Question 11.25 What are allotropes? Sketch the structure of two allotropes of carbon namely diamond and graphite. What is the impact of structure on physical properties of two allotropes?
Class XI The p-Block Elements Page 324
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An allotrope is one of a variety of forms in which an element can exist. This does not refer to the state of an element, whether solid, liquid, gas, or plasma. It refers to the tendency of an element to exist in different structural forms.
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An allotrope is one of a variety of forms in which an element can exist. This does not refer to the state of an element, whether solid, liquid, gas, or plasma. It refers to the tendency of an element to exist in different structural forms.
Hope this helps you...
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the phenomena of existence of an element into two or more forms which differ in physical properties but have same chemical properties is known as allotropy. and the different forms of elements are known as allotropes.
crystalline carbon occurs in two allotropes.
(1) graphite and (2) diamond, a third allotrope of carbon is Fullerene was discovered in 1985 by H.W Kroto, E. samlley and R.F Curl.
in diamond, Carbon is sp³ hybridized and linked to other four atoms.tetrahedrally. there is three dimensional network of carbon in diamond.
in graphite, each carbon is sp² hybridized and makes three sigma bonds with the neighboring carbon atoms. it has layered structure and the layers are held by weak van der waals force.
impact of the structures of diamond and graphite on physical propertiesof the two allotropes.
1. diamond because of its hardness, is used as an abrasive and in making dyes while graphite is so soft that it marks paper and it is used as dry lubricant in machines.
2. diamond doesn't conduct electricity whereas graphite is a good cinductor of electricity because of the presence of one free electron in each carbon atom.
3. diamond is transparent while graphite is opaque.
crystalline carbon occurs in two allotropes.
(1) graphite and (2) diamond, a third allotrope of carbon is Fullerene was discovered in 1985 by H.W Kroto, E. samlley and R.F Curl.
in diamond, Carbon is sp³ hybridized and linked to other four atoms.tetrahedrally. there is three dimensional network of carbon in diamond.
in graphite, each carbon is sp² hybridized and makes three sigma bonds with the neighboring carbon atoms. it has layered structure and the layers are held by weak van der waals force.
impact of the structures of diamond and graphite on physical propertiesof the two allotropes.
1. diamond because of its hardness, is used as an abrasive and in making dyes while graphite is so soft that it marks paper and it is used as dry lubricant in machines.
2. diamond doesn't conduct electricity whereas graphite is a good cinductor of electricity because of the presence of one free electron in each carbon atom.
3. diamond is transparent while graphite is opaque.
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