A net charge of zero, which occurs when an atom or molecule/compound has no surplus or deficit of electrons.
An ionic bond is formed through the transfer of one or more valence electrons, typically from a metal to a non-metal, which produces a cation and an anion that are bound together by an attractive electrostatic force. On a macroscopic scale, ionic compounds, such as sodium chloride (NaCl), form a crystallinelattice and are solids at normal temperatures and pressures.
The charge on the cations and anions is determined by the number of electrons required to achieve stable noble gas electronic configurations. The ionic composition is then defined by the requirement that the resulting compound be electrically neutral overall.
For example, to combine magnesium (Mg) and bromine (Br) to get an ionic compound, we first note the electronic configurations of these atoms (valence level in indicated in italics):
In order to achieve noble gas configurations, the magnesium atom needs to lose its two valence electrons, while the bromine atom, which has 7 valence electrons, requires one additional electron to fill its outer shell. Therefore, for the resulting compound to be neutral, two bromine anions must combine with one magnesium cation to form magnesium bromide (MgBr2). In addition, though any ratio of 2 bromine atoms to 1 magnesium atom will satisfy the two requirements above, the formula for ionic compounds is typically presented as the empirical formula, or the simplest whole-number ratio of atoms with positive integers.
Note that the cation always precedes the anion both in written form and in formulas. In the written form, while the cation name is generally the same as the element, the suffix of single-atom anions is changed to -ide, as in the case of sodium chloride. If the anion is a polyatomicion, its suffix can vary, but is typically either -ate or -ite,as in the cases of sodium phosphate and calcium nitrite, depending on the identity of the ion.
lithium fluoride: Li+ and F- combine to form LiF
calcium chloride: Ca2+ and Cl- combine to form CaCl2
iron (II) oxide: Fe2+ and O2- combine to form FeO
aluminum sulfide: Al3+ and S2- combine to form Al2S3
sodium sulfate: Na+ and SO42- combine to form Na2SO4
ammonium phosphate: NH4+ and PO43- combine to form (NH4)3PO4
potassium chlorite: K+ and ClO2- combine to form KClO2