In a diamond, the carbon atoms are arranged tetrahedrally. Each carbon atom is attached to four other carbon atoms 1.544 x 10-10 meter away with a C-C-C bond angle of 109.5 degrees. It is a strong, rigid three-dimensional structure that results in an infinite network of atoms.
What is the structure of the diamond?
Diamond has a giant covalent structure in which: each carbon atom is joined to four other carbon atoms by covalent bonds. the carbon atoms have a regular lattice arrangement.
What is Diamond give its structure and uses?
Structure of Diamond and Uses
The carbon atoms, here are sp3 hybridized, and the bond lengths of carbon-carbon atom are equal. Hence Diamond forms a three-dimensional network of strong covalent bonds. Diamond has a very high melting point of about 3843 K and a high density of about 3.51 g/cm3.
How do you draw the structure of a diamond?
Draw a carbon atom, and then arrange 4 others around it to look like this: It is important that you don’t draw the ones at the bottom so that they are exactly lined up with any other atom either vertically or horizontally. The arrangement around the central carbon atom is described as tetrahedral.
What type of structure does diamond and graphite have?
Diamond and graphite are different forms of the element carbon. They both have giant structures of carbon atoms , joined together by covalent bonds .
Why is diamond so hard?
The outermost shell of each carbon atom has four electrons. In diamond, these electrons are shared with four other carbon atoms to form very strong chemical bonds resulting in an extremely rigid tetrahedral crystal. It is this simple, tightly-bonded arrangement that makes diamond one of the hardest substances on Earth.
What crystal structure is Diamond?
The crystal structure of a diamond is a face-centered cubic or FCC lattice. Each carbon atom joins four other carbon atoms in regular tetrahedrons (triangular prisms).
What is Diamond used for?
The most familiar uses of diamonds today are as gemstones used for adornment, and as industrial abrasives for cutting hard materials. The markets for gem-grade and industrial-grade diamonds value diamonds differently.
What is the properties of diamond?
Besides the hardness, diamond provides an impressive combination of chemical, physical and mechanical properties: Hardness. Low coefficient of friction. High thermal conductivity.
Why is diamond so expensive?
A diamond is the hardest material on the earth and the most expensive gemstone as well. Diamonds are not rare but high-quality diamonds that can be used in the jewelry are rare. … In addition, the size and quality of the diamond also plays a major role on the price. These are the reasons why diamonds are so expensive.
What is the hybridization of diamond?
In diamond each carbon atom is attached to four different carbon atoms by sigma bonds. Hence, the hybridization of carbon is sp3 . In graphite each carbon atom is attached to three different carbon atoms by sigma bonds.
Does a diamond conduct electricity?
Diamond is a form of carbon in which each carbon atom is joined to four other carbon atoms, forming a giant covalent structure. … It does not conduct electricity as there are no delocalised electrons in the structure.
What are 5 differences between diamond and graphite?
Difference between diamond and graphite.
The p-Block Elements.
|4. It has huge three dimensional network structure.||4. It has two dimensional sheet like structure.|
|5. It does not possess any lustre||5. It a has metallic lustre.|
|6. It a has very high melting point.||6. It has low metling point.|
Does Diamond have a layered structure?
Structure and bonding
each carbon atom is joined to three other carbon atoms by covalent bonds. the carbon atoms form a hexagonal layered network structure. the layers have weak forces between them and can slide over each other.
Why Diamond is hard than graphite?
Diamond is harder than graphite because each of its carbon atoms form four covalent bonds in a tetrahedral structure and also due to the presence of strong covalent bonds in it. A chemical bond involving the exchange of electron pairs between atoms is known as a covalent bond.