Bonding, Structure and Properties

Vocabulary practice flashcards covering metallic bonding, ionic bonding, structure, and material properties.

Four Common Groups of Materials

The four main classifications of materials: ionic compounds, metals, giant covalent substances, and simple covalent substances.

Sonorous

A physical property of metals describing their ability to make a ringing sound when hit.

Ductile

A physical property of metals describing their ability to be pulled into wires.

Malleable

A physical property of metals describing their ability to be beaten into sheets.

Metallic Bonding

Bonding occurring within a metal consisting of a regular arrangement of positive metal ions surrounded by a sea of delocalised electrons.

Thermal Conduction in Metals

The transfer of thermal energy occurring because positive metal ions are tightly packed; when heated, the ions vibrate and pass on the heat energy.

Electrical Conduction in Metals

The transmission of electric current made possible by a sea of delocalised electrons that can move through the structure and carry the charge.

Melting Point Trend in Metals

The increase in melting and boiling points corresponding to higher ion charges (such as $Al^{3+}$ compared to $Mg^{2+}$ and $Na^+$), because a greater charge produces a greater electrostatic attraction to the delocalised electrons.

Ionic Bond

The electrostatic force of attraction between oppositely charged ions, formed when metals lose electrons to become positive ions and non-metals gain electrons to become negative ions.

Giant Ionic Lattice

A regular three-dimensional structure containing millions of ions held together by ionic bonds, such as sodium chloride where each ion is surrounded by 6 ions of opposite charge in a cubic lattice.

Melting Point of Ionic Compounds

A characteristic high temperature requirement caused by the presence of many strong ionic bonds in the lattice that require a large amount of heat energy to break.

Electrical Conductivity of Ionic Compounds

The ability to conduct electricity only when molten or in solution because ions are free to move, whereas in solid form the ions are fixed and cannot move.

Brittleness of Ionic Compounds

The tendency of an ionic lattice to break easily under applied pressure because ions with the same charge are forced closer together, creating repulsion.