Inter atomic bonds

• Ionic bonding is the transfer of electrons from one atom to another.
• Covalent bonds form when atoms share electrons to fill their outer shells and become stable.
• The shared electrons are attracted to the nuclei of both atoms, binding them together.
• Covalent bonding involves sharing pairs of electrons between atoms.
• Covalent bonds tend to be strong and directional.
• Metallic bonding occurs when metal atoms lose their outermost electron shell, forming positive ions that are held together by electrostatic attraction.
• Metallic bonding involves the sharing of valence electrons among metal atoms, resulting in a lattice structure that holds the metal together.
• Metallic bonding occurs between metal atoms, where delocalized electrons are shared by all atoms in the lattice structure.
• Metallic bonding involves the sharing of valence electrons between metal atoms, forming a sea of delocalised electrons that hold the positive metal ions together.
• Hydrogen bonding involves hydrogen atoms covalently bonded with other elements (such as oxygen or nitrogen) that have lone pairs on them.
• The strength of an intermolecular force depends on factors such as distance, charge distribution, and molecular shape.
• Hydrogen bonding is an electrostatic attraction between hydrogen atoms covalently bound to highly electronegative elements (such as fluorine or oxygen) and other nearby polar molecules or ions with lone pairs of electrons.
• Metallic bonding occurs between metal atoms due to the attraction between positive metal ions and delocalized electrons.
• In metallic bonding, there is no fixed structure or arrangement of ions.