Metals & Non-Metals - Vocabulary Flashcards

A vocabulary set of key terms from the Metals & Non-Metals notes, covering properties, processes, and applications.

Lustrous

Having a shining surface; characteristic metallic luster.

Metallic lustre

Shiny, reflective appearance typical of metals.

Non-lustrous

Lacking shine; opposite of lustrous (often seen in non-metals).

Hardness (metals vs non-metals)

Metals are generally hard; non-metals are generally soft.

Sonorous

Metals produce a ringing sound when struck against a hard surface.

Non-sonorous

Metals that do not produce a ringing sound when struck; examples include some non-metals.

Physical state at room temperature (metals)

All metals, except mercury, exist as solids at room temperature.

Mercury

The only metal that is liquid at room temperature.

High melting point

A property of many metals indicating they require high temperatures to melt.

Low melting point

Some metals have relatively low melting points.

Amphoteric oxide

An oxide that shows both acidic and basic properties (e.g., Al2O3, ZnO).

Allotrope

Different structural forms of the same element (e.g., carbon: graphite, diamond).

Graphite (carbon allotrope)

Lustrous form of carbon that conducts electricity.

Diamond (carbon allotrope)

Hardest natural substance with very high melting and boiling points.

Copper (Cu)

Used for cooking vessels; good conductor of heat; high melting point.

Aluminium (Al)

Used for cooking vessels; good conductor of heat; high melting point; forms protective oxide layer.

Alloy

Homogeneous mixture of two or more elements (metals or metal+non-metal).

Brass

Alloy of zinc and copper.

Bronze

Alloy of copper and tin.

Solder

Alloy of lead and tin.

Amalgam

Alloy in which one metal is mercury.

Ore

Minerals containing a high percentage of a metal suitable for profitable extraction.

Gangue

Impurities like soil or sand present in ore.

Roasting

Heating sulphide ores in excess air to form metal oxide.ptions: ZnS + O2 → ZnO + SO2.

Calcination

Heating carbonate ores in limited air to form metal oxide and CO2.

Reduction (metals from oxides)

Obtaining metal from its oxide; can be by carbon reduction or electrolytic reduction.

Electrolysis

Using electric current to extract metals; applied to very reactive metals.

Cathode

Electrode where reduction occurs in electrochemical cells.

Anode

Electrode where oxidation occurs in electrochemical cells.

Ionic (electrovalent) compound

Compound formed by electrostatic attraction between ions; solids with high mp; conduct electricity when molten or in solution.

Cation

Positively charged ion (e.g., Na⁺).

Anion

Negatively charged ion (e.g., Cl⁻).

Corrosion

Degradation of metals due to attack by environment (e.g., rusting of iron, tarnishing of copper/silver).

Rust

Iron oxide formed when iron corrodes in the presence of moisture and oxygen.

Tarnishing

Surface discoloration of metals (e.g., copper turns green; silver darkens) due to oxide/sulfide formation.

Prevention of corrosion (general)

Greasing, painting, oiling, galvanising, anodising to protect metals.

Galvanisation

Coating iron/steel with zinc, usually by electrolysis, to prevent corrosion.

Anodising

Forming a protective oxide layer on aluminum to prevent corrosion.

Electrolytic refining

Purifying impure metals (e.g., copper) by electrolysis; pure metal deposits at the cathode.

Thermit reaction

Highly exothermic reaction (Fe2O3 + Al → Al2O3 + Fe) used for welding.

Reactivity series

Order of metals by tendency to lose electrons; top is most reactive, bottom least reactive.

Displacement reaction

A more reactive metal displaces a less reactive metal from its compound.

Ore vs gangue in extraction

Ores contain high metal content; gangue is the impurity material surrounding the ore.