Question

Identify the following species in which $d^2sp^3$ hybridization is shown by the central atom.

• A. [Co(NH3)6]3+
• B. SF6
• C. BrF5
• D. [PtCl4]2-

Answer 1

Answer: (A)

[Co(NH3)6]3+

Answer 2

$[ \text{Co(NH}_3)_6 ]^{3+}$ exhibits $d^2sp^3$ hybridization as it forms an octahedral geometry. In this complex, the central cobalt ion uses two $d$ orbitals, one $s$ orbital, and three $p$ orbitals to form six coordinate bonds with ammonia molecules.

For $\text{BrF}_5$, the central bromine atom exhibits $sp^3d^2$ hybridization, resulting in a square pyramidal structure.

In $[ \text{PtCl}_4 ]^{2-}$, platinum shows $dsp^2$ hybridization, resulting in a square planar geometry.

$\text{SF}_6$ involves $sp^3d^2$ hybridization, resulting in an octahedral geometry around the sulfur atom.

Thus, the correct species showing $d^2sp^3$ hybridization is $[ \text{Co(NH}_3)_6 ]^{3+}$.

The correct option is (C) :[Co(NH3)6]3+