describe and explain hydrogen bonding, van der Waals’ forces,bond polarity and bond properties

Hydrogen Bonding: Hydrogen bonding is a special type of dipole-dipole attraction between molecules, where a hydrogen atom bound to a strongly electronegative atom such as nitrogen, oxygen or fluorine experiences attraction to some other nearby highly electronegative atom. It is stronger than a normal dipole-dipole interaction. For example, in water molecules, the hydrogen atoms are attracted to the oxygen atoms in other water molecules, forming hydrogen bonds.

Van der Waals' Forces: Van der Waals' forces are the residual attractive or repulsive forces between molecules or atomic groups that do not arise from a covalent bond, or ionic bonds. They include forces such as dispersion forces or London forces, dipole-dipole interactions and dipole-induced dipole interactions. They are generally weaker than covalent and ionic bonds.

Bond Polarity: Bond polarity refers to the separation of electric charge along a bond, leading to a molecule or its chemical groups having an electric dipole or multipole moment. It occurs due to the difference in electronegativities of the two atoms involved in a bond. The atom with higher electronegativity will pull the electron density towards itself, creating a partial negative charge, while the other atom will have a partial positive charge.

Bond Properties: Bond properties refer to the characteristics of a chemical bond such as bond length, bond angle, bond energy, etc. Bond length is the distance between the nuclei of two bonded atoms. Bond angle is the angle formed between three atoms across at least two bonds. Bond energy is the energy required to break a bond. These properties are crucial in determining the physical and chemical properties of compounds.