In which of the following molecules/ions, all bonds are equal?

Since ${\mathrm{XeF}}_4$  both$Xe$ and F are non-metal atoms, therefore the compound formed between them is considered as a covalent compound.

In ${\mathrm{BF}}_4^{-}$ , the B atom has 4 valence electrons all of which are involved in the formation of bonds with four F atoms. Hence, no lone pairs are present.

In this article, we are going to discuss the chemical bonding of silicon tetrafluoride by understanding its Lewis structure, molecular geometry, and the hybridization of the central atom. Then, we will study the polarity of ${\mathrm{SiF}}_4$ i.e., whether ${\mathrm{SiF}}_4$ is a polar or nonpolar molecule.