it dissolves in water, while the other end is hydrophobic, that is it dissolves in hydrocarbons. When soap is at the surface of water the hydrophobic ‘tail’ of soap will not be soluble in water and the soap will align along the surface of water with the ionic end in water and the hydrocarbon ‘tail’ protruding out of water. Inside water, these molecules have a unique orientation that keeps the hydrocarbon portion out of the water. This is achieved by forming clusters of molecules in which the hydrophobic tails are in the interior of the cluster and the ionic ends are on the surface of the cluster. This formation is called a micelle. Soap in the form of a micelle is able to clean, since the oily dirt will be collected in the centre of the micelle. The micelles are large enough to scatter light. Hence a soap solution appears cloudy.
When soap is used for washing clothes with hard water, a large amount of soap in water is reacting with the calcium and magnesium ions of hard water to form an insoluble precipitate called scum.
Disadvantage of using detergents:
Detergents are not biodegradable and hence cause water pollution.
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Meghna Thapar 5 years, 8 months ago
Extraction of Less Reactive Metals:
The less reactive metals are extracted by the reduction of their oxides by heat alone.
Example: Mercury (II) sulphide ore is roasted in air when mercury (II) oxide is formed. When this mercury (II) oxide is heated to about 300° C, it decomposes to form mercury metal.
Extraction of Moderately Reactive Metals:
The moderately reactive metals in the middle of the reactivity series are extracted by the reduction of their oxides with carbon, aluminium, sodium or calcium.
It is easier to obtain metals from their oxides (by reduction) than from carbonates or sulphides. So, before reduction can be done, the ore is converted into a metal oxide. The concentrated ores can be converted into metal oxides by the process of calcination or roasting.
Calcination is the process in which a carbonate ore is heated strongly in the absence of air to convert it into a metal oxide.
For example: When zinc carbonate is heated strongly in the absence of air, it decomposes to form zinc oxide and carbon dioxide. Roasting is the process in which a sulphide ore is strongly heated in the presence of air to convert it into a metal oxide.
Extracting Metals towards the Top of the Activity Series:
Metals high up in the reactivity series are very reactive. These metals have a strong affinity for oxygen. So, oxides of sodium, magnesium, calcium and aluminium cannot be reduced by carbon.
These metals are obtained by electrolytic reduction.
Sodium, magnesium and calcium are obtained by the electrolysis of their molten chlorides.
Example: Sodium metal is extracted by the electrolytic reduction of molten sodium chloride. When electric current is passed through molten sodium chloride, it decomposes to form sodium metal and chlorine gas.
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