The boiling point of Giant covalent is: 2230ºc
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,
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.
A possible compound would be silicon dioxide with giant covalent structure and strong covalent bonds.
In general, covalent compounds have lower boiling points than ionic compounds. This is because covalent compounds have weaker intermolecular forces compared to the strong electrostatic forces between ions in ionic compounds. As a result, less energy is required to overcome the intermolecular forces in covalent compounds, leading to lower boiling points.
The boiling point of a compound is influenced by various factors, including intermolecular forces and molecular weight, and cannot be accurately predicted solely based on the boiling points of elements in it. The presence of functional groups and molecular structure also play a significant role in determining the boiling point of a compound.
high boiling point low melting point
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.
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 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.
Diamond is an allotrope of carbon where all the carbon atoms are tetrahedrally bonded with each other forming a three dimensional covalent network. Since the bonds are strong (covalent, network), diamond has a very high melting point and boiling point. Iodine does not have three dimensional network and hence has very low melting/ boiling point. It fact, it will sublime at room temperature.
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 lowest boiling are small covalent molecular compounds which do not have any hydrogen bonding and because they are small have weaker dispersion forces holding them together in the liquid state. Re,memebr its intermolecular forces that keep molecules together in the solid and liquid. (Not giant molecules such as diamond they are held together in the solid by covalent bonds.)
A possible compound would be silicon dioxide with giant covalent structure and strong covalent bonds.
In general, covalent compounds have lower boiling points than ionic compounds. This is because covalent compounds have weaker intermolecular forces compared to the strong electrostatic forces between ions in ionic compounds. As a result, less energy is required to overcome the intermolecular forces in covalent compounds, leading to lower boiling points.
Metals have metallic bonds, water has a covalent bond.
All different covalent compounds have different boiling points.