Phases of matter

Three phases of water:  solid (ice); liquid (water); and gas (steam). Every day you encounter matter in one of its three phases: the floor you walk on is matter in its solid state; the water you drink during the day is in its liquid state; and the air you breathe is in its gaseous state. Each of these three phases of matter has unique characteristics. Matter in its solid state holds its shape. A liquid can change its shape by flowing to fill its container, but liquids keep their volumes constant. A gas takes the shape of its container by expanding (or contracting) its volume. Show Fourth phase of matter
At the microscopic level, the fundamental difference between solids, liquids, and gases is the average energy of its constituent particles. Atoms attract other atoms with forces that get stronger at first as two atoms get closer, then quickly becomes repulsive when the atoms start to overlap. As the thermal kinetic energy of the atoms increases, their temperature increases; higher energies can also cause the matter to transition from solid to liquid and then to gas. Solid matter stays solid because the jostling kinetic motion due to temperature is not enough to overcome the attractive forces between atoms. Matter turns into gas at high temperatures because the average thermal energies of the atoms allows them to break free completely from their intermolecular bonds.
When matter changes from one state (such as solid, liquid, or gas) to another one, we say that it undergoes a phase change. There are two important phase changes you might see every day: melting and boiling. When a solid becomes hot enough to reach the melting point, it begins the transition to a liquid through melting; likewise, when a liquid cools down sufficiently to that same melting point, it will freeze back into a solid. The same concept applies to boiling. When a liquid becomes hot enough that it reaches the boiling point, it begins the transition to a gas; when a gas cools down sufficiently, it will convert back to a liquid through condensation. Show Temperature and the microscopic view of phase changes
Energy content of ice, water, and steam at 0°C and 100 °C One kilogram of ice at the freezing point (0°C) has a thermal energy of 1.14 MJ (million joules), while one kilogram of liquid water at the same temperature has 1.48 MJ—more energy! Likewise, one kilogram of water at the boiling point (100°C) has 1.90 MJ of thermal energy, while one kilogram of steam at the same temperature has 4.15 MJ. How can gas molecules contain more thermal energy than liquid molecules at the same temperature? The answer is that a significant amount of energy had to be added to the ice to cause it to change phase to water, and much more energy had to be added to the water in order for it to change phase from liquid to steam. The added energy breaks the intermolecular bonds among the molecules. The higher energy per unit mass for steam compared to boiling water is why steam burns are so dangerous.
When water changes from a liquid to a solid, does this require energy or release energy? Show


146 Previous Page Next Page