Atoms strive to achieve a stable configuration of eight valence electrons by gaining, losing, or sharing electrons, as defined by the octet rule.
In the case of \( SF_6 \), sulfur accommodates twelve valence electrons by forming six bonds, thereby exceeding the octet rule: \[ \text{Valence electrons of S} = 6 + 6(1) = 12. \]
Comparison: Molecules such as \( H_2O \), \( CO_2 \), and \( CH_4 \) adhere to the octet rule. Conversely, \( SF_6 \) violates the octet rule due to its expanded valence shell.
The interhalogen compound formed from the reaction of bromine with excess of fluorine is a :