Metals and Non-Metals: 30 flashcards
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1. How do metals and non-metals differ in electron behaviour?
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Metals tend to lose electrons and form positive ions; non-metals tend to gain or share electrons.
2. What is lustre, and which type of element usually shows it?
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Lustre is a shiny, reflective surface. Metals usually show it; iodine is a non-metal exception.
3. Define malleability.
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The ability to be beaten into thin sheets — a typical metal property (e.g. aluminium foil).
4. Define ductility.
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The ability to be drawn into wires — a typical metal property (e.g. copper wiring).
5. What does sonorous mean?
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Making a ringing sound when struck — a property of metals (e.g. temple bells).
6. Why do metals conduct electricity?
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Because of delocalised (free) electrons that can carry charge through the metal.
7. What is the electron sea model?
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A model where metal atoms release valence electrons into a shared cloud of free electrons that holds the lattice together.
8. Which metal is liquid at room temperature?
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Mercury — the only metal that is liquid at room temperature.
9. Which non-metal conducts electricity?
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Graphite — a form of carbon that conducts because of delocalised electrons within its layers.
10. Which non-metal shows lustre?
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Iodine — a non-metal that has a shiny appearance.
11. What are metalloids? Give examples.
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Elements that show properties of both metals and non-metals — e.g. silicon, germanium, arsenic.
12. Where are metals and non-metals located on the periodic table?
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Metals occupy the left and centre; non-metals cluster at the top-right (plus hydrogen at top-left).
13. What is the reactivity series?
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A ranking of metals from highly reactive (potassium, sodium) to nearly inert (gold, platinum).
14. Why is sodium stored in kerosene?
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Because sodium reacts vigorously with air and moisture, so kerosene keeps it away from both.
15. What is galvanisation and why is it done?
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Coating iron with zinc to prevent rusting.
16. Why are copper and aluminium used in electrical wiring?
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Because they are ductile and good conductors of electricity.
17. Why are gold and silver used in jewellery?
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Because they are lustrous and malleable.
18. Give the reaction showing a metal losing an electron.
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$\text{Na} \rightarrow \text{Na}^+ + e^-$
19. Give the reaction showing a non-metal gaining an electron.
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$\text{Cl} + e^- \rightarrow \text{Cl}^-$
20. What compound forms when sodium reacts with chlorine?
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Sodium chloride ($\text{NaCl}$) — common table salt.
21. Which non-metal is essential for combustion and respiration?
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Oxygen — a non-metal gas essential for both.
22. Which non-metals are used in matches and fertilisers?
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Sulphur and phosphorus — reactive non-metals.
23. Which non-metal is fiercely reactive, and which is almost inert?
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Fluorine is fiercely reactive; nitrogen is almost inert under normal conditions.
24. Why is gold found in nature in its pure form?
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Because it is almost inert and does not readily react with other substances.
25. State the general physical state of metals and non-metals at room temperature.
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Most metals are solids (mercury is liquid); non-metals can be solids, liquids, or gases.
26. Are non-metals malleable and ductile?
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No — non-metals are generally brittle and break instead of bending.
27. What is the root cause of metallic properties like lustre and conductivity?
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The free-electron sea (delocalised electrons) inside the metal lattice.
28. Why does the metal–non-metal distinction matter chemically?
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It drives electron transfer, which is the basis of chemical bonding (e.g. forming $\text{NaCl}$).
29. Name three common metals used in everyday life and one use each.
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Copper (wiring), aluminium (foil and wiring), gold (jewellery).
30. Name three common non-metals and one use each.
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Oxygen (respiration/combustion), sulphur (matches/fertilisers), phosphorus (matches/fertilisers).
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