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London dispersion forces increase when atomic radius increase or the number of interactions between molecules.increase.
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∙ 8y ago
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∙ 11y agoYes.
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What is one type of attractive force that stabilizes molecular solids?
London dispersion forces
Do London dispersion forces act only in solids?
no
Why do molecular solids have lower boiling points than ionic solids?
In the liquid the intermolecular forces between covalent molecules are weaker than the forces between ions.
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 forces hold molecular solids?
There are different forces that are associated with solids. The main ones are normal forces and ionic bonds which hold together ionic solids.
What is one type of attractive force that stabilizes molecular solids?
London dispersion forces
What force holds molecular solids together?
London dispersion forces (also known as van der Waals forces) hold molecular solids together. or Intermolecular forces
What forces hold molecular together?
London dispersion forces (also known as van der Waals forces) hold molecular solids together. or Intermolecular forces
Do London dispersion forces act only in solids?
no
Which intermolecular force is present is present in solids and liquids that are composed of non polar molecules?
London dispersion forces (instananeous dipole - induced dipole interactions)
Why do molecular solids have lower boiling points than ionic solids?
In the liquid the intermolecular forces between covalent molecules are weaker than the forces between ions.
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 forces hold molecular solids?
There are different forces that are associated with solids. The main ones are normal forces and ionic bonds which hold together ionic solids.
What is the attraction between a solid is?
Solids are held together but different types of intermolecular forces. The nature of these forces depends on the compound. In nonpolar substances, only dispersion forces at work. In polar compounds, dipole-dipole forces also hold the molecules together. Since dipole-dipole forces are stronger than dispersion forces, polar compounds usually have a higher melting point than nonpolar ones.
What is bonding in solids. write the list of different types of bonding in solids?
Strong chemical bonds in solids are ionic bonds, covalent bonds in giant network molecules and metallic bonds. Weak bonds in solids holding discrete molecules together are hydrogen bonds in solid H2O, HF, NH3 Weak intermolecular forces including dispersion forces and permanent dipole interactions
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.
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.
