iAL CHEM - Bonding & Structure - Ionic Bonding

What is ionic bonding?

• The repulsion between like charges

• The electrostatic attraction between oppositely charged ions

• The sharing of electrons between atoms

• The formation of covalent bonds

What happens to sodium atoms when they react with chlorine?

• They remain neutral

• They form covalent bonds

• They lose electrons to become positive ions

• They gain electrons to become negative ions

Which of the following represents the formation of chloride ions?

• Cl^- + e- → Cl

• Cl₂ + 2Na → 2NaCl

• Cl₂ → 2Cl⁺ + 2e-

• Cl₂ + 2e- → 2Cl^-

What is the structure of sodium chloride in solid form?

• A random arrangement of ions

• A liquid state

• A giant lattice of oppositely charged ions

• A single molecule

What is the effect of ionic radius on the strength of ionic bonding?

• Larger ions lead to stronger bonds

• Smaller ions lead to stronger bonds

• Smaller ions lead to weaker bonds

• Smaller ions require less energy to separate

What is lattice formation enthalpy ?

• The energy needed to melt an ionic compound

• The energy released when gaseous ions form a lattice

• The energy associated with covalent bonds

• The energy required to break ionic bonds

Which of the following compounds has the highest lattice energy?

• Potassium fluoride

• Sodium chloride

• Calcium oxide

• Magnesium fluoride

What evidence supports the existence of ions in ionic compounds?

• Their ability to conduct electricity when molten or aqueous

• Their solid state at room temperature

• Their low melting points

• Their gaseous state

What occurs at the negative electrode during electrolysis of molten sodium chloride?

• Chloride ions gain electrons

• Chlorine gas is produced

• Sodium ions gain electrons

• Sodium ions lose electrons

In a dot-and-cross diagram, what do the dots represent?

• Electrons from one atom

• Nuclear charges

• Ionic bonds

• Electrons from both atoms