This is because they have extremely strong covalent bonds that operate in 3D and firmly hold together all the atoms in the lattice structure. Why the bonds are so strong? Probably (and don't quote me here) because the bonds are extremely stable as a result of hybridisation. Consequently, a lot of energy is required to break or even weaken these bonds, hence the exceptionally high melting and boiling points,
the covalent bonds in these structures are very strong, and a lot of energy is required to overcome these bonds. secondly, there are many covalent bonds in giant covalent structures, which means that a LOT of energy is required to overcome these. As a result, these structures have VERY HIGH melting and BOILING points!
hope this helps! :)
The boiling point of Giant covalent is: 2230ºc
The melting points and boiling points of molecular covalent compounds (ones with discrete molecules) are lower than ionic solids and giant molecule covalent compounds like (silica, SiO2) because the forces that attract them together in the solid and the liquid states (van der waals, hydrogen bonding and dispersion forces) are weaker than ionic (or covalent) bonds.
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.
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.
A possible compound would be silicon dioxide with giant covalent structure and strong covalent bonds.
It's likely but not definitive. Giant covalent substances like diamond also have high melting and boiling points. To be sure you would have to show that the melted or dissolved substance conducts electricity.
The boiling point of Giant covalent is: 2230ºc
The melting points and boiling points of molecular covalent compounds (ones with discrete molecules) are lower than ionic solids and giant molecule covalent compounds like (silica, SiO2) because the forces that attract them together in the solid and the liquid states (van der waals, hydrogen bonding and dispersion forces) are weaker than ionic (or covalent) bonds.
In a covalent bond electrons are shared between the atoms being bonded. Compounds containing covalent bonds are molecular, tend to have a low boiling and melting point, and they do not conduct electricity. This is because the intermolecular forces are weak , van der Waals forces. Nite that giant covalent molecules are in fact high melting.
The melting points and boiling points of molecular covalent compounds (ones with discrete molecules) are lower than ionic solids and giant molecule covalent compounds like (silica, SiO2) because the forces that attract them together in the solid and the liquid states (van der waals, hydrogen bonding and dispersion forces) are weaker than ionic or covalent bonds.
Yes. All have very strong bonds between the atoms, but much weaker forces holding the molecules together.When one of these substances melts or boils, it is these weak 'intermolecular forces' that break, not the strong covalent bonds within the molecule.
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.
The melting points and boiling points of molecular covalent compounds (ones with discrete molecules) are lower than ionic solids and giant molecule covalent compounds like (silica, SiO2) because the forces that attract them together in the solid and the liquid states (van der waals, hydrogen bonding and dispersion forces) are weaker than ionic (or covalent) bonds.
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.
A possible compound would be silicon dioxide with giant covalent structure and strong covalent bonds.
Covalent bonds do not melt. Compounds with covalent bonds melt and the melting point depends primarily on whether there are discrete molecules held together by intermolecular forces (which have lower melting points) or giant covalent networks such as in silica or diamond (which tend to have higher melting points).
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.