Which rule predicts preferred bonding patterns for many main group nonmetals?

The preferred bonding patterns for many main group nonmetals are predicted by the octet rule. This rule states that atoms tend to form bonds in such a way that they achieve a full valence shell, typically consisting of eight electrons. This arrangement mimics the electron configuration of noble gases, which are particularly stable due to their filled valence electron shells.

In forming chemical bonds, nonmetals often share, gain, or lose electrons in order to achieve this octet, thus leading to the formation of molecules or ions with stable configurations. For example, in covalent bonding, two nonmetals can share pairs of electrons, allowing each to effectively "count" the shared electrons towards their own octet.

While the duet rule applies to certain elements like hydrogen and helium, which are stable with just two electrons, it is primarily the octet rule that guides the bonding behavior of a majority of nonmetals in the main group of the periodic table. The valence shell electron pair repulsion theory relates more to the shapes of molecules rather than predicting bonding patterns, and the Pauli exclusion principle addresses electron spin within an atom, which is not directly connected to bonding patterns. Therefore, the octet rule is the most relevant principle for understanding the preferred