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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,
What else can I help you with?
What is the boiling point of giant covalent?
Giant covalent structures, such as diamond and graphite, do not have a specific boiling point because their atoms are held together by strong covalent bonds that require high temperatures to break. These structures do not boil in the traditional sense like molecular substances but rather decompose or undergo phase transitions at extremely high temperatures.
What does giant covalent mean?
Giant covalent structures are substances in which atoms are bonded together by strong covalent bonds in a continuous network, forming a three-dimensional structure. Examples include diamond, graphite, and silicon dioxide (silica). These substances typically have high melting points and are insoluble in most solvents.
Why do molecular compounds have low melting points and low boiling points relative to ionic substances?
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.
What is a physical property of a giant covalent structure?
+ High melting and boiling points+ Insoluble in water and organic solvents+ Do not conduct electricity (except when they have free electrons eg graphite)+ Solid at room temperature
Which compound has a high melting point covalent and non metals?
A possible compound would be silicon dioxide with giant covalent structure and strong covalent bonds.
Is high melting point and boiling point a sign that a compound is ionic?
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.
What is the boiling point of giant covalent?
Giant covalent structures, such as diamond and graphite, do not have a specific boiling point because their atoms are held together by strong covalent bonds that require high temperatures to break. These structures do not boil in the traditional sense like molecular substances but rather decompose or undergo phase transitions at extremely high temperatures.
What does giant covalent mean?
Giant covalent structures are substances in which atoms are bonded together by strong covalent bonds in a continuous network, forming a three-dimensional structure. Examples include diamond, graphite, and silicon dioxide (silica). These substances typically have high melting points and are insoluble in most solvents.
What are the charateristics of a covalent bond?
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.
Why are the melting point and boiling point of a covaleny substance low?
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.
Why do molecular compounds have low melting points and low boiling points relative to ionic substances?
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.
Do covalently bonded compounds have low boiling points?
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.
What is a physical property of a giant covalent structure?
+ High melting and boiling points+ Insoluble in water and organic solvents+ Do not conduct electricity (except when they have free electrons eg graphite)+ Solid at room temperature
Why do molecular compounds have low melting points and low boiling points relative to ionic substance's?
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.
Which compound has a high melting point covalent and non metals?
A possible compound would be silicon dioxide with giant covalent structure and strong covalent bonds.
Do giant covalent substance dissolve in water?
No, giant covalent substances like diamond or graphite do not dissolve in water because they have strong covalent bonds that are not easily broken by water molecules. Their rigid structure and intermolecular forces also prevent them from dissolving in water.
Does covalent structures have high or low 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.
