The general properties of metals can be summarised in the image below:
We can use the general properties of metals shown in the image above to help us figure out what the structure of a metal looks like. The table below tries to offer an explanation for some of the properties of metals and relate this property to a possible feature of the metal structure and the bonding present in the metal
| Metal property | How this relates to its structure |
|---|---|
| Metals are good conductors of electricity and heat | There must be free or delocalised electrons within the structure to conduct the electricity and heat. |
| Metals have high melting and boiling points. | Metals must have a giant structure with lots of strong bonds. |
| Metals are malleable (can be hammered into shape) and ductile (can be pulled into wire). | There are layers of particles that are able to slide over each other. |
| Metals are shiny. | Free or delocalised electrons are able to reflect light at the surface. |
| Metals are hard and dense | The particles within the metal structure are packed tightly together. |
These basic properties of metals allows us to suggest that metals consist of a giant structures of ions which are surrounded by a sea of free moving delocalised electrons. We also already know that metals are found on the left hand side of the periodic table in groups 1, 2 and 3 and that they tend to lose electrons in their reactions to form positively charged ions. This leads us to the model shown below. The dark grey balls represent positively charged metal ions (atoms which have lost their outer shell electrons). These electrons are delocalised and free to move through the giant structure of ions. This might seem odd since we might expect a giant structure of ions which all have a positive charge to repel each other and so the structure would simply break down. However we need to think about the delocalised electrons within the structure.
The negatively charged electrons are attracted to the
positively charged metal ions and
this prevents the metal ions from
repelling
each other. The electrons are attracted to the metal
ions around them. This attraction of the negatively
charged electrons to the neighbouring positively charged
metal ions is called a metallic
bond. A key feature of
this bond is the fact that metallic bonds are not permanent but are
constantly breaking and reforming
as the electrons move
freely around the structure, this is shown in the diagram below:
The fact that these metallic bonds are not permanent
but are constantly breaking and
reforming allows the layers of ions
to slide over each other. This is shown in the diagram below; which shows
a pushing force being applied to the top two
layers of ions in a metal structure.
The metallic bonds in these layers immediately break
and the layers slide along
but as soon as they stop moving the metallic bonds immediately reform.
This is why metals are malleable (can be hammered into shape) and ductile (can be pulled into wires).
Metals generally have high melting points, high densities and are good electrical and thermal conductors, though these properties can vary significantly as we cross the periodic table. Let us examine some these typical properties of metals in a little more detail