Properties and Applications of Ionic Compounds

Ionic compounds are not limited to labs; they have real-world uses like table salt and toothpaste. They share properties such as high melting points and brittleness due to their 3D lattice structure. Ionic compounds dissolve in water, dissociating into ions, which allows them to conduct electricity. This is demonstrated with copper sulfate in water. Molten ionic compounds also conduct electricity. Key properties include high melting points, brittleness, and electrical conductivity when dissolved or molten.

Which of the following is a real-life application of sodium chloride?

• Added to toothpaste

• Regular table salt

• Used in fertilizers

• Used in batteries

What structural feature contributes to the high melting points of ionic compounds?

• Van der Waals forces

• Metallic bonds

• 3D giant ionic lattice

• Covalent bonds

Why are ionic compounds brittle?

• Because of the repulsion between like-charged ions

• Because of their covalent nature

• Due to weak intermolecular forces

• Due to their metallic bonds

What happens to ionic compounds when they dissolve in water?

• They form covalent bonds

• They dissociate into ions

• They evaporate

• They become metallic

How are sodium ions stabilized in water?

• By the negative dipole of water

• By hydrogen bonding

• By the positive dipole of water

• By forming covalent bonds

What property allows ionic compounds to conduct electricity when dissolved in water?

• Brittleness

• High melting points

• Presence of free-floating ions

• Covalent bonding

In the experiment with copper sulfate, what role do the copper and zinc strips play?

• They act as electrodes

• They are the solvent

• They are the ionic compound

• They act as solutes

What happens to the lattice structure of ionic compounds at high temperatures?

• It becomes more rigid

• It breaks, allowing ions to move freely

• It becomes metallic

• It forms covalent bonds

Which of the following is NOT a key property of ionic compounds?

• High melting points

• Brittleness

• Ability to conduct electricity when molten

• Low boiling points

What allows molten ionic compounds to conduct electricity?

• Presence of free-floating ions

• High density

• Covalent bonding

• Low melting points