A full valence shell means that an atom has achieved a stable electron configuration, as it has filled all of its available valence orbitals. This results in a more energetically favorable state for the atom, making it more stable.
The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a full outer shell with eight electrons. This is because a full outer shell is more stable, and thus following the octet rule helps to increase stability in atoms.
When an atom gains or loses electrons, its valence shell may become more or less full. This can result in a more stable or less stable electron configuration, depending on the specific atom and its position on the periodic table.
Yes, the stability of a full valence shell can be influenced by external factors such as electronegativity of surrounding atoms, applied electric fields, and temperature. These factors can impact the arrangement of electrons and thus the stability of an atom's valence shell.
The stability of a full valence shell is a key factor in chemical bonding. Atoms with incomplete valence shells are more likely to form chemical bonds in order to achieve a full valence shell, resulting in increased stability. This is seen in both ionic and covalent bonding.