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In graphite which consists of fused hexagons of carbon atoms arranged in sheets there is considerable delocalisation of electrons.
In diamond the structure is "3 dimensional" with each atom of carbon tetrahedrally surronded by 4 other carbon atoms. The bonding is covalent and the electrons in each bond are localised.
What else can I help you with?
Is carbon or gold is a malleable and conducts electricity?
Carbon is not malleable but in some forms can conduct electricity. Gold is malleable and conductive.
Why does graphite conduct electricity whereas diamond does not and they are both allotropes?
Diamond and Graphite have 2 different structures, Diamond has a rigid tetrahedral network whereas Graphite has layers which completely changes the properties of both types of carbon. Basically graphite has free delocalised electrons which means electricity can be conducted, diamond however does not have any delocalised electrons which means it cannot conduct electricity. Both diamond and graphite are made up of strong covalent bonds which means they both have high melting points. Graphite is soft though because the layers which it is made up of slide, this makes it soft. Diamond is made up of carbon atoms close to each other and in a 3 layered cube shape which is a lot more rigid and this makes it 'the hardest substance on earth'. Hope this helps, Obrien9
Why does diamond not conduct electricity?
Most diamonds are not conductors, they are rather good insulators of electricity. The one exception is blue diamond, which is blue due to the addition of boron being included in the crystal lattice (normally, occasionally an excess of hydrogen can turn them blue as well but rare). The boron allows it to become a p-conductor, and thus it will conduct electricity. Note that one way to tell a real (boron doped) blue diamond from say a white diamond that has been colored blue (by irradiation, coating, etc), is to see if it will conduct electricity.
Why does carbon conduct electricity if it is a non metal?
Carbon is used as a conductor in many applications. One common conductor, automotive spark plug wires, is actually a carbon impregnated chord. A common problem in high voltage electrical systems, such as automotive ignition secondary circuits, is "carbon tracking". A distributor cap, for example, may arc from one terminal to another, leaving a carbon track behind. The current will now follow that carbon path very readily and this is one reason secondary circuit (high voltage) components have to be replaced periodically.
What are the allotropes of carbon and how are they structurall different?
diamond -it has a hard structure and crystals that shine in light and it does not conduct electricity. Graphite -it has sticky structure and has some delocalised electrons so it conducts electricity and has a slippery surface
Does carbon conduct electricity?
No, carbon in its pure form is not a good conductor of electricity. However, certain forms of carbon like graphene and carbon nanotubes can conduct electricity due to their unique structure and properties.
Do diamonds conduct electricity?
they don't conduct electricity: they have no free electrons. graphite, however, made of the same stuff as diamond (carbon) has a different structure, which means that it does have free electrons, and a lot of them. Therefore graphite is a good conductor of electricity.
Which non metal conducts electricity?
Graphite, which is a form of carbon, is a non-metal that can conduct electricity due to its unique structure that allows electrons to move freely through its layers.
Which form of carbon will passes electricity?
Graphene, graphite, and some carbon nanotubes can all conduct electricity.
Why blue diamond can conduct electricity?
Blue diamonds do not conduct electricity. Diamonds do, however, conduct heat, in fact five times better than silver. Both diamonds and graphite are produced naturally from carbon. Diamond is an excellent electrical insulator, graphite is a good conductor of electricity.
Why are diamond and graphite polymorphic?
Diamond and graphite are polymorphic because they are composed of pure carbon atoms arranged in different crystal structures. In diamond, carbon atoms are arranged in a three-dimensional network of tetrahedral shapes, resulting in a hard and transparent structure. In graphite, carbon atoms are arranged in layered sheets that are weakly bonded between layers, giving graphite its lubricating properties and ability to conduct electricity.
Is carbon or gold is a malleable and conducts electricity?
Carbon is not malleable but in some forms can conduct electricity. Gold is malleable and conductive.
Why does graphite conduct electricity and diamond does not?
: Diamond is made up of pure carbon. In the structure of diamond one carbon atom is attached to four other carbon atoms forming a covalent bond. All the electrons of each carbon atom is shared and the octet rule is satisfied. Hence no free electron is left for the conductance of electricity. : In case of graphite the carbon atoms naturally combine covalently with three other carbon atoms so every combined carbon has one unshared or free electron. Now this free electron is responsible for conductance in graphite. : Graphite and metals have free electrons to conduct electricity.
Diamond is an insulator while graphite conducts electricity?
Diamond is considered the hardest mineral known to man, while graphite is one of the softest. Diamond is an excellent electrical insulator, while graphite is a good conductor of electricity. This is due to the way the carbon atoms are arranged in each mineral.
Why does graphite conduct electricity whereas diamond does not and they are both allotropes?
Diamond and Graphite have 2 different structures, Diamond has a rigid tetrahedral network whereas Graphite has layers which completely changes the properties of both types of carbon. Basically graphite has free delocalised electrons which means electricity can be conducted, diamond however does not have any delocalised electrons which means it cannot conduct electricity. Both diamond and graphite are made up of strong covalent bonds which means they both have high melting points. Graphite is soft though because the layers which it is made up of slide, this makes it soft. Diamond is made up of carbon atoms close to each other and in a 3 layered cube shape which is a lot more rigid and this makes it 'the hardest substance on earth'. Hope this helps, Obrien9
Why does diamond not conduct electricity?
Most diamonds are not conductors, they are rather good insulators of electricity. The one exception is blue diamond, which is blue due to the addition of boron being included in the crystal lattice (normally, occasionally an excess of hydrogen can turn them blue as well but rare). The boron allows it to become a p-conductor, and thus it will conduct electricity. Note that one way to tell a real (boron doped) blue diamond from say a white diamond that has been colored blue (by irradiation, coating, etc), is to see if it will conduct electricity.
Is carbon an insulator or a conductor?
It depends on the type, or allotrope, of carbon you're talking about. For a material to conduct electricity, it should have free electrons to carry the electrical current. In diamond, an allotrope of carbon, there are no such free electrons. This means that diamond does not conduct electricity. However, graphite, another allotrope of carbon, conducts electricity very well because it has an entire "sea" of free electrons.
