hydrogen bonding between the nitrogen of one molecule and the hydrogen of another, followed by dipole-dipole interactions and finally the very weak but ever present Van Der Waals forces.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
attractive force present between ammonia ions repulsive force also exist but not at high rate
NH3 exhibits hydrogen bonding in addition to dispersion forces. This significantly increases the intermolecular force, and raises the boiling point. PH3 does not exhibit hydrogen bonding and the dominant intermolecular force holding these molecules together is dispersion forces. (Dispersion forces also known as Van Der Waal Force)
Ion-dipole force
Dipole forces and London forces are present between these molecules.
The intermolecular force of ClF is dipole-dipole interaction. This is because ClF is a polar molecule, with a significant difference in electronegativity between chlorine and fluorine causing a partial positive and partial negative charge, leading to attraction between the molecules.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
attractive force present between ammonia ions repulsive force also exist but not at high rate
The most important intermolecular force between CH3Cl molecules is dipole-dipole interactions. CH3Cl is a polar molecule due to the difference in electronegativity between carbon and chlorine, causing a partial positive charge on the carbon and a partial negative charge on the chlorine atom. These dipole-dipole interactions play a significant role in holding the molecules together in a pure sample of CH3Cl.
The predominant type of intermolecular force in OF2 is dipole-dipole interactions. This is because OF2 is a polar molecule due to the difference in electronegativity between oxygen and fluorine atoms, creating partial positive and negative charges that allow for dipole-dipole interactions between molecules.
The predominant intermolecular force in non-polar molecules is London dispersion forces, also known as Van der Waals forces. These forces are due to temporary fluctuations in electron distribution within the molecule, creating temporary dipoles that attract each other.
The intermolecular force in AgNO3 is mainly ionic bonding, as silver nitrate is a salt composed of positively charged silver ions (Ag+) and negatively charged nitrate ions (NO3-). This strong electrostatic attraction between the charged ions holds the crystal lattice together.
No, covalent bonds are intramolecular forces that hold atoms together within a molecule. Intermolecular forces are interactions between molecules that are weaker than covalent bonds, such as hydrogen bonding, dipole-dipole interactions, and van der Waals forces.
The forces of attraction between molecules in a molecular compound are generally weaker than those in an ionic compound. These forces are typically known as van der Waals forces or London dispersion forces, which are based on temporary fluctuations in electron distribution within the molecules. The strength of these forces can vary depending on the molecular structure and shape of the compound.
The intermolecular forces are London dispersion forces.C2H4 is ethene molecule. The bonding is calledthe covalent compound,which the molecules share their electrons in order to achieve the stable electron arrangement.
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.
Solid state matter has maximum intermolecular force.