Metals

Metals are found on the left-hand side of the periodic table and are known for their high electrical and thermal conductivity, luster, malleability, and ductility. These properties arise due to the arrangement of electrons in metal atoms and their ability to easily lose electrons and form positive ions.

Key Features And Properties Of Metals

• Metallic luster: Metals have a shiny, reflective surface when polished, which is due to the ability of their delocalized electrons to absorb and re-emit light.
• Electrical conductivity: Metals are excellent conductors of electricity due to the presence of mobile, delocalized electrons that can move freely within the metal lattice, facilitating the flow of electric current.
• Thermal conductivity: Metals also exhibit high thermal conductivity, meaning they efficiently transfer heat due to the movement of delocalized electrons.
• Solid state (at room temperature): Most metals are solid at room temperature, with exceptions like mercury, which is liquid.
  
• High melting and boiling points: Metals generally have high melting and boiling points compared to nonmetals, due to the strong metallic bonds between the positively charged metal ions and delocalized electrons.

Examples of metals include common elements like Iron (Fe), Copper (Cu), Gold (Au), Silver (Ag), Aluminum (Al), and Calcium (Ca).