Why does graphite conduct electricity whereas diamond does not?

Asked By: Brennan Senger
Date created: Thu, Apr 29, 2021 3:34 PM
Best answers
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.
Answered By: Olga Shields
Date created: Fri, Apr 30, 2021 5:37 PM

Why diamond is non conductor and graphite is conductor

Why diamond is non conductor and graphite is conductor
Why does graphite conduct electricity whereas diamond does not? Graphite is a good conductor of electricity since each carbon atom is linked to three of its neighbouring carbon atoms. So the fourth electron is free to move, which can carry a charge. In contrast, diamond has no free mobile electron, so diamond is a bad conductor of electricity.
Answered By: Dejon Kirlin
Date created: Sat, May 1, 2021 3:17 AM
graphite conduct electricity where as diamond does not because in diamond the carbon atoms are bonded to for others atoms. whereas graphite each carbon atom is only bonded to three other atoms. therefore, there are delocalised (free) electrons in graphite, which can move and carry a charge so graphite conducts electricty.
Answered By: Madge Rolfson
Date created: Sun, May 2, 2021 3:51 AM
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.
Answered By: Amya Tillman
Date created: Sun, May 2, 2021 11:40 AM
Graphite can conduct electricity because of the delocalised electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. Generally, in diamond, all the 4 outer electrons on each carbon atom are used in covalent bonding, so there are no other delocalised electrons. 249 views
Answered By: Willa Wolf
Date created: Mon, May 3, 2021 1:47 PM
Why can graphite conduct electricity but diamond can not? In diamond the carbon atoms are bonded to four other atoms. Whereas, in graphite each carbon atom is only bonded to three other atoms. Therefore, there are delocalised (free) electrons in graphite, which can move and carry a charge so graphite conducts electricty.
Answered By: Demetris Greenfelder
Date created: Tue, May 4, 2021 3:35 AM
Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor. Graphite on the other hand, although also only made up of carbon atoms, is the only non-metal that can conduct electricity.
Answered By: Alberta Schmitt
Date created: Tue, May 4, 2021 9:33 PM
Click here 👆 to get an answer to your question ️ Why does graphite conduct electricity whereas diamond does not 0? wafulamoses7301 wafulamoses7301 23.03.2019 Physics Secondary School Why does graphite conduct electricity whereas diamond does not 0? 1 See answer wafulamoses7301 is waiting for your help. Add your answer and earn points…
Answered By: Jamil Powlowski
Date created: Wed, May 5, 2021 6:43 AM
Graphite conducts electricity whereas diamond does not. Diamond is a transparent object which has extraordinary shine and lustre whereas graphite is an opaque and greyish-black object. The difference in these physical properties is due to the fact that they have different molecular structure. 4. The carbon atoms in graphite are covalently bonded to three other carbon atoms, forming sheets that are able to slide over and past each other, thus making graphite soft and slippery and conductive ...
Answered By: Claudie Cassin
Date created: Wed, May 5, 2021 5:05 PM
Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. This makes graphite useful for electrodes...
Answered By: Mekhi McLaughlin
Date created: Thu, May 6, 2021 7:52 AM
Variable electrical conductivity – diamond does not conduct electricity, whereas graphite contains free electrons so it does conduct electricity. Why do diamond and graphite have such different physical properties? Since they are both made of carbon their chemical properties are the same.
Answered By: Esteban Witting
Date created: Fri, May 7, 2021 4:02 AM
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
Answered By: Melyssa Stanton
Date created: Fri, May 7, 2021 4:14 PM
0 votes. 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.
Answered By: Cierra Kessler
Date created: Fri, May 7, 2021 9:49 PM
Why can graphite conduct electricity but diamonds can’t? True, both diamonds and graphite are made from carbon. However, their structures are significantly different. Remember how graphite carbon atoms have a free electron? The same isn’t true for diamond: all four electrons have formed strong single bonds with other atoms.
Answered By: Else Dickinson
Date created: Sat, May 8, 2021 9:04 PM
Diamond does not conduct electricity because it has no charged particles that are free to move. Graphite does conduct electricity because it has delocalised electrons which move between the layers.
Answered By: Christy Erdman
Date created: Sun, May 9, 2021 12:10 PM
Thus, no free electrons are available. In the structure of graphite, three electrons in the valence shell of carbon are involved in covalent bond formation, The fourth electron is free to move. Therefore, graphite is a good conductor of electricity.
Answered By: Kaylin Barrows
Date created: Mon, May 10, 2021 1:14 AM
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.
Answered By: Ashton Blick
Date created: Mon, May 10, 2021 10:10 AM
FAQ
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Summary: diamond vs graphite | gcse chemistry (9-1) | kayscience.com

Summary: diamond vs graphite | gcse chemistry (9-1) | kayscience.com
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