Dr. Gaurav Jhaa Blogs

  Metallic bonding is a type of chemical bonding that is characterized by the sharing of electrons between metal atoms. This type of bonding is responsible for many of the unique properties of metals, including their high melting and boiling points, electrical conductivity, and ductility. In this blog, we will explore metallic bonding in detail, including its definition, properties, and examples. Definition of Metallic Bonding Metallic bonding refers to the sharing of electrons between metal atoms in a crystal lattice structure. In metallic bonding, the electrons are free to move throughout the crystal lattice, resulting in a sea of electrons that surrounds the positively charged metal ions. This sea of electrons gives rise to many of the unique properties of metals, including their high electrical conductivity and their ability to conduct heat. Properties of Metallic Bonding High Melting and Boiling Points: Metals have high melting and boiling points due to the strong metalli

  Hydrogen bonding is a type of chemical bond that occurs between or within molecules (Inter/intramolecular hydrogen bonding). It is a highly attractive interaction between a hydrogen atom that is covalently bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and another electronegative atom. The hydrogen atom donates its electron pair to the electronegative atom, resulting in a positive charge on the hydrogen and a negative charge on the electronegative atom. This creates an electrostatic attraction between the hydrogen and electronegative atom, resulting in a hydrogen bond. Hydrogen bonds are much weaker than covalent bonds, but they are still significant and play a critical role in many biological and chemical processes. They are responsible for the stability of DNA and proteins, as well as the unique physical properties of water. In water, hydrogen bonds between water molecules create a highly cohesive liquid, with a high boiling point and surface