The positive metal ions and the negative ions produced when metals and non-metals react to form an ionic compound will be attracted to each other and pack as closely together as possible in a regular way. Structures with regular arrangements of atoms or ions are often referred to as being crystalline. The electrostatic attraction of positive and negative ions is called an ionic bond. Ionic compounds consist of a giant structure made of these ions. These giant structures of ions are often referred to as an ionic lattice. The smaller the ions and the more highly charged they are will mean that they can pack together more closely and form a stronger ionic bond. Sodium chloride is an ionic compound formed when sodium; a group I metal reacts with the halogen chlorine. Sodium will form an ion with a +1 charge. Chlorine a group 7 halogen will form an ion with a -1 charge. If you look at grains of sodium chloride, an ionic compound under the microscope you will see that they have a cubic shape. The image below shows the structure of the sodium chloride lattice. The green spheres represent chloride ions (Cl-) and the blue spheres sodium ions (Na+).
If you were to count the ions in the model you would notice that
there are equal numbers of sodium ions, Na+, and
chloride ions, Cl-. This is simply because when the ions pack together they do in
such a way that the charges always
cancel out. The +1 charge on the sodium ion is cancelled out by the -1 charge on th
chloride ion. So the ratio of
the ions is 1:1. This simple ratio of ions enables you to calculate the empirical (simplest) formula for the compound.
So in the case of sodium chloride it is NaCl. Its ionic formula is Na+Cl-.
You will often see the lattice structure for ionic compounds shown in different ways. This is to try and help you visualize what the giant structure looks like. Opposite is shown the cubic lattice for sodium chloride (Cl- shown in green, Na+ is a yellow/green colour), but this time there are bonds shown between the ions. In reality there would be no gaps between the ions as they will pack together as closely as possible but it does allow you to view the interior of the structure which is not possible from the first model. Both model allow you to visualize how the ions are arranged in the structure.
None of the models for sodium chloride shown allow
you to spot immediately how the crystal structure is built. If
you pick out one sodium ion you should see that it has six immediate neighbours. One
chloride above it and one below,
one to its left and one to its right and one in front and one behind. This is shown opposite. The same is true if you
pick a chloride ion. Each sodium or chloride
ion has 6 immediate neighbours, the ions are described as 6 co-ordinate.
All ionic compounds have a giant lattice structure made up of ions. However not all ionic lattices have a face centred cubic structure like sodium chloride. Remember the ions will always try and pack together as closely as possible, but in a way that maximises the attraction between oppositely charged ions and reduces the repulsion between ions of a similar charge. However the different size of the ions in the compound will limit how closely they can pack together to maximise attractions and reduce repulsion.
Caesium like sodium is an alkali metal, however caesium being in period 6 is a much larger atom than sodium.
Caesium like sodium has one outer shell valency electron and so will form an ion with a 1+ charge, Cs+. This means that
caesium chloride will have the formula CsCl where the caesium and chloride ions are in the ratio of 1:1,
exactly the same as sodium chloride, NaCl. However caesium chloride has a different lattice structure from NaCl. The larger caesium
ion allows 8 chloride ions to fit around it, that is its coordination number is 8, compared to 6 with sodium chloride.
This is shown opposite:
Note that in the cell shown for both the NaCl and the CsCl lattice the metal ion is shown at the centre with the chloride ions surrounding it, to visualise the coordination number for chloride ion simply swap the position of the metal and the chloride ions around, put the chloride ion at the centre of the cell with the metal ions around it!
In caesium chloride you can visualise the caesium ions at the centre of a box with the chloride ions at the corner of this box. This type of structure is often referred to as body centred cubic (bcc). The coordination number for both the chloride and caesium ions is 8, this may be easier to visualise in the image below which shows a number of the CsCl cells that link to form part of the lattice structure for CsCl. The coordination number for each ion in the crystal must be the same since the ions are present in the ratio of 1:1.
The image below shows ball and stick models for the structure of the calcium fluoride lattice. Clearly it is not cubic like the sodium chloride lattice because the ions are different in size and charge. In the models the red ions are Ca2+ and the blue ions are F-.
|Group ion||Elements present||Charge||Formula|
When working out the formula of compounds containing these ions we just use the same rules as before e.g.
|Swap over the valencies||2||1|
|The ionic formula is simply the formula with the charges on the ions present. The charges on the ions are simply the number of electrons lost or gained when the element reacts. This is the same as its valency and for group ions it is probably easiest if you simply memorise the formula for these ions!|
|Ionic formula formula||Na2+SO42-|
|Swap over the valencies||1||2|
|When writing out the formula for calcium nitrate the calcium ions and nitrate ions are in the ratio of 1:2. The brackets are required around the nitrate simply because if they are omitted then we have NO32, which reads as 1 nitrogen and 32 oxygens, which is obviously not what we want.|
|Ionic formula formula||Ca(NO3)2-|