0.1 States of matter and the kinetic molecular theory  (Page 5/7)

The properties of matter

Let us now look at what we have learned about chemical bonds, intermolecular forces and the kinetic theory of matter, and see whetherthis can help us to understand some of the macroscopic properties of materials.

1. Melting point

   Melting point

   The temperature at which a solid changes its phase or state to become a liquid . The process is called melting and the reverse process (change in phase from liquidto solid) is called freezing .

   In order for a solid to melt, the energy of the particles must increase enough to overcome the bonds that are holding the particlestogether. It makes sense then that a solid which is held together by strong bonds will have a higher melting point than one where the bonds are weak, because more energy (heat) is needed to breakthe bonds. In the examples we have looked at metals, ionic solids and some atomic lattices (e.g. diamond) have high melting points, whereas the meltingpoints for molecular solids and other atomic lattices (e.g. graphite) are much lower. Generally, the intermolecular forces between molecular solids are weaker than those between ionic and metallic solids.
2. Boiling point

   Boiling point

   The temperature at which a liquid changes its phase to become a gas . The process is called evaporation and the reverse process is called condensation

   When the temperature of a liquid increases, the average kinetic energy of the particles also increases and they are able to overcomethe bonding forces that are holding them in the liquid. When boiling point is reached, evaporation takes place and some particles in the liquid become a gas. In other words, the energy of theparticles is too great for them to be held in a liquid anymore. The stronger the bonds within a liquid, the higher the boiling point needs to be in order tobreak these bonds. Metallic and ionic compounds have high boiling points while the boiling point for molecular liquids is lower.The data in [link] below may help you to understand some of the concepts we have explained. Not all of the substances in the table aresolids at room temperature, so for now, let's just focus on the boiling points for each of these substances. What do you notice?

   Substance	Melting point ( ${}^{°}\mathrm{C}$ )	Boiling point ( ${}^{°}\mathrm{C}$ )
   Ethanol ( ${\mathrm{C}}_2{\mathrm{H}}_6\mathrm{O}$ )	- 114,3	78,4
   Water	0	100
   Mercury	-38,83	356,73
   Sodium chloride	801	1465

   You will have seen that substances such as ethanol, with relatively weak intermolecular forces, have the lowest boiling point, while substances withstronger intermolecular forces such as sodium chloride and mercury, must be heated much more if the particles are to have enough energy to overcome theforces that are holding them together in the liquid. See the section below for a further exercise on boiling point.
3. Density and viscosity
   Density and viscosity is not in CAPS - Included for Completeness

   Density

   Density is a measure of the mass of a substance per unit volume.

   The density of a solid is generally higher than that of a liquid because the particles are held much more closely together and therefore thereare more particles packed together in a particular volume. In other words, there is a greater mass of the substance in a particular volume. In general, densityincreases as the strength of the intermolecular forces increases.

   Viscosity

   Viscosity is a measure of how resistant a liquid is to flowing (in other words, how easy it is to pour the liquid from one container toanother).

   Viscosity is also sometimes described as the 'thickness' of a fluid. Think for example of syrup and how slowly it pours from one container intoanother. Now compare this to how easy it is to pour water. The viscosity of syrup is greater than the viscosity of water. Once again, the stronger theintermolecular forces in the liquid, the greater its viscosity.