1. Gaining or Losing Electrons:
* Gaining electrons: Atoms with a high electronegativity (like nonmetals) tend to gain electrons to achieve a stable octet configuration in their outermost shell. This results in the formation of a negatively charged ion (anion).
* Losing electrons: Atoms with a low electronegativity (like metals) tend to lose electrons to achieve a stable configuration by removing electrons from their outermost shell. This results in the formation of a positively charged ion (cation).
2. Sharing Electrons:
* Covalent bonding: Atoms share electrons to achieve a stable octet configuration. This sharing results in the formation of a covalent bond, where both atoms have a shared electron pair in their outermost shell.
Example:
* Sodium (Na) has one electron in its outermost shell. When it forms an ionic bond with chlorine (Cl), it loses this electron to become a Na+ ion with a stable electron configuration like Neon (Ne).
* Chlorine (Cl) has seven electrons in its outermost shell. It gains one electron from sodium to become a Cl- ion, achieving a stable electron configuration like Argon (Ar).
Important Points:
* The change in electron configuration is driven by the desire to achieve a stable octet configuration in the outermost shell, following the octet rule.
* The type of bond formed depends on the electronegativity difference between the atoms.
* The electron configuration changes only in the outermost shell, while the inner shells remain unaffected.
Let me know if you would like to know more about specific examples or have any further questions.
