Atomic Stability and Bonding Rules
📌 Atoms (excluding hydrogen) aim to have eight electrons in their outer shell to achieve chemical stability, known as the Octet Rule.
⚛️ Atoms achieve the Octet Rule by giving up, accepting, or sharing electrons when forming compounds.

Covalent Bonding
🔗 A covalent bond occurs when atoms share electrons to satisfy the octet rule.
🧪 Carbon atoms, having four outer electrons, can share with other atoms (like four hydrogen atoms to form methane) to achieve a stable octet for carbon and a stable two-electron configuration for hydrogen.

Ionic Bonding
⚡ An ionic bond forms due to the attraction between opposite charges resulting from electron transfer.
➕ Sodium (Na) tends to give up one electron, resulting in a slightly positive charge ($\text{Na}^+$), and thus achieving an octet in its remaining outer shell.
➖ Chlorine (Cl), possessing seven outer electrons, tends to gain one electron to complete its octet, becoming slightly negative ($\text{Cl}^-$).
🧂 The attraction between the resulting positive sodium ion and negative chlorine ion forms sodium chloride ($\text{NaCl}$), commonly known as table salt.

Key Points & Insights
➡️ The Octet Rule dictates that most atoms strive for eight valence electrons for maximum stability.
➡️ Covalent bonds involve sharing electrons (e.g., in the sharing between Carbon and Hydrogen).
➡️ Ionic bonds result from the transfer of electrons, creating charged particles called ions that attract each other.

📸 Video summarized with SummaryTube.com on Jan 08, 2026, 11:49 UTC