because the strong covalent bonds that operate in 3D and firmly hold together all the atoms within the structure.
yes covalent does
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.
Molecular covalent compounds have lower melting points because the inetrmolecular forces are weaker than ionic bonds. Note that giant covalent structures, such as silicon dioxide, can have very high melting points, the key factor is not simply the nature of the bond.
No they have high melting and boiling points. Don't get confused with simple molecular structures such as water and carbon dioxide which have simple covalent structures. When you heat them you are overcoming the forces BETWEEN THE MOLECULES (intermolecular/van der waals forces of attraction), NOT the actual covalent bonds themselves, like the bond betwen the C and either O in carbon dioxide.
Ionic compounds have strong electrostatic force of attraction and hence have higher melting points than covalent compounds.
yes covalent does
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.
Molecular covalent compounds have lower melting points because the inetrmolecular forces are weaker than ionic bonds. Note that giant covalent structures, such as silicon dioxide, can have very high melting points, the key factor is not simply the nature of the bond.
No they have high melting and boiling points. Don't get confused with simple molecular structures such as water and carbon dioxide which have simple covalent structures. When you heat them you are overcoming the forces BETWEEN THE MOLECULES (intermolecular/van der waals forces of attraction), NOT the actual covalent bonds themselves, like the bond betwen the C and either O in carbon dioxide.
Ionic compounds have strong electrostatic force of attraction and hence have higher melting points than covalent compounds.
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,
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).
Ionic compounds have higher melting points because the bond olding the ionic crystal together is stronger than the intermolecular forces (van der Waals) holding covalent molecules together. Giant covalent molecules such as dialmond and silicon dioxide have very high melting points because the lattice is held together by stong covalent bonds
Compounds bonded by covalent bonds do not necessarily have low melting points. Some have whereas some don't have.Some polymers and hydrocarbons have very high melting points. But it can be said that they don't have melting points as high as ionic compounds. It is so because ionic bonds are stronger than the covalent bonds.
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
Covalent, Metallic, and Ionic crystals have high melting points and densities, but molecular crystals tend to be soft and has a lower melting point. Covalent crystal=covalent bond and Ionic crystal=ionic bond.
Because they have interlocking electrons as the different elements' electrons have been 'tangled'