They vary- most decompose into smaller units which may be molecules or atoms or free radicals. there is no hard and fast rule- usually we are talking of very high temperature gases.
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.
Ionic bonded always. Also giant covalent structures- like diamond and silicon dioxide. It is NOT just ionic compounds!
Indeed they can. A common example of Carbon covalently bonding with carbon is in what we refer to as Giant Covalent Structures, which are multiple of an atom bonded together in a set, lattice-like shape. Examples of giant covalent structures made from carbon are diamond where the atoms are arranged in a pyramid shape, and graphite, where they are arranged in flat layers.
Unlike most Giant Covalent Structures like diamond that form four covalent bonds, Graphite only forms 3, meaning it has a free electron meaning that graphite can conduct electricity.
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".
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.
COVALENT
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.
Some do- for example molten silicon conducts like ametal when molten.
Ionic bonded always. Also giant covalent structures- like diamond and silicon dioxide. It is NOT just ionic compounds!
Indeed they can. A common example of Carbon covalently bonding with carbon is in what we refer to as Giant Covalent Structures, which are multiple of an atom bonded together in a set, lattice-like shape. Examples of giant covalent structures made from carbon are diamond where the atoms are arranged in a pyramid shape, and graphite, where they are arranged in flat layers.
Unlike most Giant Covalent Structures like diamond that form four covalent bonds, Graphite only forms 3, meaning it has a free electron meaning that graphite can conduct electricity.
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 bonds are formed by electron sharing between atoms. They create structures called molecules.
No, they don't. As giant covalent substances are non-polar, means having no dipole moment. Only polar or substances having charges like ionic compounds are soluble in water.
It's due to the facts that simple covalent bonds like single bonds are weaker and longer than others bonds with tighter interactions like pi bonds (double bonds) or ionic bonds. Once the heat is turned up it excites the electrons to move from their bonded positions and the bond breaks
A giant covalent structure is an element made with very strong bonds between the atoms too create various materials. A couple of examples are Diamond and Buckminster Fullerine. Graphite is also one but has weak bonds aswell. like...