Octet rule:
The octet rule is a chemical principle that states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration resembling the noble gases. This stable electron configuration typically involves having eight valence electrons, known as the octet configuration.

Sharing or transfer of electrons:
Atoms can achieve the stable octet configuration by either sharing electrons or transferring electrons from one atom to another.

Sharing of electrons:
In covalent bonding, atoms share electrons in order to achieve a complete octet. This occurs when two non-metal atoms share electrons to fill their outer energy level. Each atom contributes one or more electrons to the shared pair, resulting in a bond.

Transfer of electrons:
In ionic bonding, electrons are transferred from one atom to another to achieve a complete octet. This occurs between a metal and a non-metal atom. The metal atom donates one or more electrons to the non-metal atom, resulting in the formation of positive and negative ions that are held together by electrostatic forces.

Importance of stable octet configuration:
The stable octet configuration is important because it represents a state of low energy and high stability for the atom. By achieving a complete octet, atoms can attain a more stable electron configuration similar to the noble gases, which have full valence shells.

Exceptions to the octet rule:
There are a few exceptions to the octet rule. Some elements, such as hydrogen (H), helium (He), lithium (Li), and beryllium (Be), can achieve stability with fewer than eight valence electrons. These elements follow the duet rule (H and He) or the triplet rule (Li and Be).

In summary, the sharing or transfer of electrons from one atom to another to attain a stable octet configuration follows the octet rule. This rule states that atoms tend to gain, lose, or share electrons in order to have eight valence electrons and achieve a stable electron configuration.