Question
Polarity of BF4-
Answers
GPT-4o mini
The ion \( \text{BF}_4^- \) (tetrafluoroborate) has a symmetrical tetrahedral molecular geometry due to the arrangement of the four fluorine atoms around the boron atom. As a result of this symmetry, the individual bond dipoles cancel each other out.
Since the molecule has an even distribution of charge and a symmetrical shape, \( \text{BF}_4^- \) is considered nonpolar despite the presence of polar bonds (the B-F bonds). Thus, \( \text{BF}_4^- \) is a nonpolar ion.
In summary, the polarity of \( \text{BF}_4^- \) is nonpolar.
Since the molecule has an even distribution of charge and a symmetrical shape, \( \text{BF}_4^- \) is considered nonpolar despite the presence of polar bonds (the B-F bonds). Thus, \( \text{BF}_4^- \) is a nonpolar ion.
In summary, the polarity of \( \text{BF}_4^- \) is nonpolar.