Compare the physical and chemical properties of metals and non-metals, explore the reactivity series, and see how ionic bonds form.
Metals are generally shiny, malleable, ductile, and good conductors of heat and electricity. Non-metals are usually dull, brittle (if solid), and poor conductors.
A sample can be hammered into thin sheets without breaking. Is it more likely a metal or a non-metal?
A metal — this property is called malleability
4Na + O₂ → 2Na₂O is a combination reaction. Is it balanced?
Yes — 4 Na and 2 O atoms on each side
Metals can be arranged in order of how readily they react. A more reactive metal can displace a less reactive one from its compound.
(Most reactive → least reactive)
Fe + CuSO₄ → FeSO₄ + Cu — why does this reaction happen?
Iron is more reactive than copper, so it displaces copper from copper sulphate
Metals tend to lose electrons to form positive ions (cations); non-metals tend to gain electrons to form negative ions (anions). The attraction between oppositely charged ions is an ionic bond.
In NaCl, sodium loses one electron and chlorine gains one. What ions are formed?
Na⁺ (sodium ion) and Cl⁻ (chloride ion)
1. Which property lets a metal be drawn into wires?
2. Between Zn and Cu, which is more reactive according to the reactivity series?
3. Will Zn + CuSO₄ → ZnSO₄ + Cu happen? Why or why not?
4. When a metal atom forms an ion, does it usually gain or lose electrons?
5. Is a non-metal more likely to be a good or a poor conductor of electricity?