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Question

How many hybrid orbitals are present in the molecule PCl5?


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Solution

Hybridization:

  • Hybridization is known as the concept of mixing two atomic orbitals of comparable energies to give rise to a new set of types of hybridized orbitals.
  • This intermixing generally results in the formation of hybrid orbitals having entirely different energies, shapes, etc.
  • Basically, these hybrid orbitals are quite useful in explaining atomic bonding properties and molecular geometry.

Hybrid orbitals for the molecule PCl5:

  • Hybridization is known as the process of mixing atomic orbitals of similar energy to generate a new set of orbitals.
  • In the case of the given molecule PCl5 ; the P atom requires five orbitals to form the five P-Cl bonds.
  • The outermost valence shell electronic configuration of P in the ground state is given as =3s23p3.
  • Here, the P atom has only one 3s orbital and three 3p orbitals, therefore it uses one of its 3d orbitals to form the fifth bond.
  • Hence, the electronic configuration of P in the excited state is given as =3s13p33d1
  • These five mentioned orbitals are hybridized to form five sp3d orbitals and form a trigonal bipyramid geometry given as;

Overlap

  • Here, 3 hybrid orbitals directed towards the corners of an equilateral triangle are called equatorial hybrid orbitals which are planar and have a bond angle of 120°.
  • Whereas the 2 hybrid orbitals which are perpendicular to the plane of the equatorial hybrid orbital are called axial hybrid orbitals and form a 90° angle with the equatorial hybrid orbitals.

Hence, hybrid orbitals are present in the molecule PCl5, are five sp3d orbitals that generate the trigonal bipyramid geometry.


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