Hydrogen Bond

Polar molecules have weak, partially negative, and partially positive charges. For example, in water, the negative charge is an oxygen atom and the hydrogen atom in water is a positive one. When water molecules approach each other, positively and negatively charged regions are attracted to oppositely charged regions or nearby molecules. The dotted line in the figure is called a hydrogen bond. Each water molecule is bound to the other four molecules. Hydrogen bonds formed between water molecules are part of the fundamental and unique properties of water.

A water molecule can form up to four hydrogen bonds by accepting two hydrogen atoms and providing two hydrogen atoms. Hydrogen bonding is a relatively weak attractive force compared to the covalent bond (intramolecular bond) in the water molecules themselves, which is the cause of many physical properties of water. One of the features is that the melting point and boiling point are relatively high and more energy is required to break the intermolecular hydrogen bond to convert to a higher energy phase.

Hydrogen bonding has a very important effect on the characteristics of water and ice. Hydrogen bonding is also important in the process of proteins, nucleic acids, and life. The opening of the DNA is a hydrogen bond cleavage which helps to hold the two chains of the double helix together. This is because hydrogen bonding is very important to us. To attract hydrogen bonds, hydrogen must be very positive, but the other must be negative to bond the bond, "hydrogen bonding"

Hydrogen bonding is the third type of van der Waals forces. It has exactly the same interaction as a dipole-dipole, it just gets a special name. Hydrogen bonds are dipole dipole interactions occurring between any molecule having a bond between a hydrogen atom and any oxygen / fluorine / nitrogen. Hydrogen bonding is only dipole dipole force, but it is very strong compared to dipole dipole force like HCl. F N and O are very good at attracting electrons and H is very powerful as it is very good at losing them. Therefore, basically, because binding is unilateral, leading to extreme dipole states, they are called hydrogen bonds. Extreme frontalities of molecules are extremely negatively oriented with other molecules

Can you explain about the power of Van der Waals and why they need energy to evaporate water?

At lower temperatures, hydrogen bonding of water molecules forms ice crystals. Hydrogen bonds are more stable and retain their crystalline form. Because hydrogen bonds are spaced from one another, ice (solid water) is less dense than water. The low density is the reason that the iceberg is allowed to float, and only the top of the lake is frozen. Water forms hydrogen bonds and becomes a powerful solvent. Water molecules are attracted to other molecules, including perfect charges such as ions, partial charge or polarity. The salt (NA + CL -) is soluble in water. The water molecules surround the salt molecules and separate NA + from CL- by forming a hydrated shell around two separate ions