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The type of covalent bond in a diamond is a 'giant covalent' bond in a crystalline structure. Actually, I think it's called a covalent network solid. I don't think chemists and physicists would like to use a layman's term like "giant".
Covalent, and has a network structure
A covalent lattice is a type of bond that occurs between non-metal atoms. The atoms bond to an certain number of atoms which bond to more atoms etc. Examples include graphite, diamond and silica.
These are giant molecular lattice structures. This implies that strong covalent bonding holds their atoms together in a highly regular extended network. The bonding between the atoms goes on and on in three dimensions. Melting requires the separation of the species comprising the soild state, and boiling the separation of the species comprising the liquid state. Because of the large amount of energy needed to break huge numbers of covalent bonds, all giant covalent network structures have high melting points and boiling points and are insoluble in water. Diamond, graphite (allotropes of carbon) and quartz (silicon(IV) oxide, SiO2) are examples.
Diamond has an octahedral structure.
The type of covalent bond in a diamond is a 'giant covalent' bond in a crystalline structure. Actually, I think it's called a covalent network solid. I don't think chemists and physicists would like to use a layman's term like "giant".
high hardness
No, diamond is a covalent network solid.
Covalent, and has a network structure
Network
A diamond is a non-organic structure of carbons all covalently bonded to each other, creating a network covalent bonded, single crystalline molecule
According to Wikipedia:"A diamond is a transparent crystal of tetrahedrally-bonded carbon atoms in a covalent network lattice that crystallizes into the diamond lattice which is a variation of the face centered cubic structure."
Not sure what that means... but both silicon dioxide (sand) and diamond are covalent networks.
A covalent lattice is a type of bond that occurs between non-metal atoms. The atoms bond to an certain number of atoms which bond to more atoms etc. Examples include graphite, diamond and silica.
These are giant molecular lattice structures. This implies that strong covalent bonding holds their atoms together in a highly regular extended network. The bonding between the atoms goes on and on in three dimensions. Melting requires the separation of the species comprising the soild state, and boiling the separation of the species comprising the liquid state. Because of the large amount of energy needed to break huge numbers of covalent bonds, all giant covalent network structures have high melting points and boiling points and are insoluble in water. Diamond, graphite (allotropes of carbon) and quartz (silicon(IV) oxide, SiO2) are examples.
The tetrahedral covalent structure of carbon is known as diamond.
Diamond has an octahedral structure.