According to VSEPR theory, how should the molecular shape of AsF3 be classified?

Question

(1 point)
Responses

tetrahedral, because the arsenic atom forms bonds with the three atoms and the lone pair
tetrahedral, because the arsenic atom forms bonds with the three atoms and the lone pair

trigonal planar, because the arsenic atom forms three single covalent bonds and has no lone pairs
trigonal planar, because the arsenic atom forms three single covalent bonds and has no lone pairs

linear, because the arsenic atom forms bonds with only one other type of atom
linear, because the arsenic atom forms bonds with only one other type of atom

trigonal pyramidal, because the arsenic atom forms three single covalent bonds and has one lone pair
trigonal pyramidal, because the arsenic atom forms three single covalent bonds and has one lone pair

Answer 1

According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the molecular shape of AsF3 should be classified as trigonal pyramidal, because the arsenic atom forms three single covalent bonds with fluorine atoms and has one lone pair of electrons. This lone pair affects the geometry of the molecule, resulting in a trigonal pyramidal shape rather than a tetrahedral one.

So the correct response is:

trigonal pyramidal, because the arsenic atom forms three single covalent bonds and has one lone pair.