How does atomic structure explain the properties of metals and non-metals?

Atomic structure explains the properties of metals and non-metals through the arrangement and behaviour of their electrons.

Metals and non-metals differ greatly in their properties, and this is largely due to the differences in their atomic structures. Metals, for instance, have a unique atomic structure that allows them to conduct electricity and heat, be malleable and ductile, and exhibit a shiny lustre. These properties are due to the 'sea of electrons' model in which metal atoms lose their outermost electrons to form a 'sea' of free electrons. These free electrons can move around, allowing metals to conduct electricity and heat. The positive metal ions are packed closely together in a regular pattern, but the layers can slide over each other making metals malleable and ductile. The free electrons also interact with light, giving metals their characteristic shiny appearance.

Non-metals, on the other hand, have a different atomic structure. They tend to gain or share electrons to achieve a stable electron configuration, forming negative ions or covalent bonds. This results in non-metals generally being poor conductors of heat and electricity, as they lack the free electrons that metals have. Non-metals are also usually brittle and lack the lustre of metals. Their atomic structure leads to a variety of physical states at room temperature, including gases, liquids, and solids.

In summary, the atomic structure of metals and non-metals, particularly the behaviour of their electrons, is key to understanding their distinct properties. The 'sea of electrons' model in metals leads to their conductivity, malleability, ductility, and lustre, while the gaining or sharing of electrons in non-metals results in their generally poor conductivity, brittleness, and variety of physical states.