Metals, Bonding, and Extraction: Key Concepts Explained

Metals, Bonding, and Extraction: Key Concepts

Attractive forces in a metallic structure arise because positive ions and electrons attract each other.

High Melting Points

Why does X have a high melting point? Due to its giant covalent structure, a lot of energy is needed to break the strong covalent bonds.

Lattice Structure of Metals

Why do metals have a lattice structure? The atoms in a pure metal are arranged in closely packed layers, which makes them strong.

Alloys

Alloy: A mixture of a metal with at least one other element.

Isotopes

Isotope: An atom with a different number of neutrons.

• The more reactive the metal, the more likely it is to corrode from oxygen and water.

Ores

Ore: A rock that contains enough metal to make mining and extraction economical.

Metal Extraction Methods

Two main ways to extract metals from their ores:

• Electrolysis
• Burning ores with carbon (reduction)

Aluminium Properties

Why does aluminium have a low density and resist corrosion? A thin layer of oxide quickly forms on the surface and prevents any further reaction from taking place, which is very important in the aerospace industry.

Amphoteric Substances

Amphoteric: Able to react both as a base and as an acid.

Alkali and Alkaline Earth Metals

• Very reactive with water
• Low densities
• High and shiny
• High melting points (lower than transition metals)

Transition and Inner Transition Metals

• Reactive with acids
• Higher melting and boiling points than other metals
• High densities
• High and shiny
• Malleable and ductile
• Radioactive

General Properties of Metals

Metals: Shiny, malleable, ductile, high melting point, good conductors of electricity and heat.

General Properties of Non-Metals

Non-metals: Brittle, dull, low melting and boiling point, poor conductors of electricity and heat.

Covalent Bonding

Covalent bonding: A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms (non-metal atoms only).

Ionic Bonding

Ionic bonding: An ionic bond is formed when electrons are lost and gained by two or more atoms (metal and non-metal atoms).

Metallic Bonding

Metallic bonding: The metallic bond is the force of attraction between these free-moving (delocalised) electrons and positive metal ions (metal atoms only).

Ionic compounds do not conduct electricity when they are solid because the ions are packed together and cannot move.

When molten or dissolved in water, however, the lattice breaks up and the ions are free to move, then they conduct electricity.

When copper nitrate is heated strongly, it produces copper oxide, nitrogen dioxide, and oxygen.