Diamond and Graphite
Diamond and Graphite: Overview
This topic explains the structures and uses of diamond and graphite. Diamond, Graphite are allotropes of carbon. Diamond is a colourless, transparent substance having extraordinary brilliance and Graphite is a greyish-black, opaque substance.
Important Questions on Diamond and Graphite
The form of carbon which is used as a lubricant at high temperature is _____.(graphite/diamond/fullerene)
The form of carbon which is known as black lead is _____. (diamond/graphite/fullerene)
Name the hardest natural substance known.
Name the element whose allotropic form is graphite.
Diamond and graphite are the covalent compounds of carbon elements (C).
The pencil leads are made of mainly:
A diamond-toothed saw is usually used for cutting:
State any two uses of graphite.
Why is graphite a good conductor of electricity but diamond is a non-conductor of electricity?
Describe the structure of graphite with the help of a labelled diagram.
What is graphite? Of what substance is graphite made?
State any two uses of diamond.
Explain why, diamond has a high melting point.
Describe the structure of diamond. Draw a simple diagram to show the arrangement of carbon atoms in diamond.
What is diamond? Of what substance is diamond made?
State one use of diamond which depends on its 'extraordinary brilliance' and one use of graphite which depends on its being 'black and quite soft'.
Explain why, diamond can be used in rock drilling equipment but graphite cannot.
Explain why, graphite can be used as a lubricant but diamond cannot.
Write two points of difference in the structures of diamond and graphite.
Explain why diamond is hard while graphite is soft (though both are made of carbon atoms).
