dipole-dipole
intermolecular forces. In the case of HF, hydrogen bonding exists between HF molecules, which results in stronger intermolecular attractions compared to the London dispersion forces present in H2 and F2. These stronger intermolecular forces in HF allow it to exist as a liquid at room temperature.
Noble gases usually exist as monatomic (single atom) gases because they have a stable electron configuration and are inert, meaning they do not easily react with other elements. This makes them chemically unreactive and often found in their elemental form in nature.
All inert gases exist as gases in nature; but today the name inert remain only traditional. The so-called noble gases has known compounds (excepting neon).
Dispersion forces, also known as London dispersion forces, are present in all molecules and atoms. These forces are the weakest type of intermolecular interaction and arise from temporary fluctuations in electron distribution within a molecule or atom.
The intermolecular force in CCl4 is dispersion forces. This occurs when slight variations in electron distribution effect the electron distribution of other molecules. Because CCl4 is non polar, it does not have other intermolecular forces holding the molecules together.
intermolecular forces. In the case of HF, hydrogen bonding exists between HF molecules, which results in stronger intermolecular attractions compared to the London dispersion forces present in H2 and F2. These stronger intermolecular forces in HF allow it to exist as a liquid at room temperature.
Helium is a noble gas, so it exhibits weak dispersion forces, also known as London dispersion forces, as its primary intermolecular force. These forces arise from temporary fluctuations in electron distribution around the atom.
Yes... When water is heated, the intermolecular force of attraction between water atoms become weak and they start losing the intermolecular force of attraction... at temperature known as boiling point of water this intermolecular force become so weak that water lose its state and converts into gasious state... but this expansion is not considerable... :)
All elements and compounds can exist as a gas if heated sufficiently.
The intermolecular force in XeF4 is London dispersion forces, which are also known as van der Waals forces. These forces are caused by temporary dipoles that occur due to fluctuations in electron distribution around the atoms.
Noble gases usually exist as monatomic (single atom) gases because they have a stable electron configuration and are inert, meaning they do not easily react with other elements. This makes them chemically unreactive and often found in their elemental form in nature.
The type of intermolecular force present in Br2 is London dispersion forces. These forces are the weakest of the intermolecular forces and result from temporary fluctuations in electron distribution around the molecule, leading to a temporary dipole moment.
The attractive force between masses is known as gravity. It is responsible for keeping planets in orbit around stars and objects on Earth grounded.
This is an intermolecular attraction of water molecules, associated by hydrogen bonds.
The electrostatic attraction known as hydrogen bonds that form directional intermolecular associations.
All inert gases exist as gases in nature; but today the name inert remain only traditional. The so-called noble gases has known compounds (excepting neon).
Cohesive force is the attractive force between like molecules. Cohesive forces are also known as intermolecular forces and can also be repulsion forces.