Chemical Structures
Ionic compounds are formed due to the electrostatic
attraction between oppositely charged ion. Ionic compounds consist of
- A metal (an element on the lower left side of the periodic table), which loses one or more electrons to become a positively charged ion (cation) and
- A non-metal (an element on the upper right side of the periodic table), which gains one or more electrons to become a negatively charged ion (anion).
The charge of many elements can be predicted based on their
position on the periodic table.
Ionic compounds differ from molecular compounds in several important
ways. For example,
- Ionic compounds typically have higher melting points.
- Ionic compounds are typically found as crystalline materials.
- Ionic compounds often dissolve in water.
- Solutions of ionic compounds in water conduct electricity.
- Ionic compounds do not form discrete molecules (see below).
Table Salt, NaCl
Many of the most important features of ionic compounds can be illustrated
using NaCl as an example. This compound contains the metal sodium (Na) and
the non-metal chlorine (Cl). In ionic compounds, the charges of Na and Cl can
be determined by referring to the periodic table (see above), giving:
- Sodium loses one electron to become Na+1
- Chlorine gains one electron to become Ca-1
Atoms are incredibly small. In order for a compound to exist as a stable
solid, the total charge must be zero. (Otherwise, the incredible number of
charges would give rise to a huge electrostatic repulsive force, which would
tear the material apart). In sodium chloride, the +1 charge on the sodium ion
is exactly balanced by the -1 charge on the chloride.
The simplest picture of NaCl is a single pair of Na+1 and
Cl-1 ions as shown below. However, this diagram suggests that each
Na ion is only attached to or surrounded by a single chloride (and vice
versa), which is not correct.
A more realistic picture of NaCl can be drawn be imagining that a sodium ion
is placed on a flat surface. This ion can then be surrounded by four (4)
chloride ions. In turn, each of these chloride ions, is surrounded by four
sodium ions. This process can be repeated in two-dimensions as long as ions
remain. A small sample of this could look like is shown in the
two-dimensional drawing shown below.
However, molecules are not really 'flat' but instead exist in
three-dimensions. In ions are placed above and below the layers shown above,
a 'three-dimensional' image can be drawn. This image reflects that
crystalline structure of sodium chloride.
Note that each layer is 'offset' so that Na+1 ions are not placed
on top of each other, but are placed over (or below) Cl-1
ions.
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