The table shows electrical conductivity values for the elements sodium to argon, relative to aluminium (which I have set at 1).
| Element | Symbol | Atomic number | Electrical conductivity |
|---|---|---|---|
| Sodium | Na | 11 | 0.55 |
| Magnesium | Mg | 12 | 0.61 |
| Aluminium | Al | 13 | 1 |
| Silicon | Si | 14 | 0.10 |
| Phosphorus | P | 15 | 0 |
| Sulfur | S | 16 | 0 |
| Chlorine | Cl | 17 | 0 |
| Argon | Ar | 18 | 0 |
Substances conduct electricity if they contain charged particles that can move from place to place when a potential difference is applied.
The table below gives some information about different substances.
| Type of substance | Notes |
|---|---|
| Metal | Conduct when solid or liquid |
| Covalent substance | Do not conduct (graphite is an exception) |
| Ionic compound | Conduct when dissolved or when liquid |
The graph shows how electrical conductivity varies across period 3.
There is a lot going on in this graph, so it is often easier to divide it into three sections. The table below gives a brief summary of these sections.
| Element(s) | Type of element | Type of structure | Description |
|---|---|---|---|
| Na, Mg, Al | Metal | Metallic | Conductivity increases from Na to Al |
| Si | Metalloid | Giant covalent | Conductivity much less than Na, Mg and Al |
| P, S, Cl, Ar | Non-metal | Simple molecular (Ar is monatomic) | Do not conduct electricity |
When you click on the download symbol, you will be able to download the graph as an image file or pdf file, save its data, annotate it, and print it.
Sodium, magnesium and aluminium are all metals. They have metallic bonding, in which the nuclei of metal atoms are attracted to delocalised electrons.
Going from sodium to aluminium:
Metallic bonding is often described as the attraction between positive metal ions and delocalised electrons. This is incorrect because metals still consist of atoms, but the outer electrons are delocalised and are free to move through the structure.
Silicon has a giant covalent structure. It is a semiconductor, so it is not a good conductor or a good insulator.
The giant lattice structure of silicon is similar to that of diamond. Each silicon atom is covalently bonded to four other silicon atoms in a tetrahedral arrangement.
The remaining elements in period 3 do not conduct electricity. They have no free electrons that can move around and carry charge from place to place.
The atoms in molecules of phosphorus, sulfur or chlorine are attracted to each other by covalent bonds.
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