ionic bond

Cation

A positively charged ion formed by losing electrons.

Anion

A negatively charged ion formed by gaining electrons.

Ionic bond

The electrostatic attraction between cations and anions formed by the transfer of electrons.

Lewis symbols

Notation that represents atoms with their chemical symbol surrounded by dots indicating valence electrons.

Lewis structures

Diagrams that show the formation of bonds and the arrangement of electrons in molecules.

Lattice energy

The energy released when gaseous ions form an ionic solid; indicates the strength of ionic bonds.

Ionization energy (IE)

The energy required to remove an electron from an atom, which influences cation formation.

Electron affinity (EA)

The energy change when an atom gains an electron, important for anion formation.

Born-Haber cycle

A thermochemical cycle that relates lattice energy to other energy changes involved in ionic compound formation.

Electrostatic attraction

The force that attracts oppositely charged ions toward each other in an ionic bond.

Energetic favorability

Condition in which the energy released during ionic lattice formation compensates for the energy absorbed in ion formation.

Size of ions

A factor affecting lattice energy; smaller ions with higher charges create stronger ionic bonds.

Octet rule exception

Condition for some atoms that can achieve a stable configuration with fewer than eight electrons.

18-electron rule

A guideline for transition metals indicating they often seek to fill d orbitals alongside s orbitals.

High melting point

Characteristic of ionic compounds typically resulting from strong ionic bonds influenced by high lattice energy.

Solubility in water

The ability of ionic compounds to dissolve in water, often correlated with lattice energy.

Transition Metals

Elements that often do not follow the octet rule due to involvement of d orbitals.

Stability of ionic compounds

Related to the lattice energy where higher lattice energy makes compounds more stable.

Stable ionic configuration

A state attained by atoms in ionic compounds, often involving the complete transfer of electrons.

Affecting ionic bonds

Factors such as ion size, charge, and electron affinities that influence the strength and formation of ionic bonds.