Chemical Bonding and Structure

Flashcards covering Metallic, Ionic, and Covalent (Molecular and Network) bonding, including their definitions, properties, and specific examples.

Metallic Bonding

Formed when delocalized valence electrons are shared among a lattice of positively charged metal ions.

Electrical conductivity in metals

Contain delocalized valence electrons that can move through the structure and carry charge through the lattice.

Malleability & Ductility (Metallic)

Layers of ions can slide while remaining attracted to the delocalized electrons, so the metallic bond doesn’t break.

Ionic Bonding

Electrostatic attraction between positively charged metal cations and negatively charged non‑metal anions after electrons are transferred.

Brittleness (Ionic)

Caused by like charges lining up and repelling strongly when the crystal is struck, causing it to shatter.

Conductivity of Ionic Compounds

They only conduct when molten or aqueous because ions are mobile and can carry charge; in the solid state, ions are locked in place.

Covalent Bonding (Covalent Molecular)

The sharing of electrons between non‑metal atoms to form molecules.

Melting and Boiling points (Covalent Molecular)

Low, because weak intermolecular forces require little energy to overcome.

Buckminsterfullerene ($C_{60}$)

A covalent molecular substance because it exists as individual molecules, not a continuous covalent network.

Covalent Bonding (Covalent Network)

A giant 3D lattice of atoms held together by strong covalent bonds throughout the entire structure.

Melting points (Covalent Network)

Very high, because atoms are held by strong covalent bonds in a giant 3D network, and breaking these requires huge amounts of energy.

Diamond

A covalent network where carbon has 4 bonds, resulting in a hard, high melting point structure that does not conduct electricity.

Graphite

A covalent network where carbon has 3 bonds and delocalized electrons between layers allow it to conduct electricity; its layers can slide, making it soft.

Silicon ($Si$)

A semiconductive covalent network element similar in structure to diamond.

Silicon dioxide ($SiO_2$)

A giant covalent network that is hard, has a high melting point, and is used in glass.

Naming Covalent Compounds

Add a prefix to the 1st and 2nd element and add -ide to the 2nd element, though mono- is never added to the 1st element.