Table of Contents
What are structures of diamond and graphite?
In diamonds, one carbon atom is bonded with four others to create a dense, cage-like crystal structure that is very hard. In graphite, one carbon bonds with three others to form flat layers that stack like a deck of cards and can slide apart (as seen by the trail of pencil lead).
What are diamond and graphite examples of?
Diamond, graphite and fullerenes (substances that include nanotubes and ‘buckyballs’ , such as buckminsterfullerene) are three allotropes of pure carbon.
What makes a diamond different from a graphite?
Diamond and graphite are different forms of the element carbon. They both have giant structures of carbon atoms, joined together by covalent bonds. However, their structures are different so some of their properties are different. The rigid network of carbon atoms, held together by strong covalent bonds, makes diamond very hard.
How does a graphite have a giant covalent structure?
Graphite has a giant covalent structure in which: 1 each carbon atom is joined to three other carbon atoms by covalent bonds 2 the carbon atoms form layers with a hexagonal arrangement of atoms 3 the layers have weak forces between them 4 each carbon atom has one non-bonded outer electron, which becomes delocalised More
What’s the difference between graphite and precious stone?
Precious stone and graphite have shift structures which represent their diverse properties, and both are pure carbon. However, the graphite’s particles join to the three atoms of carbon and get associated with the plates that are parallel to each other. The particles of Diamond enter the four atoms of carbon in a gem frame.
What is the structure of a graphite ring?
The carbon atoms in the Graphite structure are sp 2 hybridized and are directed in the same plane thus forming hexagonal rings. The rings have many layers of particles. Graphite is said to exhibit low electrical conductivity with a low density of about 2.26 g/cm 3.