Chemistery

You've met ionic bonds (electrons transferred) and covalent bonds (electrons shared). But what holds a lump of pure copper or iron together, when there's only one kind of atom and nobody to trade with? That's the job of the third great bond type: metallic bonding . The short answer: metallic bonding is the attraction between positively charged metal ions and a " sea " of shared, freely moving electrons. Metal atoms give up their outer (valence) electrons into a common pool that flows through the whole structure, and the electrostatic pull between the fixed positive ions and this mobile electron sea holds the metal together. What metallic bonding actually is Picture a metal as a neat 3D lattice of positive ions (metal atoms that have released their valence electrons) sitting in a shared pool of those delocalised electrons . "Delocalised" means the electrons don't belong to any single atom — they roam freely across the entire piece of metal. The...

Look at a periodic table and most of it is metals — but the small patch of nonmetals on the right side includes oxygen, carbon, and nitrogen, the elements life is made of. Telling the two groups apart is one of the first skills that makes the periodic table feel readable. The short answer: metals tend to be shiny, conduct electricity, bend without breaking, and lose electrons. Nonmetals tend to be dull, don't conduct, are brittle when solid, and gain or share electrons. On the periodic table, a zig-zag staircase line separates the metals (left and centre) from the nonmetals (upper right). Quick comparison at a glance Feature Metals Nonmetals Position on the table Left and centre (most of it) Upper right Appearance Shiny (lustrous) Dull Electrical/heat conductivity Good conductors Poor (insulators) When solid Malleable & ductile (bend, stretch) Brittle (shatter) State at room temperature Mostly solid (mercury is liquid) Gases, liquids, or ...