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".
Network Covalent
Almost all of the compounds of carbon are formed by covalent bonding. Compounds such as diamond and graphite show strict covalent character in bonding.
The carbon to carbon bonding in Diamond is a covalent bonding.
Polar covalent
Covalent bonding is a type not found in metals (there mainly metal bonds or ionic bonds) In nonmetals more covalent bonding is common.
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.
it has covalent bonding
Network
Almost all of the compounds of carbon are formed by covalent bonding. Compounds such as diamond and graphite show strict covalent character in bonding.
The carbon to carbon bonding in Diamond is a covalent bonding.
Covalent Bonding
Covalent bonding. This means the atoms share electrons, producing a strong inter-linkage.
Polar covalent
Covalent bonding is a type not found in metals (there mainly metal bonds or ionic bonds) In nonmetals more covalent bonding is common.
there is covalent bond in hydrogen sulfide.
covalent bonding
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.
Bonds in organic compounds from oil are covalent.