Metals contain delocalized electrons forming a 'sea' of electrons. Metal atoms lose electrons to form positive metal ions. Metallic bonding is the attraction between delocalized electrons and positive ions
Chemical bonding unites atoms through electron redistribution for stable electronic states. Four main types exist: ionic, covalent, hydrogen, and metallic
Primary bonds hold atoms in molecules, secondary bonds hold molecules together. Primary bonds include ionic, covalent, and metallic bonds. Secondary bonds include dispersion, dipole, and hydrogen bonds
Metals exhibit luster, malleability, ductility, and conductivity due to metallic bonding. Term "metal" comes from Greek "metallon" meaning mine. Copper was discovered around 9000 BC, leading to early metal use
Chemical bonds form between atoms or ions to create molecules and structures. Strong bonds include covalent, ionic, and metallic bonds. Weak bonds consist of dipole-dipole, London dispersion, and hydrogen bonding
Metallic bonding arises from electron cloud between metal ions and conduction electrons. Electrons are delocalized in all three dimensions, forming a single molecule. Electron deficiency allows electrons to migrate and change states easily