Science, asked by Anonymous, 1 year ago

diffrence bwtween ....daimond and graphite and fullerenes

Answers

Answered by 1Anushka12
3
Hey mate here is your answer

☆Diamond- Diamond is a solid form of carbon with a diamond cubic crystal structure. At room temperature and pressure it is metastable and graphite is the stable form, but diamond almost never converts to graphite.

☆Graphite- Graphite, archaically referred to as plumbago, is a crystalline allotrope of carbon, a semimetal, a native element mineral, and a form of coal. Graphite is the most stable form of carbon under standard conditions.

☆Fullerenes- A fullerene is an allotrope of carbon in the form of a hollow sphere, ellipsoid, tube, and many other shapes. Spherical fullerenes, also referred to as Buckminsterfullerenes or buckyballs, resemble the balls used in association football. Cylindrical fullerenes are also called carbon nanotubes.

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Answered by Anonymous
1
HEY ❤️ ❤️ ❤️

Diamond and graphite are both giant covalent substances made entirely of carbon atoms. Both have chemical formula , but they do not have a molecular formula.

 <b>Molecular structure</b>

 <b>Diamond:</b> Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.

 <b>Graphite: </b> It is also Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.

 <b>Hardness</b>

 <b>Diamond: </b> Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.

 <b>Graphite: </b> Soft. Layers of hexagonally arranged carbon atoms can slide over one another.

 <b>Electrical conductivity</b>

 <b>Diamond:</b> Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.

 <b>Graphite:</b> Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.

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