dipole-dipole
The strongest intermolecular force present in hydrogen bromide (HBr) is dipole-dipole interaction.
To determine the strongest intermolecular force in a substance, you need to consider the types of molecules present. Look for hydrogen bonding, which is the strongest intermolecular force. If hydrogen bonding is not present, then consider dipole-dipole interactions and London dispersion forces in determining the strength of intermolecular forces.
London forces are present in chlorine molecules.
The intermolecular force in phosphorus trichloride (PCl3) is primarily dipole-dipole interactions. This is due to the polar nature of the P-Cl bonds, where the chlorine atom is more electronegative than the phosphorus atom, creating partial charges and leading to attractive forces between the molecules.
The type of intermolecular force present in KOH is hydrogen bonding. Hydrogen bonding occurs between the hydrogen atom of one molecule and the oxygen atom of another molecule when hydrogen is bonded to a highly electronegative atom such as oxygen.
The strongest intermolecular force present in hydrogen bromide (HBr) is dipole-dipole interaction.
To determine the strongest intermolecular force in a substance, you need to consider the types of molecules present. Look for hydrogen bonding, which is the strongest intermolecular force. If hydrogen bonding is not present, then consider dipole-dipole interactions and London dispersion forces in determining the strength of intermolecular forces.
Because there is the present of intermolecular force and intramolecular force
London forces are present in chlorine molecules.
The intermolecular force in phosphorus trichloride (PCl3) is primarily dipole-dipole interactions. This is due to the polar nature of the P-Cl bonds, where the chlorine atom is more electronegative than the phosphorus atom, creating partial charges and leading to attractive forces between the molecules.
The type of intermolecular force present in KOH is hydrogen bonding. Hydrogen bonding occurs between the hydrogen atom of one molecule and the oxygen atom of another molecule when hydrogen is bonded to a highly electronegative atom such as oxygen.
Dimethyl ether exhibits dipole-dipole interactions as the main intermolecular force. It also experiences weak London dispersion forces.
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.
Dipole forces and London forces are present between these molecules.
Water (H2O) has stronger intermolecular forces than ammonia (NH3) due to hydrogen bonding in water molecules. Hydrogen bonding is a type of intermolecular force that is stronger than the dipole-dipole interactions present in ammonia molecules.
London dispersion forces (instananeous dipole - induced dipole interactions)
intermolecular force