Class 10th Science: Metals and Non-Metals

Comprehensive vocabulary flashcards covering key definitions, physical and chemical properties, extraction processes, refining methods, and alloys from Class 10th Science Chapter 'Metals and Non-Metals'.

Malleability

The physical property of a metal that allows it to be hammered or beaten into thin sheets without breaking (e.g., aluminium, iron), with exceptions including zinc, arsenic, and mercury.

Ductility

The physical property of a metal that allows it to be drawn or stretched into thin wires (e.g., copper, aluminium), with mercury and zinc being notable exceptions.

Sonority

The characteristic property of metals to produce a ringing sound when struck (sonorous), seen in metals like iron and copper, with mercury being non-sonorous.

Metallic Lustre

The shiny surface appearance characteristic of metals in their pure state (e.g., gold, aluminium). Non-metals are typically dull, with iodine being a lustrous exception.

Amphoteric Metals

Metals whose oxides exhibit both acidic and basic characteristics, reacting with both acids and bases to yield salt and water (e.g., beryllium, zinc, tin, lead, aluminium, and antimony).

Aqua Regia

A highly corrosive fuming mixture consisting of concentrated hydrochloric acid and concentrated nitric acid in a $3:1$ ratio, capable of dissolving noble metals such as gold ($\text{Au}$) and platinum ($\text{Pt}$).

Reactivity Series

A vertical arrangement of metals placed in decreasing order of their chemical reactivity, with potassium ($\text{K}$) at the top as most reactive and gold ($\text{Au}$) at the bottom as least reactive.

Ionic Bond

A chemical bond formed via electrostatic attraction between oppositely charged ions resulting from the complete transfer of one or more valence electrons from a metal atom to a non-metal atom.

Ionic Compounds

Compounds consisting of cations and anions held together by strong inter-ionic electrostatic forces, resulting in high melting and boiling points, solubility in water, and electrical conductivity only in molten or aqueous states.

Metallurgy

The science and technology involved in studying the properties of metals and their extraction, production, and purification from their ores.

Minerals

Naturally occurring inorganic elements or compounds found in the Earth's crust (e.g., salt, clay, marble) that may or may not contain metals in commercially viable amounts.

Ores

Naturally occurring minerals containing a sufficiently high percentage of a metal from which that metal can be extracted conveniently, profitably, and economically (e.g., bauxite, hematite, rock salt).

Gangue Particles

The undesirable, commercially worthless impurities—such as sand, rock, soil, or oil—present alongside the desired metal compound in naturally mined ores.

Enrichment of Ore (Concentration)

The initial physical or chemical process of separating and removing gangue particles from mined ore prior to the extraction of the metal.

Roasting

A metallurgical process in which a concentrated ore (typically a sulphide ore) is heated strongly in the presence of excess air or oxygen to convert it into a metal oxide, accompanied by the release of $\text{SO}_2$ gas.

Calcination

A metallurgical process in which an ore (typically a carbonate or hydrated ore) is heated strongly below its melting point in the presence of limited air or oxygen to expel volatile impurities and carbon dioxide.

Thermit Reaction

A highly exothermic reduction reaction where iron(III) oxide is reduced by aluminium powder ($\text{Fe}_2\text{O}_3 + 2\text{Al} \rightarrow 2\text{Fe} + \text{Al}_2\text{O}_3$), releasing enough heat to produce molten iron used for joining railway tracks or cracked machine parts.

Electrolytic Refining

A purification technique for metals (such as copper, zinc, tin, nickel, silver, and gold) using an electrolytic cell where impure metal serves as the anode, a thin pure metal strip serves as the cathode, and a metal salt solution acts as the electrolyte.

Anode Mud

The insoluble residue and impurities that drop and settle at the bottom of the tank directly beneath the positive electrode (anode) during the electrolytic refining process.

Corrosion

The gradual destruction of metals caused by chemical reactions with environmental agents like moist air, oxygen, and carbon dioxide (e.g., tarnishing of silver into black $\text{Ag}_2\text{S}$, formation of green $\text{CuCO}_3 \cdot \text{Cu(OH)}_2$ on copper, and rusting of iron into hydrated iron oxide $\text{Fe}_2\text{O}_3 \cdot x\text{H}_2\text{O}$).

Alloy

A homogeneous mixture of two or more metals, or a metal with a non-metal, formed to alter physical properties such as increasing hardness, lowering melting point, or reducing electrical conductivity.

Brass

An alloy composed of copper and zinc ($\text{Cu} + \text{Zn}$) that is a poorer conductor of electricity than pure copper.

Bronze

An alloy composed of copper and tin ($\text{Cu} + \text{Sn}$) that exhibits significantly lower electrical conductivity compared to pure copper.

Solder

An alloy composed of lead and tin ($\text{Pb} + \text{Sn}$) with a notably low melting point, making it suitable for welding and joining electrical components.

22 Carat Gold

A gold alloy consisting of 22 parts by weight of pure gold alloyed with 2 parts of either copper or silver, providing the hardness necessary for crafting jewellery.