Ionic Bonding and Electron Transfer

Metals have low ionization energies, making electron loss easier to achieve a stable octet configuration. Nonmetals have high electron affinities and readily accept electrons to complete their valence shells. This electron transfer between oppositely charged ions creates strong electrostatic attractions that form ionic bonds, lowering the overall potential energy of the system.

Use the Lewis model to determine how many electrons each atom must lose or gain to reach a stable octet. The cation loses valence electrons while the anion gains them. The formula reflects the simplest ratio ensuring equal positive and negative charges. For example, strontium loses two electrons and chlorine gains one, creating the 1:2 ratio in strontium chloride.

Ionic compounds form hard, well-defined three-dimensional crystal lattice structures due to strong electrostatic attraction between oppositely charged ions. The attractive forces are isotropic, meaning each ion is equally attracted to all nearby ions of opposite charge. This regular arrangement results in high melting points and brittleness characteristic of ionic solids.

S-block metals on the left side of the periodic table have low ionization energies and readily form cations by losing electrons. P-block nonmetals in the upper-right corner have high electron affinities and readily form anions by gaining electrons. This periodic trend reflects the ease of electron transfer needed to achieve stable electron configurations.

In solid ionic compounds, strong electrostatic forces hold ions in fixed positions within the crystal lattice, preventing free movement. When melted or dissolved in water, ions can move freely through the liquid, allowing electrical current to flow. This mobility of charged particles makes molten and aqueous ionic solutions excellent conductors of electricity.

Coulomb's law describes the electrostatic force of attraction between oppositely charged ions. The force is proportional to the product of the charges and inversely proportional to the distance between them. In ionic compounds like lithium fluoride, this law explains why the positively charged lithium cation and negatively charged fluoride anion attract each other strongly to form a stable neutral compound.

Transition metal cations typically have 2+ or 3+ charges resulting from loss of outermost s electrons first, followed by d electrons from the next-to-outermost shell. Main group elements lose all valence electrons to achieve a noble gas configuration. This difference occurs because transition metals have accessible d orbitals, allowing variable oxidation states unlike main group elements.