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If both molecular solids and network solids contain covalent bonds why do network solids have such higher melting points than molecular solids?
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Is Glucose covalent molecular or covalent network?
network molecular
Are phosphorus and argon molecular covalent or network covalent?
Phosphorus - covalent network Argon - covalent molecular
Is cyclohexane ionic covalent molecular or covalent network?
Covalent molecule
What solid is stronger ionic solid or covalent network solids?
Network solids are held together by covalent bonds to each other. They're usually very hard and have high melting points, and are also poor heat and electrical conductors. Think of diamond and graphite. These are covalent network solids. Molecular solids, on the other hand, are molecules held together by weak intermolecular forces (such as dipole-dipole, ion-dipole, or London dispersion forces). These are usually soft with low melting points, and are also poor conductors of heat and electricity. Some examples of molecular solids would be carbon dioxide and benzene. The way I think about it, to help it make more sense to me, is that in covalent network solids, each atom is BONDED to all the other atoms around it. In molecular solids, you have completely separate molecules that are just weakly held together by intermolecular forces, they're not actually bonded to each other.
What are covalent-network solids?
Network Solids are atomic solids that contain strong directional covalent bonds to form a solid that might be best viewed as a giant molecule.
Is Glucose covalent molecular or covalent network?
network molecular
Are phosphorus and argon molecular covalent or network covalent?
Phosphorus - covalent network Argon - covalent molecular
Is cyclohexane ionic covalent molecular or covalent network?
Covalent molecule
Is HNO2 ionic network covalent molecular or metallic?
HNO3 (nitric acid) is ionic.
What are some common types of bonds?
ionic, covalent (molecular and network), and metallic
What solid is stronger ionic solid or covalent network solids?
Network solids are held together by covalent bonds to each other. They're usually very hard and have high melting points, and are also poor heat and electrical conductors. Think of diamond and graphite. These are covalent network solids. Molecular solids, on the other hand, are molecules held together by weak intermolecular forces (such as dipole-dipole, ion-dipole, or London dispersion forces). These are usually soft with low melting points, and are also poor conductors of heat and electricity. Some examples of molecular solids would be carbon dioxide and benzene. The way I think about it, to help it make more sense to me, is that in covalent network solids, each atom is BONDED to all the other atoms around it. In molecular solids, you have completely separate molecules that are just weakly held together by intermolecular forces, they're not actually bonded to each other.
What are covalent-network solids?
Network Solids are atomic solids that contain strong directional covalent bonds to form a solid that might be best viewed as a giant molecule.
What is the type of covalent bond that is found in a diamond?
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.
Why do molecular substances with strong intermolecular forces have high melting points?
There are two molecular network structures that result in high melting points. The covalent structure of carbon forms rigidity of diamond. A diamond can in fact boil but it requires an extreme temperature because of this structure. Salt (NaCl) has a rigid ionic lattice structure between its sodium and chloride atoms. This gives salt a melting point of some 801 degrees Celsius.
How are solids designated on the periodic table?
It can be categorised into -Ionic -Covalent molecular -Metallic -Covalent network
Why melting point of diamond is higher than that of silicon carbide?
Diamond is a covalent network solid, and those types of compounds have higher melting points than other types of compound.
What is strength of sand?
Sand (SiO2) is a network covalent solid. It's considered to be extremely strong with relatively high melting points (>1550'C). It is made by atoms making multiple bonds with other atoms in the "network". To compare, another example of a network covalent solid is diamonds.
