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Why does graphite conduct electricity but diamond doesn t?
Graphite can conduct electricity because of the delocalised (free) electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.
Why is diamond not a good conductor of electricity?
As we know diamond is a giant covalent structure i.e. each carbon atom is covalently bonded with other carbon atoms. So the four outermost electrons, four carbon atoms, are engaged or trapped in the covalent bonds which means that there are no free electrons. So diamond is a bad conductor of electricity.
Why does diamond have a high melting and boiling point?
Diamond has a very high melting point because a large amount of energy is needed to overcome the many strong covalent bonds. There are no electrons or other charged particles that are free to move so diamond does not conduct electricity.
Can electricity pass through diamond?
Diamond does not conduct electricity although it is a good thermal conductor. It is not possible for Pure diamond to conduct electricity as it does not have any delocalized free electrons in the outer shell of the carbon atom. Pure diamond is made of only carbon atoms combined in covalent bonds with other carbon atoms.
Why do both diamond and graphite have high melting points?
Very high melting points – this is because a lot of strong covalent bonds must be broken. Graphite, for example, has a melting point of more than 3,600°C. Variable electrical conductivity – diamond does not conduct electricity, whereas graphite contains free electrons so it does conduct electricity.
Why diamond is high melting point?
Because covalent bonds are strong, diamond contains many covalent bonds. As high temperatures are required to break such strong bonds, diamond melts at a very high temperature.
Why is graphite a good conductor of electricity and soft?
Each carbon atom is bonded into its layer with three strong covalent bonds. This leaves each atom with a spare electron, which together form a delocalised ‘sea’ of electrons loosely bonding the layers together. These delocalised electrons can all move along together – making graphite a good electrical conductor.
Why is graphite a good conductor of electricity but not Diamond?
answered Apr 25, 2019 by muskan15 (-3,990 points) (a) In a graphite molecule, one valence electron of each carbon atom remains free, Thus making graphite a good conductor of electricity. Whereas in diamond, they have no free mobile electron. Thats why diamond are bad conductor electricity.
Why does graphite have a high melting point than diamond?
Like silica, diamond has a very high melting point and it does not conduct electricity. Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity.
Why is diamond a bad conductor of electricity?
Diamond is a bad conductor of electricity because it does not have any delocalized electron like graphite. However graphite and diamond both are allotropes of carbon having the same composition but different structures. Free electrons are carriers of electric current.
How are the atoms of Diamond and graphite bound together?
In these allotropes of carbon, the atoms consisting of carbon atoms in that of the Diamond and Graphite, are bound together by strong covalent bonds with different arrangements. Precious stone and graphite have shift structures which represent their diverse properties, and both are pure carbon.