Compare and Explain the Different Properties of Graphite and Diamond

Diamond has four covalent bonds around one carbon atom. In diamond there is a three dimensional network of strong covalent bonds.

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Because of hardness diamond is used in making cutting and grinding tools.

. The answer lies in ordinary different atomic structures of friendly and graphite. Graphite has planar hexagonal layers of carbon atoms held together by weak Vander Waals forces and C is. The fact that pure carbon has so many forms with so many different properties is why chemists keep doing chemistry.

C 60 in solution along with its atomic structure. Each C atom is s p 2 hybridized and forms 3 sigma bonds with 3 other C atoms. Diamond has a face-centered cubic crystal structure while graphite has a planar structure.

Start studying Compare Diamonds and Graphite. In diamond strong three-dimensional networks are formed due to the. Diamonds have a tetrahedral-like composition while graphite has a hexagonal-like arrangement layered in sheets.

Fourth electron forms pi bond. They are chemically identical but very different physically which is why they are called polymorphous. Allotropes are compounds of the same composition but exists in two or more different forms due to the different bonding.

Diamond does not conduct electricity because it has no charged particles that are free to move. Diamond is expensive whereas graphite is cheap. In diamond C atom is s p 3 hybridised due to tetrahedral structure.

Diamonds and graphite are both allotropes of Carbon. Diamond and graphite are two allotropic forms of carbon and their crystal structure is different from each other as shown in figure. Some differences that Diamonds and Graphite have are that Diamonds are very hard whereas Graphite is very soft and easy to break.

Diamond graphite and fullerene are different allotropes of the chemical element carbon. The key difference between diamond graphite and fullerene is that diamond has a diamond cubic crystal structure and graphite has a hexagonal crystal structure while fullerene occurs as a large spheroidal molecule. All these compounds have only carbon atoms in the.

The geometry is tetrahedral. Diamond is vary hard whereas graphite is soft. The particles of Diamond enter the four atoms of carbon in a gem frame.

Diamond is not a good conductor whereas graphite is a good conductor of electricity. 7 rows 1 It has a layered structure. Diamond is a very stable allotrope of carbon that is composed of sp3 hybridized carbon atoms.

This makes diamond extremely hard. Graphite is an allotrope of carbon that is made out of sp2 hybridized carbon atoms. Difference between the electrical conductivity of diamond and graphite.

Image adapted from source1 source2. The fourth valence electrons. Graphite does conduct electricity because it has delocalised electrons.

Unlike diamond graphite can be used as a lubricant or in pencils because the layers cleave readily. However the graphites particles join to the three atoms of carbon and get associated with the plates that are parallel to each other. The difference in the properties of diamond and graphite can be easily explained in terms their structures.

Properties and uses The delocalised electrons are free to move through the structure so graphite can conduct electricity. 5 rows Diamond. Also a Diamonds density is greater than that of Graphite.

Difference between the electrical conductivity of diamond and graphite are discussed as follows. The geometry is planar C-C bond length is 154 pm. Diamond has a face-centered cubic crystal structure.

Diamond has four covalent bonds around one carbon atom. Diamond and graphite are the same chemically but utterly different in atomic as well as in crystal structures. Graphite has a planar structure.

In graphite each carbon atom is covalently bonded to only three neighboring carbon atoms and these form layers of hexagonal network which are separated by a large distance. Graphite has three covalent bonds around one carbon atom. The fullerenes have properties different yet again from diamond or graphite.

2 It has a planar geometry. It is soft and slippery and its hardness is less than one on the Mohs scale. Precious stone and graphite have shift structures which represent their diverse properties and both are pure carbon.

Why metals compare pure diamonds are utilized in crystal structure between the confidence for announcements and collated tabular data to three difference between properties of diamond and graphite the covalent bonds present in the melting point on. It has layered structure Each C is s p 3 hybridzed and forms 4 covalent bonds with neighboring C atoms. 2 It is made up of tetrahedral units.

For example C 60 is purple and can be dissolved in oily liquids. Graphite It has crystalline nature. Learn vocabulary terms and more with flashcards games and other study tools.

This makes graphite useful for electrodes in batteries and for electrolysis.

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