Metals – History, Properties & Reactions

Vocabulary flashcards covering key historical periods, mineral terminology, Group 1 properties, metallic bonding, alloys, reactivity, redox concepts, electrolysis and blast-furnace extraction from the lecture notes.

Alkali Metals (Group 1)

Highly reactive metals—Li, Na, K, Rb, Cs, Fr—with one valence electron.

Lithium flame

red flame

Sodium flame

yellow flame

Potassium flame

lilac flame colour.

Softness (Alkali Metals)

Physical trait allowing Li, Na, K to be cut with a knife.

Density Trend (Group 1)

Density generally increases down the group

Atomic Size (Group 1 Trend)

Atoms get larger down the group, contributing to higher reactivity.

Steel

Alloy of iron and carbon; stronger and more versatile than pure iron.

Transition Metals

Block of 30 center-table elements known for hardness, high melting points and variable oxidation states.

Metallic Bonding

Attraction between positive metal ions and a ‘sea’ of delocalised electrons in a lattice.

Delocalised Electrons

Valence electrons free to move through a metal lattice, enabling conductivity.

Metal Lattice

Regular three-dimensional arrangement of positive metal ions in a solid metal.

Malleability

Ability of a metal to be hammered or rolled into shapes without breaking.

Ductility

Capability of a metal to be drawn into a wire.

Alloy

Mixture of two or more elements (often metals) designed to improve properties.

Substitutional Alloy

Alloy where similar-size atoms replace host atoms in lattice (e.g., brass).

Interstitial Alloy

Alloy where smaller atoms occupy spaces between larger atoms (e.g., steel).

Hardness (Metals)

Resistance to scratching or indentation; depends on metallic bond strength.

Reactivity Series

Ranking of metals from most to least reactive based on tendency to lose electrons.

Metal Oxide

Compound formed when a metal reacts with oxygen (e.g., ZnO).

Metal Hydroxide

Product of metal reacting with water, alongside hydrogen gas (e.g., NaOH).

Displacement Reaction

Reaction where a more reactive metal displaces a less reactive metal from solution.

Electrolysis

Process using electric current to decompose molten or aqueous ionic compounds into elements.

Electrolyte

Molten or dissolved ionic compound that conducts electricity during electrolysis.

Cathode

Negative electrode where cations gain electrons (reduction) in electrolysis.

Anode

Positive electrode where anions lose electrons (oxidation) in electrolysis.

Direct Current (DC)

Unidirectional electric flow essential for consistent ion movement in electrolysis.

Redox Reaction

Chemical reaction featuring simultaneous oxidation and reduction (electron transfer).

Oxidation

Loss of electrons or gain of oxygen by a substance.

Reduction

Gain of electrons or loss of oxygen by a substance.

Oxidising Agent

Substance that causes oxidation, gets reduced by accepting electrons.

Reducing Agent

Substance that causes reduction, gets oxidised by donating electrons.

Half-Equation

Equation showing electron loss or gain for either oxidation or reduction part of a redox reaction.

Potassium Flame Colour

Light purple flame

Corrosion

Gradual destruction of metals by chemical reactions with environment (e.g., rusting of iron).

Rusting

Formation of hydrated iron(III) oxide when iron reacts with oxygen and water.

Catalyst (Transition Metals)

Substance that speeds up reactions without being consumed; many transition metals act as catalysts.

Electrical Conductivity (Metals)

Property resulting from free electrons; silver is the best conductor, followed by copper.

Lustre

Shiny appearance of metals caused by reflection of light by free electrons.

Metal Density

High mass per unit volume due to closely packed lattice of metal ions.

Melting Point (Metals)

Temperature where metallic lattice breaks; higher when metallic bonds are stronger.

Charge Density

Ratio of ionic charge to size; higher charge density strengthens metallic bonds.

Group 1 Reactivity Trend

Reactivity increases down the group as outer electron is lost more easily.

Colourless Ionic Solutions (Group 1)

Alkali-metal compounds (e.g., NaCl) dissolve to form colourless solutions.

Lithium Flame Colour

Crimson-red flame produced when Li compounds burn.

Sodium Flame Colour

Bright yellow flame seen when Na compounds burn.