Ionic Bonding — Flashcards & Quiz

Q1: Describe ionic bonding and the properties of ionic compounds.

Ionic bonds form when electrons are transferred from a metal to a non-metal, creating oppositely charged ions (cations + anions) held together by electrostatic attraction in a crystal lattice. Properties: high melting/boiling points, hard and brittle, conduct electricity when molten or dissolved (mobile ions), soluble in water.

Q2: What is a lattice energy and how does it relate to ionic compound stability?

Lattice energy is the energy released when gaseous ions come together to form an ionic crystal lattice. Higher lattice energy = more stable compound = higher melting point. Lattice energy increases with higher ion charges and smaller ion sizes (stronger electrostatic attraction).

Q1: Ionic compounds conduct electricity in the solid state.

Answer: FALSE

Solid ionic compounds do NOT conduct because ions are fixed in the crystal lattice. They conduct when molten or dissolved because ions become mobile.

Q2: Ionic bonds form between metals and non-metals through electron transfer.

Answer: TRUE

Metals lose electrons (form cations) and non-metals gain electrons (form anions). The electrostatic attraction between these ions is an ionic bond.

Q3: Lattice energy increases when ion charges increase and ion sizes decrease.

Answer: TRUE

Higher charges and smaller ions mean stronger electrostatic attraction (Coulomb's law), resulting in greater lattice energy and higher melting points.