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Atomic Structure
Non-metals have atoms with 4-8 electrons in their outermost shell. They tend to gain electrons to achieve stable configuration. Unlike metals, their electrons are tightly bound to the nucleus.
This electron configuration explains why non-metals are poor conductors!
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Physical States
Non-metals exist in all three states at room temperature: Solids (Carbon, Sulfur, Iodine), Liquids (Bromine - the only liquid non-metal), and Gases (Oxygen, Nitrogen, Hydrogen, Chlorine).
Bromine is unique - it's the only non-metal that's liquid at room temperature!
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Brittleness
Solid non-metals are brittle - they break or shatter when struck with force. This happens because their atoms are held by covalent bonds in fixed positions and cannot slide past each other like metals.
When you hit sulfur with a hammer, it breaks into powder instead of flattening!
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Carbon Allotropes
Carbon is special - it can exist in different forms called allotropes. Diamond (hardest natural substance, doesn't conduct electricity), Graphite (soft, conducts electricity), and Fullerenes (soccer ball-shaped molecules).
Same element, completely different properties - that's the magic of allotropes!
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Notable Exceptions
Not all non-metals follow the typical rules! Iodine has metallic lustre despite being a non-metal. Graphite conducts electricity due to delocalized electrons. Diamond has an extremely high melting point (3500°C).
These exceptions make chemistry fascinating and show that nature doesn't always follow simple rules!