Hybridization of XeF4

The term ‘Hybridization’ refers to the formation of newly hybridized orbitals by fusing the atomic orbitals. On the other hand, these newly formed hybridized orbitals affect molecular geometry and bonding properties. 

Also, the process of hybridization is the development of the valence bond theory. For exploring this knowledge in advance, we will apply three kinds of hydrocarbon compounds to explain sp³, sp², and sp hybridization.

As we know, in the case of XeF₄ or xenon tetrafluoride, the hybridization of xeof₄ occurs in the central atom, which is Xenon (Xe). In this case, if we gaze upon the valence shell of Xe, the total amount of electrons is six in the 5p orbital as well as two electrons in the 5s orbital. 

Let’s keep an observation on the 5th orbital; we will find that some of the orbitals such as d orbital and f orbital exist which possess no electrons. 

There are two 5p orbital electrons present. We can say that these orbitals are in an excited state. These orbitals transfer to complete the empty 5d orbitals in the process of making the XeF₄. 

This results in 4 unpaired hybridized electrons which consist of 2 in 5p and 2 in 5d orbitals. So, finally, we get the actual orbital used in XeF₄ development, and it results in sp²d² hybridization.

But if we consider fluorine, there are four F atoms combined with these four half-filled orbitals. The placement of the fluorine atoms will then be on both sides of the central atom.

Hybridization of XeOF₄

Do you know about the hybridization of XeOF₄? As we discussed earlier, the concept is the same. The s-orbital is used by the central atom as usual and the mixing of the p-orbitals as well as the rest of the d-orbitals together to create the hybrid orbitals.

Thus, in the case of XeOF₄ formation, s orbital will be needed for Xe along with its three p-orbitals as well as 2d-orbitals. So, sp³d² or d²sp³ will be its hybridization state.

The Brief Details of Xeof₄ Hybridization are Given in the Table Below.

XeF₄ consists of two lone pair electrons. Let’s consider the VSEPR theory, which says that there is a repulsion experienced between the bond pair electrons and lone pair electrons. 

(Image will be uploaded Soon)

With the help of the structure, they will obtain a stable state. The sole pairs of Xenon stay in the vertical surface in an octahedral arrangement. This is the reason behind the square planar geometry for the XeF₄ molecule.

The angles of the bond are 90^o or 180°. The singular couples stay on the contrary sides of the molecule fundamentally at 180° from each other.

Xeof₄ Structure Hybridization

• The geometry of Xeof₄ is square pyramidal. 

• As we have learned before the s-orbital will be used by the central atom, the hybrid orbitals will be mixed via its p-orbitals along with its d-orbitals as much as available. 

• Xenon will require its s orbital along with its p-orbitals which are three in number, and 2 of its d-orbitals to form the hybridization state as sp³d², or d²sp³.

Iodine Pentafluoride Hybridization

By adding the number of σ-bonds designed by the chosen atom (in this case ‘I’) and the lone pair’s number on it, we can simply distinguish the hybridization of it.

• If the addition is 2 → hybridization−sp

• If the addition is 3 → hybridization−sp²

• If the addition is 4 → hybridization−sp³

• If the addition is 5 → hybridization−sp³d

• If the addition is 6 → hybridization−sp³d²

Reviewing the Lewis structure of IF5

(Image will be uploaded Soon)

In this case, 5 sigma bonds and 1 lone pair of electrons is possessed by the IF5. That’s why the sum is 6. So, the hybridization of it is sp³d². We can also observe the hybridization process of IF5 in this picture.

(Image will be uploaded Soon)

Yes, this is known as iodine pentafluoride. It is a wonderful illustration of a molecule that doesn't satisfy the simple Lewis theory. 

Sometimes you will discover that this is the case for weightier elements frequently, where the electrons from numerous subshells can donate to the bonding.

Well here in iodine, the subshells such as 5p and 5s and also the 4d subshells are pretty close in energy to each other, and all are valence subshells.

As such, iodine utilizes the entire electrons in chemical bonding: these are viz:

2 in the 5s, 

5 in the 5p, and 

up to 10 in the 4d, even if it needs only to use 4 of its 4d electrons for bonding. Therefore, it can have more than 8 electrons to be involved in its bonding process.

“sp³d² hybridized bonding” method has been used by the molecule. We can explain it simply in brief such as the iodine produces one standard covalent bond to an F-atom, four dative covalent bonds to 4 F-atoms, by keeping one lone pair as of its remaining.

Xef₅ Hybridization

Do you know certain facts regarding Xef₅ hybridization? 

Central atom: Xe whose configuration is 5s² 5p⁶

Number of valence electrons: 8 

Number of BP = 5 

Number of lone LP = 2 

Number of e-pairs = BP + LP = 5 + 2 =7 

Hybridization: sp³d³ 

Electron pair geometry: Pentagonal bipyramid 

Molecular geometry:

(Image will be uploaded Soon)

Characteristics of Hybridization: 

• Ions with similar energies or configurations are hybridized.

• Hybridization takes place if the orbitals belong to the same atom. 

• The hybrid orbitals can make stronger or more stable bonds than the pure atom orbitals.

• All the hybrid orbitals are equivalent in energy and shape.

• Hybridization leads to the production of equivalent orbitals. This gives the orbitals its maximum symmetry.

• Hybridization explains the behavior of the molecule in an orbit.

Is this page helpful?