Answer
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The boron trifluoride (BF3) molecule does not follow the octet rule due to the formal charge considerations.
The octet rule states that atoms tend to form stable compounds by attaining a full valence electron configuration of eight electrons. However, in the case of BF3, the boron atom has only six valence electrons, which is less than the preferred octet configuration.
Formal charge is a concept used to determine the distribution of electrons in a molecule. It is calculated as follows:
Formal charge = Valence electrons - Nonbonding electrons - (1/2) × Bonding electrons
For the boron atom in BF3, the formal charge calculation is:
Formal charge (B) = 3 (valence electrons) - 0 (nonbonding electrons) - (1/2) × 6 (bonding electrons)
Formal charge (B) = 0
This means that the boron atom in BF3 has a formal charge of 0, which is lower than the preferred octet configuration. The molecule is stable because the formal charge is minimized, and the overall electronic configuration is more favorable than the octet rule.
