Question

the substances shown are ordered (from left to right) in order of increasing a density b kinetic energy. c potential energy d intermolecular attractions

Explanation:

Step1: Analyze density

Density of ice is \(0.92\ g/cm^{3}\), water is \(1\ g/cm^{3}\), steam (gas) has very low density (much less than liquid water). So order of density is steam < ice < water. So option A is wrong.

Step2: Analyze kinetic energy

Kinetic energy of particles is related to temperature and state. In solid (ice) particles vibrate in fixed positions (low kinetic energy). In liquid (water) particles move more freely (higher kinetic energy than solid). In gas (steam) particles move randomly at high speeds (highest kinetic energy). So order of kinetic energy is ice < water < steam.

Step3: Analyze potential energy

Potential energy in phase - change context: When ice melts (solid to liquid), potential energy increases (breaking some intermolecular bonds). When water vaporizes (liquid to gas), potential energy increases more (breaking more intermolecular bonds). But the order given in the problem (left - right: ice, water, steam) for potential energy would be ice < water < steam. But let's check other options.

Step4: Analyze intermolecular attractions

Intermolecular attractions are strongest in solid (ice), weaker in liquid (water) and weakest in gas (steam). So order of intermolecular attractions is steam < water < ice. So option D is wrong.

Since the order of kinetic energy (ice < water < steam) matches the left - right order of the substances (A: ice, B: water, C: steam) in the problem.

Answer:

B. kinetic energy