Chemistry - CHEMICAL BONDING Question with Solution | TestHub
Which of the following species have all bonds are identical?
Options:
Answer:
Solution:
To determine which species has all identical bonds, we need to analyze their VSEPR geometries and hybridization.
A. SF₄: Sulfur has 6 valence electrons. With 4 F atoms, there are 4 bonding pairs and 1 lone pair. The steric number is 5, leading to a trigonal bipyramidal electron geometry. The lone pair occupies an equatorial position, resulting in a seesaw molecular geometry. In a seesaw geometry, axial and equatorial bonds are not identical.
B. XeF₅⁻: Xenon has 8 valence electrons. With 5 F atoms and a -1 charge, there are 5 bonding pairs and 2 lone pairs ( electrons, pairs). The steric number is 7, leading to a pentagonal bipyramidal electron geometry. The two lone pairs occupy axial positions, resulting in a square planar molecular geometry. In a square planar geometry, all Xe-F bonds are identical.
C. XeF₅⁺: Xenon has 8 valence electrons. With 5 F atoms and a +1 charge, there are 5 bonding pairs and 1 lone pair ( electrons, pairs). The steric number is 6, leading to an octahedral electron geometry. The lone pair occupies one position, resulting in a square pyramidal molecular geometry. In a square pyramidal geometry, the apical bond is different from the basal bonds.
D. BrF₃: Bromine has 7 valence electrons. With 3 F atoms, there are 3 bonding pairs and 2 lone pairs. The steric number is 5, leading to a trigonal bipyramidal electron geometry. The two lone pairs occupy equatorial positions, resulting in a T-shaped molecular geometry. In a T-shaped geometry, the axial and equatorial bonds are not identical.
Therefore, only XeF₅⁻ has all identical bonds due to its square planar molecular geometry.
The final answer is .