yes a diamond is classified as a covalent crystal
Yes, a tetrahedral array of carbons bonding covalently only to other carbons forms a diamond.
Yes, the covalent structure of diamond is responsible to its high MP and BP too.
Damond is covalently bonded, a giant molecule
Yes, diamonds are pure carbon ( almost ) and the carbon forms many tetrahedral structures by being covalently bonded; one carbon to another. Carbon catenation.
Silicon (like carbon) can form covalent bonds, it forms a giant molecule with the diamond structure. Silicon dioxide is also a giant structure with polar covalent bonds. Silica reacts with basic oxides to form silicates- and these are generally giant structures, polar covalent bonds again, that form a very large proportion of the minerals in the earths crust.
silicon (IV) oxide or silicon dioxide has giant covalent structure
yes, it is bonded in a giant covalent lattice and has a tetrahedral structure, and is very hard to break apart
because it has many strong covalent bonds in a lattice structure (such as diamond)
Four. they are arranged tetrahedrally. The structure is similar to diamond.
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".
The giant structure involve an enormous number of atoms.
Silicon (like carbon) can form covalent bonds, it forms a giant molecule with the diamond structure. Silicon dioxide is also a giant structure with polar covalent bonds. Silica reacts with basic oxides to form silicates- and these are generally giant structures, polar covalent bonds again, that form a very large proportion of the minerals in the earths crust.
It depends on the type of structure; simple covalent structures (like water) generally have low boiling points, while giant covalent structures (like diamond) have high boiling points.
silicon (IV) oxide or silicon dioxide has giant covalent structure
Damond is covalently bonded, a giant molecule
Silica
The tetrahedral covalent structure of carbon is known as diamond.
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.
That's a very good question and there are arguments for both. I would class it more as a simple molecular substance because a sample will contain many separate molecules, with forces other than covalent bonds between them. A giant covalent structure like diamond is wholly held together by covalent bonds.
Such compounds can have either a giant or a simple molecular structure. Cellulose is an example of a material with a giant structure, and carbon monoxide has a very simple one.