The table compares the properties of two compounds. Compound J is an ionic compound and compound L is a simple molecular compound. Property Compound J Compo...

This question contrasts a giant ionic compound (J) with a simple molecular compound (L), using structure and bonding to explain every property.

(a) Compound J has a giant ionic lattice (giant ionic structure) [1]. [1]

(b) Within a molecule of the simple molecular compound L, the atoms are joined by covalent bonds (shared pairs of electrons) [1]. [1]

(c) J is a giant ionic lattice with strong electrostatic forces of attraction between oppositely charged ions, so a lot of energy is needed to break them [1][1]; L is simple molecular, with only weak intermolecular forces between separate molecules that need little energy to overcome [1]. This is why J melts at 850 °C but L at \(-85\) °C. [3]

(d) In solid J the ions are held in fixed positions in the lattice and cannot move [1]; when J is molten the lattice breaks down and the ions become free to move [1]; the moving ions then carry the electric charge, so molten J conducts [1]. [3]

(e) The strong forces between the ions in J hold the particles firmly together, so it is a solid at room temperature [1]; the weak forces between L's molecules are so easily overcome that L is a gas at room temperature [1]. [2]

(f) When J dissolves, the lattice breaks up and the ions separate and become free to move [1]; these mobile ions carry the charge through the solution, so it conducts [1]. [2]

(g) L contains no ions and no other free-moving charged particles (its electrons are held in fixed covalent bonds), so it cannot conduct in any state [1]. [1]

(h) The charged particles in J are ions [1] - specifically positive cations and negative anions [1]. [2]