Is Cl2XeF2 polar or nonpolar? - Polarity of XeCl2F2
The question is –
Is Cl2XeF2 polar or non-polar?
Answer:
⇒ Cis- Cl2XeF2 is polar while trans-Cl2XeF2 is a non-polar molecule.
Explanation:
The polarity of Cl2XeF2 or XeCl2F2 depends on the arrangement of two chlorine (Cl) and two fluorine (F) atoms around the central xenon (Xe) atom.
Cis-trans isomerism exists in this molecule. In the cis-form, two Cl and two F-atoms are each present on the same side of the molecule.
Contrarily, in trans-Cl2XeF2, two Cl-atoms and two F-atoms each occupy the opposite sides of the molecule, a complementary pair facing each other.
Each Xe-Cl and Xe-F bond is individually polar owing to an electronegativity difference of 0.56 units and 1.38 units, respectively, between the bonded atoms.
Each of the Cl and F-atoms thus gains partial negative charges (δ–) while the central Xe-atom attains a partial positive charge (δ+) in the Cl2XeF2 molecule.
The Cl2XeF2 molecule possesses a square planar geometry. 2 lone pairs of electrons surround the central Xe-atom, one on each side of the molecule, which leads to an overall symmetrical shape.
The individual Xe-Cl and Xe-F dipole moments get canceled in opposite directions in the trans-form. Thus trans-Cl2XeF2 is overall non-polar (net µ = 0).
In contrast, the stronger Xe-F dipole moment does not get canceled with the oppositely-facing Xe-Cl dipole moment in the cis-form of Cl2XeF2.
The charged electron cloud stays non-uniformly distributed. Consequently, cis-Cl2XeF2 is overall polar (net µ > 0).
⇒ How to know if a compound is polar or nonpolar?
FAQ
Is Cl2XeF2 or XeCl2F2 polar or nonpolar? |
The overall polarity of Cl2XeF2 depends on the arrangement of its atoms. The trans-form of the Cl2XeF2 or XeCl2F2 is non-polar (net µ = 0) due to the cancellation of the individual Xe-Cl and Xe-F dipole moments in opposite directions. In contrast, the cis-form of Cl2XeF2 or XeCl2F2 is polar (net µ > 0) due to the stronger Xe-F dipole moment not getting canceled with the oppositely-facing Xe-Cl dipole moment. |
What is the geometry of Cl2XeF2? |
Cl2XeF2 has a square planar geometry, meaning that the molecule is shaped like a square and all the atoms lie in the same plane. The central Xe-atom is surrounded by two lone pairs of electrons, one on each side of the molecule, which contributes to its symmetrical shape. |
What causes the polarity of Cl2XeF2? |
The polarity of Cl2XeF2 is caused by the electronegativity differences between the bonded atoms (Xe, Cl, and F). Each Xe-Cl and Xe-F bond is individually polar, with the Cl and F-atoms gaining partial negative charges (δ–) and the central Xe-atom attaining a partial positive charge (δ+). This uneven distribution of charge creates a dipole moment, which results in the overall polarity of the molecule. |
What is the difference between cis- and trans-Cl2XeF2? |
The difference between cis- and trans-Cl2XeF2 lies in the arrangement of the Cl and F-atoms around the central Xe-atom. In the cis-form, two Cl and two F-atoms are each present on the same side of the molecule. In contrast, in trans-Cl2XeF2, two Cl-atoms and two F-atoms each occupy opposite sides of the molecule, facing each other in a complementary pair. This difference in arrangement determines the net polarity of the molecule, with cis-Cl2XeF2 being polar and trans-Cl2XeF2 being non-polar. |
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