Ionic Bonding Review

Question-and-answer flashcards summarising key concepts of ionic bonding, its formation, lattice structure, properties, and factors influencing bond strength.

What is ionic bonding?

The electrostatic attraction between oppositely charged ions, typically a metal cation and a non-metal anion.

How are ions formed in ionic bonding?

Metals lose electrons to become positively charged cations, while non-metals gain electrons to become negatively charged anions.

What electron arrangement do ions achieve after ionic bonding?

A full outer electron shell, resulting in a stable noble-gas configuration.

Which kinds of elements usually form ionic bonds?

Metals (forming positive ions) and non-metals (forming negative ions).

Describe the process of ionic bond formation.

A metal atom loses electrons to form a cation, a non-metal atom gains those electrons to form an anion, and the resulting opposite charges attract strongly.

What is a giant ionic lattice?

A three-dimensional, regular, repeating structure of billions of ions held together by strong ionic bonds.

List four key properties of ionic compounds.

High melting/boiling points, solubility in polar solvents (e.g., water), electrical conductivity when molten or in solution, and hard but brittle solid form.

Why do ionic compounds conduct electricity when molten or dissolved but not when solid?

In the solid lattice, ions are fixed and cannot move; when molten or dissolved, ions are free to move and carry charge.

How does ionic radius affect the strength of ionic bonding?

Smaller ions with a higher charge density produce stronger electrostatic attractions, strengthening the bond.

How does ionic charge affect the strength of ionic bonding?

Higher ionic charges increase electrostatic forces, resulting in stronger ionic bonds.

What is lattice enthalpy?

The energy released when one mole of an ionic lattice forms from its gaseous ions, reflecting bond strength.

How does lattice enthalpy relate to bond strength in ionic compounds?

A larger (more negative) lattice enthalpy indicates stronger ionic bonding within the lattice.