Final answer:
Common ions form by losing or gaining electrons, impacting chemical bonding and reactivity. Ionic bonds involve transfer of electrons and attraction of opposite charges, while covalent bonds involve sharing electrons to achieve stability. This knowledge is key for predicting compound formulae and understanding material properties.
Step-by-step explanation:
The charge of common ions formed by atoms contributes significantly to chemical bonding and reactivity. Atoms form ions by either losing or gaining electrons to achieve a stable electronic arrangement. Ions typically have the electronic configuration of the nearest noble gas. For elements in Groups 1A, 2A, and 3A, the loss of electrons to form cations with 1+, 2+, and 3+ charges, respectively, is a trend seen in the periodic table.
Ionic bonding occurs when oppositely charged ions attract each other to form a neutral compound. This is done through the complete transfer of electrons from one atom to another, rendering one ion positively charged (cation) and the other negatively charged (anion). In contrast, covalent bonding involves the sharing of electrons between atoms, which allows elements in group 6A, for example, to satisfy the octet rule by sharing electrons with one another, forming a stable molecule.
Understanding the common charges of ions is crucial in chemistry, especially when predicting the formulae of ionic compounds. A synthesis reaction between sodium (Na) and chlorine (Cl) for instance results in an ionic compound NaCl, because Na typically forms a Na+ ion and Cl forms a Cl- ion; their opposite charges attract and result in an ionic bond. The nature of chemical bonds greatly affects the properties and reactivity of substances.