Metals vs Non-Metals: The Basics
You'll spot metals straight away because they're the shiny, strong materials that feel solid in your hands. All metals have metallic bonding, which gives them their signature properties: they're tough to break, malleable (you can hammer them into different shapes), and they're brilliant at conducting heat and electricity. They also need loads of energy to melt or boil.
Non-metals are completely different beasts. Without metallic bonding, they tend to look dull and are much more brittle - they'll snap rather than bend. Most importantly for your exams, they generally won't conduct electricity (though there are exceptions like graphite).
Transition metals are what most people picture when they think "metal" - they're the dense, shiny, strong materials that make excellent catalysts in chemical reactions. These are your "typical metals" that tick all the metallic property boxes.
Group 1 elements (the alkali metals) might surprise you though. Despite being metals, they're actually soft and have low density because they're so desperate to lose that single outer electron - this makes them incredibly reactive.
Key Point: The number of outer shell electrons determines how an element behaves, not just whether it's a metal or non-metal.