Plenary 6.2 - Ionic bonds and Ionic Compounds

Which of the following is not an ionic compound?

• magnesium oxide

• sodium chloride

• dihydrogen monoxide

• barium sulfate

Identify the binary ionic compound.

• H₂O

• NaCl

• C₆H₁₂O₆

• Be₃Al₂Si₆O₁₈

What term best describes the structure formed by the strong attractions among the positive ions and the negative ions in an ionic compound?

• a mineral

• an oxide

• a salt crystal

• a crystal lattice

Which of the following is true of ionic crystals?

• Ionic bonds are strong, so ionic crystals require a large amount of energy to be broken.

• Ionic crystals have low melting points and high boiling points.

• Ionic crystals are malleable, not brittle.

• Ionic crystals always conduct electricity.

Which of the following is correct?

• Lattice energy is the energy needed for 1 mol of positive ions to bond with 1 mol of negative ions.

• Ions in an ionic compound are arranged in a random pattern.

• Ionic compounds are never electrolytes.

• Ionic compound properties are related to ionic bonding.

Why are solid ionic compounds poor conductors of electricity?

• They are non-metals.  

• They are electrolytes.

• They have electrons that   cannot flow freely.

• Solids do not conduct electricity

What is the electrostatic charge holding two ions together?

• covalent bond

• pseudo-noble gas bond

• crystal lattice bond

• ionic bond