Structure of Solids

Flashcards covering key concepts on the structure of solids, including ionic bonds, covalent structures, properties of materials like diamond and graphite, and the unique properties of ice and iodine.

Ionic Bond

The electrostatic force between a positively charged metal ion (cation) and a negatively charged non-metal ion (anion).

Giant Ionic Lattices

Regular repeating arrangements of cations and anions held together via strong electrostatic forces.

Coordination Number

The number of atoms or ions that surround a central atom or ion in a lattice; in NaCl, each ion is 6-coordinate.

Covalent Bond

A bond between non-metals in which electrons are shared between the atoms.

Simple Molecular Lattices

Structures where covalent compounds are arranged; examples include iodine and ice.

Hydrogen Bonds

Weak interactions that occur between polar molecules, such as in liquid water.

Face-centered Cubic (fcc) Structure

A crystal structure consisting of an atom at each cube corner and an atom in the center of each cube face.

Diamond

A giant covalent structure that is very hard, has a high melting point, and does not conduct electricity.

Graphite

A form of carbon that has a high melting point, is soft and slippery, and conducts electricity due to delocalised electrons.

Silicon Dioxide

A hard material with a high melting point that does not conduct electricity and is insoluble in water and organic solvents.

Unique Density of Ice

Ice is less dense than liquid water, allowing it to float and insulating liquid water below it during winter.

Iodine

A dark grey crystalline solid with a low melting point and a face-centered cubic structure.