Ionic Compounds and Metals

Ion

A charged particle formed when an atom gains or loses electrons.

Ionic bond

The electrostatic attraction between oppositely charged ions, usually formed when a metal transfers electrons to a nonmetal.

Metallic bond

The attraction between positive metal ions and a sea of freely moving, delocalized valence electrons.

Oxyanion

A polyatomic ion containing oxygen bonded to another element.

Exothermic

A process that releases energy.

Endothermic

A process that absorbs energy.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Formula unit

The simplest whole-number ratio of ions in an ionic compound.

Ionic crystal lattice

An ordered, three-dimensional arrangement of positive and negative ions held together by strong electrostatic attractions.

Metallic crystal lattice

An ordered arrangement of metal particles held together by metallic bonds.

Electrolyte

A substance that produces ions in solution and allows the solution to conduct electricity.

Lattice energy

The energy released when a mole of an ionic crystal forms from its gaseous ions.

Metal

An element that generally loses electrons and forms positive ions called cations.

Nonmetal

An element that generally gains electrons and forms negative ions called anions.

Delocalized electrons

Electrons that are free to move throughout a metallic structure.

Highest lattice energy

Look for the smallest ions and the largest charge magnitudes.

Lowest lattice energy

Look for larger ions and smaller charge magnitudes.

Metallic bonding

Positive metal ions are surrounded by a sea of freely moving electrons.

Metal electrical conductivity

Metals conduct electricity because their delocalized valence electrons can move freely.

Metal heat conductivity

Metals conduct heat because their mobile electrons help transfer energy.

Metal malleability

Metals can be shaped because layers of atoms can slide past each other while metallic bonding holds the structure together.

Metal ductility

Metals can be stretched into wires because their layers can slide past each other.

Ionic compound hardness

Ionic compounds are generally hard because their ions are held together by strong attractions.

Ionic compound melting point

Ionic compounds generally have high melting points because strong attractions require lots of energy to overcome.

Ionic compound boiling point

Ionic compounds generally have high boiling points because strong attractions require lots of energy to overcome.

Ionic compound brittleness

Ionic compounds are brittle because shifting their layers causes like-charged ions to repel each other.

Ionic compound ductility

Ionic compounds are not ductile because their crystal structures break instead of bending.

Solid ionic conductivity

Solid ionic compounds do not conduct electricity because their ions are locked in place.

Aqueous ionic conductivity

Dissolved ionic compounds conduct electricity because their ions are free to move and carry electrical current.

Molten ionic conductivity

Melted ionic compounds conduct electricity because their ions are free to move.

Ionic bond formation

Exothermic because energy is released when oppositely charged gaseous ions come together to form an ionic crystal.

Ionic compound attraction

Positive and negative ions attract each other through strong electrostatic forces.

Ionic compound high melting point

Strong attractions between oppositely charged ions require a large amount of energy to overcome.

Naming ionic compounds

Name the metal first and the nonmetal second, changing the nonmetal ending to -ide.