The reason behind this is that the polarity of XeF4 can be quite confusing, as some of its properties can be polar or nonpolar. XeF4 is a chemical compound composed of a Xenon atom and Fluorine atoms. XeF4 is widely used to degrade silicone rubber because XeF4 leaves a residue of metal impurities.
There are twelve atoms in the central Xe atom, wherein the eight atoms share the four Fluorine bonds. The two lone pairs of electrons, on the other hand, are nonbonding electrons. The central atom Xenon is bonded chemically with four fluorine atoms creating a square planar molecular geometry [1].
Although the individual Xe-F are polar, the Xenon Tetrafluoride is a nonpolar molecule because it cancels each other, making the net dipole moment zero.
There are four Xe-F bonds, and each has individual bond dipoles with direction and magnitude. Since it creates molecules in a symmetrical shape, XeF4 is nonpolar. The chemical compound Xenon Tetrafluoride forms when a Xenon as the central atom reacts with Fluorine atoms.
When the four electrons bond with the half-filled orbitals, it is placed on either side of the atom. There will be octahedral geometry of the molecule when the hybridization of Xenon and Fluorine takes place. The Xe valence shell consists of six electrons in 5p orbital and two electrons in 5s.
When the two electrons in the excited state fill the vacancies, there will be sp2d2 hybridization. There are a total of 36 valence electrons in XeF4. Because the central Xenon atom has two lone pairs of valence electrons of a molecule, the molecular geometry will help with the repulsion. The two pairs, which are nonbonding pairs, will be in a perpendicular plane to maintain minimal repulsion.
There are no electrons in d-orbitals and f-orbitals in the ground state of Xenon. But when this atom is in an excited state, two electrons in the p-orbitals move to d-orbitals; as a result, there are four unpaired electrons in total. Out of which, two are in p-orbitals, and the other two unpaired electrons are in d-orbitals.
These hybridized orbitals lead to sp3d2 hybridization in XeF4. It is easier to understand the molecular geometry of a given molecule once we know its Lewis structure. As Xenon has two lone pairs of electrons, it will take up a structure that helps these lone pairs avoid the repulsion forces. To keep these repulsions at a minimum, the lone pairs will be in a perpendicular plane. And as there are four fluorine atoms, the molecule will have an arrangement such that its molecular geometry is square planar.
XeF4 has an electronic geometry of octahedral, making the molecular geometry of Xenon Tetrafluoride square planar. The bond angles of F-Xe-F are 90 degrees, and lone pairs have angles of degrees. These bond angles contribute to the formation of square planar molecular geometry.
Although the bonds between Xenon and Fluorine atoms are polar , XeF4 is a nonpolar molecule. Wondering how? All the Xe-F bonds are in opposition with each other mutually, making the sum of dipole moment zero.
As there are four electrons on the Xenon atom, which are localized as nonbonding pairs of electrons. As the overall arrangement of the atoms and electrons in the molecule is such that the vector sum of the dipoles is zero, XeF4 is a nonpolar molecule. Xenon Tetrafluoride is one of those molecules that is relatively easy to understand. Its Lewis structure is one of the least complicated structures, as all the Fluorine atoms are arranged in the symmetric pattern. The lone pairs in the molecule are located in a perpendicular plane in an octahedral shape to keep their repulsive forces at a minimum.
To summarize this blog post, we can say that XeF4 has 36 valence electrons. In XeF4, there are four fluorine atoms are bonded with a central xenon atom.
Also, there are two lone pair of nonbonding electrons are localized on the central Xe atom. The Xe-F bonds are polar as the electronegativity difference between xenon 2. But we know molecular polarity is a vector quantity which means net polarity is the vector sum of individual bond dipoles. The molecule is symmetrical so that all the Xe-F bond dipoles are opposing each other, as a result, the net dipole charge becomes zero.
And there is not any dipole charge presence on the molecule which makes XeF4 a nonpolar molecule. These are some of the major factors which are used to determine the polarity of the compounds:. Electronegativity is a kind of force exerted by atoms on their bonding partners at the time of bond formation. All the atoms have their own electronegativity value which varies from atom to atom.
Some have higher EN value and some have lower EN value. The atoms having higher electronegativity value attract the electrons pair from the bonding partners. It means higher the electronegativity difference between atoms, the more uneven sharing of electrons takes place.
In the periodic table, the fluorine F atom has the highest electronegativity value of 4. In the XeF4 compound, the electronegativity difference between fluorine 4. The central atom of XeF4 Xe has a total of 12 electrons localized in the form of 8 as Xe-F bonding and 4 as non-bonding pairs.
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